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Air Pollution Aspects of Emission Sources
SULFURIC ACID MANUFACTURING
A Bibliography with Abstracts
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U. S. ENVIRONMENTAL PROTECTION AGENCY
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AIR POLLUTION ASPECTS
OF EMISSION SOURCES:
SULFURIC ACID MANUFACTURING-
A BIBLIOGRAPHY WITH ABSTRACTS
Office of Technical Information and Publications
Air Pollution Technical Information Center
U.S. EPA-NE1C LIBRARY
Denver Federal Center
Building 25, Ent. E-3
P.O. Box 25227
Denver, CO 80225-0227
ENVIRONMENTAL PROTECTION AGENCY
Office of Air Programs
Research Triangle Park, North Carolina
May 1971
For sale by the. Superintendent of Documents, U.S. Government Printing Office, Washington, D.C. 20402 - Price Co cents
Stock Number 5503-0007
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The AP series of reports is issued by the Office of Air Programs, Environmental Protec-
tion Agency, to report the results of scientific and engineering studies, and information of
general interest in the field of air pollution. Information reported in this series includes
coverage of Air Program intramural activities and of cooperative studies conducted in con-
junction with state and local agencies, research institutes, and industrial organizations.
Copies of AP reports are available free of charge to Federal employees, current contrac-
tors and grantees, and nonprofit organizations - as supplies permit - from the Office of
Technical Information and Publications, Office of Air Programs, Environmental Protection
Agency, P.O. Box 12055, Research Triangle Park, North Carolina 27709. Other requestors
may purchase copies from the Superintendent of Documents, Washington, D. C. 20402.
Office of Air Programs Publication No. AP-95
11
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BIBLIOGRAPHIES IN THIS SERIES
r\
AP-92, Air Pollution Aspects of Emission Sources:
Municipal Incineration — A Bibliography with Abstracts
AP-93, Air Pollution Aspects of Emission Sources:
Nitric Acid Manufacturing —A Bibliography with Abstracts
AP-94, Air Pollution Aspects of Emission Sources:
Sulfuric Acid Manufacturing — A Bibliography with Abstracts
AP-95, Air Pollution Aspects of Emission Sources:
Cement Manufacturing — A Bibliography with Abstracts
AP-96, Air Pollution Aspects of Emission Sources:
Electric Power Production —A Bibliography with Abstracts
L 1 B ift A R Y
Environm^^i ;'nt^;n n-
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CONTENTS
INTRODUCTION vii
BIBLIOGRAPHY
A. Emission Sources I
B. Control Methods 5
C. Measurement Methods 26
D. Air Quality Measurements 32
E. Atmospheric Interaction 33
F. Basic Science and Technology „ 34
G. Effects - Human Health 39
H. Effects - Plants and Livestock (None)
I. Effects - Materials 41
J. Effects - Economic 42
K. Standards and Criteria 44
L. Legal and Administrative 45
M. Social Aspects (None)
N. General 47
AUTHOR INDEX 49
SUBJECT INDEX 51
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AIR POLLUTION ASPECTS
OF EMISSION SOURCES:
SULFURIC ACID MANUFACTURING-
A BIBLIOGRAPHY WITH ABSTRACTS
INTRODUCTION
Sulfuric acid manufacturing contributes significantly to the overall air pollution level
in the United States. To aid efforts to improve air quality, the Air Pollution Technical
Information Center (APTIC) of the Office of Technical Information and Publications, Office
of Air Programs has compiled this bibliography relevant to the problem and its solution.
Approximately 200 abstracts have been selectively screened from the contents of
APTIC's information storage and retrieval system to cover the 14 categories set forth in
the table of contents. The compilation is intended to be representative of available litera-
ture, and no claim is made to all-inclusiveness.
Subject and author indexes refer to the abstracts by category letter and APTIC acces-
sion number. Generally, higher accession numbers, representing the latest acquisitions,
cover the most recent material.
All documents abstracted herein are currently on file at the Air Pollution Technical
Information Center, Office of Air Programs, Environmental Protection Agency, P. O. Box
12055, Research Triangle Park, North Carolina 27709. Readers outside the Environmental
Protection Agency may seek duplicates of documents directly from libraries, publishers,
or authors.
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A. EMISSION SOURCES
02235
SULFURIC ACID MANUFACTURE, REPORT NO. 2. J. Air
Pollution Control Assoc. 13, (10) 499-502, Oct. 1963.
This report, published as Informative Rpt. No. 2 of the Air
Pollution Control Association's TI-2 Chemical Committee, rr-
presents the 'best thinking of the Association' on the subject
of Sulfuric Acid Manufacture. Of all the chemicals made in
the U.S., sulfuric acid is probably produced in the greatest
quantity. In 1961 the U.S. Department of Commerce reported
production of 17,847,812 short tons. Inasmuch as one ton of
sulfur produces nearly three tons of sulfuric acid, the large
proportion coming from sulfur is apparent. The following
processes are reviewed in regard to operations and air pollu-
tion aspects: Contact Process, Chamber Process, Acid
Recovery Processes.
04946
A. F. Snowball
DEVELOPMENT OF AN AIR POLLUTION CONTROL PRO-
GRAM AT COMINCO'S KIMBERLEY OPERATION. J. Air
Pollution Control Assoc. 16, (2) 59-62, Feb. 1966.
During the concentration of lead and zinc sulfides from
Cominco's Sullivan Mine at Kimberley, British Columbia,
there is also produced an iron sulfide concentrate as a
byproduct. A portion of these iron concentrates is roasted and
the resulting calcine is treated in electric furnaces to produce
300 tons of pig iron per day. The sulfur dioxide produced in
the roasting process is used to make sulfuric acid which is em-
ployed in the manufacture of ammonium phosphate fertilizers.
Problems in the control of air pollution resulting from the iron
sintering, iron smelting, and fertilizer operations at Kimberley
are discussed, including those arising as a result of almost con-
tinuous expansion of these facilities since their establishment
12 years ago. (Author abstract)
10749
Gobson, F. W.
NEW BUICK LEAD SMELTER INCORPORATES FORTY
YEARS OF TECHNICAL ADVANCES. Eng. and Mining J.,
169(7):62-67, July 1968.
Four significant innovations in the design and operation of
lead smelters will be combined for the first time when the new
Buick complex goes on stream this year near Bixby, Mo. The
plant, designed to produce 100,000 tpy of 99.99% lead, will
feature: updraft sintering, air pollution control through produc-
tion of sulfuric acid, continuous tapping of molten lead, and
vacuum dezincing. While none of these processes is new, this
will be the first plant to utilize all four.
12633
F. E. Ireland
POLLUTION BY OXIDES OF SULPHUR. Chem. Eng., No.
221, CE261 -262, Sept. 1968.
The sources of sulfur oxide pollution include the combustion
of sulfur-bearing fuels such as coal, coke, and fuel oil, the
manufacture of sulfuric acid, miscellaneous uses of sulfur
dioxide, and the combustion of sulfur compounds in waste
gases from manufacturing processes. This is a brief report of
these pollution sources made to the Working Party on Air Pol-
lution of the European Federation of Chemical Engineering.
12751
McKee, Arthur G. and Co., San Francisco, Calif., Western
Knapp Engineering Div.
SYSTEMS STUDY FOR CONTROL OF EMISSIONS. PRIMA-
RY NONFERROUS SMELTING INDUSTRY. (FINAL RE-
PORT). VOLUME H: APPENDICES A AND B. Contract PH
86-65-85, Rept. 993, 88p., June 1969. 72 refs. CFSTI: PB 184
885
A systems study of the primary copper, lead, and zinc smelt-
ing industries is presented to make clear the technological and
economi factors that bear on the problem of control of sulfur
oxide emissions. Sulfur oxide emissions for various types of
smelting operations are tabulated, including gas flows and
compositions and an analysis of sulfur oxides generation and
recovery. Smelter flow diagrams are presented for the control
methods of contact sulfuric acid, absorption, reduction to ele-
mental sulfur, lime wet scrubbing, and limestone wet
scrubbing. Sulfur oxide recovery processes that were in-
vestigated and rejected as not being suitable for economic
analysis are listed. Cost estimates for various control
processes are given.
12823
McKee, Arthur G. and Co., San Francisco, Calif., Western
Knapp Engineering Div.
SYSTEMS STUDY FOR CONTROL OF EMISSIONS. PRIMA-
RY NONFERROUS SMELTING INDUSTRY. (FINAL RE-
PORT). VOL I. Contract PH 86-65-85 Rept. 993, 188p., June
1969. CFSTI: PB 184 884
A systems study of the primary copper, zinc, and lead smelt-
ing industries is presented to make clear the technological and
economic factors that bear on the problem of control of sulfur
oxide emissions. The nature of smelting practice is described,
and potential air pollution problems in smelter areas are
revealed. Five processes for the control of sulfur oxides are
presented, including contact sulfuric acid, absorption, reduc-
tion to elemental sulfur, lime wet scrubbing, and limestone wet
scrubbing. Current sulfur oxide emissions from U. S. smelters
are given, and forseeabl emission trends are discussed. Mar-
kets for sulfur byproducts are mentioned, the costs of control
by available methods are tabulated, and control method
evaluation with plant models is considered. A research and
development program for control methods and smelting
process technology is recommended.
13403
Ganz, S. N., I. Y. Kuznetsov, V. A. Shlifer, and L. I. Leykin
REMOVAL OF NITROGEN OXIDES, SULFUR DIOXIDE,
AND SULFURIC ACID MIST AND SPRAY FROM INDUSTRI-
AL EXHAUST GASES USING ALKALINE PEAT SORBENTS.
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SULFURIC ACID MANUFACTURING
(Ochistka vykhlopnykh gazov ot okislov azota, semistogo
gaza, tumana i bryzg sernoy kisloty torfoshchelochynymi sor-
betami v zavodskikh usloviyakh.) Text in Russian. Zh. Prikl.
Khim., 41(4):720-725, 1968. 1 ref.
Studies on the purification of exhaust gases from the Mills-
Packard process under industrial conditions revealed that the
most effective additive to the peat sorbents was ammonia, the
sorption of gases producing a useful organomineral fertilizer.
Addition of the ammonia directly to the boiling layer of sor-
bent was the most efficient method, and three sorbent layers
were used. Successive layer thicknesses were 200-300, 300-
400, and 400-450 mm with moisture content 35-40, 40-45, and
45-55 percent, respectively. Raw material requirements for
sanitary purification of 60,000 cu m/hr are (in tons per hr):
0.294 ammonia, 1.5 dry peat, and 3 peat with 50 percent
moisture. The ton-per-hour trapping rate was: 0.318 nitrogen
oxides, 0.405 sulfur dioxide, and 0.012 sulfuric acid. Data are
given for the effectiveness of the resultant fertilizer deter-
mined from agricultural study.
13596
Cunningham, George H. and Allen C. Jephson
ELECTROLYTIC ZINC AT CORPUS CHRIST!, TEXAS.
Trans AIMEE (Am. Inst. Mining Metallurgical and Petroleum
Engrs.), Vol. 159, p. 194-209, 1944.
The design of the plant includes the use of Trail suspension
roasting equipment, contact acid equipment, and batch
leaching in mechanically agitated tanks. Pressure filtering and
washing of leach pulp and batch purification are followed by
clarification in filter presses and cooling of purified solution
by evaporation. Electrolysis is carried out in cells using Tain-
ton alloy anodes and aluminum cathodes. Cell temperatures
are held within desired limits by circulating cell solution
through cooling towers. Steam-driven generators are used to
provide direct current for electrolysis. The cathode zinc is
melted and cast into slabs for shipment. Plant roasting capaci-
ty is 140 to 240 tpd. Steam is generated in three boilers, each
with a capacity of 6000 to 12,000 Ib of steam per hr at 150 psi,
and amounts to about 0.7 Ib per Ib of concentrate roasted.
Boiler gas at 8500 to 10,500 cu ft per min and 320 C is fed to
separate cyclone units. The gas is passed from the cyclones to
two cottrell precipitators, each with a capacity of 18,500 cu ft
per min at 250 C, and on to the acid plant. The H2S04 section
consists of a standard Leonard Monsanto contact unit using
vanadium mass converters to produce 125 tons of 100% acid
daily.
13841
Lewis, W. K. and E. D. Ries
INFLUENCE OF REACTION RATE ON OPERATING CON-
DITIONS IN CONTACT SULFURIC ACID MANUFACTURE.
n. Ind. Eng. Chem., 19(7):830- 837, 1927. 7 refs.
Using the data of Knietsch, the authors had previously calcu-
lated correct operating conditions for the catalytic oxidation of
sulfur dioxide to sulfur trioxide in the presence of platinum.
Further reaction rate data were obtained under strictly isother-
mal conditions simulating plant practice. From these data, a
new equation was developed. While it does not explain the
mechanism of the reaction, it accurately predicts conversion
under any given set of circumstances. It applies equally to
SO2 and O2 runs. Optimum operating temperatures calculated
by means of the equation are found to correspond closely with
good plant practice. A comparison is made between existing
equations and the new one, and the shortcomings, both practi-
cal and theoretical, of the earlier forms are discussed in detail.
13850
Thompson, A. Paul
PLATINUM VS. VANADIUM PENTOXIDE AS CATALYSTS
FOR SULFURIC ACID MANUFACTURE. Trans. Am. Inst.
Chem. Engrs., vol. 27:264-309, Dec. 1931.
Platinum catalysts, including platinized asbestos, platinized
magnesium sulfate, and platinized silica gel, are compared
economically and technically with vanadium catalysts on the
basis of data derived from sulfuric plant operations. The
catalysts are evaluated by such factors as initial costs, cost of
catalyst per daily ton of 100% acid per year, ultimate cost,
ability to handle gas with a low oxygen to sulfur dioxide ratio,
converter space required, relationship of gas loading or space
velocity to conversion, and life expectancy. Platinized contact
masses are shown to be cheaper from every standpoint than
vanadium masses. The 1931 cost of an ounce of platinum is
only 8.57 cents per ton of acid produced. The costs for vanadi-
um masses are 2.8 to 5.1 times higher, with one vanadium
catalyst costing nearly 46 cents per ton of acid produced. With
regard to relative effectiveness, platinized catalysts have a
lower kindling temperature, a greater activity over a much
wider temperature range, and they excel in handling gases
whose sulfur dioxide content varies from time to time. Their
greater activity with gases of varying sulfur dioxide content
over broad temperature ranges simplifies converter design and
operation. Like vanadium catalysts, platinized silica gel is not
poisoned by arsenic present in the gas being treated. Addi-
tional cost and purification data on contact sulfuric acid
catalysts are given in a discussion appended to the article.
15517
Public Health Service, Washington, D. C., National Air
Pollution Control Administration
CONTROL TECHNIQUES FOR SULFUR OXIDE Affi POL-
LUTANTS. NAPCA Publ. AP-52, 122p., Jan. 1969. 274 refs.
About 75% of sulfur oxide emissions in 1966 resulted from the
combustion of sulfur-bearing fuels, with coal combustion ac-
counting for the largest part. The economic and technical
aspects of various techniques for controlling these emissions
are examined in detail; they are categorized as (1) change-over
to fuels with lower sulfur content or to another energy source,
such as hydroelectric or nuclear power; (2) desulfurization of
coal or residual fuel oil; (3) removal of sulfur oxides from flue
gas by various processes, including limestone-dolomite injec-
tion and alkalized alumina sorption; and (4) increase in com-
bustion efficiency. Of the industrial sources of SO2 emissions,
nonferrous primary smelting of sulfide-containing metallic ores
such as copper, zinc, and lead is the largest emitter. About
half of the primary smelters in the U. S. now use sulfuric acid
recovery to reduce emissions and at the same time offset
smelter operating costs. Smelters, oil refineries, pulp and
paper mills, steel plants, sulfuric acid plants, waste disposal
processes, and a number of other industrial sources are con-
sidered in terms of present technology for reducing emissions.
The costs of dispersion of sulfur oxides by tall stacks are
briefly discussed as an approach toward reducing the frequen-
cy of high concentrations at ground level in some areas, and
an extensive bibliography on gas dispersion is included. An ap-
pendix on chemical coal processing describes the current state
of development of such methods as gasification and liquefac-
tion for reducing the sulfur content of high-sulfur coal.
18305
Lindau, L.
AIR POLLUTION AND THE MANUFACTURE OF INOR-
GANIC CHEMICALS. (Luftfororening vid framstallning av
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A. EMISSION SOURCES
oorganiska baskemikalier.) Text in Swedish. Statens Natur-
vardsverk, Stockholm, Publikationer No. 4, 66p., 10 refs.
The investigation deals with air pollution problems in connec-
tion with the manufacture of basic inorganic chemicals such as
sulphuric acid, hydrochloric acid, phosphoric acid, ammonia,
nitric acid, chlorine and sodium hydroxide. The report con-
tains a survey of present conditions, an analysis of various
technical methods to reduce the emissions, and a discussion of
the economic consequences of these methods. The purpose of
the survey is to supply information to the Swedish authorities
dealing with air pollution control. The rates of emission from
the chemical plants are described as kg/ton product. The costs
of air pollution abatement vary. In certain cases, e.g., the
recovery of sulphur in connection with the production of am-
monia, the necessary investments can be written off. In other
cases, e.g., introduction of the double-contact process for the
manufacture of sulphuric acid, the increasing yield can only
partially motivate the investments required. There are also
cases when the costs entirely belong to the air pollution ac-
count. A comparison between Swedish and foreign plants in-
dicates that emissions are of the same magnitude. Essential
improvements are possible to obtain in new plants and the
latest Swedish production units have applied this to a great ex-
tent.
21221
Pels, M. and H. L. Crawford
FEASIBILITY STUDY OF CENTRALIZED AIR-POLLUTION
ABATEMENT. (FINAL REPORT). Battelle Memorial List.,
Columbus, Ohio, Columbus Labs. NAPCA Contract PH-86-68-
84, TAsk 12, 51p., Nov. 17, 1969. 35 refs. CFSTI: PB 190486
The technical and economic aspects of a centralized air-pollu-
tion control plant located a distance from seven industrial
plants were investigated. The plants chosen were as follows:
lime, 200 tons/day; cement, 4500 barrels/day; sulfuric acid, 400
ton/day; power, 25 Mw; fertilizer, 570 tons/day; gray iron,
1440 tons/day; and electric arc, 2600 tons/day. Gaseous and
particulate-emission levels were taken from literature sources,
and as far as possible, average values were used for each in-
dustry. The total amount of gases from the plants was 627,000
cfm at 320 F and after mixing. While the centralized control
facility is less expensive to build and operate than individual
control devices, transportation costs are so high as to make
the centralized concept unattractive. The economics would
favor centralized abatement only if each of the seven plants
were located at about 1/2 mile from the central facility. This
distance is considered to be unrealistically close from the
standpoint of an individual plant's land requirements. In addi-
tion to transportation costs, the centralized plant would render
emissions from lime, cement, and sulfuric acid plants value-
less, and any equipment malfunction would release large quan-
tities of pollutants over a relatively small area. Finally, vegeta-
tion growth over buried pipes would be inhibited, leading to
potential esthetic problems. (Author summary modified)
23044
Ireland, F. E.
POLLUTION BY OXIDES OF SULPHUR. Chem. Engr. (Lon-
don), 46(7): CE261-CE262, Sept. 1968.
Sulfur oxides arise from the combustion of sulfur-containing
fuels such as coal, coke, and fuel oil; from sulfuric acid plants
and miscellaneous uses of sulfur dioxide; and from the com-
bustion of sulfur compounds in waste gases from manufactur-
ing processes. Many investigations have been carried out on
the removal of sulfur from fuel and on the removal of sulfur
oxides from waste gases, but no generally practical methods
have been developed. Thus, recourse is made to dispersion
from suitably tall chimneys to reduce ground-level concentra-
tions to acceptable limits. By controlling burner conditions to
limit excess air in the gases, large users of fuel oil and electric
power plants can reduce sulfur trioxide in waste gases from
40-50 ppm to about 5-10 ppm. In most countries, sulfuric acid
is produced by contact processes that give a final acid emis-
sion to not more than two percent of the sulfur burned. Pro-
vided contact plants are equipped with adequate facilities for
preheating, there should be no adverse local conditions
produced by emissions. However, there is scope for research
into acid mist formation and methods for its prevention at the
source. Emissions from some chemical processes are often
more concentrated than those from the combustion of fuel. It
is common practice to remove the sulfur dioxide in these emis-
sions by scrubbing with alkali solutions.
23972
Weissenberger, G. and L. Piatti
RECOVERY OF SULFUR DIOXIDE FROM WASTE GASES
BY MEANS OF CYCLICAL KETONES I. (Ueber die Gewin-
nung von Schwefeldioxyd aus Abgasen mil Hilfe cyclischer
Ketone. L). Text in German. Chemiker Z., 53(25):245-247,
March 27, 1929. Part H. Ibid., 53(26):266-267, April 10, 1929.
Sulfur dioxide present in waste gas from a sulfuric acid plant
(contact process) in a quantity of 6-7 g per cu m was absorbed
in laboratory experiments by clear technical cyclohexanone
(boiling begin 150/152 Q and by clear technical methyl-
cyclohexanone at 15 to 20 C in wash bottles and the absorbed
SO2 was subsequently recovered by heating the solvents to 80
C. The absorbed SO2 was determined by titration with an
iodine solution. The quantity of SO2 absorbed by the two sol-
vents varied with temperature, at a practical operating tem-
perature of 15-20 C approximately 0.25% by weight S02 was
absorbed. The addition of metallic mercury to the solvents had
a marked positive or negative effect on the SO2 absorption
capacity of both solvents depending on temperature. The per-
centage of SO2 in the waste gas affected positively the absorp-
tion capacity of the two solvents from 0 to 5% SO2.
25178
Teworte, W. M.
SPECDJ1C Am POLLUTION CONTROL ARRANGEMENTS
AT NON-FERROUS METAL WORKS. Preprint, International
Union of Air Pollution Prevention Associations, 41p., 1970. 20
refs. (Presented at the Internationa Clean Air Congress, 2nd,
Washington, D. C., Dec. 6-11, Paper EN-28B.)
Information on the cost problem and on the necessity for air
pollution control technology in the field of non-ferrous metals
production is presented. Their price, high in comparison with
that of steel, is an incentive to developing any means of in-
creasing the yield and, thus, to recovering the metals from flue
dusts. Therefore, the center of air pollution control arrange-
ments shifts to the side of extracting accompanying elements
in the ores, auxiliary materials, and highly volatile compounds.
The negative biological effects of a large number of metals
require particularly effective arrangements for waste gas pu-
rification. More recent specific methods of air pollution con-
trol are illustrated by several examples. Fluorine emissions
from the flux are fought in aluminum works by means of ef-
fective wet purification processes; dry absorption methods are
also being tried. Fluorine levels of 0.5-1.5 ppb were detected
even in industrial areas where there was no aluminum produc-
tion at all. Waste gas purification at aluminum re-melting
works presents a particularly difficult problem with regard to
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SULFURIC ACID MANUFACTURING
the extraction of very fine salt fumes. The utilization of the
sulfur content in the non-ferrous metal ores is discussed in
detail. Here, the solution to the economic problem of market-
ing a sulfuric acid, aptly called 'acide fatal' by Belgian smelt-
ing works, is as important as the solution to the process
technical problem. The latter was dealt with very successfully
by means of the development of a double-contact process with
intermediate absorption for roasting gases poor in sulfur diox-
ide. The final gases contain less than 0.5% of the SO2 charge.
More and more processes favorable to air hygiene are being
used by zinc metallurgy. Methods of recovery that cannot be
controlled by waste gas technology, will be discarded. General
and particular information is given on the cost problem of air
pollution control. Frequently, the wrong conclusions are drawn
from the fact that only 0.2% of the value of industrial produc-
tion are required for direct steps, with secondary injurious ef-
fects, amounting to 1-2%, being prevented in this manner.
Production at some works is hard hit by specific costs of 1-5%
of the proceeds from sales. (Author abstract)
25605
Fulton, Charles H.
METALLURGICAL SMOKE. Bull. Bureau Mines, no. 84:7-94,
1915. 44 refs.
The problem of metallurgical smoke (defined as gases and
vapors, an the fine dust entrained by them) that issues from
stacks of smeltin and ore roasting plants is considered. Sulfur
dioxide and trioxide are two of the major gases in this case.
They can combine with atmospheric water to form sulfuric
and sulfurous acid. The dust that is carried by the gases con-
sists of small particles of the different ores, fluxes, or fuel.
These emissions can, when combined with certain meteorolog-
ical conditions, cause extensive plant damage, as well as inju-
ry to animals and humans. The physica and chemical proper-
ties governing the actions of stack emissions ar discussed. The
effect of the effluent flow speed on the compositio of the flue
dust is considered, and design practices for dust chambers and
stacks are related. Methods for the control of dust emissions
include settling chambers, bag-houses, and electrostatic
precipitation. Several operating examples of these controls are
presented. Several processes for the removal of SO2 from
stack gases and its conversion to H2SO4 are given, including
absorption and alkaline additives. Some legal aspects of
smelter emissions problems are discussed in terms of actual
litigation.
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B. CONTROL METHODS
00587
J.A. Brink, Jr., W.F. Burggrabe, L.E. Greenwell
MIST REMOVAL FROM COMPRESSED GASES. Chem. Eng.
Progr., 62(4):60-66, April 1966.
Fiber mist eliminators have been successfully used to purify
gases and solve difficult air pollution problems involving:
methanol synthesis gas, sulfonation and chlorination process
gases, nitric acid process gases, chlorine, and compressed air.
Extensive research and development work resulted in the
development of fiber mist eliminators for the collection of sub-
micron mist particles. The first plant-scale installations were
made for the control of air pollution from sulfuric and
phosphoric acid plants. After full-scale units had been proven
highly efficient on stack gases containing submicron particles,
further research was undertaken to develop fiber mist elimina-
tors which would be most economical for the collection of par-
ticles which are predominantly 1 to 20 microns in diameter.
The installation of fiber mist eliminators within various
processes to purify gases was started after several difficult air
pollution problems had been solved. The widespread applica-
tion of fiber units to chlorine plants was reported in detail, but
the applications to many other processes has not been re-
ported previously. It should be noted that mists are present in
many chemical processes at pressures ranging up to 5,500
Ib./sq. in. gauge. The temperatures at whcih mists are present
are usually moderate since many mists vaporize at higher tem-
peratures.
00800
E.P. Stastny
ELECTROSTATIC PRECIPITATION. Chem. bSeng. Prog, 62,
(4) 47-50, Apr. 1966.
The electrostatic precipitator has proven to be the answer to
an important consideration in the production of oleum in the
sulfuric acid industry. Through its utilization, in addition to its
air pollution abatement role, important production gains have
been made possible. Look not only at what it can do for your
present operation conditions, but establish its design criteria
for ultimate plant capacity so as to insure full satisfaction at
maximum outputs under future air pollution codes.
01125
D. Zanon and D. Sordelli
PRACTICAL SOLUTIONS OF AIR POLLUTION PROBLEMS
FROM CHEMICAL PROCESSES . (Realizzazioni nel Campo
delia Prevenzione dell' inquinamento Atmosferico di Origine
Industriale.) Translated from Italian. Chim. Ind. (Milan),
48(2):251-261, March 1966.
A strict control of pollutant to be dispersed in the atmosphere
offers technical and economic problems, both in the design
and the operation of chemical processing units. Three exam-
ples of processes for which pollution control has been
established are described: SO2 derived from contact sulfuric
acid and from hydroxylamine sulfate plants, nitrous gas from
low and high-pressure nitric acid plants, and fluorine-contain-
ing effluents from hydrogen fluoride production. The general
approach, kind of abatement process adopted, materials and
construction costs are discussed.
02355
S.T. Cuffe CM. Dean
ATMOSPHERIC EMISSIONS FROM SULFURIC ACID
MANUFACTURING PROCESS; A COMPREHENSIVE AB-
STRACT. Preprint. (Presented at the 58th Annual Meeting, Air
Pollution Control Association, Toronto, Ontario, Canada, June
1965.)
This paper includes basic descriptions of both the chamber
and contact processes. Variations in process conditions that
may appreciably change the magnitude of emissions, e.g., the
manufacture of oleum or the use of different sulfur bearing
feed materials, are noted. Concentrations of both nitrogen ox-
ides and sulfur dioxide emissions from chamber plants were
found to range from about 0.1 to 0.2 volume percent. The con-
centration of combined acid mist and spray from chamber
plants varied from about5 to 30 milligrams per cubic foot. For
contact plants, the range of sulfur dioxide concentrations in
the absorber exit stack ranged from 0.13-0.54 volume percent;
while acid mist concentrations varied from 1.1 to 4.8 milli-
grams per cubic foot. The test data show that it is possible to
recover 99 percent of all of the acid mist and spray emissions
by adding commercially available mist elimination. (Author ab-
stract)
02985
K. Stopperka
ELECTROPREdPITATION OF SULFURIC ACID MISTS
FROM THE WASTE GAS OF A SULFURIC ACID PRODUC-
TION PLANT. Staub (English Transl.) 25, (11) 70-4, NOV.
1965. CFSTI TT66-51040/11
Optimum conditions for electroprecipitation of sulfuric acid
mist from waste gas in sulphuric acid production have been in-
vestigated in a pilot plant. The specific effect of the shape of
the discharge electrode has been tested in addition to the in-
fluence of collecting electrode dimensions and different
moisture contents on separation efficiency. The tests which
have been carried out with a 'Korobon' filter pipe (electrode
graphite) indicate that the corrosion problem has been solved
permanently. (Author summary)
03129
Avy., A. P.
METHODS OF REDUCING POLLUTION CAUSED BY
SPECIFIC INDUSTRIES. (CHAPTER VI. CHEMICAL INDUS-
TRY). European Conf. of Air Pollution, Strasburg, 1964. p
337-356.
The pollutants discharged by the chemical industry may be
subdivided into several classes. The first and most important
class is that of harmful products emitted in large quantities by
the 'heavy' chemical industry and, in particular, organic
chemical works: Sulphur dioxide, sulphuric acid, chlorine,
whether manufactured or in the form of impurities in the basic
-------
SULFURIC ACID MANUFACTURING
material: fluorine in the case of fertilizers and fluorine again in
aluminum electroechemistry. The chemical industry has a wide
range of special problems which is in a constant state of flux
owing to the wide and ever-increasing variety of new synthetic
products (intermediate and finished) in the organic chemical
industry. From the technical point of view, the prevention of
pollution by such products depends on their presentation and
manner of application. A problem directly connected with
chemical manufacture is that of smell: mercaptans, hydrogen
phosphide, methylamines, etc., although, of course, it does not
arise in the chemical industry alone. Technical methods used
to reduce pollution are highly devellped for dusts and smoke
and there is a wide choice of apparatus. The chemical indus-
try, like all others, is subject to laws and regulations governing
industrial air pollution. A fairly sharp distinction, however,
should be drawn between laws, which lay down in general
terms the objects to be attained and the obligations to be ful-
filled, and the regulations which embody detailes of the limits
imposed and the degree of reduction demanded. In this last re-
port, caution is necessary and impossible or unnecessary stan-
dards should not be set. It is clear that international liaison or
even international collaboration is not only desirable, but
necessary.
03945
F. T. Meinhold
THREE-WAY PAYOUT FOR H2SO4 GAS CLEANER. Chem.
Progress 29, (3) 63-4, Mar. 1966.
A compact and efficient acid gas cleaner was installed in the
top of each absorber and was adapted to the acid absorbers.
Another potential air pollution source was quenched in the
plant which involved the acid drying towers. Elimination of
the course mist not only prevents corrosion in the connecting
duct, but also reduces the over-all vol. of mist leaving the ab-
sorbers. Each of the 900-tpd. acid plants was completed on a
turn-key basis in 8 months. The exhaust stacks cleared in only
50 min. and now, after regular scheduled shut-downs, the
stacks are usually cleared in 5 to 30 minutes, depending on the
length of shut-down.
04067
E. O. Kossovskii
SANITIZATION OF IRON PYRITES GRINDING AT THE
M.B. FRUNZE SULFURIC ACID PLANT. Gigiena i Sanit. 28,
(1) 77-9, Jan. 1963. Russ. (Tr.) (Translated by B. S. Levine in
U.S.S.R. Literature on Air Pollution and Related Occupational
Diseases, Vol. 12.)
The iron pyrite grinding department at the M. F. Frunze sul-
furic acid plant was an intense source of fine air-suspended
dust which was coming from the transportation, unloading,
grinding, and loading of the groundbore onto the small transfer
cars. The entire pyrite grinding process was accomplished in
an inclosed brick building. Fine dust was intensely liberated
into the surrounding air at each step of the procedure. The
density of the air-suspended pyrite dust was inversely propor-
tional to the moisture content of raw ore, but the temperature
of the air generally reduced the initial moisture of the raw
pyrite by 65-70%, and under the prevailing ore grinding condi-
tions it was not possible to raise the moisture content of the
material artificially. Attempts to sanitize the working condi-
tions had to be limited to encasing points of dust generation
and to establish a suitable system of leak-proof ventilation.
Before the sanitary improvements in the process of iron
pyrites grinding were instituted the density of the generated
and air suspended pyrite dust was great and constituted a seri-
ous sanitary problem. The density of the iron pyrite dust in the
air surrounding the process was to a degree inversely propor-
tional to the moisture content in the raw ore. The sanitary im-
provements consisted basically in leak-proof encasing of
strategic dust generating production points and in instituting an
arterial ventilation system.
05079
N. Morash, M. Krouse, and W. P. Vosseller
REMOVING SOLID AND MIST PARTICLES. Chem. Eng.
Progr. 63, (3) 70-4, Mar. 1967.
The laboratory and pilot plant development work for a
technique which successfully removes submicron size dust and
acid mist particles from exhaust gases is described. The result
obtained when an irrigated, thin, felted fiber filter is used to
remove a mixture of fine titanium dioxide and sulfuric acid
mist particles from the exhaust gases of pigment calciners is
discussed.
05514
R. L. Gotham
ELECTROSTATIC PRECIPITATION OF SULPHURIC ACID
MISTS. Proc. Clean Air Conf., Univ. New South Wales, 1962,
Paper 20, Vol. 2, 16 p.
The most important feature of electrostatic precipitators is
their ability to remove very small concentrations of finely di-
vided particulate matter, at high efficiency, from extremely
large gas flows, in a plant of moderate size with a low pres-
sure drop across the equipment. Although little is known in re-
gard to the phenomena encountered, the process of electro-
static precipitation has gained world-wide acceptance as one of
the most efficient collection systems known, and for many
years has been successfully applied to the problem of sulphu-
ric acid mist removal. In this application, single-stage Cottrell
precipitators with a wire and tube electrode arrangement are
usual. Industrial precipitators are normally operated with their
discharge electrodes at as high a negative potential as possible
without sparking in order to obtain maximum particle migra-
tion velocities. For the treatment of gaseous effluent from
contact sulphuric acid plants, efficiency tests have indicated
average migration velocities in the range of 0.40 to 0.60 ft/sec
with attendant fficiencies in the order of 99.7%. The Deutsch
Equation, relating efficiency with migration velocity and
specific collecting area, is a satisfactory basis for equipment
design and comparisons provided that the value of migration
velocity used in the equation is an empirical or average value
determined from plant wxperience or pilot plant studies on a
similar application. (Author abstract)
05567
L. Silverman
HIGH TEMPERATURE GAS AND AEROSOL REMOVAL
WITH FD3ROUS FILTERS. Proc. Air Water Pollution Abate-
ment Conf., 1957. pp. 10-23m.
The use of a slag wool fiber filter as an inexpensive cleaner of
high temperature gases and fumes produced in open hearth
steel furnaces was described and evaluated. These fibers are
small (4 microns mean diameter) and are refractory, thus able
to withstand temperatures of 1100 F. ;or high efficiency
separation of fine aerosols, fine targets in large number are
necessary which packed slag fiber layers can provide.
Theoretical, laboratory and field studies show that slag wool
filters show efficiencies ranging from 90 to 99%, depending
upon fiber layer compositions, density, and thickness. The
chief separating mechanisms appear to be diffusion and impac-
tion. Results are presented of the air flow resistance charac-
-------
B. CONTROL METHODS
teristics of a rotary screw agglomerator, used to provide
dynamic gas treatment to increase particle size of the efficien-
cy of the screw as an inertial collector for iron oxide fume.
The collection efficiency and resistance characteristics of slag
wool fiber filters was extended to other aerosols and gases
such as fly ash, sulfur dioxide, hydrofluoric acid and sulfuric
acid mist. The filter (one inch thickness, five pounds per cubic
foot density) at velocities used for collecting iron fume (50 to
150 feet per minute) showed efficiencies for SO2 of approxi-
mately 30% when moist and zero when dry. For hydrogen
fluoride (dry and wet), efficiencies range from 70 to 90%. For
fly ash resuspended from Cottrell ash, efficiencies ranged
from 60 to 90%, whereas when feeshly formed fly ash was
created by burning powdered fuel, efficiencies ranged from 93
to 99%. A revised pilot model slag wool filter was constructed
for 750 to 1000 cfm gas flow based on results of the first field
unit.
06247
SULFURIC ACID MIST IS CLEANED FROM AIR BY FOG
FILTER SYSTEM. ((Air Eng.)) 9(3):24-25, Mar. 1967.
In the making of TNT, contaminants such as sulfuric acid mist
are emitted to the air. A relatively new method of cleaning air,
the fog filtration system is essentially a high pressure
scrubbing operation in which vaporized water cleans the pol-
luted air is silo- shaped chambers spaced about 50 ft. apart.
The air-cleaning system is actually a three-stage operation. Its
functioning is described: (1) Polluted air is drawn through one
of seven Cottrell electrostatic precipitators, where entrained
moisture receives electric charges from electrodes, (2) The
now partially clean air is drawn into one of the three fog fil-
ters, where it is washed under high pressure, pulled downward
in a swirling pattern, is then drawn up through a pipe and ex-
pelled, with virtually all impurities removed, and (3) The ef-
fluent (dirty) water flows from the bottom of the filter to a
collecting basin several hundred feet away, where it is treated
and discharged. These three powerful fans draw the con-
taminated air from the electrostatic precipitators are big units:
21 ft. high, 20 ft. wide, and 10 ft. deep. Once the acid-polluted
air is drawn into them, the suspended matter in the air
acquires a charge and is precipitated at the ground surface.
Droplets so precipitated unite to form a liquid which drains
down the sides of the tubes and is collected below. The next
step is the suction of the still acidic polluted fumes through
the fog filters. Then the air is given a thorough scrubbing with
fog particles. The wetting nature of the high pressure fog per-
mits fine particles to be 'centrifuged' out of the air by a simu-
lated cyclone action in the wetted gases. Fog particles from
high pressure nozzles provide an excellent induced draft air
pump, because all air entrained must necessarily move with
substantially the same velocity as that of the fog particle. The
system is virtually maintenance-free, even though the filters
are operating on a 24 hour a days basis to keep the air clean.
Beyond a routine schedule of cleaning the filter chambers,
there is no requirement for maintenance manpower.
06282
A. S. Arkhipov, A. N. Boytsov
TOXIC AIR POLLUTION FROM SULFURIC ACID PRODUC-
TION. Gigiena i Sanit., Vol. 31, p. 12-17, Sept. 1962. 5 refs.
Engl. transl. by JPRS-R-8824-D, p. 1-7, Nov. 11, 1967.
In order to analyze working conditions in the production of
sulfuric acid against a background of technical progress and
modernization of the progress, data on air pollution were col-
lected in furnace sections of sulfuric acid shops at 12 chemical
plants. Technical progress, the introduction of new calcining
methods for pyrite, the mechanization of many manual opera-
tions, the introduction of automation features, better ventila-
tion and other means have improved working conditions in
kiln shops of sulfuric acid plants. The concentrations of S02
in a number of plants producing sulfuric acid have dropped to
permissible levels. The reduction in SO2 concentration to per-
missible levels and the marked reduction in clinker dust have
been achieved even during increased technical progress,
greater charges of raw materials and gas per cubic meter of
furnace and cubic meter of building volume and the greater
production of sulfuric acid plants.
07535
W. Leithe
CLEAN AIR MAINTENANCE - AN IMPORTANT TASK FOR
CHEMISTRY AND ECONOMY. (Reinhaltung der Luft ein
dringendes Anliegen fur Chemie und Wirtschaft.) Text in Ger-
man. Allgem. Prakt. Chem. (Vienna), 18(8):239-241, Sept. 10-
17, 1967. 4 refs.
This article is a summary of two lectures given at meetings of
chemical societies. The problem of air pollution and some con-
trol methods are outlined. Typical examples of well-known air
pollution problems are mentioned: London's smog chiefly
caused by domestic heating, the smog of Los Angeles due to
automobiles, the sun, and temperature inversions, and the in-
dustrial air pollution of the Ruhr Valley. Some characteristic
data for all three examples are quoted. The techniques for the
control of dust emissions are farthest advanced. This is
verified by the fact that in Germany, emission of cement dusts
decreased to one third while the production of cement tripled
in the last 17 years. Far less satisfactory is the control of SO2
emissions. About twice as much sulfur is blown into the air
than is used for the production of sulfuric acid. Some wet and
dry processes for the elimination of SO2 from smoke are men-
tioned, but no method is known today which is both effective
and economical. The chemical industry tackled its problems
mostly by reducing the emission of air polluting substances by
increasing the efficiencies of the relevant chemical processes.
Examples are the production of sulfuric acid and nitric acid.
Organic compounds can be recovered by either absorption on
activated charcoal or oxidation by catalytic afterburners.
07552
Billings, Charles E., Charles Kurker, Jr., and Leslie Silverman
SIMULTANEOUS REMOVAL OF ACID GASES, MISTS, AND
FUMES WITH MINERAL WOOL FILTERS. J. Air Pollution
Control Assoc., 8(3): 195-202, Nov. 1958. 20 refs. (Presented at
the 51st Annual Meeting, Air Pollution Control Assoc.,
Philadelphia, Pa., May 26-29, 1958.)
Investigations have indicated that two in. thick filters at four
Ib/cu. ft. packing density will remove up to 80% of acid mist
and up to 99% of acid gases and fumes. Total filter life de-
pends upon concentration of contaminant in the entering air. A
summary of filter performance is given. Estimated operating
life based upon one use of the filter material can be obtained
from the data given. With particulates such as iron oxide and
fly ash, it has been found possible to wash and reuse filters
about ten times. When iron oxide was collected simultaneously
with SO2, filters were reused about eight times. Acid gas col-
lection is significantly improved by the presence of moisture
on slag wool filters. Mineral wool filters have several features
such as, low cost (about 1 cents/lg.), small fiber diameter (4
micron and ability to withstand high temperatures (1000 deg
F.). Slag wool will simultaneously remove sub-micron particu-
late materials with 90 to 99% efficiency. Resistance to flow
through two in. slag wool filters (with an HF efficiency of
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8
SULFURIC ACID MANUFACTURING
95%) is on the order of one or two in. of water, or if continu-
ously moistened, at most 6 in. of water.
07925
Beighton, J.
THE SPECIAL INDUSTRIAL PROCESSES. Roy. Soc. Health
J. (London). 87(4):215-218, July-Aug. 1967. 2 refs. (London)
The air pollution problems of a group of industries which
produce: sulfuric acid, nitric acid, petroleum and petrochemi-
cals, iron and steel, copper, aluminum, gas, ceramics and elec-
tric power are reviewed. The basic technical approach is to
avoid the formation of the emission by design of the process,
then to require the treatment of any unavoidable emission, and
finally to require adequate dispersal of any residual amount
which has to be discharged. The legislation is designed to com-
promise between safeguarding of public health and amenities
and providing for a realistic acceptance with adequate control
of special processes. Although the loss of gases in the manu-
facture of sulfuric acid is limited to 2% of the sulfur burned,
the loss from a contact acid plant with a 500-ton-per-day
capacity may be considerable so that chimney heights as high
as 450 ft may be required. Acid mist from contact plants burn-
ing sulfur is a special problem as it is difficult to control and
its occurrence is unpredictable. There are two nitric acid
plants in Britain equipped with catalytic tail-gas reduction
units which should solve the problem of brown nitrous fume
emission to the air. The use of special flares is required to
control H2S and mercaptans emitted by oil refineries. In the
steel industry the development of the Fuel-Oxygen-Scrap
process is regarded as an alternative to the electric arc fur-
nace. It is claimed that melting and refining can be carried out
without exceeding a fume level of 0.05 grains per cu ft.
08181
Varlamov, M. L., G. A. Manakin, and Y. I. Starosel'skii
PURIFICATION OF EXHAUST GASES OF A SULFURIC
ACID TOWER PLANT BY A FLOWMETER PIPE TYPE OF
APPARATUS. Zh. Prikl. Khim., 31(2): 178-186, 1958. 19 refs.
Translated from Russian by Bture on Air Pollution and Related
4, p. 68-77, Aug. 1960. CFSTI: TT 60-21913
A venturi apparatus for the recovery of spray, sulfuric acid
aerosol, and nitrogen oxides from the exhaust gases of a sul-
furic acid tower plant is described. The experimental arrange-
ment consisted of two units: a small assembly, producing up
to 50 cu in/hour, and a larger one producing up to 500 cu
m/hour. In one apparatus, the fluid entered the main channel
at an angle; in a second apparatus, the fluid entered tangen-
tially and became distributed evenly over the perimeter of the
diffuser. A third apparatus had a radial fluid feed in relation to
its main axis. The separator walls of the small unit were ar-
ranged concentrically which forced the passing gas to impinge
upon the surface of the liquid twice in succession. Another
type of tube was tested in connection with the large unit. This
tube had two radial fluid feeds set at 90 deg, and a separator
of the type of abbreviated cyclone TsKTI. The power con-
sumed in the operation of the flowmeter tube type of ap-
paratus in the purification of exhaust gases emitted by the
tower nitrose system ranged between 5 6 kilowatt-hours per
ton of H2SO4, or 10 to 12% of the total power used in the
production of one ton of sulfuric acid by the nitrose method.
09126
Moeller, W. and K. Winkler
THE DOUBLE CONTACT PROCESS FOR SULFURIC ACID
PRODUCTION. J. Air Pollution Control Assoc., 18(5):324-325,
May 1968. 1 ref. (Presented at the 60th Annual Meeting, Air
Pollution Control Assoc., Cleveland, Ohio, June 11-16, 1967,
Paper No. 67-115.)
In the Bayer double contact process the reaction is interrupted
after approx. 90% SO2 has been converted to SOS. The SOS is
removed in a first absorption stage the so-called intermediate
absorption and the remaining SO2-air mixture is once more
reacted at the contacts. By removing the SOS during the inter-
mediate absorption, the distance of the remaining gas mixture
from the state of equilibrium is increased and this permits
further reaction, which means higher degrees of conversion.
Theoretically, the double contact process allows the conver-
sion degree to be increased from approx. 98% for the normal
contact process to approx. 99.8%, and thus a reduction of S02
emitted by a factor of ten. After the intermediate absorption,
the temperature at which the catalyst begins to respond is
about 50 degrees C lower than usual. This greatly helps to con-
trol air pollution, since the more favourable state of equilibri-
um further cuts down the quantity of emitted SO2 by at least
50% at a temperature which is 50 degrees C lower. The SO2
concentration emitted by the double contact plant, based on
elemental sulfur, does not exceed 240 ppm at 20% overload
and is as low as 100 120 ppm SO2 at normal load. Plants which
have now been operating for 3 years on the basis of pyrites
still give the same degree of conversion of 99.7%.
09559
Hensinger, C. E., R. E. Wakefield, and K. E. Glaus
TURNING POLLUTION GASES INTO PROFITS. Eng. Mining
J., 169(2): 131-135, Feb. 1968.
Fluid Column zinc roasters have been developed to process
pelletized zinc concentrates with the resulting sulphur dioxide
in the roaster gas used to produce sulphuric acid in a contact
plant. These installations reflect the modem trend toward
more efficient roasting processes and sulphuric acid plants of
larger tonnage. In Fluid Column roasting several contiguous
fluidized beds of pelletized zinc concentrates of varying
OoJagmtienai BttrtnJeaceVate superimposed one on top of the
other without intervening mechanical grates. Air is the primary
fluidizing agent, however, provision is made for the introduc-
tion of other gases to produce different conditions in each
bed, e.g. the lowest may be oxidizing while the upper bed may
be reducing. The roasting process and the sulfuric acid plant
are described in some detail.
09913
Guyot, G. L. and J. P. Zwilling
SNPA'S PROCESS FOR H2SO4 PRODUCTION DEVELOPED
WITH EYE ON ADX POLLUTION. Oil Gas J., 64(47):198-200,
Nov. 21, 1966.
A new process provides for reducing the sulfur content of
residual gases to a very low level and converting the removed
sulfur into high concentration (92 to 94%) H2SO4. The new
process purifies exhaust gases containing up to 30 vol % steam
and 0.8 to 3.0 vol % sulfur derivatives. The gases, after trans-
formation of sulfur compounds into SO2 go through a mul-
tibed catalytic converter to transform SO2 into SOS. The con-
version rate varies from 90 to 95%, depending on initial SO2
concentration. The SOS is condensed, in the form of sulfuric
acid of 92 to 94% concentration. The SOS-rich gases are
cooled to a temperature slightly higher than their dew point.
-------
B. CONTROL METHODS
Then they are sent to an absorption tower for countercurrent
washing and cooling by the acid already produced. No filters
or electrostatic precipitators are needed. An acid of 92 to 94
wt% concentration can be made from a gas with less than 1%
SO2 and up to 30% water.
11058
W. Teske
IMPROVEMENTS IN THE PROCESSES AND OPERATION
OF PLANTS IN THE CHEMICAL INDUSTRY LEADING TO
REDUCED EMISSION. Staub (English translation), 28(3):25-
33, March 1968. CFSTI: TT 68-50448/3
The emissions from chemical plants can be reduced, in special
cases, by changing the production process or, in general, by
using a gas cleaning method. Change in the production process
may be achieved by a basic alteration of the process itself, by
changing the mode of operation, by modifying the equipment
and by using a different raw material. For this purpose, the
doublecontact method for sulphuric acid production, the pres-
sure method for nitric acid recovery and the introduction of a
covered carbide furnace are mentioned as examples. The su-
perphosphate process, viscose process, production of
betanaphthol, production of thermal phosphoric acid and
production of calcium chloride are given as examples for
waste gas cleaning. (Author's summary)
11146
Anon.
SULPHUR. A HIDDEN ASSET IN SMELTER GASES. PART
4. Eng. Mining 169(8):59-66, Aug. 1968.
Smelter and converter gases and their contained sulfur are a
specialized problem which may be turned into an asset for
profit. The worldwide application of technology to this
problem is reviewed Process description and applications are
discussed.
11235
J. A. Brink, Jr., W. F. Burggrabe, and L. E. Greenwell
FIBER MIST ELIMINATORS FOR SULFURIC ACID
PLANTS. Preprint, Monsanto Co., St. Louis, Mo., ((31))p.,
1968. 10 refs. (Presented at the Symposium on Sulfur, Sulfuric
Acid and the Future, Part n, 61st Annual Meeting, American
Institute of Chemical Engineers, Los Angeles, Calif., Dec. 1-5,
1968, Paper 6-F.)
Fiber mist eliminators not only utilize the mechanisms of im-
paction and interception on the large and intermediate size
particles, respectively, but also are the only type of equipment
which can be designed to utilize the Brownian movement of
particles to effect extremely high collection efficiencies in the
low and sub-micron ranges. Collection efficiences on particles
greater than 3 microns are essentially 100% while efficiencies
as high as 99.98% on all remaining particles 3 microns and less
in size can be achieved depending on design and economics.
High efficiency fiber mist eliminator elements for sulfuric acid
plants plants consist of fibers packed between two concentric
screens. Mist particles collected on the surface of the fibers,
become a part of the liquid film which wets the fibers. The
liquid film is moved horizontally through the fiber bed by the
drag of the gases and is moved downward by gravity. The
Liquid drains down the inner screen to the bottom of the ele-
ment and then to a liquid seal pot. The liquid overflows the
seal pot continuously back to the process.
11238
R. R. Dukes, and M. D. Farkas
SULFUR SHORTAGE VS PLANT DESIGN. Preprint, Leonard
Construction Co., Chicago, LI., 25p., 1968. 5 refs. (Presented
at the 61st Annual Meeting, American Institute of Chemical
Engineers, Symposium on Sulfur, Sulfuric Acid and the Fu-
ture, Part I, Los Angeles, Calif., Dec. 1-5, 1968, Paper 5-C.)
Sulfuric acid plants can be built using SO2 bearing gases from
various sources. The most important characteristic from the
viewpoint of economics is the SO2 concentrations. Catalyst
poisons such as fluorides should be avoided, and the SO3 and
paniculate contents should be as low as possible. If the S02
content is low, the operating costs will be high because of in-
creased utility requirements as fuel to keep the plant in ther-
mal balance, and a power to supply refrigerated water. The
amortization costs will be high because of the increased capital
requirements. (Authors' summary)
11250
C. F. Scheidel
SULPHUR DIOXIDE REMOVAL FROM TAIL GAS BY THE
SULFACID PROCESS. Preprint, Lurgi Apparatebau
Gesellschaft mbh, Frankfurt (Germany), ((25))p., 1968.
(Presented ath the 61st Annual Meeting, Symposium on Sul-
fur, Sulfuric Acid and the Future, Part n, Los Angeles, Calif.,
Dec. 1-5, 1968, Paper 6 E.)
A sulfur dioxide removal process is described. Gases contain-
ing SO2 are passed through an activated carbon reactor and
optimum removal of SO2 is reached if the gas is saturated
with water at a temperature of approximately 160 degree F.
The bed of activated carbon is sprayed with water. The fol-
lowing process steps are required for wet catalytic conversion
to sulfuric acid: 1) adsorption of SO2 milecules 2) oxidation of
SO2 3) removal of SO3 by flushing with water 4) increase of
solubility of S02 with lower sulfuric acid concentration in
liquid film 5) the rate of H2SO4 adsorption increases with
H2SO4 concentration which slows down SO2 diffusion in ad-
sorbent. A description of the chemical plant and equipment
used in this process is given along with operating costs.
11629
Zwilling, J. P. and G. Guyot
RECOVERY OF THE WASTE GASES FROM CLAUS UNITS
FOR THE PRODUCTION OF SULFURIC ACD3. Erdoel Kohle
(Hamburg), 21(5):290-292, May 1968. (Presented at the 19th
Annual Meeting of the German Society for Petrology and Coal
Chemistry, Hamburg, Oct. 6, 1967.) Translated from German.
8p.
At a natural gas purification plant, separated acid gas is
processed to sulfur in a Claus unit. Since five percent of the
sulfur was removed as sulfur dioxide with the waste gases, a
continuous catalytic oxidation process was developed to con-
vert sulfur compounds to sulfur trioxide and to recover con-
centrated sulfuric acid. The oxidation of the sulfur compounds
is preceded by the combustion of residual gases at 540 C to
oxidize hydrogen sulfide to sulfur dioxide and by the sub-
sequent cooling of the combustion gases at 410 C. The sulfur-
containing gases are then contacted with a vanadium catalyst
in an adiabatic converter; oxidation takes place with the
release of heat. Gases leaving the converter are cooled to 275
C and then passed to a concentration tower where they are
contacted with 90-94% sulfuric acid in a counterflow
precedure. Gases from the concentration tower flow- to an ab-
sorption tower where the sulfuric acid vapors are scrubbed
with 80-85% sulfuric acid. The gases impart their heat to the
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10
SULFURIC ACID MANUFACTURING
acid; since the absorption by the sulfuric acid also generates
heat, the circulation absorption-sulfuric acid is cooled in gra-
phite exchangers. Any acid remaining in the gases is removed
by a Teflon filter; no electrostatic filters are required. Produc-
tion of sulfuric acid is 65,000 to 140,000 ton/yr. The concentra-
tion of the acid is 91-94%.
11906
Hilder, Wolfgang
A NEW SULPHURIC ACID INSTALLATION REDUCES
SULPHER DIOXIDE EMISSION. ((Neue Schwefelsaureanlage
verringert Schwefeldioxidemission.)) Text in German. Stad-
tehygiene, 19(6):125-127, June 1968.
An increased (24%) consumption of sulfuric acid (H2SO4)
(used in the manufacture of fertilizers, vitamin pigments, ar-
tificial fibers, etc.) in the German Federated Republic over the
last 5 years, a 78% H2S04 made in the Chamber and Tower
Process which did not fulfill all purity requirements, and a
shortage of elemental sulfur caused interest in the Pyrite-roast-
ing Process of H2SO4 production. Copper, zinc, and a purple
ore which is a valuable raw material in the iron industry, are
also by-products of this process. With a daily production of
650 tons, the new pyrite-buming, H2SO4 installation of the
Hoechst Dye Works is one of the largest plants of its kind.
This non-urban, modern factory, which utilizes a closed com-
bustion and exhaust system and a highly effective noise-isola-
tion system, performs 4 operations: heat utilization, gas clean-
ing, contact, and absorption. The dust-containing mixture of
SO2 and air is freed of floating particles and moisture in
hot,roasting ovens used also in the manufacture of steam and
electricity. The dust from the ovens and from the gas cleaning
is collected for further utilization. The cleaned gases, emitting
only 1/5 the amount of SO2 as the earlier process, escape after
final absorption through a stack 135 m in height. The improved
contact operation, which oxidizes SO2 to SO3, produces most
of the H2SO4 in the Federal Republic (90%) and U.S.A. (95%).
Since only 2% of the SO2 emissions are contributed by all
H2SO4 manufacturers in West Germany, it is a fallacy to be-
lieve that the new installation will reduce atmospheric SO2
pollution substantially. The overwhelming portion of SO2 pol-
lution is emitted from heat or electricity-producing fossil fuel
installations.
13206
Bulicka, Milan, Jaroslav Podmolik, and Josef Hajek
ECONOMY OF ABSORPTION UNIT INSERTED FOR
LOWERING OF EXHALATIONS FROM SULPHURIC ACID
PRODUCTION PLANT. (Ekonomie vyroby kyseliny sirove s
vlozenou absorpci). Text in Czech. Chem. Prumysl (Prague),
19(3):140-142, 1969. 5 refs.
When the daily production of sulfuric acid ranged to 100 t/day,
with 95 to 97% conversion and with an average absorption of
99%, even with relatively low chimney heights, the immediate
vicinity of factory was free from emissions. When production
exceeded 300 t/day, higher chimneys did not sufficiently
reduce the local concentrations. In most plants using the
heterogeneous oxidation manufacturing method, SO2 emis-
sions are 0.2 to 0.4%, SO3 emissions are 0.02 to 0.1%, and
H2SO4 emissions are 0.075%. For the work in Prerov, which
produces 100,000 t/year, a two stage exothermic process of
catalytic oxidation of SO2 was adopted. Output is higher than
103,000 t/year, and 10 kg of sulfur are recovered for 1 t of the
manufactured sulfuric acid. The process uses a closed circuit
of cooling water which requires 20% more water than with
traditional methods, and 3.5 kWh/t more sulfuric acid, and
which produces 10 kg less of steam per ton of sulfuric acid.
The cost of the absorption equipment is offset by the value of
the sulfur recovered. The greatest advantage of the unit is its
reduction of harmful emissions.
13337
Emicke, Klaus
A METHOD OF REMOVING SULPHUR DIOXIDE FROM
GAS CONTAINING SULPHUR DIOXIDE. (Nor Deutsche Af-
finerie, Hamburg, Germany), British Pat. 1,107,626. 5p.,
March 27, 1968. (Appl. June 11, 1965, 12 claims).
A method of removing SO2 from exhaust gases is described.
The gas is brought into contact with an aqueous solution of
selenious acid in reaction vessels through which the solution is
passed in countercurrent to the gas which contains SO2. The
removal of the SO2 is performed in two stages. The selenium
which is formed in the first stage is removed from the circulat-
ing liquor, and the SO2 is completely removed from the gas in
the second stage. It is possible to perform this method
economically and to remove the SO2 completely because the
selenium formed is precipitated in solid form and does not dis-
solve in the H2SO4 which is formed simultaneously.
13667
Lehle, W. W.
PROCESSING OF WASTE GASES FROM SULFURIC ACID
PLANTS. In: The Manufacture of Sulfuric Acid, Werner W.
Duecker and James R. West (eds.), Am. Chem. Soc. Mono-
graph Series, New York, Reinhold Publishing Corp., 1959,
Chapt. 20, p. 346-358. 25 refs.
Tail gases from contact sulfuric acid plants consist mainly of
nitrogen, oxygen, carbon dioxide, and a small amount of sul-
fur dioxide. Though present normally in small concentrations,
sulfur dioxide, sulfur trioxide, and sulfuric acid can exceed
permissible limits during start-ups and plant upset conditions.
Sulfur trioxide and sulfuric acid vapor both form sulfuric acid
mists which produce visible plumes from acid plant stacks.
Processes for treating tail gases of sulfuric acid plants include
scrubbing sulfur dioxide from waste with water, soda ash solu-
tions, lime slurries, salt solutions, and ammonia solutions; the
exorption process developed by the Consolidated Mining and
Smelting Company; and the Katasulf modified autoclave
process. As illustrated by the Cominco sulfur dioxide recovery
system, an automated two-stage scrubber method using am-
monia solutions has a number of advantages. It will reduce
sulfur dioxide concentrations in tail gases to 0.03, handle gas
concentrations as high as 0.9% sulfur dioxide, produce a
scrubber liquid which has commercial value, and, by eliminat-
ing pollution, allow a plant to operate at an overload capacity
on the order of 20%. Pease-Anthony Venturi scrubbers and
Calder-Fox scrubbers are not efficient for sulfuric acid mists
less than 10 microns. Of the equipment available for mist
removal, wire-mesh eliminators and ceramic filters are more
effective than cyclone separators, baffles, Vane-type separa-
tors, and packed-bed separators. The costs of wire-mesh
removals is modest, though the possibilities of corrosion must
be considered in selecting the mesh-wire material. The ceramic
filter tube requires considerably more filtering area.
13672
KENNECOTT STARTS UP HUGE H2SO4 PLANT. Chem
Eng. News., 45(13):59-61, 1967.
Kennecott Copper's sulfuric acid plant near Salt Lake City is
autothermal and designed to run on smelter gas containing 2-
6% SO2. Gas from copper converters first goes through a glass
cleaning section comprising a Cottrell precipitator, a large
-------
B. CONTROL METHODS
11
Peabody scrubber, and Cottrell mist eliminators. The cleaned
gas passes through a drying tower, two 2000 hp blowers, and
into a series of five gas-to-gas heat exchangers before entering
a three-pass converter where SO2 is converted to SO3. From
the converter, the gas goes to the absorbing tower where the
SO3 is absorbed by 98% sulfuric acid. The efficiency of the
absorption towers is considered to be doubled by the use of 3
in. interlocked saddles, which allow a higher throughput of
gas, and by an increased number of distribution ports for the
acid that contacts the gas. The mist eliminator installed at the
top of the absorption tower is a two-stage device with a Teflon
mesh.
13728
Guyot, G.
PRODUCTION OF CONCENTRATED SULFURIC ACID
FROM SULPHUROUS GASES WITH HIGH WATER
VAPOUR CONTENT. (Fabrication d'acide sulfurique concen-
tre a partir de gaz sulfureux a forte teneur en vapeur d'eau).
Text in French. Chim. Ind. (Paris), 101(6):813-816, March 1969.
Although the contact process is applicable to both dry and wet
gases, the sulfuric acid produced from wet gases by this
method has a relatively low concentration (80%). A process is
described for producing commercial concentrations (94%) of
the acid from sulfurous gases with a high content of water
vapor, even when the sulfur dioxide content is lower than 1%.
The unit operating at Lacq is given as an example of the
economics and applications of the process. (Author abstract
modified)
13806
SULFURIC ACID PROCESS REDUCES POLLUTION. Chem.
Eng. News, 42(40):42-43, Dec. 21, 1964.
The Bayer process for H2SO4 production is based on a double
pass of SO2-bearing gases through the converter. The first
contact is accomplished in three stages of varying depths of
vanadium pentoxide. The second contact is accomplished in
the fourth stage. The gases increase in temperature from 450
to 600 C in the first stage and must be cooled before entering
the second stage. Cooling is accomplished by adding a side
stream of cold SO2-containing gas to the reactor just below
the first stage. A series of heat exchangers remove the heat of
reaction in the remaining three stages. The SOS-rich gas is
removed from the converter and the S03 is absorbed in
H2SO4 after the first three stages. The unreacted SO2 is recy-
cled back through heat exchangers to the fourth stage. Up to
99.7% of the original SO2 has been removed after the fourth
stage. The gas has an analysis of about 0.7% SO3, 0.03% S02,
5% O3, and the remainder nitrogen. The SOS is absorbed in a
packed tower. Sulfur dioxide sent to the stack is one-seventh
to one-tenth the concentration found in conventional
processes.
13880
Siedlewski, J.
THE MECHANISM OF CATALYTIC OXIDATION ON AC-
TIVATED CARBON. THE ROLE OF FREE CARBON RADI-
CALS IN THE OXIDATION OF SO2 TO SO3. Intern. Chem.
Eng., 5(4):608-612, Oct. 1965. 14 refs. (Also: Roczniki Chem.,
39(2):263-271, 1965.)
Free carbon radicals have been shown to have no influence on
the maximum quantity of physically adsorbed SO2; rather,
they constitute the active centers of the carbon surface in the
chemisorption of SO2. The quantity of chemisorbed SO2 in-
creases with a rise in concentration of free radicals on the car-
bon surface. If SO2 and O2 are introduced on the catalyst
simultaneously, the increase in the mass of the catalyst as a
result of the adsorption and oxidation processes which occur
is found to be proportional to the size of the catalyst surface.
However, the quantity of SOB formed does not depend on the
total amount of adsorbed reactants, but on the number of
chemisorbed molecules. Samples of carbon characterized by
the strongest signal in resonance spectrum have been found to
have the maximum catalytic activity.
14030
Guyot, G.
S.N.P.A. PROCESS FOR THE TREATMENT OF RESIDUAL
GASES WITH LOW CONCENTRATION IN SO2. (Precede
developpe par la Societe Nationale des Petroles d'Aquitaine
pour trailer des gaz residuaires charges de faibles teneurs de
SO2). Text in French. Chim. Ind. (Paris), 101(l):31-34, Jan.
1969.
The sulfuric acid plant of the Societe Nationale des Petroles
d'Aquitaine at Lacq is able to produce a sulfuric acid with a
concentration of 94% from gases containing only 1.5% by
volume of SO2 and H2S, and 30% water vapor. The process
involves the oxidation of H2S to SO2, followed by the oxida-
tion of SO2 to SOS on a vanadium catalyst in an adiabatic
reactor, gas-liquid contact in a bed of Raschig rings, and,
finally, the absorption of SO3 by diluted acid circulated and
cooled in graphite exhangers. After leaving the absorption
unit, the gas is passed through a Teflon filter which retains
any drops of acid that are carried along with the gas. To avoid
the condensation of acid in the chimney, gases are lightly
heated before being exhausted into the atmosphere. Gases
emitted from the plant contain 75 mg/cu m SO3 at the most.
14386
Smyslov, N. I.
MEANS OF ELIMINATING HARMFUL WASTES FROM
SULFURIC ACID TOWERS. (Puti likvidatsii vrednykh
vybrosov bashennykh semokislotnykh sistem). Text in Rus-
sian. Ochistka Ispol'z. Stochn. Vod Prom. Vybrosov, Kiev,
Sb., 1964:88-93.
Various causes of instability in tower operation, and hence in-
creases in the amount of harmful wastes above permissible
levels together with a decrease in productivity, are discussed
in general terms. Measures adopted in 1954 to normalize
operating conditions and limit each plant to operation with a
single raw material type were only partially implemented but
did yield positive results; by 1962, the average consumption of
nitrogen oxides per ton of products for all plants had been
reduced from 28 kg (1954) to 20 kg; leading plants reduced
HNO3 consumption to as low as 10 kg. The so-called cross-
reflux scheme has recently been proven effective and is
recommended for adoption. Conversion to a combined con-
tact-tower system at the Odessa plant has been completed; it
can be applied to plants operating with pure sulfur or pyrite. It
is concluded that sufficient means are available for improving
sulfuric acid systems and for eliminating harmful wastes; ac-
celerated implementation is urged.
14533
A METHOD FOR THE RECOVERY OF NITROGEN OXIDES.
(Werkwijze voor het winnen van stikstofoxyden). Text in
Dutch. (Universal Oil Products Co., Des Plaines, m.) Dutch
Pat. 6,607,036. 13p., Nov. 25, 1966. (Appl. May 23, 1966, 8
claims).
-------
12
SULFURIC ACID MANUFACTURING
The system is particularly suited to handling tail gases from a
nitric acid factory and from the lead chamber process of a sul-
furic acid factory. This method also gives a distinct improve-
ment in the output of a nitric acid plant. The waste gas is
passed over a bed of adsorbing coal particles followed by a
hot fluid desorption medium to remove the adsorbed nitrogen
oxides from the particles. The desorption medium consists of
steam at about 10 atm at a temperature greater than 157 C and
preferably more than 177 C. The nitrogen oxide-containing
steam is cooled and the mixture obtained is returned to the ad-
sorption zone of the nitric acid plant. The desorption medium
can also be hot air. The depth of the bed should not exceed
0.3m to prevent a large pressure drop. The stream waste gas
through the adsorption bed is diverted upon saturation with
nitrogen oxides to another bed of adsorbing coal. The coal in
the first bed is then desorbed until the second bed is saturated
and the cycle is repeated. Waste gas from sulfuric acid plants
is treated the same way. The advantages of this method are
better removal of nitrogen oxides with cost reduction, since no
extra fuel is required. Due to integration of the units for
preparation of acid and for recovery, higher output is ob-
tained; output of a nitric acid plant can be increased by 5% by
more complete use of NO2.
14568
SafiuUin, N. Sh. and M. I. Olevinskiy
RENDERING HARMLESS THE WASTE GASES FROM SUL-
FURIC ACID TOWER SYSTEMS. (Obezvrezhivaniye otk-
hodyashchikh gazov bashennykh sernokislotnykh sistem). Text
in Russian. Khim. Prom. (Moscow), no. 3:132-136, 1955.
It is reported that a complex consisting of a precipitation sec-
tion irrigated with strong acid and a moist electrofilter will as-
sure reliable purification of waste gases from tower systems.
Such a system reduces the aerosol and vapor sulfuric acid
content to 0.04-0.10 g/cu m, a 20-fold reduction. Complete ab-
sorption of an equimolar mixture of nitrogen oxides results in
a reduction in specific consumption rate of nitric acid by 6-8
kg/ton. Absorption of nitrogen oxides and reduction of nitric
acid discharge rate may be increased significantly by supplying
the equipment with nitrogen oxides with a degree of oxidation
of 45-50%. In order to assure normal operation of the equip-
ment, the amount of original sulfuric acid circulating in it must
be not less than 88%. Joint operation of both the irrigating
system and the electrofilter is imperative for proper purifica-
tion of waste gases.
14660
Herzog, G.
DESULFURIZATION OF FLUE GASES - PROBLEMS AND
SOLUTIONS. (Die Entschwefelung von Rauchgasen
Probleme und Losungswege). Text in German. Energietechnik,
17(12):539-542, Dec. 1967. 9 refs.
The state of the art of desulfurization methods in East Ger-
many is reviewed. The main emission sources for S02 in East
Germany are the power production plants and the sulfuric acid
industry. In 1965, the power plants emitted a total of 685,000
tons of S02. The sulfuric acid plants emitted about 17,500 tons
of SO2 in 1966. No economic desulfurization method yet ex-
ists to cope with these enormous emission quantities. The wet
processes based on absorption of SO2 by aqueous or alkaline
suspensions or solutions have three specific disadvantages.
The gases must be cooled prior to the desulfurization process,
which leads to corrosion problems in the heat exchanger; there
is a waste water problem; and the cold, wet gases have no
thermal buoyancy. Due to such problems, industry has turned
to dry methods in recent years. The Reinluft process for ox-
idation of SO2 to sulfuric acid over an activated carbon
catalyst has been of prime interest, although it is not economi-
cal. A brief outline of the essential principles of this method is
given. Oxidation of SO2 to SO3 and subsequent removal of
the latter by condensation with water to form H2SO4 or by
adsorption on activated coal is mentioned. Studies are
presently underway in East Germany on the binding of SO2 to
alkaline substances such as ash.
15739
Popovici, N., P. Potop, L. Brindue, and P. Anghel
PROPOSED EQUIPMENT FOR RETAINING SO2-CONTAIN-
ING RESIDUAL GASES DERIVED FROM THE MANUFAC-
TURE OF SULFURIC ACID, IN THE CONTEXT OF A FER-
TILIZER MANUFACTURING PLANT AND UNDER
FAVORABLE ECONOMIC CONDITIONS. (Proiectarea unei
instalatii de retinere a gazelor reziduale cu SO2 de la
fabricarea acidului sulfuric in cadrul unei uzine de in-
grasaminte complexe, in conditii economice avantajoase). Text
in Romanian. Rev Chim. (Bucharest), 18(l):40-44, 1967. 17
refs.
Economic development of Rumania calls for increasing the
production of chemical fertilizers, including ammonium
phosphate, to 340,000 tons in 1965 and 1,300,000 tons in 1970.
The need for industrial sulfuric acid is also increasing. Am-
monia can be used to remove SO2 from exhaust gases and
phosphoric acid to decompose the ammonium sulfite-bisulfite
solution. Optimum values, when working with an SO2 concen-
tration of 0.2-0.3%, are a liquid-gas relationship of about 3.5
per thousand; a SO2/NH3 ratio of 0.7; a maximum and 50 C
maximum concentration of ammonium sulfite bisulfite in solu-
tion of 700 grams per liter; absorption temperature. Phosphoric
acid is used as decomposing agent of the bisulfite solution,
preferably with a gas flow of 75 meters per second. Optimum
values to be achieved include: a 50% P205 concentration in the
phosphoric acid; an H3P04/NH3 ratio of 2.2 minimum; an
operating temperature of 95 C; and a liquid-gas ratio of .0043.
Under these conditions a 90% recovery of SO2 is possible. A
device designed to achieve these conditions can process about
44,000 Nm3 per hour of residual gases containing 0.2-0.3%
SO2 at a minimum operating cost. This cost (for water, steam,
and electrical energy) is offset by the amount of extra sulfuric
acid obtained: about 3,500 tons per year.
15846
Koto, K.
REMOVAL OF SULFUR DIOXIDE FROM EXHAUST GAS.
(Haigasu chu no aryusan gasu shori-ho). Text in Japanese.
(Toa Gosei Chemical Industry Co., Japan) Japanese Pat.
174,880. 2p., June 6, 1948. (Appl. Dec. 28, 1943, claims not
given).
The coal dust and inorganic compounds (SiO2, Fe2O3, A1203,
CaO) resulting from coal gas production are used to remove
sulfur dioxide gas from factories engaged in sulfuric acid
manufacture. This coal dust is activated by the high tempera-
ture, oxygen, and steam, and shows a tremendous adsorptive
power for SO2. In addition, the inorganic compounds included
in large amounts with the coal dust (40.23 to 57.96%), neutral-
ize the SO2 present in the water. Thus, 600 1 of coal dust is
homogenized with 1.7 1 of water and is scattered inside a
cylinder in which SO2 (0.7% of the total exhaust gas) passes at
the rate of 135 cu m/min. The washed exhaust gas includes
only 0.04% of SO2 at a temperature of 12 C. The coal dust can
be used in this procedure for 48 hrs.
-------
B. CONTROL METHODS
13
15879
IMPROVEMENTS IN OR RELATING TO A PROCESS FOR
RECOVERING SULPHUR DIOXIDE FROM A GAS MIX-
TURE CONTAINING THE SAME. (American Smelting and
Refining Co., New York) British Pat. 564, 734. 5p., Oct. 11,
1944. (Appl. June 29, 1942, 16 claims).
In a cyclic process for recovering sulfur dioxide from smelter
smoke, flue gases, etc., sulfur dioxide-containing gas is first
absorbed in an aromatic amine reagent of the aniline class and
its homologues and derivatives preferably dirnethylaniline. The
exit gases are then scrubbed with sodium carbonate and sul-
furic acid solutions to remove the reagent, following which the
resulting solutions' are combined and heated by steam to
release the sulfur dioxide and the regenerated amine esters.
The released reagent is returned to absorb additional sulfur
dioxide. While various types of scrubbers may be employed in
the process, best results are obtained with bubble towers.
Compared to other processes, the operation greatly reduces re-
agent losses and regenerative costs.
15991
Fleming, Edward P. and T. Cleon Fitt
RECOVERY OF SULPHUR DIOXIDE FROM GAS MIX-
TURES. (American Smelting and Refining Co., New York) U.
S. Pat. 2,295,587. 3p., Sept. 15, 1942. (Appl. Nov. 25, 1939, 7
claims).
A cyclic process for recovering sulfur dioxide from smelter
smoke, flue gases, and the like uses an aromatic amine as the
reagent absorbant. Compared to other methods, the process,
which preferably takes place in a bubble tower, greatly
reduces reagent losses and regenerative costs. Sulfur dioxide-
bearing gases, after cleaning to remove nongaseous contami-
nants, are passed to the bottom of an absorber where they
flow upward in countercurrent to the absorbent, preferably
dimethylaniline. Within the absorber, the sulfur dioxide is
transferred from the gas mixture to the dimethylaniline, with
the efficiency of the transfer enhanced by controlled cooling
of the absorber. The sulfur dioxide-depleted gases are passed
through sodium carbonate and sulfuric acid solutions and
steam is added to free the gases from the regeant. The aro-
matic amine and sulfur dioxide mixture is passed through a
heat exchanger on its way to the stripping tower. The excess
steam and reagent vapors are brought into contact with the
aromatic amine and sulfur dioxide mixture to expel the latter
and yield a warm stripped reagent. The stripped reagent is
further cooled and separated into two components, mainly
water and reagent. The anhydrous reagent is returned for
treating additional volumes of sulfur dioxide-bearing gases.
16289
Yeselev, I. M., I. P. Mukhlenov, and D. G. Traber
CERTAIN QUESTIONS ABOUT THE OPERATING REGIME
OF A COMBINED CONTACT-TOWER SYSTEM. (Nekoto-
ryye voprosy rezhima raboty kombinirovannoy kontaktno-
bashennoy sistemy). Text in Russian. Zh. Prikl. Khim., vol.
37:1204-1210, May-Aug., 1964.13 refs.
Analysis of data from the literatures showed that optimum
temperatures in the preliminary catalytic oxidizing arrange-
ment with a fluidized catalyst bed are subject to the same de-
pendences as in arrangements with a stationary bed. Formu-
lated calculations indicate that a system producing 315,000
tons of sulfuric acid per year is economically feasible with a
preliminary oxidation arrangement using an iron oxide catalyst
with a particle size ranging from 0.80 to 1.30 mm.
16290
Yeseleve, I. M., I. P. Mukhlenov, and D. G. Traber
USE OF DION CATALYST IN THE CONTACT-TOWER
PROCESS. H. (K voprosu ispol'zovaniya zheleznogo kataliza-
tora v kontaktno-bashennom protsesse). Text in Russian. Zh.
Prikl. Khim., vol. 37:972-979, May-Aug., 1964. 14 refs.
The rate of sulfur dioxide oxidation in a reactor with a
fluidized iron oxide catalyst bed is reduced as compared with
a reactor with a stationary layer. The degree of reduction in
rate is characterized by the ratio of contact time required to
achieve a given degree of conversion in a fluidized catalyst
bed to the analogous contact time for a stationary layer, all
other conditions being equal. Empirical formulas derived for
determining this ratio are shown to describe the kinetics of
SO2 oxidation in an arrangement with a fluidized catalyst bed
with sufficient accuracy. Verification on a pilot installation has
demonstrated complete suitability of these equations for desig-
ning industrial reactors.
16291
Lastochkin, Yu. V., I. P. Mukhlenov, I. G. Lesokhin, Ye. S.
Rumyantseva, and T. P. Bondarchuk
OXIDATION OF SULFUR DIOXIDE IN AN ARRANGEMENT
WITH A PSEUDO FLUIDIZED BED OF HtON OXIDE
CATALYST UNDER CONDITIONS OF CONTACT-TOWER
PRODUCTION OF SULFURIC ACID. (Okisleniye semistogo
gaza v apparate s psevdoozhizhennym sloyem okisnozhelez-
nogo katalizatora v usloviyakh kontaktno-bashennogo proiz-
vodstva semoy kisloty). Text in Russian. Khim. Prom.
(Moscow), 42(6):45-48, 1966. 4 refs.
Optimum conditions for sulfuric acid production in a pseudo
fluidized bed of an iron oxide catalyst were studied on both a
laboratory and industrial scale. Data indicated that, with a sul-
fur dioxide content of 12% at an optimum temperature of 680-
700 C, there is a sharp rise in catalyst productivity with an in-
crease in volumetric gas flow rate. With a constant linear gas
flow rate, there is a resultant decrease in hydraulic resistance
of the system and an increase in the volumetric flow rate, at
the same time, a minimum required degree of preliminary ox-
idation is assured. Increasing the volumetric flow rate also
reduces catalyst consumption to five times below existing
systems using vanadium catalysts.
16447
Tamm, O. M. and E. M. Vasil'eva
MEASURES FOR REDUCING ATMOSPHERIC POLLUTION
IN CTITES OF THE ESTONIAN SSR. (Meropriyatiya po sniz-
heniyu zagryazneniya atsmofernogo vosdukha v gorodakh
Estonskoy SSR). Text in Russian. In: Sanitation Measures
Against Air and Water Pollution in the Planning of Cities. (Oz-
dorovleniye vozdushnogo i vodnogo basseynov gorodov).
Government Committee on Civil Building and Architecture
(ed.), Lecture series no.2, Kiev, Budivel 'nik, 1968, p.39-40.
Air pollution problems in Estonia center around the cities of
Tallinn and Kohtla-Jarve. A paper and pulp plant, a sulfuric
acid plant, a mineral-enriching installation, and a shale
processing combine are cited as major air pollution sources in
the Kohtla-Jarve area and some of the measures taken to con-
trol these sources are mentioned. Control measures widely in-
stituted in the country include: conversion to gas and liquid
fuels, the use of central heating plants, removal from the cities
of large pollution sources such as asphalt-concrete plants, and
the closing of installations which do not lend themselves to air
pollution control (e.g., the stone crushing facility at the Tallinn
concrete plant, and the asphalt-concrete plant at Toyl).
-------
14
SULFURIC ACID MANUFACTURING
16480
Boreskov, G. K., L. G. Rimmer, and E. I. Volkova
IGNITION TEMPERATURE OF VANADIUM SULFURIC
ACID CATALYSTS. (Temperature zazhiganiya vanadievykh
sernokislotnykh katalizatorov) Text in Russian. Zh. Prikl.
Khim., 13(3):250-260, 1949. 7 refs.
A thermographic method of determining the ignition tempera-
ture of the catalytic mass was developed and verified. The ig-
nition temperature of sulfuric acid-vanadium catalysts was ex-
perimentally determined for gas mixtures containing from 7-
95% sulfur dioxide and 5-75% oxygen at initial degrees of
catalysis of 0 to 50%. It was shown that a change in the igni-
tion temperature of vanadium catalysts in relation to the com-
position of the gas was dependent on the shift of the tempera-
ture of the phase transformation of the catalytically active
polyvanadates into vanadyl sulfates and with a change in the
reaction rate. Equations are proposed and a diagram con-
structed for determining of the ignition temperature of gas
mixtures of varying composition. At a constant concentration
of oxygen, the ignition temperature was practically indepen-
dent of the sulfur dioxide concentration. With an increase in
oxygen concentration, the ignition temperature decreased. For
gas obtained by roasting pyrites and containing 7% sulfur diox-
ide and 11% oxygen, the ignition temperature was 423 C. For a
stoichiometric mixture (66.7% sulfur dioxide, 33.3% oxygen),
the ignition temperature equalled 394 C. An increase in the
degree of catalysis to 50% increased the ignition temperature
20-30 deg. A decrease in the activity of the vanadium catalysts
as a result of terminal treatment or lengthy processing in-
creased the ignition temperature which was directly propor-
tional to the logarithm of the ratio of thyinitial and final values
of the reaction rate constant. The temperature of extinction
was determined for gas mixtures containing 7% sulfur dioxide;
11% oxygen and 50% sulfur dioxide; and 50% oxygen. At a
hypothetical linear gas flow rate equal to 0.15 m/sec, the tem-
perature of extinction in the first case was 7 deg and in the
second, 85 deg below the temperature of ignition. The dif-
ference in the temperatures of ignition and extinction cor-
responded well with the difference in surface temperature of
the grains in the first layer of catalyst and gas, calculated ac-
cording to the rate of heat loss. This indicates that catalytic
oxidation of sulfur dioxide is carried out entirely at the surface
of the catalyst.
16718
Remirez, Raul
DOUBLE-ABSORPTION GETS U.S. FOOTHOLD. Chem.
Eng., 76(2):80-82, Jan. 27, 1969.
The first sulfuric acid plant in the Western Hemisphere to use
a double-absorption process will soon be constructed. The
process has been popular in Europe not only for its antipollu-
tion properties but also because the higher conversion (99.5%)
results in attractive raw-material savings. However, installation
and operating costs still appear to be substantially higher than
for single absorption units. When sulfur emission control laws
are enacted it is probable that single absorption plants now in
existence will find it desirable to either convert to the double
absorption process or improve the efficiency of the present in-
stallation. Some of the possible avenues open to improve the
single absorption units are discussed.
17053
Connor, John M.
NEW METHOD REDUCE AIR POLLUTION IN OLDER SUL-
FURIC ACID PLANTS. Water Sewage Works, 117(1):IW/16-
IW/19, Jan.-Feb. 1970.
There are a large number of plants in operation and in good
shape, producing large quantities of acid, which were not
designed according to current conversion standards and which
cannot, without modification, meet the proposed new air pol-
lution standards. Many of the smaller plants will probably be
shut down, but the larger plants in good condition can be
modified. Two schemes are offered for removing the sulfur
dioxide from sulfuric acid plant stacks. Flow charts are given.
A modified version of the first scheme could be designed to
suit roaster gas plants in some cases, but the problem in con-
nection with these plants is much more complex and each
plant would have to be considered individually. The second
scheme is simpler to install in an existing plant, and can poten-
tially increase the total output of the plant by 10 to 20% and
improve conversion at the same time. By taking advantage of
the fact that the double absorption process is usually operated
with 10% SO2 in the converter feed, compared to 8% in the
standard plant, scheme 2 could be used to increase production
by as much as 35%.
17810
Srbek, Josef, Rostislav Klimecek, and Lubomir Jager
PROCESS OF RECOVERING SULFUR DIOXIDE FROM EX.
HAUST GASES. (Zpusob zachycovani kyslicniku siriciteho z
odpadnich plynu). Text in Czech. (Assignee not given.) Czech.
Pat. 108093. 3p., Aug. 15, 1963. (Appl. Nov. 15, 1958, 2
claims).
A process of recovering sulfur dioxide during the last stages of
sulfuric acid manufacture is presented. The exhaust gas is
channelled to the absorption device, where a solid compound
of zinc is in water suspension. The process is characterized by
using only that amount of the water suspension of zinc oxide
or hydroxide which corresponds to the amount of the ab-
sorbed SO2 from the exhaust gases. To prevent solidifying the
suspension, a very diluted suspension below 3% of the total
amount of zinc should be used.
17887
Garbato, Carlo
PROCEDURE FOR CATALYTIC OXIDATION OF SUL-
FUROUS GASES, NO MATTER HOW PRODUCED, AS A
MEANS OF MANUFACTURING SULFURIC ACID AND OLE-
UM, USING CATALYSTS DISPERSED AS A FINE DUST IN
THE REAGENT GAS AND CmCULATTNG WITH IT:
MEANS AND DEVICES FOR ITS APPLICATION. (Procedi-
mento per 1'ossidazione catalitica di gas solforosi, comunque
prodotti, per la fabbricazione di acido solforico ed oleum a
mezzo di catalizzatori dispersi in povere fine nella massa gas-
sosa reagente, e con essa fluenti mezzi e apparecchiatura per
realizzarlo). Text in Italian. (Assignee not given.) Italian Pat.
435,452. 3p., May 18, 1948. (Appl. April 11, 1946, 6 claims). In
the process of making sulfuric acid from sulfurous gases, the
principle of a 'flowing' rather than a 'static' catalyst is
preferred, wherein the catalyst is pulverized to a suitable parti-
cle size and is circulated directly with the gas itself throughout
the apparatus. This avoids the problem, encountered with the
stationary catalyst, of the accumulation of heat in the catalyst,
which if not dissipated in some way or other causes the reac-
tion temperature to rise, disturbing the relationship of SOS to
SO2, thereby reducing the yield of sulfuric acid. The preferred
catalyst is an iron oxide produced by roasting powdered iron
pyrite. The pyrite roasting and the SO2 oxidation take place in
the same apparatus, the iron oxide produced being used im-
mediately as catalyst for the oxidation of SO2. Catalysis takes
place in a special apparatus consisting of a metal chamber,
which is cooled by the circulation of some type of fluid which
-------
B. CONTROL METHODS
15
absorbs excess heat produced by the reaction. The apparatus
is constructed so as to resist pressures above atmospheric
pressure. A partial catalysis may also be performed with a cir-
culating catalyst wherein the process is completed with the
conventional 'static' process.
17889
Roesner, Gerhard
UTILIZATION OF INDUSTRIAL AND RESIDUAL GASES BY
THE METHODS OF THE LURGI ENTERPRISES. (L'Utilisa-
tion de Gaz Industrials et Residuels par les Precedes des
Societes Lurgi). Text in French. Metallges. Periodic Rev., no.
13:22-31, 1938. 8 refs.
The modern trend in the chemical industry is to utilize
processes in which the chemical reactions take place in the gas
phase. This raises the problems of cleaning gases prior to their
reaction, as well as of processing the residual gases of that
reaction. The Lurgi enterprises address themselves to the task
of providing engineering solutions to these kinds of problems,
including processes of purification of reacting gases of sub-
stances which 'poison the catalyst' used to accelerate or to
make possible the desired reaction and processes of remove!
of dust and other participate solids, of condensable vapors,
and of gaseous constituents from the residual gases, with the
objective of their recovery or of prevention of their discharge
into the atmosphere. Various devices and existing industrial in-
stallations are reviewed, such as 'Multiklon' centrifugal dust
separators, electrostatic filters for removal not only dry dusts
but also condensable mists, scrubbing towers for selective ab-
sorption of gases or mists by liquid absorbents and the
'Benzobon' process of absorption by solid charcoal of benzene
from city gas or coking-plant gas. A large section of the paper
is devoted to the removal of sulfur dioxide and hydrogen sul-
fide from waste gases, the production of ammonium sulfate
and particularly the production of sulfuric acid.
19033
Roll, Kempton H.
CONTROLLING CORROSIVE AIR POLLUTANTS. J. Air Pol-
lution Control Assoc., 1(6):6-10, May 1952.
Control of an aerosol, such as sulfuric acid mist, is a problem
of collection, but an entirely different technique must be util-
ized in the case of a gas such as sulfur dioxide. Conversion of
SO2 to H2SO4 is a possibility, as is absorption of the gas in
chemicals from which it can be recovered as pure SO2.
Hydrogen sulfide is now being treated in a number of oil
refineries by burning it in air to convert it to sulfur dioxide
and water vapor or by burning it in the presence of sulfur
dioxide to convert it to elemental sulfur and water vapor. It is
common practice to add an electrostatic precipitator at the end
of the processing circuit through which all gases bearing sul-
furic acid mist must pass. As the gases pass through the
precipitator, they receive electrical charges which cause them
to coalesce, whereas the sonic collector operates on the princi-
ple that high intensity sound will cause particulate matter to
agglomerate and descend to the bottom for removal. One of
the newest and most successful methods of converting sulfur
dioxide to liquid involves dissolving the impure gas in cool
dimethylaniline and extracting it as pure SO2 by heating the
pregnant dimethylaniline solution.
19228
Drechsel, Herbert, Karl-Heinz Doerr, and Hugo Grimm
METHOD FOR THE CATALYTIC OXIDATION OF SO2 TO
SO3 IN SO2 LADEN GASES AND PRODUCTION OF SUL-
FURIC ACID. (Verfahren zur katalytischen Oxydation von
SO2 in SO2-haltigen Gasen zu SOS und Herstellung von
Schwefelsaeure). Text in German. (Metallgesellschaft A. G.,
Frankfurt (W. Germany)) Swiss Pat. 478,712. 4p., Sept. 30,
1969. (Appl. Oct. 25,1963, 5 claims).
A method for the catalytic oxidation of sulfur dioxide in SO2-
laden gases to SOS with the aid of oxygen containing gases
and production of sulfuric acid by absorption of the formed
SOS is described. The SO2-laden gases are heated by heat
exchange with the formed SO3 containing gases. The SO2 con-
tent in the gases is increased prior to catalytic oxidation by
mixing with gases from the combustion of sulfur. The inven-
tion pertains to the use of primary gases with an SO2 content
at 9% or less by volume. The hot gases from the combustion
of sulfur are mixed at least with part of the heated flow of pri-
mary gas after it has left the heat exchanger and prior to the
entrance into the catalytic oxidation chamber. The sulfur and
oxygen quantities must be selected so that the sum of the heat
developing at the combustion of sulfur to S02 plus the heat
developing at the oxidation of SO2 to SOS suffices to compen-
sate for the heat loss suffered at the intermediate absorption
of SOS. The sulfur dioxide content of the mixture of primary
gas/sulfur combustion gas may not exceed 9% by volume. A
branch of non-heated SO2 containing primary gas is added to
this gas mixture to obtain a temperature of 440 C (maximum).
If the primary gas contains less than 9% SO2, 3 to 4 kg,
preferably 3.5 kg, sulfur per 1000 cu m primary gas are burned
for each missing percentage and added to the gas.
19370
Ganz, S. N., I. E. Kuznetsov, V. A. Shlifer, and L. I. Leikin
REMOVAL OF NITROGEN OXIDES, SULFUR DIOXIDE,
MIST, AND SULFURIC ACID SPRAY FROM EXHAUST GAS
BY PEAT-ALKALI SORBENTS UNDER PRODUCTION CON-
DITIONS. J. Appl. Chem. USSR (English translation from
Russian of: Zh. Prikl. Khim.), 41(4):700-704, April 1968. 1 ref.
Optimal conditions were determined for the absorption of
nitrogen oxides, sulfur dioxide, mist, and sulfuric acid spray
from sulfuric acid tower systems by means of peat-alkali ab-
sorbents. Shredded peat with a moisture content up to 50%
was used for absorption; solid ash, apatite concentrate, aque-
ous ammonia, and ammonia gas were used as additives to the
peat. The moisture content of the peat in the absorber must
not be below 25-30%, as at lower moisture contents the peat
begins to form dust and the absorption process deteriorates
considerably. Ammonia introduced directly to the fluidized
beds was the most effective additive, removing 90% of the
acidic components of the waste gas in 90 min. For 80% purifi-
cation of the gas in one hr, it is sufficient to have one or two
beds with a total sorbent height of about 500 mm. A sulfuric
acid plant with a gas output of up to 60,000 cu m/hr will
require 0.294 tons ammonia, 1.5 tons of dry peat, and 3 tons of
peat (with a moisture content of 50%) per hr for gas decon-
tamination. Sorption of the gases by the peat-ammonia sorbent
yields an effective organomineral fertilizer.
19383
SO2 ABSORBER: TWO SCRUBS BETTER THAN ONE.
Chem. Eng., 62(2):132-134, Feb. 1965.
Sulfur dioxide in concentrations as high as 0.9% is effectively
removed from sulfuric acid plant fumes in a double scrubbing
tower that comprises two separate scrubbers built one above
the other. The scrubbing system utilizes ammonium sulfite-
bisulfite solutions. Inlet gases pass countercurrent to the first
scrubbing solution in the lower scrubber, where most of the
sulfur dioxide is recovered. Gas then moves through a chim-
^ .,
LIBRARY
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16
SULFURIC ACID MANUFACTURING
ney to the upper section, where a weaker solution removes the
remaining sulfur dioxide. Tail gases discharged to the at-
mosphere contain less than 0.3% sulfur dioxide. Ammonium
sulfate is recovered as a by-product by passing the solution
from the lower scruober to a stripping tower and reacting it
with sulfuric acid from the acid unit. The ammonium sulfate is
pumped to an adjacent fertilizer plant.
19469
Woollam, J. P. V. and A. Jackson
THE REMOVAL OF OXIDES OF SULPHUR FROM EXIT
GASES. Trans. Inst. Chem. Engrs. (London), vol. 23:43-51,
1945. 33 refs. (Presented at the Institution of Chemical En-
gineers North Western Branch Meeting, Manchester, England,
March 17, 1945.)
A process is described for removing sulfur dioxide and triox-
ide from the exit gases of contact acid plants, boiler installa-
tions, and smelting processes. It consists of scrubbing the
gases with a solution of ammonium sulfite, bisulfite, and
sulfate mixture, keeping the pH value at a predetermined
figure by the addition of aqueous ammonia, and bleeding off
the make of solution to an autoclave where it is heated with
steam to form ammonium sulfate solution and sulfur. On the
basis of encouraging preliminary tests, a large-scale process
facility was built at a contact acid plant. Testing and results
are given in detail, and permit definition of the limits for op-
timum conditions. The SO2 and SOS present in the exit gases
can be reduced to less than 5% of their original value, and the
price of the ammonia feed can be reduced to 60% of that for
the pure 25% ammonia by the use of 18-20% concentrated gas
works liquor. Two applications of the process are briefly
discussed: acid plant exit gas treatment, and 'devil gas' treat-
ment with reference to a 15% hydrogen sulfide gas mixture.
19486
Hara, Maruichi
RESEARCHES ON CONTACT REACTION RATE FOR SO2-
OXTOATION. Ann. Genie Chim., 1967:187-196, 1967. 6 refs.
The velocities of contact reaction rates for sulfur dioxide ox-
idation over vanadium pentoxide-industrial catalyst were mea-
sured for both forward and reverse reactions using a dif-
ferential reactor. For gas phase reactions, an approximate rate
formula of catalytic reaction was derived theoretically in case
of the reactions being in stationary state and having no side
and no consecutive reactions. Results of applying the derived
formula to the experimental data and to many reactor designs
for sulfuric acid factories in Japan were satisfactory. (Author
abstract modified)
19592
Takeuchi, Tsugio and Tamotsu Tanaka
DRY REMOVAL PROCESS OF SULFUR COMPOUNDS IN
EXHAUST STACKS. Translated from Japanese. Franklin Inst.
Research Labs., Philadelphia, Pa., Science Info. Services, 3p.,
Oct. 29, 1969.
The ability of activated charcoal to remove sulfur dioxide
from exhaust gas in the form of sulfuric acid was tested by
passing the treated gas through a hydrogen peroxide solution
and titrating by alkali the H2SO4 that was produced in the
solution. The amount of sulfur dioxide entrained by the char-
coal varied greatly with the linear velocity of the gas and with
space velocity. In addition, activated charcoal wetted with am-
monium sulfate captured about three times as much sulfur
dioxide as the original activated charcoal. Presumably, the sul-
furic acid produced on the charcoal reacts with ammonium
sulfate to yield ammonium hydrosuifate and to free sulfuric
acid not produced on the charcoal. The experiments demon-
strate that ammonium sulfate can be used to regenerate the ac-
tivated carbon and that crystallized ammonium sulfate can be
easily recovered as a by-product.
19593
Chemical Construction Corp., New York, N. Y., Consulting
Div.
A BD3LIOGRAPHY OF REMOVAL OF NITROGEN OXIDES
FROM WASTE GASES, EXCEPT METHODS BASED ON
REDUCTION AT HIGH TEMPERATURE AND CATALYTIC
DE-COMPOSITION, 1907-1968, WITH ABSTRACTS. (PART
4). In: Engineering Analysis of Emissions Control Technology
for Sulfuric Acid Manufacturing Processes. Volume 2. Litera-
ture Search. Contract CPA 22-69-81, 52p., March 1970. 158
refs. CFSTI: PB190471
References and abstract from U. S. and foreign sources, in-
cluding patents, are arranged and indexed by a variety of in-
dividual adsorption and absorption control methods, within
one of two major subdivisions. Part One pertains to the
removal of nitrogen oxides from chamber and Mills-Packard
sulfuric acid plant tail gases, while Part Two is concerned with
the removal of low concentrations of nitrogen oxides from
waste gases.
19594
Chemical Construction Corp., New York, N. Y., Consulting
Div.
A BD3LIOGRAPHY OF SULFUR TRIOXTOE AND SULFURIC
ACID MIST EMISSIONS AND THEm CONTROL, 1907-1968,
WITH ABSTRACTS. (PART 3). In: Engineering Analysis of
Emissions Control Technology for Sulfuric Acid Manufactur-
ing Processes. Volume 2. Literature Search. Contract CPA 22-
69-81, 32p., March 1970. 105 refs. CFSTI: PB 190471
References and abstracts from U. S. and foreign sources, in-
cluding patents, are arranged and indexed by subject into
seven major categories. These are: sulfuric acid mist forma-
tion; physical behavior of H2SO4 mists; sulfuric acid mist
emissions and their control; mist removal in general; sulfuric
acid mist removal; sulfur trioxide removal; and analytical
methods.
19595
Chemical Construction Corp., New York, N. Y., Consulting
Div.
A BIBLIOGRAPHY OF SULFUR DIOXIDE REMOVAL AND
RECOVERY FROM WASTE GASES AND SULFURIC ACID
PLANT TAIL GASES, EXCLUDING THE LIMESTONE AND
DOLOMITE INJECTION PROCESSES, 1953-1968, WITH AB-
STRACTS. (PART H). In: Engineering Analysis of Emissions
Control Technology for Sulfuric Acid Manufacturing
Processes. Volume 2. Literature Search. Contract CPA 22-69-
81. 58p., March 1970. 223 refs. CFSTI: PB 190471
References and abstracts from U. S. and foreign sources, in-
cluding patents, are arranged and indexed by subject within 13
major categories. These are: data on SO2 emissions; toxicity
and tolerance of SO2 in the atmosphere; absorption of SO2 in
water; absorption of SO2 in inorganic aqueous salt solutions;
aqueous slurries; sorption by solid materials; molten salts;
aqueous solutions of organic compounds; oxidation of SO2 to
SO3; removal of SO2 by reduction; chromatographic separa-
tion; general reviews and economic aspects; and bibliogra-
phies. Several tables of data on SO2 air pollution are also in-
cluded.
-------
B. CONTROL METHODS
17
19606
Burgess, Wilfred Duncan
TREATMENT OF FLUE GASES. (Consolidated Mining and
Smelting Co. of Canada, Ltd., Montreal (Quebec)) U. S. Pat.
2,862,789. 8p., Dec. 2, 1958. 8 refs. (Appl. May 17, 1954, 4
claims).
A method of economically recovering sulfur from flue gases
which contain very small amounts of sulfur oxides is
presented. The process employs ammonium sulfate as an ab-
sorbing agent, and involves a series of cooling and concentrat-
ing steps and treatment with sulfuric acid. Previously, in ap-
plying this absorption process to the treatment of gases from
combustion furnaces, a number of difficulties were encoun-
tered, such as: high cost of cooling gases to the desired tem-
perature, problems with fly ash acting as condensation nuclei,
and evaporation of large quantities of water in order to avoid a
very dilute concentration of ammonium sulfate. These difficul-
ties are successfully overcome by the process described.
19644
Tsudo, Kozaburo
OPERATION OF SO2 GAS ABSORBING PLANT. Nippon
Kokan Giho (Tokyo), 19(1): 1-6, 1966. Translated from
Japanese Belov and Associates, Denver, Colo., 19p., April 21,
1970.
A method for controlling sulfur emissions from a sulfuric acid
plant is described. This method is a limestone-gypsum injec-
tion where the sulfurous acid gas and sulfur dioxide are
neutralized, and the gypsum is recovered. Lime milk is
sprayed into an elimination tower where the SO2 and acid are
absorbed. The solution containing SO2 is sent to a pH tower
where it is regulated to a suitable pH by an acidification reac-
tion. Calcium sulfite, formed in the elimination tower, is sent
to an acid tower. Here it is acidified to calcium sulfate to form
gypsum by minute mist. The gypsum is transported to a gyp-
sum thickener where it is separated, washed, and deliquidated.
The operation and production data of this system are also in-
cluded.
19682
Amelin, A. G.
CONDENSATION OF SULPHURIC ACID. Ann. Genie Chim.,
1967:52-61, 1967. 12 refs.
The process of sulfuric acid condensation is complicated by
several concurrent processes which are specific for the
production of sulfuric acid. Therefore, proper corrections
should be introduced into average calculation formulae.
Moreover, sulfuric acid vapor is easily condensed in volume,
forming a stable mist which causes great difficulties in produc-
tion processes. When a vapor-gas mixture contacts a colder
surface, two independent processes occur simultaneously cool-
ing of the gas and condensation of the vapor. The rates of
these processes are in such a relation that at the beginning,
vapor oversaturation increases, reaches the maximum value,
and then goes down. When oversaturation reaches the critical
value, the vapor condenses in volume forming nuclei which
later increase because of condensation growth. While consider-
ing the process of vapor condensation on the surface, it is
necessary to differentiate strictly between conditions before
and after mist formation. In the first case, the process of con-
densation can be calculated according to well-known formulae,
in the second case a stage-by-stage method of calculation is
used. The results of investigations show that the necessary
data are available for establishing such condensations under
which the formation of mist can be eliminated. However, this
is usually connected with the decrease of condensation
process rate. Therefore it often appears very profitable to con-
duct the process at high rates with the formation of larger
drops of mist and then to remove that mist in filters. Minimum
material expenses for the realization of the process are deter-
mined by vapor condensation on the surface and by the condi-
tions of mist evolution in filters. (Author abstract modified)
19856
Postnikov, V. F. and T. I. Kunin
ON THE RECOVERY OF SO2 FROM WASTE GASES FROM
CONTACT SULFURIC-ACID PLANTS. (K voprosu Iz-
vlecheniya SO2 iz otkhodyashchikh gazov kontaktnykh Ser-
nokislotnykh zavodov). Text in Russian. In: Tr. Ivanovsk.
Khim. Tekhnol. Inst., no. 2, p. 56-70, 1939.
The use of a quinoline-water mixture as a sulfur dioxide ab-
sorber was studied experimentally, and a 1:1 ratio was found
to be optimum. Absorption was significant, but neither the
degree of SO2 accumulation, nor the frequency of regenera-
tion, were determined. Studies were made at 20-100 C with gas
mixtures containing 0.7% SO2 and 0.2-0.3% SO3, and with gas
flow rates ranging 0.09-0.24 m/sec.
19886
Bacon, Raymond F. and Isaac Bencowitz
RECOVERY OF SULPHUR. (Raymond F. Bacon) U. S. Pat.
1,917,234. 5p., July 11, 1933. (Appl. July 29, 1930, 11 claims).
In various processes suggested for recovering elemental sulfur
from roaster gases, the sulfur dioxide gases are usually treated
at some point removed from their source. This results in loss
of the sensible heat of the gases, and the necessity of supply-
ing supplemental heat to replace the lost heat. A process is
described for recovering elemental sulfur from SO2 gases in
which the high sensible heat of the gases is retained, and addi-
tional heat is derived from the furnace itself. The hot gases are
first sent to a collector to remove any fine dust entrained in
the SO2. The cleaned gases are passed into the reaction
chamber where they are contacted with a reducing gas, such
as natural gas, water gas, or producer gas. The temperature of
the reducing gas is raised when it is mixed with the hot SO2
gases, and by absorption of heat from the burner. The reaction
between the S02 and the reducing gas is rapid and exothermic.
As the gases leave the chamber they are cooled in a waste
heat boiler, and treated with an electrostatic precipitator or by
absorption to remove the sulfur. The residual gases may be
catalytically oxidized to remove hydrogen sulfide and recover
additional sulfur.
19943
Grodzovskiy, M. K.
MECHANISM OF CATALYTIC OXTOATION OF SO2 IN A
SOLUTION OF MANGANESE SALTS. H. THE EFFECT OF
OZONE ON MANGANESE SALT SOLUTIONS. (Mekhanizm
kataliticheskogo okisleniya SO2 v rastvore solei margantsa. II.
Deystviye ozona na rastvor zaMsnoy soli marganitsa). Text in
Russian. Zh. Fiz. Khim., vol. 6:496-510, 1935.
Studies of sulfur dioxide oxidation in manganese salt solutions
have led to the following conclusions: SO2 concentrations of
0.3-0.4% do not provide sufficient conversion of Mn-2 to Mn-3
when used as the catalyst in amounts of about 5%; low O2
partial pressure (5-10%) in the flue gases also hampers this
conversion, or renders it nonexistent with poor absorption
equipment; as acidity increases, alpha 02 decreases to 30-40%
sulfuric acid, and the rate of induced oxidation diminishes to
zero due to inhibition of complex formation, oxidation, and to
a drop in regenerative capability of the catalyst resulting from
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18
SULFURIC ACID MANUFACTURING
formation of stable Mn2(SO4)3; increasing catalyst concentra-
tion above 0.025% has no further effect, especially when the
oxygen partial pressure is low; increasing the solution volume
in itself yields no improvement; negative catalysts poison the
manganese; the action of ozone is necessary to counteract the
above factors so as to maintain manganese activity; gradually
increasing the ozone concentration maintains oxidation and
regeneration up to a practical H2SO4 level of 50% (60-65%
maximum) even with low SO2 and O2 concentrations; ozone
should lead both to accelerated oxidation of MNSO2 and to
direct oxidation of Mn-2; these and other effects of ozone
form a basis for evaluating the use of ozone to produce con-
centrated sulfuric acid from flue gases; since SO2 oxidation
proceeds by means of Mn oxidation, perhaps more economical
means are possible, such as electro-oxidation.
20024
Yeselev, I. M., I. P. Mukhlenov, and D. G. Traber
USE OF IRON CATALYST IN THE CONTACT-TOWER
PROCESS. (K voprosu ispol'zovaniya zheleznogo katalizatora
v kontaktno-bashennom protsesse). Text in Russian. Zh. Prikl.
Khim., vol. 37:722-727, Jan.-April 1964. 22 refs.
Equations were verified for calculating the contact time of gas
on an iron catalyst that were sufficient to yield a given degree
of conversion. Sulfur dioxide was oxidized over a stationary
iron catalyst layer with a grain size of 0.75 mm. The gas flow
rate was 0.975 m/sec and rate constants were determined over
the range 610-730 C. Estimations of the energy of activation
were about 126 kJ/mole for temperatures above 640 C, and 280
kJ/mole below 640 C. The discountinuity at 640 C is explained
by the conversion of active ferric oxide to the inert sulfate.
The literature is reviewed with respect to the reaction kinetics
for SO2 absorption on an iron catalyst with both stationary
and fluidized beds.
20248
Public Health Service, Cincinnati, Ohio, National Air Pollution
Control Administration
A STATUS REPORT: PROCESS CONTROL ENGINEERING;
R & D FOR AIR POLLUTION CONTROL. 37p., Nov. 1969.
The various phases of the work of the Process Control En-
gineering Division of the National Air Pollution Control Ad-
ministration are described as of late 1969. These include sulfur
oxides control (dry and wet limestone processes, coal clean-
ing, and new processes such as those employing molten alkali
carbonates), industrial process control (nonferrous smelting,
iron and steel, sulfuric acid, papermaking, graphic arts, iron
foundries, aluminum smelting, etc.), combustion emissions
control (e.g., fluidized-bed combustion, nitrogen oxides), ap-
plied equipment research (wet scrubbers, fabric filters, electro-
static precipitators, incinerator control), supporting measure-
ments (detection, spectroscopy, dust and gas-sampling analy-
sis, holographic determinations, continuous monitors, etc.),
and advisory and supporting services. A special report is also
given on the alkalized alumina process for control of SO2. A
list of 110 specific research projects and 11 services is given.
More than eleven million dollars was budgeted for the Process
Control Engineering programs in 1969. The 1970 budget is ex-
pected to be more limited, necessitating an emphasis on
sustaining rather than new programs.
20416
(Inventor not given.)
PROCEDURE FOR PRODUCTION OF SULFURIC ACID.
(Precede de production d'acide sulfurique). Text in French.
(Mitsubishi shipbuilding and Engineering Co., Ltd., Japan)
French Pat. 1,348,923. 7p., Dec. 2, 1963. (Appl. Feb. 28, 1963,
5 claims.)
Two procedures are presented for producing sulfuric acid from
a gas containing sulfur oxides and from a suspension. In the
first case, the gas is brought into contact with an aqueous
suspension of a manganese oxide, of a concentration at which
it remains fluid, to form MnSO4. If the latter reacts with HC1,
H2SO4 and a crystalline precipitate of MnC12 are formed. In
the presence of O2 and H2O vapor at an elevated temperature,
MnC12 decomposes into HC1 gas and a Mn oxide, which are
returned to the operations of H2SO4 formation and MnC12
precipitation and of preparation of an aqueous suspension of a
Mn oxide. In the second case, from an aqueous suspension of
crystalline MnSO4, a gas containing hydrochloric acid is in-
troduced into the aqueous suspension at a temperature not ex-
ceeding 50 C and, preferably, at ambient temperature to
produce H2SO4 and crystalline MnC12. After separating the
latter from H2SO4, it is reacted with a gas containing O2 and
H2O vapor at a temperature between 350 and 600 C in order
to oxidize it to HC1 and a Mn oxide. The resulting gas contain-
ing hydrochloric acid is re-used for production of MnC12 from
MnSO4. In addition, a hot gas containing hydrochloric acid
produced in the oxidation of MnC12 is used to eliminate HC1
remaining in H2SO4 after its separation from MnC12. This gas
is cooled in an indirect heat exchanger by transferring its heat
to H2SO4, yet to undergo the HC1 elimination treatment. Air
is brought into contact with the HCl-bearing H2O condensate
of that heat exchanger to obtain air containing HC1 and H2O
vapor to be used for MnC12 oxidation.
20670
Furkert, Herbert
METHOD OF RECOVERY OF SULPHURIC ACID.
(Chemiebau Dr. A. Zieren G.m.b.H. and Co. K. G., Cologne-
Braunsfeld (West Germany)) U. S. Pat. 3,490,868. 5p., Jan. 20,
1970. 4 refs. (Appl. March 4, 1968, 6 claims).
Sulfuric acid is produced from sulfur dioxide-containing gases
by a multi-stage catalytic oxidation process and a two-stage
sulfur trioxide absorption. The first absorption stage is ar-
ranged before the last oxidation stage and the second absorp-
tion stage is arranged after the last oxidation stage. Sulfur
trioxide-free exhaust gas leaving the first absorption stage is
reheated to the starting temperature for the last oxidation
stage with superheated steam. The steam is obtained from an
exothermic step of the overall sulfuric acid recovery process
starting with a sulfur containing raw material. (Author ab-
stract)
20777
Tamura, Zensuke and Yukio Hishinuma
A PROCESS AND APPARATUS FOR THE DESULFURIZA-
TION OF INDUSTRIAL WASTE GASES. (Hitachi, Ltd.,
Tokyo (Japan)) U. S. Pat. 3,486,852. 6p., Dec. 30, 1969. 4 refs.
(Appl. Sept. 21, 1967, 20 claims).
A process and apparatus for desulfurizing industrial waste gas
and recovering sulfuric acid as a byproduct are described. A
portion of the waste gases are introduced into an adsorption
tank to remove the sulfur oxides by contacting them with ac-
tive carbon, while the remaining portion is sent to a region for
drying the active carbon which has been wet in a proceeding
rinse-desorption step. From the drying tank the gases are led
to the adsorption tank. Waste gases free of sulfur oxides are
released to the atmosphere from the adsorption stage. Sulfur
oxides are removed from the active carbon by rinsing with
-------
B. CONTROL METHODS
19
water, and the washings are removed and sent to a concentra-
tion tank where they are heated and sulfuric acid is recovered.
The functions of the respective regions is the adsorption-
desorption apparatus are shifted one after another at a certain
time interval, so that a cycle of operation consisting of adsorp-
tion, rinsing-desportion and drying, is carried out concurrently
repeatedly.
21309
Argenbright, L. P. and Bennett Preble
SO2 FROM SMELTERS: THREE PROCESSES FORM AN
OVERVIEW OF RECOVERY COSTS. Environ. Sci. Technol.,
4(7):554-561, July 1970.
About 2.2 million long tons per year of sulfur is contained in
the sulfur oxide gases generated in the operation of copper,
zinc, and lead smelters in the western United States. Nearly
23% of this is recovered, mostly as sulfuric acid. A study was
made to identify and evaluate the technological and economic
problems associated with controlling the sulfur oxide emis-
sions of these smelting operations. Three processes for control
and by-product recovery were considered: the contact sulfuric
acid process, the Cominco absorption process, and the ASAR-
CO reduction process. All three are adversely affected by the
low percentage of sulfur in the exhaust gases. Similarly, all are
limited in optimum size, since the capital investment for larger
operations off-sets the reduction in operating cost. Of the
three processes considered, the contact sulfuric acid process is
the least costly, both in terms of initial cost and operating
cost.
21203
Romovacek, Jiri and Jaroslav Fohl
APPARATUS FOR THE PREPARATION OF GASEOUS MIX-
TURES WITH LOW SO2 CONCENTRATION. (Apparatur zur
Herstellung von Gasgemischen mil kleiner SO2-Konzentra-
tion). Text in German. Erdoel Kohle (Hamburg), 23(5):294-296,
May 1970. 13 refs.
A gaseous mixture with sulfur dioxide concentrations of 0 to 1
mg/cu m is obtained by continuously adding dichlorsulfitomer-
curate-(II) to sulfuric acid and by diluting the liberated SO2
with a regulated flow of carrier gas. The solution of dichlorsul-
fitomercurate-(II) is pumped peristaltically into a spiral-shaped
glass column simultaneously with the H2SO4. The spiral
column has an inner diameter of 8 mm and a length of 800
mm. The carrier gas nitrogen is taken from a pressurized gas
bomb, and is cleaned with solid NaOH. The speed of the carri-
er gas is controlled by a manometer. A constant SO2 concen-
tration was produced in long-term experiments.
21824
Chemical Construction Corp., New York, N. Y., Consulting
Div.
ENGINEERING ANALYSIS OF EMISSIONS CONTROL
TECHNOLOGY FOR SULFURIC ACID MANUFACTURING
PROCESSES. Contract CPA 22-69-81, 276p., March 1970. CF-
STI: PB 19093
The capabilities and state of development of the available
processes and devices to effect control for both existing and
new plants were evaluated to determine the cost of control by
various methods, and to outline programs for further develop-
ment of systems which appear to have the greatest overall
potential for reducing undesirable emissions from sulfuric acid
plants in the United States at the lowest cost. Existing plants
can reduce their emissions somewhat by modifying their
operating conditions with little capital expenditure, but this
control is limited to about 2000 ppm of sulfur dioxide. Present
technology can achieve a control effectiveness of 500 ppm of
SO2 via the dual absorption route, and excellent acid mist con-
trol in the order of 0.1 mg/SCF. No fully developed acid plant
control systems are commercially operated in the U. S. which
achieve an effectiveness of 100 ppm of S02, but there are
promising ones in various stages of development. It is doubtful
that there is any contact plant in the U. S. to which some type
of control system could not be applied to reduce emissions to
less than 500 ppm SO2, but to do so economically may be a
different story. Cost of emission control varies widely with
plant capacity, type of control system and other factors. Cost
of less than 500 ppm SO2 control for a 250 T/D contact plant
varies from about $.75 to over $3 per ton of acid. Mist control
costs vary from $.02 to $.35/tons of acid. These costs are
predicated on an asssumption that promising processes will
work as expected. Control cost is lower for large plants.
Recommended areas for study include development of resin
and molecular sieve adsorbents, oxidation inhibitor develop-
ment for tail gas recovery processes, study of stack dispersion
and factors affecting it, plus development work on several
processes, both for treatment of tail gas and improved in-plant
conversion.
22055
Snowball, A. F.
A CYCLIC PROCESS OF SULPHURIC ACID MANUFAC-
TURE AT TRAIL, B. C. Can. Chem. Process, vol. 31:1110-
1114, Dec. 1947. 2 refs. (Presented at the C.I.C. Meeting,
Banff, Ontario, June 8-11, 1947.)
In a cyclic process of sulfuric acid production, pure sulfur
dioxide and oxygen are fed to a circulating gas stream that is
moved by centrifugal blowers through heat exchangers to
cylindrical steel converters packed with vanadium catalyst.
The converted gas containing sulfur trioxide at high tempera-
ture is first cooled in the heat exchangers, then in air-cooled
pipes before entering absorber towers where the sulfur triox-
ide is removed in contact with 98.4% sulfuric acid. The cycle
is complete when the gas passes through spray catchers and
coke filters back to the blowers. Measured quantities of ox-
ygen and 100% sulfur dioxide gas are added during and after
absorption, replacing sulfur trioxide and bringing the gas con-
centration back to the ideal operating percentages of 25% sul-
fur dioxide, 30% oxygen, and 54% nitrogen. Control of
catalyst temperature in the converter is reviewed, as are the
steps taken to prevent metal corrosion. Efficiency of the plant,
which is operated by one attendant through centralized con-
trol, is 99.5%.
22182
(Inventor Not Given.)
METHOD OF REGENERATING ADSORBING COKES
CHARGED WITH SULFURIC ACID. (Precede de regeneration
de cokes adsorbants charges d'acide sulfurique). Text in
French. (Bergwerksverband G.m.b.H., Essen, W. Germany)
Belg. Pat. 707,739. 9p., June 10, 1968. (Appl. Dec. 8, 1967. 4
claims).
A method is described for the regeneration of adsorbing cokes
charged with sulfuric acid after having served to fix sulfur
dioxide obtained from gas containing SO2 in the presence of
oxygen and water vapor. The adsorbing coke charged with
H2SO4 is first washed in the known manner by means of hot
water or of aqueous solutions. Between 1 and 5% (by weight)
sodium or potassium hydroxide is added to the wet coke and
the coke is heated in an inert atmosphere at a nominal 600-
1000 C (400 C minimum) for 1/2 4 hours. The thermal treat-
ment includes simultaneous rinsing by means of an inert gas.
-------
20
SULFURIC ACID MANUFACTURING
22943
Hammond, Roll
ELIMINATING DUST IN CHEMICAL PLANT. Chem. Age,
(New York), vol. 77:431-433, March 9, 1957.
Among new equipment for eliminating dust from chemical
plant flue gases is a multi-wash collector that removes sub-
micron particles with maximum efficiency. The collector com-
prises a cylindrical stainless steel tower with six and one-half
vaned impingement stages. An entrainment separator placed
above the units forms a seventh tier. Air enters the tower just
below its conical base, which acts as a wet cyclone to collect
the heavier particles upon entry. A water curtain descending
from the top of the tower combines with spray and impinge-
ment to envelop the particles rising with the air, carrying them
down into the cone and out of the collector. When most of the
dust is above the submicron range, collectors with fewer
stages are employed. These collectors are equally effective on
both soluble and insoluble dusts and on soluble gases. For the
removal of gaseous contaminants such as hydrogen sulfide,
sulfur dioxide, hydrochloric or hydrofluoric acid vapors, al-
kaline solutions are added to the recirculated liquid. For the 0.1
to 5 micron particles found in pharmaceutical and bacteriologi-
cal work, an esparto grass-based paper filter with asbestos
fibers has an efficiency of 99.95%. This filter can be accom-
modated in a very small place. A reverse-jet type filter has
proved very efficient for vaporized silica of 0.6 micron and
less. Electrostatic precipitators are used to remove dust and
fumes from pyrite roasters, sulfuric acid mist from wet
catalyst sulfuric acid plants, and sulfuric acid mist from coal
roaster gases. Static rectifiers for the precipitators are availa-
ble that dispense with the high-tension connections formerly
required. Alternating current is rectified and used without
high-frequency effect on the wave-form, as in the case of
mechanical rectifiers.
23048
TIME TO RETHINK SULFURIC SOURCES. Chem. Week,
102(19):55-56, May 11, 1968.
Slightly more than a year ago, engineers agreed that while
chemical process technology is readily available to make sul-
furic acid from pyrite concentrate or gypsum, the methods
could not compete economically with sulfuric from elemental
sulfur. However, the handicaps associated with pyrites and
gypsum are beginning to disappear, now that the price of sul-
fur is $42 per long ton. Total plant investment costs are com-
pared on the basis of 400,000 short tons of acid per year
produced from brimstone, pyrite, and gypsum. For each
method, the total plant investment is equal to 125% of the bat-
tery-limit costs. Total indirect costs are 16.6% of the entire
plant investment. The economics of the gypsum process are
expected to become more attractive with the development of a
fluid-bed process for recovering sulfur from calcium sulfate in
the form of waste gypsum. There are two steps to the process:
first, dry gypsum is preheated in a fluid bed and the two mols
of combined water are driven off at a temperature high enough
to support combustion of residual hydrocarbons; secondly, the
calcium sulfate is reduced in a second chamber to calcium sul-
fide at approximately 1560 F. The latter is recovered as a
suspension in water, where it is carbonated with carbon diox-
ide gas to yield calcium carbonate and also sulfur in the form
of hydrogen sulfide gas. The gas is burned with air to form the
sulfur dioxide gas feeding the sulfuric acid plant.
23070
Averbukh, T. D., I. A. Apakhov, O. V. Maydurova, N. P.
Bakina, N. P. Blinova, A. A. Burba, and I. V. Avdeyeva
REMOVAL OF SULFUR FROM COPPER-SULFUR PLANT
WASTE GASES BY THE AFTERBURNING METHOD.
(Ochistka otkhodyashchykh gazov mednosernyk zavodov ot
sery metodom dozhiganiya). Text in Russian. Khim. Prom.
(Moscow), no. 4:51-58, 1962. 7 refs.
Catalytic afterburning of waste gases containing about 3 vol.
% carbon disulfide, carbon sulfide, hydrogen sulfide, and sul-
fur dioxide (50 g/cu m of sulfur) to produce sulfuric acid was
studied experimentally at temperatures of 200-600 C using 16
different catalysts. Data are given for the following catalysts:
various types of bauxite, barium-aluminum-vanadium (BAV),
and chamotte treated with nickel and aluminum nitrates. Pilot
studies made at flow rates of 800-1200 cu m/h using bauxite
and BAV catalysts are reported, and a proposed production in-
stallation is described.
23264
Adachi, Noriyoshi, Makoto Kimura, and Seiko Hashimoto
ELECTRIC FILTRATION OF SO2. Taiki Osen Kenkyu (J.
Japan Soc. Air Pollution), 2(1):98-100, 1967. Translated from
Japanese. 8p.
To develop equipment for the removal of sulfur dioxide in flue
gas, a wet-type electric precipitator was constructed and a
basic study of electric filtration of SO2 was performed. Liquid
was dropped along the inside wall of a glass cylinder of 35 mm
inner diameter. The corona electrode was placed at the center
of the cylinder and voltage was applied between the corona
electrode and the liquid surface. A known concentration of
SO2 gas was introduced from the bottom of the cylinder,
passed through the corona discharge, and was taken out from
the top of the cylinder. Sampling of SO2 was in accordance
with Japan Industrial Standard JIS-KO103-1963; titration was
employed for the analysis of SO2. As SO2 is an electronega-
tive gas on which electrons are easily attached, its collection
efficiency was increased at a corona starting voltage of 5 kV
and the efficiency was constant with voltages larger than a
certain value. The collection efficiency was always higher with
a negative corona electrode voltage than with a positive one.
With positive voltage above a certain level, collection was not
achieved steadily. A flow rate of about 100 ml/min. was most
adequate. Gas collection efficiency was greater than 95% with
an applied voltage of 9 kV and SO2 concentration below
0.45%. In the preceding results, water was employed as the
collection medium. Further experiments were conducted using
a 5% aqueous solution of Na2CO3 and a 10% aqueous solution
of sulfuric acid. The collection efficiency was reduced with
the increase of SO2 concentration; this tendency was more
pronounced with the sulfuric acid solution. With a voltage of 7
kV, the efficiency with the Na2CO3 solution was almost
100%, whereas with the sulfuric acid solution it was only 35%.
23556
Clauss, N. W.
THE REDUCTION OF ATMOSPHERIC POLLUTION FROM
SULFURIC ACID RECOVERY PROCESSES. Manufacturing
Chemists Association, Washington, D. C. Air Pollution Abate-
ment Committee and Manufacturing Chemists Association,
Washington, D. C., Water Pollution Abatement Committee
Proc. Mfg. Chem. Ass. 1952-53 Pollution Abatement Conf., 9p.
Effluent gases from air-blown sulfuric acid concentrators con-
tain sulfuric acid mist and sulfur dioxide resulting from the
decomposition of sulfuric acid by carbonaceous materials
-------
B. CONTROL METHODS
21
present in the spent acid. A pflot plant was designed to study
the removal of the mist by low-pressure water sprays, high-
pressure water sprays, bag filters, and decomposition by heat
When the data obtained suggested that the high-pressure water
spray system was most effective, a plant-scale acid mist
removal unit was put into service. The sulfuric acid mist
removal of the plant-scale unit appears to be higher than the
efficiency obtained in the pilot spray unit, probably due to the
elimination of wall effects. It is concluded that when the full
capacity of the system is made available, the system can be
operated, at a net operating cost (1953) of $5000 year, at max-
imum production rates with no pollution of the atmosphere by
sulfuric acid mist.
23939
Nagibin, V. D.
SMELTING CONCENTRATES IN CONVERTERS AND
PRODUCTION OF SULFUR DIOXIDE FOR SULFURIC ACID
MANUFACTURE. Soviet J. Non-Ferrous Metals (English
translation from Russian of: Tsvetn. Metal.), vol. 9(10):39-42,
Oct. 1968.
Industrial tests were performed on the converter smelting of
copper matte in an air blast enriched with up to 24-27% ox-
ygen. The output capacity of converters increased propor-
tionally to the percentage of oxygen in a blast. The tempera-
ture of the molten charge in converters increased sharply as a
result of the heat of exothermic reactions; this permitted the
processing of cold additions in the form of ore, concentrate,
and other copper containing materials. Concentrations of sul-
fur dioxide in the waste gases of the converter increased by
1.5-2.5% (in absolute value), varying during the second blow-
ing period by 5-10%. The operating regime of the converters
decreased markedly when enriched blasts were used during the
first and second blowing stages. On the basis of these findings,
programs were developed for the smelting of pelletized copper
concentrates and for the production of sulfuric acid from con-
verter waste gases alone. The latter process is based on a
starting concentration of about 4% SO2 in converter waste
gases fed to a contact-reaction vessel and on special condi-
tions for matte blowing. At least two converters are con-
tinually on blast, the blast consumption of each varying
between 30,000 to 45,000 cu m/hr. Before being passed to the
sulfuric acid production plant, the exhaust gases are pressure
fed by a blower to electrostatic dust separators. An automatic
switching system for changing the direction of the gases from
the sulfuric acid units to stack exhaust makes it possible to
stabilize the content of sulfur dioxide being shipped to the
former.
24103
Browder, Timothy J., Jr.
METHOD OF SULFURIC ACID MANUFACTURE. (Parsons
(Ralph M.) Co., Los Angeles, Calif.) U. S. Pat. 3,525,587. 4p.,
Aug. 25, 1970. 3 refs. (Appl. July 19, 1968, 12 claims).
A process is described for the production of sulfuric acid by
the catalytic oxidation of sulfur dioxide containing gas and the
multiple stage absorption of sulfur trioxide produced by such
catalytic oxidation. Sulfur dioxide containing gas can be
produced by a variety of reactions, such as by the oxidation of
hydrogen sulfide or hydrocarbon mercaptans, or by metallurgi-
cal smelting. Conventional multiple oxidation stage processes
which utilize intermediate absorption between stages are defi-
cient in that they fail to allow the desired flexibility of initia-
tion of optimum inlet or exit temperatures for each of the ox-
idation stages. The present method utilizes a portion of the ex-
othermic reaction heat of gas exiting from the first of at least
three successive oxidation stages, having an intermediate ab-
sorption stage between the second and third stages for pre-
heating gas passing into the third oxidation stage. Exit gas
from the first oxidation stage is preferably split into two
streams; one stream is fed to a heat exchanger for pre-heating
gas to be fed into the first oxidation stage, and the other
stream is utilized to pre-heat gas passing from the intermediate
absorption stage to the third oxidation stage.
24110
Berly, Edward M., Melvin W. First, and Leslie Silverman
RECOVERY OF SOLUBLE GAS AND AEROSOLS FROM
AIR STREAMS. Ind. Eng. Chem., 46(9):1769-1777, Sept. 1954.
18 refs.
High efficiency absorption of soluble or reactive gases was ob-
tained with wetted fiber beds. Wetted fibers were five to 10
times more efficient than Raschig rings or Berl saddles, com-
pared on the basis of equal volumes. When compared on the
basis of weight of packing, 1 pound of 78-micron-diameter
saran fibers was 75 times more effective for the absorption of
hydrogen fluoride gas than 1 pound of 1/2 inch Berl saddles.
In addition to hydrogen fluoride gas, cleaning efficiency for
sulfuric acid and ammonium bifluoride mists, ammonium
bifluoride and aluminum chloride fumes, and silica, tale, and
atmospheric dusts was investigated. High efficiency collection
(greather than 99.9%) generally required the addition of a
droplet eliminator composed of a 1 to 2-inch depth of dry
fibers less than 5 microns in diameter. Although absorption of
the gas was complete, a significant quantity of fluorides
passed the scrubber in the form of fine (less than 10 micron)
mist droplets formed from condensation of hydrogen fluoride
gas in the humid atmosphere of the scrubber or from fine
droplets formed by the sprays. When gas streams containing
inert particles were treated, the absorbing stages were pro-
tected from fouling and plugging by the use of an impingment
device such as a Neva-Clog screen as a prefilter. Over-all re-
sistance of the scrubber was proportional to the flow rate. For
gas flows of 200 cu ft/min, sq ft of scrubber face area, high
efficiency scrubbing of gas and submicron paniculate matter
was obtained with resistances not exceeding 6 inches of water
gauge For atmospheric pollution control of stack gas, emis-
sions resistances less than half this may be adequate. (Author
summary)
24246
Farrar, G. L.
LACQ LEADS IN SULFUR-RECOVERY OPERATIONS. Oil
Gas J., 68(42):72- 75, Oct. 19, 1970. 2 refs.
Already the largest single producer of chemically derived sul-
fur in the world, and with one of the largest gas throughputs
anywhere, the Lacq gas processing plant in southern France is
now the leading pioneer in recovering sulfur from plant ex-
haust gases. The air-pollution-prevention attack is three
pronged. The sulfur plants are automated to insure that sulfur-
content of effluent gases from Claus sulfur units is at an ab-
solute minimum. A sulfuric acid plant, operating on a part of
the sulfur-plant off gas, makes a salable product and reduces
the sulfur content in the effluent gas to the hundreds of ppm
range. A new sulfur recovery process, operating on another
part of Claus off gas, utilizes a special catalyst, which is active
at reactive conditions and low operating temperatures to
drastically cut the concentration of sulfurous gases in the ef-
fluent. In the new (Sulfreen) process, the feed gas is first
cleaned by contacting it with liquid sulfur, then passed to a
battery of six reactors where Claus reactions are carried out at
temperatures lower than those utilized in the sulfur plant.
-------
22
SULFURIC ACID MANUFACTURING
These temperatures insure that product sulfur deposits are
deposited on the catalyst as a liquid. A stream of nitrogen
sweeps the catalyst clean while the liquid sulfur product is
drained off to liquid storage. The feasibility of installing other
Sulfreen units is being studied.
24256
Yashke, Ye. V., A. G. Amelin, V. A. Petrovskiy, and V. A.
Osmul'kevich
GLASS-FIBER FILTERS FOR TRAPPING SULFURIC ACID
MIST. (Steklovoloknistyye fil'ty dlya ulavlivaniya tumana ser-
noy kisloty). Text in Russian. Khim. Prom. (Moscow), no.
3:196-200, March 1965. 16 refs.
The use of alkali glass fibers as filter material for the collec-
tion of sulfuric acid mist was studied experimentally for sul-
furic acid concentrations of 75-98%, with mist droplets 0.2-0.5
micron in diameter. Procedures for estimating degree of
deposition as a function of droplet size, mist density, gas flow
rate, gas viscosity, fiber diameter, and filter packing density
are discussed. Data on the operation of such a filter in an in-
dustrial installation in combination with an electrofilter are
presented. This filter handles 10,000-15,000 cu m of mist per
hour, effecting 99.7% removal.
24451
Petersson, Stig
CONCENTRATING SULFUR-CONTAINING GASES FROM
SMELTING PLANTS. (Koncentrering av svaveldioxidhaltiga
smaeltverksgaser). Text in Swedish. Kem. Tidsskr., 82(1):34-
38, Jan. 1970.
Copper, lead, and zinc are usually present in nature in sulfide
ores. When these ores are processed by industrial operations,
gases containing sulfur dioxide are liberated. The SO2 concen-
tration varies depending upon the process. A primary control
method for S02 involves absorption of the gas by water or an
organic solution, followed by healing and condensing to liquid
SO2 for sulfuric acid manufacturing. A Swedish plant is
described which produces liquid SO2 from smelter plant gases.
The plant capacity is 50,000 cu m/hr at 4.5% SO2. The liquid
SO2 is partly sold and partly used to raise the gaseous SO2
content at a sulfuric acid plant. The absorption tower is
designed for an efficiency of 98% calculated at maximum load
and at a water temperature of 11 C. The plant raises the use of
SO2 in the gases from the smelting plant from 75% to 95%.
The plant was motivated by both production efficiency and en-
vironmental concern.
24594
Rosendahl, Fritz
RECENT PROCESSES FOR THE REMOVAL OF SULFUR
COMPOUNDS FROM GASES, AS SEEN IN GERMAN
PATENTS FOR THE YEAR 1964. (Neuere Verfahren zur Ent-
fernung von Schwefelverbindungen aus Gasen-dargestellt an
Hand deutscher Patent von 1964). Text in German. Gas Was-
serfach (Munich), 106(31):857-859, Aug. 6, 1965. 19 refs.
German patent literature is reviewed, summarizing achieve-
ments in the field of dry gas removal, wet ammonia processes
and other wet processes, reactions between hydrogen sulfide
and sulfur dioxide, and the removal of organic sulfur com-
pounds. An iron oxide is obtained from the roasting of pyrite,
the fine granular form of which can absorb 93.3% S. One am-
monia process, making use of waste water from a coke plant,
gives a 70-80% sulfuric acid yield. Wet processes use not only
water but also various organic solvents such as methanol, pyr-
rolidone, or piperidone. The advantage of the two last-men-
tioned solvents is their relatively high boiling point. Acetone,
methanol, or ethanol can also be added to the water used in
scrubbers (5-20 vol. %), reducing the viscosity and making
possible a lower operating temperature. Hydrogen sulfide and
carbon monoxide can be removed from waste gases under
pressure by using various esters and ester mixtures. The
removal of organic sulfur compounds can be achieved with an
efficiency of at least 90%. The removal of hydrogen sulfide
from gases by the use of activated charcoal requires a pore
diameter of more than 60 A, while the removal of organic sul-
fur compounds requires a diameter on the order of 20-40 A.
24628
Drechsel, Herbert, Karl-Heinz Doerr, and Hugo Grim
PRODUCTION OF SULFUR TRIOXTOE AND SULFURIC
ACID. (Metallgesellschaft A. G., Frankfurt (W. Germany)) U.
S. Pat. 3,525,586. 7p., Aug. 25, 1970. (Appl. Oct. 12, 1966, 4
claims).
A catalytic oxidation process is described which utilizes sulfur
dioxide-containing gases to produce sulfur trioxide and sulfuric
acid. The SO2 content of the gas must be at least 9% in order
for this process to work. The process involves a series of heat
exchange and oxidation steps and a hot single stage inter-
mediate absorption step. It is self-sufficient as to sensible heat
requirements, actually producing recoverable excess heat to be
utilized for other purposes. The advantages of this process
over previous ones are that the initial concentration of S02 in
the starting gas can vary over a specified range, and that this
process produces excess heat while other processes require
heat inputs to function properly. This process results in a high
degree of conversion, making it economically desirable.
24673
Asano, Toyoshi
DISPOSAL OF WASTE GAS CONTAINING DELUTE SUL-
FUR OXIDE. (Kihaku sanka iou ganyu gasu no kaishu). Text
in Japanese. Kogyo Kagaku Zasshi (J. Chem. Soc. Japan),
73(7):1731-1732, July 5, 1970. 3 refs.
Disposal of sulfur dioxide in pyrites roasting, petrochemical
industry, or power plant waste gas is discussed. In a conven-
tional wet disposal method, SO2 is merely neutralized by an
agent like lime or ammonia, but a very large quantity of the
neutralization agent is needed. Another disadvantage of the
conventional method is that its sulfur oxide absorption effi-
ciency drops with substances formed as a result of the
neutralization process. When SO2 gas was made to flow coun-
tercurrent to manganese ore suspension in a tower, SO2 was
reduced to sulfuric acid of a densit about the same as that ob-
tained in a lead chamber method, and practically no SO2 was
contained hi the gas discharged from the tower. A 10% man-
ganese-ore suspension was used in an experimental device in
which the suspension was heated to the desired temperatures
and, when vaporized by the heating, automatically reduced
from gas to liquid. Ore composed of Mn(27.96%),
SiO2(37.32%), Fe(8.16%) and P(0.03%) was pulverized to 80-
mesh grains and mixed with water at a 10:90 ratio to make the
suspension used as the absorbing agent. From the results of
this test, it was determined that the higher temperature of the
suspension, the higher its SO2 absorption efficiency; the
amount of SO2 absorbed decreased with increasing sulfuric
acid density in the suspension; at 50 C, the quantity of sulfuric
acid contained in the suspension reached 74.3 g/100 ml. The
contact time of SO2 gas with the suspension was 5.7 sec and
the gas injection speed 8 cm/min. The device maintained about
100% SO2 absorption efficiency for 20 hrs, indicating that the
manganese oxide suspension can be effectively used as an
SO2 absorbing agent.
-------
B. CONTROL METHODS
23
24695
Fairs, G. Lowrie
HIGH-EFFICIENCY FIBRE FILTERS FOR THE TREAT-
MENT OF FINE MISTS. Trans. Inst. Chem. Engrs. (London),
vol. 36:476-485, 1958. 3 refs.
The treatment of contact process sulfuric acid plant tail gases
to remove completely a sulfuric acid mist with particles of less
than two micron was studied. If a filter of fine glass-wool is
treated with a silicone to provide a water repellent surface, the
acidity of the gases leaving the filter is reduced to 0.2% of the
inlet acidity as compared with 2.5% for untreated wool under
similar operating conditions. This twelve-fold improvement of
scrubbing efficiency is important, since the gases scrubbed
with the silicone-treated fiber were invisible when vented to
the atmosphere, while a visible plume persisted after scrubbing
with the untreated fiber. A scrubbing efficiency of 99.6% was
obtained with a garnetted Terylene polyester fiber, which is in
itself water repellent. Comparative performance data for the
two filters are summarized. (Author abstract modified)
24833
York, Otto H. and E. W. Poppele
TWO-STAGE MIST ELIMINATORS FOR SULFURIC ACID
PLANTS. Chem. Eng. Progr., 66(ll):67-72, Nov. 1970. 5 refs.
Sulfuric acid plants, and plants producing oleum in addition to
sulfuric acid, are a major source of concern to air pollution
authorities because of the dense and highly corrosive acid mist
discharged with the absorption tower tail gas. Modern air pol-
lution codes require that mist emissions from existing plants
be reduced to below 2 mg/std cu ft. Compliance with these
regulations is achieved at minimum cost by means of a two-
stage scrubber, one stage designed for the removal of the
coarse fraction of the mist and the other for removal of very
fine mist particles. Fluorocarbon fibers are used for the con-
tact stages as they combine complete corrosion resistance with
high separation efficiency at moderate pressure drop. Efficien-
cy of the scrubbers, unlike that of two-stage wire mesh mist
eliminators, is essentially 100% for particles down to about
one micron. Reduction of particles down to 0.3 micron is also
substantial.
25133
Donovan, J. R. and P. J. Stuber
AIR POLLUTION SLASHED AT SULFURIC-ACID PLANT.
Chem. Eng., 77(25): 47-49, Nov. 30, 1970.
Among processss for controlling emissions from sulfuric acid
production, attention is now being given to interabsorption, or
double-catalysis. This system markedly lowers sulfur dioxide
emissions and gives higher conversion to acid at generally
modest cost penalties. While in a conventional contact-acid
plant, SO2 is converted into sulfur trioxide in one operation,
interabsorption instead interrupts the reaction to remove some
of the SO2 product. This has a favorable effect on both the
kinetics and the equilibriu of further conversion. Equipment
required for an interabsorption plant is similar to that of con-
ventional facilities with the addition of heat exchangers and an
interpass absorption tower. Conversion of 99.5% can be
guaranteed by the process as compared to 98% for a conven-
tional plant. Capital and operating costs, together with indirect
charges, are itemized for the first facility in the Western
Hemisphere to use this German-based process
25275
Nilsson, Folke and Bengt Rudling
AIR POLLUTION CONTROL AT THE BOLIDEN COPPER
AND LEAD SMELTING PLANT, ROENNSKAERSVERKEN,
SWEDEN. Preprint, International Union of Air Pollution
Prevention Associations, 36p., 1970. (Presented at the Interna-
tional Clean Air Congress, 2nd, Washington, D. C., Dec. 6-11,
1970, Paper SU-24D.)
Factors considered when the Boliden Company's copper and
lead smelter was erected in Sweden in 1928-1930 are reviewed.
Built for smelting copper-arsenopyrite ore from the Boliden
mine, the smelter was placed on a peninsula at the Bothnian
Gulf. To utilize excess sulfur in the ore as pyrite and thereby
reduce the sulfur dioxide emission by about 50%, the ore was
concentrated. After World War n a sulfuric acid plant took
care of the roaster gases and ten years later the production
was increased three-fold by further SO2-utilization. Hereafter
no effect can be seen on forest, crop, or garden. The concen-
tration of SO2 in ambient air around the the smelter is far
beneath the official limit. The production of liquid SO2 for the
paper and pulp industry will now make it possible to utilize
over 90% of the SO2. The SO2-recovery is made by absorp-
tion in water. This process is economical when a good supply
of cold water for cooling and inexpensive surplus steam is
available. Along with diversified and increased production,
dust cleaning has been extended and modernized. The results
of these activities have been followed up by medical studies of
the population. (Author abstract modified)
25370
Quitter, Volker
ELECTROSTATIC SEPARATION OF SO3 MISTS. Staub (En-
glish translation from German of: Staub, Reinhaltung Luft),
30(4):8-10, April 1970. 2 refs.
Electrostatic precipitators with special electrodes have been
used successfully for precipitating sulfur trioxide mists.
Production of sulfuric acid and oleum on an anhydrite base en-
tails the generation of waste gases with high sulfur dioxide and
SO3 contents which cause heavy damage to agriculture and
forestry. Tail gas precipitators were manufactured and in-
vestigated under a variety of operational conditions. Lead and
'korobon' plates were used as collecting electrodes, while the
discharge electrodes consisted of barbed lead wire. SO2 and
S03 contents, temperature, and gas humidity were measured
upstream and downstream of the precipitator. While rising
SO3 content causes the current consumption to fall, collection
efficiency on the other hand will rise. The flashover limit is as-
sociated with the gas velocity and with the composition of the
tail gas.
25468
Glowiak, Bohdan and Adam Gostomczyk
SULFUR DIOXIDE SORPTION ON ANION EXCHANGERS.
Preprint, International Union of Air Pollution Prevention As-
sociations, 19p., 1970. 10 refs. (Presented at the International
Clean Air Congress, 2nd, Washington, D. C., Dec. 6-11, 1970,
Paper EN-23E.)
The experiment of using anion-renewable exchangers in sulfur
dioxid sorption from gases was conducted in three stages. An
artificially created mixture of sulfur dioxide and air was
passed through a column 50 mm in diameter in the first stage.
The column was filled with an anion layer 300 mm high. Next,
a laboratory device was use for obtaining SO2 from the ex-
haust gases which were emitted by a boiler-house. The gases
had to be dedusted and cooled before passing through the
-------
24
SULFURIC ACID MANUFACTURING
column with anion. At the third stage, a pilot apparatus was
installed in a sulfuric acid works, and the characteristic fea-
tures of an installation working at this stage are described. The
method which was utilized consisted of forcing gases with
countercurrents through a layer of anion exchanger resin
which was sprayed with hydroxide solution. This method can
be used for purification of gases which have a temperature
lower than 60 C and which do not contain dust. Efficiency in-
creases slightly, simultaneous with the increasing concentra-
tion of spraying solution and with that of SO2 in the purified
gas. (Author abstract modified)
25491
Franz, Milan and Rostislav Klimecek
PROCESSING OF SULFUR DIOXIDE FROM COMBUSTION
GASES. (Zpusob zpracovani kyslicniku siriciteho ze spalin).
Text in Czech. (Czechoslovak Republic) Czech. Pat. 110,995.
3p., Dec. 15, 1963. (Appl. July 22, 1961, 1 claim).
Sulfur dioxide from combustion gases (from the manufacture
of contact gas in the production of sulfuric acid) is absorbed
by a solution of sodium hydroxide with the formation of sodi-
um hydrogen sulfite. A surplus of sulfuric acid is then added
to the absorption solution to obtain a pH of approximately 1,
yielding concentrated SO2 which escapes and sodium sulfate
which remains in solution. The sodium hydroxide needed for
the absorption and the sulfuric acid needed for the decomposi-
tion are recovered from the sodium sulfate solution electrolyti-
cally. Electrolysis generates oxygen in a quantity equivalent to
the quantity of the sodium hydroxide recovered and thus also
equal to the quantity of absorbed SO2; the oxygen oxidizes
SO2 to SO3. Sulfur trioxide from the combustion gases causes
a disequilibrium between sodium and sulfate ions in the solu-
tion with a resulting accumulation of free sulfuric acid. This
excess must be neutralized before electrolysis and part of the
solution of sodium sulfate equivalent to the SO3 content hi the
combustion gas is removed and the sulfate is recovered by
crystallization. The method works at normal temperatures.
25643
Sykes, W. and F. Broomhead
PROBLEMS OF ELECTRICAL PRECIPITATION
REVIEWED. Gas World, 134(3494):98-104, Aug. 4, 1951. 5
refs.
Aspects of the design, construction, and operation of the elec-
trical precipitator are discussed. The great advantage of this
device is its ability to remove with high efficiency dust of par-
ticle size much smaller than that removable by mechanical or
cyclone separators. Back pressure, and power needs to
produce the corona discharge, a very small; however initial
costs are much higher. Problems considered at length include
removal efficiency and its relation to time contact of the gases
in the field, design of the precipitation chamber, insulator
breakdown, gas distribution across the precipitator, removal of
deposits from electrodes, and electrical equipment require-
ments. Five essential design factors are given: correct time
contact, good gas distribution throughout the fields, design and
arrangement of the electrodes, maintenance of clean elec-
trodes, and maintenance of correct voltage. Examples of the
following typical application are described and the principal
design features are indicated in each case to point up the great
variety of constructions required by specific and differing
operating conditions: detailing of producer gas from coal and
coke, chamber and contact process sulfuric acid manufacture,
aluminum and cement production, boiler flyash precipitation,
gypsum dust removal, sodium sulfate recovery in the Kraft
pulp industry, cleaning of blast furnace gas, air conditioning,
and spray painting.
25717
Brink, Joseph A., Jr.
LIQUID MIST COLLECTION. (Monsanto Enviro-Chem
Systems, Inc., Chicago, LI.) U. S. Pat. 3,540,190. 7p., Nov. 17,
1970. 5 refs. (Appl. May 16, 1963, 5 claims).
A finely divided mist is separated and collected from a gas in
which the mist is disposed by passing the gas through a bed of
inorganic fibers (preferably glass fibers), composed almost en-
tirely from fibers having diameters within the range of about 5
to 30 micron and compressed to a density of about 5-20
pounds per cubic foot. The mist is collected upon the surfaces
of the fibers, then drained from the fiber bed by gravity flow
in a continuous liquid phase. The apparatus is particularly use-
ful with respect to the removal and recovery of acid mists,
such as sulfuric or phosphoric acids.
25742
Nakazono, T.
REMOVAL OF SO2 GAS. (Aryusan gasu kaishu hoho). Text in
Japanese. (Koga Mine Industrial Co. (Japan)) Japan. Pat.
172,814. 6p., May 31, 1946. (Appl. Oct. 28, 1940, claims not
given).
Sodium formate and/or calcium formate were used as the ab-
sorbents for the removal of sulfur dioxide gas of low concen-
tration under low temperature. The amount of SO2 gas ab-
sorbed was remarkably increased with an increase in the
amount of absorbents. With an increased amount of SO2 gas,
using the same concentration of formate, the amount of S02
absorbed increased until SO2 concentration reached 4%; it in-
creased the least amount thereafter. The SO2 gas obtained by
heating (55 to 100 degree) the formate solution which had ab-
sorbed SO2 gas was utilized for producing sulfuric acid in in-
dustry. The formic acid, produced by the sulfuric acid which
was an intermediate product during this procedure was
neutralized with alkaline salt(s) to regenerate the sodium or
calcium formate. This method is economical and can be util-
ized for the long-term removal of SO2 gas.
25768
Skrivanek, Jaroslav and Vladimir Cada
ABSORPTION OF SULFUR DIOXIDE IN A VENTURI TUBE.
(Absorpce kyslicniku siriciteho ve Venturiho trubici). Text in
Czech. Chem. Prumysl (Prague), 7(32):340-343, 1957. 6 refs.
Gas containing 0.2% SO2 emanating from the manufacture of
H2SO4 was absorbed in a venturi tube by a soda ash solution
dispersed by the gas stream in the constricted neck of the
tube. The degree of absorption and loss of pressure were stu-
died with the view of testing the industrial feasibility of this
method of recovery of sulfur. The venturi tube can be used
only where the pipeline gas pressure exceeds 50 cm H2O and
for comparatively low concentrations of gas to be absorbed.
The theoretical relationship between gas absorption, gas flow
volume and velocity was analyzed, an equation for the depen-
dence of the absorption constant on gas flow volume, on
liquid flow volume and on the intitial soda ash concentration
derived. The experimental arrangement and the method of
determining the residual concentration of S02 in the gas fol-
lowing absorption is described. The absorption constant in-
creases with increasing gas flow velocity and decreases with
increasing absorption liquid volume. The absorption constant
rise with rising gas flow velocity is greater than linear. The ef-
fectiveness of the venturi tube increases with increasing gas
flow velocity, even though the contact between the phases is
shortened, because of the positive effect of flow velocity on
the absorption constant.
-------
B. CONTROL METHODS
25
26095
Brink, J. A., Jr., W. F. Burggrabe, and J. A. Rauscher
FIBER MIST ELIMINATORS FOR HIGHER VELOCITIES.
Chem. Eng, Progr., 60(ll):68-73, Nov. 1964. 8 refs.
Fiber mist eliminators are now installed in various chemical
processes for air pollution control and gas purification. The
design superficial velocity of the gas through the fibers in
most of the eliminators has been 5 to 30 ft/min. Now, as a
result of extensive testing, eliminators are available with su-
perficial velocities of 30 to 90 ft/min, or even higher. These
new units are smaller and less expensive than previous
designs. Performance data is presented for high-velocity units
on sulfuric acid and phosphoric acid mist. At a large-scale sul-
furic acid plant, collection efficiencies as high as 96% are ob-
tained for particles three microns and smaller, and pressure
drop is constant at 7.5 to 8.0 in. of water. The efficiency of the
unit does decrease on smal submicron particles when oleum is
produced.
26254
Perrine, Richard L. and Limin Hsueh
MISCELLANEOUS INDUSTRIAL EMISSIONS. In: Project
Clean Air. California, Univ., Berkeley, Task Force 5, Vol. 1,
Section 14, 5p., Sept. 1, 1970. 3 refs.
Five broad categories of industrial polluters are briefly con-
sidered, as weU as their kinds of emissions and control
problems. The inorganic chemical industry has problems with
hydrochloric acid, hydrofluoric acid, nitric acid, sulfuric acid,
calcium oxide, chlorine, soaps and detergents. Steel produc-
tion is a major industry, but the open hearth furnaces are
gradually being replaced by the basic oxygen furnace.
Although this also produces fumes, the new plants can be con-
structed with proper control equipment. Foundries may change
the work they do from day to day so that control problems are
at their worst, but methods to trap particles and fumes are
available. The handling of large volumes of minerals normally
involves problems with dust, while the special biological ef-
fects of asbestos must be noted. Glass fibers can also be a
problem, as well as fluoride-containing ores. Copper lead, and
zinc mining and milling operations involve dust problems,
while sulfur oxides may be released during smelting. Hydrogen
sulfide, mercaptans, sulfide and polysulfides which have very
bad odors, and other noxious gases are emitted during wood
pulp processing. Typical gaseous emissions from Kraft pulping
are presented tabularly. Coffee roasting plants, slaughter-
houses, and pickel plants emit strong odors. An areas of con-
cern is new processes to break down waste and return it to a
state useful in natural processes without problems of storage.
A particularly important point which needs to be considered is
site location.
-------
26
C. MEASUREMENT METHODS
00040
ATMOSPHERIC EMISSIONS FROM SULFURIC ACID
MANUFACTURING PROCESSES. Public Health Service, Cin-
cinnati, Ohio, Division of Air pollution and Manufacturing
Chemists' Association, Washington, D.C. (999-AP-13.) 1965.
127 pp.
Emissions to the atmosphere from the manufacture of sulfuric
acid were investigated jointly by the Manufacturing Chemists'
Association, Inc. and the U. S. Public Health Service; the
study was the first in a cooperative program for evaluation of
emissions from selected chemical manufacturing processes.
The report describes the growth and potential of the sulfuric
acid industry, types of raw materials used, design of plants,
process variables, emissions from plants under normal operat-
ing conditions, and the methods and devices used to limit and
control emissions. The sampling and analytical techniques by
which emissions were assessed are presented in detail.
(Authors' abstract)
00381
W. L. Crider
HYDROGEN FLAME EMISSION SPECTROPHOTOMETRY
IN MONITORING AD* FOR SO2 AND SULFURIC ACID
AEROSOL. Anal. Chem. 37, 1770-3, Dec. 1965.
The principle of hydrogen flame emission spectrophotometry
is demonstrated to be of practical use in monitoring the at-
mosphere of animal exposure chambers for SO2 in concentra-
tions from 0.1 ppm (v./v.) to 100 ppm and for airborne droplets
of H2SO4 in the concentration range from 0.17 to 5.2 mg per
cu meter. Some parameters influencing emission intensity are
explored. (Author)
00482
F. P. Scaringelli, R. E. Boone, and G. A. Jutze
DYNAMIC CALIBRATION OF AN ACID AEROSOL
ANALYZER. J. Air Pollution Control Assoc. 16(6):310-313,
June 1966.
A method is described for dynamic calibration of an acid
aerosol analyzer based on a commercial modification of the
Thomas Autometer. This automated instrument removes acid
aerosol from an air stream by sonic impaction, and the sulfuric
acid collected is determined conductometrically. An all-glass
aerosol generator based on the reaction of water vapor with
sulfur trioxide vapor released from fuming sulfuric acid was
built for the calibration. Air samples were withdrawn for in-
strument calibration before and after the concentration of the
acid aerosol was determined by titration. The apparent particle
size as determined by an Andersen sampler ranged from 2.0
microns to less than 0.68 micron and exhibited a sharp peak
with mass median diameter at 1.3 microns in the distribution
curve. The size of the aerosol, within certain limits, could be
controlled by humidity. Data indicated a linear response with
an aerosol collection efficiency of 80% in the important
respirable size range. (Author abstract)
01387
J.V. Kerrigan K. Snajberk
STUDIES ON SULFURIC ACID MIST DOWNWIND FROM A
SULFURIC ACID MANUFACTURING PLANT. J. Air Pollu-
tion Control Assoc., 15(7):316-39, July 1965.
Air pollution downstream from a sulfuric acid manufacturing
plant is comprised of two aspects, the amount of acid mist fal-
lout and the concentratuon in the atmosphere. This investiga-
tion shows that it is desirable to determine each of these by an
independent method of collection. Pans of distilled water were
used to collect and determine the sulfuric acid mist concentra-
tion in the atmosphere. The use of Stokes' Law to convert the
results obtained by one method to those obtained by the other
requires a knowledge of the particle size of the sulfuric acid
mist droplets. Data presented show that the use of an average
particle size can yield a picture of pollution which is in error
by many orders of magnitude. The study shows that areas ad-
jacent to a plant may be subjected to fallout of rather large
particle size when there are not adequate methods for removal
from the emission or byproduct gases. (Author abstract)
01819
R.E. Boone R.M. Brice
CONTINUOUS MEASUREMENT OF ACID AEROSOL IN
THE ATMOSPHERE. Preprint. (Presented at the 58th Annual
Meeting, Air Pollution Control Association, Toronto, Canada,
June 20-24, 19659)
Experience in operating a combination acid aerosol and sulfur
dioxide automatic analyzer in ambient air at an urban site is
reported. Data for a 1-month period showed an average con-
centration of 9.2 micrograms/cu m of acid aerosol as sulfuric
acid and 550 micrograms/cu m of sulfur dioxide. Limitations
of the instrumentation have been determined and indicate ap-
preciable variation in acid aerosol due to losses from in-
complete impaction and from measurement of nonacid elec-
trolytes as acid aerosol in the conductivity cell. The overall
factors for converting instrument reading to actual acid aerosol
concentration averaged from 0.52 to 0.70 when determined by
3 methods. The appreciable variations in instrument response
to total acid aerosol in the air sampled, the range of variations
in impaction efficiencies for acid aerosol, and significant varia-
tions in instrument response to nonacid electrolytes suggest
that much more study is necessary before the practicability of
the present instrumentation for monitoring acid aerosol can be
determined. (Author abstract)
03035
M. Hayashi, S. Koshi, and H. Sakabe
DETERMINATION OF MIST SIZE BY METAL COATED
GLASS SLIDE. Bull. Nat. Inst. Indust. Health (Kawasaki
Japan) 6, 35-42, 1961
A new method for the determination of mist size and numbers
of mist particles is described, which is useful in air pollution
research as well as in industrial hygiene. A glass slide was
coated with a very thin layer of metal film; iron was the best
-------
C. MEASUREMENT METHODS
27
of three metals tried. The slides were placed in an Owens type
dust counter or a cascade impactor for the collection of mist
particles. Both acid and alkaline mists were tested. As the cor-
rosive particles hit the slide, metal was dissolved and the
transparent holes which were formed could be detected under
an optical microscope. Methods for calculating true particle
size from the holes in the metal-coated slide are given.
03852
E. S. Kohen
INDICATOR TUBE FOR THE INSTANTANEOUS DETER-
MINATION OF THE SO2 CONTENT OF THE AIR. Indikator-
rohrchen zur Soforthestimmung des So2 - Gehaltes der Luft
Chem. Tech. (Berlin) 18, (11) 688, Nov. 1966. Text in Ger.
The tube was developed to facilitate the rapid determination of
SO2 required for worker protection in the rapidly expanding
sulfuric acid and sulfide ore industry. The operation of the
tube is based on standard reaction tests for S2 and SO32-
using sodium nitroprusside in an alkaline medium. The adsor-
bent is Fajan's powder. The preparation of the adsorbent and
the complete indicator powder is described in detail. A calibra-
tion table (ranging from a length of coloring of 2mm for an
S02 concentration of 0.01 mg per liter to 60 mm for 0.64 mg
per liter) is given. The sensitivity of the tube is about 0.01 mg
per liter. Tubes tested in sulfuric acid plants gave accurately
reproducible results. H2S does not affect the results unless
present in very high concentrations. The tubes are found to be
superior to those of the firm 'drager' (adsorbent, silical gel; re-
agent, potassium iodide and starch) with respect to cost, ease
of manufacture, accuracy, and sensitivity. The tubes last about
10 months.
09033
Scaringelli, F. P. and K. A. Rehme
DETERMINATION OF ATMOSPHERIC CONCENTRATIONS
OF SULFURIC ACID AEROSOL. Preprint, Public Health Ser-
vice, Cincinnati, Ohio, National Center for Air Pollution Con-
trol, ((10))p., 1968. 32 refs. (Presented at the Division of
Water, Air, and Waste Chemistry, American Chemical
Society, San Francisco, Calif., April 3, 1968.)
A new sensitive, relatively specific method has been
developed for sulfuric acid aerosol. It is based on the collec-
tion of the aerosol by sonic impaction on a copper disc, or by
filtration on glass fiber filters. The free sulfuric acid or the
prepared metal salt is thermally decomposed under a stream of
nitrogen to sulfur trioxide. The sulfur trioxide is converted to
sulfur dioxide by a catalytic bed of hot copper. The resulting
sulfur dioxide is determined spectrophotometrically or by titra-
tion in a microcoulometer. Most salts of sulfuric acid do not
interfere. Ammonium sulfate responds quantitatively, but this
fact is not considered objectionable. This salt, in all likelihood,
results from the reaction of sulfuric acid and ammonia in the
atmosphere. The method is reproducible and is suitable for the
determination of sulfuric acid in the parts per billion range.
09295
N. N. Basargin, N. K. Oleinikova
DETERMINATION OF SULFURIC ACID MIST IN THE
GASES FROM SULFURIC ACID CONTACT PLANTS. Ind.
Lab. (USSRXEnglish Transl.), 32(8): 1118-1119, Aug. 1966. 4
refs.
In order to meet the need for a method for the rapid and
precise determination of H2SO4 mist in gases containing acid
components and arsenic, a direct volumetric method was
developed for titrating sulfate ion with a barium salt in the
presence of a new indicator for barium, namely
nitrochromazo. Special features in the structure of
nitrochromazo enable it to react with barium in an acid medi-
um. The titration can be carried out at pH 2.0, which
completely eliminates the effect of arsenates. The basis of the
method was the direct titration of absorbed sulfuric acid, in a
50 percent aqueous acetone or aqueous alcohol medium, with
a solution of barium chloride in the presence of
nitrochromazo. The equivalent point was shown by a sharp
change in the color of the indicator from violet to blue (com-
plex with barium). The gas was drawn through the system by a
vacuum pump. The sampling rate was 1 liter/min. The H2SO4
mist content of the sample should be 20 to 40 mg. The filter
with absorbed sulfuric acid was washed through with distilled
water by means of a water pump. The wash water was col-
lected in a 100 ml graduated flask. The sampling tube was
washed out into the same flask, and the volume was made up
to the mark with water. An aliquot portion (10 to 20 ml) of this
solution was transferred to a 100 ml conical flask, the pH was
adjusted to 2.0 as judged by universal indicator paper, and the
liquid was acidified with a few drops of N HCL. An equal
volume of acetone or alcohol was added, and the solution was
treated with 1 to 2 drops of 0.2 percent nitrochromazo solution
in water and titrated, with shaking, with 0.02 N BaC12 solution
until the color changed. The strength of the BaC12 solution
was determined by titration of 0.02 N H2SO4 solution under
the same conditions, in the presence of nitrochromazo. A
blank titration was carried out to check the purity of the water
and acetone or alcohol. The titration with nitrochromazo as in-
dicator was checked with pure acid solutions. The proposed
method was tested under laboratory conditions and at two sul-
furic acid plants. Results for the determination of H2SO4 mist
in production gases by the alkalimetric and nitrochromazo
titration methods are compared; the former method gave high
results in most cases.
09369
Wilson, H. N. and G. M. Duff
INDUSTRIAL GAS ANALYSIS: A LITERATURE REVIEW.
Analyst, 92(1101):723-758, Dec. 1967. 712 refs.
Analytical methods are reviewed for: permanent and inorganic
gases; analysis of liquefied or pure gases; fuel gases; flue
gases; motor exhaust gases; analysis of micro samples; and at-
mospheric pollutants. The years from 1958 to about mid-1966
were covered. In no branch of analysis is the swing towards
physical methods more marked than in gas analysis. There
have been no important developments of the conventional
methods during the last ten years; the chief advances have
been the application of galvanic methods to 'trace' of certain
gases, and gas chromatography. The rapid spread of the elec-
trogalvanic methods for the 'on-stream' determination of
traces is also most significant. The other most noticeable fea-
ture is the vast and increasing attention being paid to at-
mospheric pollutants of all kinds, particularly sulphur dioxide,
sulphuric acid and hydrocarbons.
09633
Green, W. D.
SENSITIZED FILMS FOR THE DETECTION AND ANALY-
SIS OF CHEMICAL AEROSOLS. Preprint, Meteorology
Research, Inc., Altadena, Calif., 12p., 1968. 4 refs. (Presented
at the 9th Conference on Methods in Air Pollution and Indus-
trial Hygiene Studies, Pasadena, Calif., Feb. 7-9, 1968.)
The chemical species to be detected in the aerosol undergoes a
specific reaction with the indicator in the film following impac-
tin and absorption of the particle. At the present time, films
-------
28
SULFURIC ACID MANUFACTURING
for the detection of sulfate, halide, iodine, iodide, oxidants,
nonspecific acids and bases, and sulfuric acid have been
developed. Semi quantitative analysis of the ion concentration
in single particles particles is possible by precalibration of the
films with droplets aerosolized from solutions of known con-
centration. These films have been used on various air pollution
oriented programs to trace sulfates, halides, and acid aerosols
in the Los Angeles Basin and near San Juan, Puerto Rico, and
to detect halides and acid aerosols in automobile exhaust.
(Author's abstract, modified)
09983
Ubl, Z.
UNIFIED METHODS FOR THE ANALYSIS OF POLLU-
TANTS IN THE FREE ATMOS- PHERE. Acta Hygienica, No.
1, Suppl, 1966. 84p. 24 refs.
Methods for the analysis of pollutants in the air are presented
with precise and complete notes dealing with procedure, ap-
paratus, reagents, and possible problems. Procedures are given
for determining the following compounds in the air: SO2, CO,
NO2, NOx, sulfuric acid aerosols, C12, H2S, Pb compounds,
CS2, phenol, As, F2, NH3, soot, Mn compounds, SiO2, and
formaldehyde. Also discussed are methods of air sampling,
calibration methods, calculations, sensitivity and error in the
determinations interferences from other compounds, and the
principle involved in the method.
11089
Scaringelli, F. P. and K. A. Rehme
DETERMINATION OF ATMOSPHERIC CONCENTRATIONS
OF SULFURIC ACH) AEROSOL BY SPEC-
TROPHOTOMETRY, COULOMETRY, AND FLAME
PHOTOMETRY. Preprint, Public Health Service, Cincinnati,
Ohio, National Air Pollution Control Administrstion, 27p.,
1968. 34 refs. (Presented before the American Chemical
Society, Div. of Water, Air and Waste Chemistry, San Fran-
cisco, Calif., April 3, 1968.)
A sensitive, relatively specific method for sulfuric acid aerosol
has been developed. The method is based on the collection of
the aerosol by sonic impaction on a copper disc, or by filtra-
tion on glass fiber filters. The free sulfuric acid or the
prepared metal salt is thermally decomposed under a stream of
nitrogen to sulfur trioxide. The sulfur trioxide is converted to
sulfur dioxide by a catalytic bed of hot copper. The resulting
sulfur dioxide is determined spectrophotometrically or by titra-
tion in a microcoulometer. Most salts of sulfuric acid do not
interfere. Ammonium sulfate responds quantitatively, but this
fact is not considered objectionable. This salt, in all likelihood,
results from the reaction of sulfuric acid and ammonia in the
atmosphere. The method is reproducible and is suitable for the
determination of sulfuric acid in the parts per billion range.
(Authors' abstract, modified)
11140
Cares, Janet Walkley
THE DETERMINATION OF OXIDES OF SULFUR BY X-RAY
EMISSION SPECTROMETRY. Am. Ind. Hyg. Assoc. J.,
29(4):386-389, July -Aug. 1968.
Determination of sulfur dioxide, sulfur trioxide, or sulfuric
acid mist becomes difficult in the presence of other acid gases
or where collected samples are highly colored or turbid. A
method is described by which all oxides of sulfur are oxidized
arid precipitated as barium sulfate. The barium in the
precipitate is determined by measuring the intensity of the L-
alpha emission produced by x-ray excitation. The method is
useful for about 0.05 to 10 micromoles of oxides of sulfur in
the aliquot analyzed. (Author's abstract)
12596
O'Keeffe, Andrew E.
Affi POLLUTION INSTRUMENTATION. STATE OF THE
ART. Preprint, National Air Pollution Control Administration,
Washington, D. C., Methods Development Section, 23p., 1968
(?). (Presented at the American Council of Independent
Laboratories, Inc., Annual Meeting, Washington, D. C., Oct.
20, 1968.)
Brief descriptions of a number of new air pollution monitoring
instruments being developed are presented. A key feature of
these devices is their ability to sense and measure pollutants
without use of reagents in solution. A flame photometric sulfur
detector is being modified to read sulfur dioxide by gas chro-
matography. Fuel cells can be made for burning carbon
monoxide, methane, SO2, or other compounds of interest.
Semiconductors, such as zinc oxide change resistance when
exposed to certain compounds. Microwave plasma detectors,
in conjunction with spectrophotometers, can analyze certain
gases. A chemiluminescent ozone monitor can measur ozone
due to a release of light energy in direct proportion to the par-
tial pressure of ozone. The permeation tube primary standard
emits a constant supply of a desired gas, a feature which
makes it desirable as a standard. Variations of gas chromatog-
raphy and mass spectrometry are discussed. A system for the
analysis of sulfur trioxide (sulfuric acid mist) is described. Not
all of these methods will necessarily be commercial successes,
but a number of them will certainly prove to be of great value
in the detection of air pollutants.
14486
Uhi, K.
THE DETERMINATION OF ACIDIC GASES IN WORKING
ENVIRONMENTS BY ALKALI FILTER PAPER. (Alkali roshi
ho ni yoru sagyo kankyo chu sansei gas no sokutei). Text in
Japanese. Nippon Eiseigaku Zasshi (Japan J. Hyg.), 24(1):49,
April 1969.
The alkali filter paper method for determining acid gases in
working environments entails soaking filter paper in a 30%
potassium carbonate solution, drying the paper in air, and
putting it in a vinyl holder having an exposure area of 64 sq
cm. Absorbed gases are extracted with distilled water and
determined qualitatively and quantitatively. The required expo-
sure time is determined by the type of acid being measured,
the production process, and the sensitivity of the determina-
tion method. Generally, 1 to 8 hrs are appropriate for acidic
gases like S02, HC1, and NO2, and 8 to 24 hrs for acid mists
of sulfuric, phosphoric, and chromic acids. One hour is usually
required for SO2 measurements by the para-rosaniline for-
maline method; the CL-Ba method requires 8 to 24 hrs. When
the relationship between the amount of SO2 adsorbed on the
filter paper and the average gas concentration in the working
environment is plotted, a curve is obtained. Thus, on a per day
basis, the coefficient of conversion depends on the amount ad-
sorbed. However, the graph for an hour of exposure time is
linear, suggesting that shorter exposure times would be con-
venient for the calculation.
14735
Steinke, Irmhild
CONTRD3UTION TO THE DETERMINATION OF SO2 AND
SOS IN WASTE GASES. (Beitrag zur potentiometrischen
Bestimmung von SO2 und SOS in Abgasen). Text in German
Z. Anal. Chem., 244(4):253-254, 1969. 3 refs.
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C. MEASUREMENT METHODS
29
In the determination of sulfur trioxide and sulfuric acid
aerosols in the presence of sulfur dioxide, the latter substance
is oxidized to SO3 and both oxides are determined jointly.
After additional determination of the S02 content, the SO3
content is obtained from the difference. In experiments to test
this method, both oxides were absorbed in NaOH/H2O2 solu-
tion. Woulf's absorbing flask was used for this purpose. Gas
components which are not immediately absorbed will be ab-
sorbed after shaking. In this alkaline solution, the SOS (com-
posed of SOS and the oxidized SO2) is present in form of
sulfate ions, which are best determined by the method of Bau-
disch, Beilstein, and Neuenhausen to an accuracy of plus or
minus 0.16 mg. The SO2 concentration was separately deter-
mined by absorption in Na2(HgC14) solution (West and Gaeke
method). By this approach, the SO2 and SOS concentrations in
waste gases from sulfuric acid plants can be determined to a
minimum concentration of 1 g/cu m plus or minus 0.07 g/cu m.
15745
Dubois, L., R. S. Thomas, T. Teichman, and J. L. Monkman
A GENERAL METHOD OF ANALYSIS FOR HIGH VOLUME
AIR SAMPLES. I. SULFATE AND SULFURIC ACID.
Microchim. Acta, vol. 6:1268-1275, Nov. 1969. 11 refs.
A method for analyzing high volume samples, particularly with
respect to sulfates and sulfuric acid, was described which
makes use of microdiffusion at 200 C to separate the volatile
sulfate fraction from an aliquot portion of an air sample on a
glass fiber. This separation ensures that only fixed sulfate is
left in the aliquot disc after heating, and that the sulfuric acid,
if originally present, will be removed. At the same time, any
sulfuric acid evolved is trapped in a sodium hydroxide absor-
bent, which can be analyzed for fixed soluble sulfate using a
method specifically for sulfates. The measurement of the
separated volatile sulfate may then be carried out by
microtitration or by square wave polarography. The polaro-
graphic method is more rapid and agrees with values found by
microtitration; it is readily adapted to large scale analyses, and
analytical speed can be improved. The proposed method is
free from inaccuracies and ambiquities associated with
procedures which depend upon pH measurement or non-
specific acid-base titration.
19384
Taylor, H. D.
THE CONDENSATION OF SULPHURIC ACID ON COOLED
SURFACES EXPOSED TO HOT GASES CONTAINING
SULPHUR TRIOXIDE. Trans. Faraday Soc., vol. 47:1114-
1120, 1951. 8 refs.
Laboratory apparatus and techniques are described for sam-
pling and analyzing the sulfuric acid condensing from a hot gas
mixture of known water vapor and sulfur trioxide contents.
The essential feature of the technique is the vaporization of
sulfuric acid into an air stream of known composition and its
condensation upon a surface held at a known temperature in
such a manner that the condensate could be sampled and
analyzed. Over the range of gas composition studied (from 60
to 600 ppm of SO3), the concentration of the condensate is not
affected by the proportion of sulfur trioxide present. It is a
function only of the surface temperature and the water vapor
content of the gases and, independent of the latter, there is a
peak in the rate of condensation at a surface temperature ap-
proximately 45-50 C below the dewpoint. The magnitude of
this peak increases with increasing dewpoint. (Author abstract
modified)
20595
Wyszynska, Halina, Konrad Kosinksi, Stefan Maziarka, Z.
Misiakiewicz, and Artur Strusinsky
METHODS FOR THE SANITARY INVESTIGATION OF AT-
MOSPHERIC AIR DEVELOPED BY THE SECTION OF
SANITATION LABORATORIES FOR THE PROTECTION OF
ATMOSPHERIC Ant. (Metody sam'tarnego badania powietrza
atmosferycznego opracowanie zespolu Pracowni Sanitamej
Ochrony Powietrza Atmosferycznego). Wydawnictwa
Metodyczne Panstwowego Zakladu Higieny (Methodologic
Study Govt. Dept. Hyg.), no. 4(26); issue no. 10, 149p., 1968.
78 refs. Translated from Polish. Franklin Inst. Research Labs.,
Philadelphia, Pa., Science Info. Services, Oct. 14, 1969.
Methods are presented for determing atmospheric pollutants,
with the exception of carbon monoxide and gasoline, the con-
centrations of which are defined by Polish law. In addition,
methods are given for the determination of pollutants present
in the atmosphere in quantities sufficient to create sanitation
problems or to cause plant damage and corrosion to buildings.
Some of the methods have been checked and tested extensive-
ly in the laboratory and in the field. Others have not yet been
widely tested but are included for their potential usefulness in
laboratory studies. The methods include the measurement of
dust collected by the deposition method with respect to tars,
sulfates, free silica, heavy metals, calcium, and fluorine. The
other methods are the aspiration and contact methods for sul-
fur dioxide; the method employing thorium nitrate and
eriochromecyanin R for sulfur trioxide-sulfuric acid; the para-
aminodimethylaniline method for hydrogen sulfide; methylene
blue and diethylamine and copper methods for carbon disul-
fide; the Saltzman method for nitrogen oxides; titration with
thorium nitrate and colorimetric determination with
eriochromecyanin and zirconium oxychloride for fluorine; o-
tolidine for chlorine; titration for hydrogen chloride; buffered
potassium iodide and the Heigal method for ozone; the
Schryver method for formaldehyde; para-aminodimethylaniline
and diazo-p-nitroaniline for phenol; nitration for benzene and
chlorobenzene; and the indophenol method for aniline.
21056
Takahashi, Akira
ELECTROCONDUCTrvTry ANALYZER. (Taikichu no SO2
sokuteiho. 3. Yoeki dodenritsuho). Text in Japanese. Netsu
Kami (Tokyo) (Heat Eng.), 22(2):60-64, Feb. 28, 1970. 1 ref.
An electroconductivity analyzer was adopted to monitor sulfur
oxides in a specified area in conformity with the requirements
of the air pollution prevention law. The conductivity of an ab-
sorbent reaction solution is increased by sulfuric acid, which is
formed by a reaction of hydrogen peroxide with the sample at-
mosphere. The density of the sulfur oxides is measured as an
increase in conductivity. Measurement can be intermittent, au-
tomatic, or continuous. In one procedure the reagent used is a
solution of 0.006% H202 and .00005 N sulfuric acid. The re-
agent will last for 20 days if 20 liters are used. A recorder can
simultaneously measure the oxidized sulfur substance and
floating gas. Sampling should be made to extract a representa-
tive sample of atmosphere at a specified district.
21415
Larrat, P. and J. Louise
CONTINUOUS DETERMINATION OF TRACE AMOUNTS
OF SO2 IN THE ATMOSPHERE AND IN OTHER GAS MIX-
TURES. (Dosage continu de traces de SO2 dans 1'atmosphere
et autres melanges gazeux). Text in French. Chim. Anal.
(Paris), 52(4):397-399, April 1970. 3 refs.
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30
SULFURIC ACID MANUFACTURING
A method is proposed for making a wide range of sulfur diox-
ide content determinations: from concentrations on the order
of 10 to the minus 6th power to those on the order of 10 to the
minus 2 power. It offers the advantage that it does not require
reference gas mixtures but only titred sulfuric acid solutions.
The sulfur dioxide is first oxidized with hydrogen peroxide,
after which the resulting sulfuric acid is determined by the
conductimetric method. The method was tested with a gas rate
of flow of 20 1/hr using 100 cu cm/hr of the liquid reagent. Ab-
sorption of SO2 was complete, and the relative accuracy of
measurement was plus or minus 3 %.
22645
Barton, Sydney C. and Henry G. McAdie
PREPARATION OF GLASS FIBER FILTERS FOR SUL-
FURIC ACID AEROSOL COLLECTION. Environ. Sci.
Technol., 4(9):769-770, Sept. 1970. 5 refs.
When using glass fiber filters for sampling air containing
microgram quantities of sulfuric acid, close attention must be
given to blank effects since the residual alkali content of the
filters can result in H2SO4 losses of 0.4 to 7.8 micrograms per
sq cm of filter. In a new procedure, the sulfur contaminants
responsible for the irreversible absorption of H2SO4 on the
filter are deactivated by soaking the filter in 20% H2SO4 for
two to three days, then rinsing it in distilled water, 80%
isopropanal, and acetone. No H2SO4 losses have been ob-
served in filters treated in this manner.
23771
Patton, W. F. and J. A. Brink, Jr.
NEW EQUIPMENT AND TECHNIQUES FOR SAMPLING
CHEMICAL PROCESS GASES. J. Air Pollution Control As-
soc., 13(4):162-166, April 1963. 7 refs (Presented at the Air
Pollution Control Association, 55th Annual Meeting, Chicago,
May 20-24, 1962.)
When the need for improved sampling equipment and
techniques was recognized at Monsanto a number of years
ago, a cascade impactor suitable for adiabatic measurements
on process gases was developed. Simpler equipment, suitable
for routine control of air pollution, can determine accurately
the weight or chemical composition of the particles in a gas
stream, as well as separately determine the loading of particles
greater than three micron in diameter from particles smaller
than this. The dust or mist sampling device is contained in a
small case with a carrying handle and removable sides similar
to an Orsat analyzer. Gases first enter the cyclone where the
larger particles are collected, while the smaller particles are
carried over and collected by the filter. Sampling preparations
are discussed for large particles, fine particles, and isokinetic
sampling. The procedures for sampling are outlined, as well as
an example for sulfuric acid mist. Calculations of loadings
from sampling data are also indicated. Eight sets of the sam-
pling equipment have been utilized for sulfuric, phosphoric,
and nitric acid mists, mercury mist, various phosphate salt
dust, ammonium chloride fume, ammonium nitrate fume, and
several organic mists.
24970
Heilingoetter, R.
ANALYTICAL METHODS USED TO DETERMINE DAMAGE
BY ACIDS IN THE ATMOSPHERE. (Die chemische Unter-
suchungsmethoden des Luftsaeureschaedenexperten). Text in
German. Chemiker-Zeitung, 51(45):429-433, June 8, 1927.
The three methods available for the assessment of damage
caused by atmospheric acids are the so called leaf and needle
ash analysis which directly measures damage caused to plants,
atmospheric acid analysis by which the harmful content of
acids can be measured on the spot and the qualitative deter-
mination of small quantities of acid in the atmosphere. The
first method is based on the accumulation of acid in the ex-
posed plants. In the ash of such exposed plant material (nee-
dles of conifers for example) water soluble sulfuric acid,
chlorine, fluorine, and nitrogen are determined and the excess
over normal levels is calculated. The second method, analyz-
ing air acidity directly, uses a series of absorption bottles filled
with different absorbent liquids designed to retain carbon diox-
ide, sulfur dioxide, sulfur trioxide, nitrogen oxides, ammonia,
chlorides and hydrochloric acid which are then measured by
appropriate analytical methods and the respective acidity is
calculated. Toxicity limits are for SO2 3 mg/cu m, for N204
50 mg/cu m, for NH3 30 mg/cu m, for HC1 110 mg/cu m, for
C12 64 mg/cu m and for HF 0.00033 vol %. The qualitative
method uses cotton cloth dipped in a barium hydroxide solu-
tion and in lime water to determine the presence in the at-
mosphere of SO2 and of F respectively.
25445
Barton, S. C. and H. G. McAdie
A SPECIFIC METHOD FOR THE AUTOMATIC DETER-
MINATION OF AMBIENT H2SO4 AEROSOL. Preprint, Inter-
national Union of Air Pollution Prevention Associations, 19p.,
1970. 25 refs. (Presented at the International Clean Air Con-
gress, 2nd, Washington, D. C., Dec. 6-11 1970, Paper CP-7D.)
Although the importance of sulfuric acid (H2SO4) aerosol as a
toxic air pollutant is well established, the aerosol has received
limited attention due to the lack of a satisfactory method for
its determination. An instrument that employs new and im-
proved versions of the established techniques of collection by
filtration and colorimetric analysis provides a convenient
method for the automatic determination of ambient H2SO4
aerosols under field conditions. The aerosol is collected,
together with other particulates, on a Nuclepore polycarbonate
membrane filter, then selectively eluted with 1-propanol for
colorimetric analysis by the barium chloranilate method. Air is
sampled at the rate of 20 1 reciprocal min, and one-hour sam-
pling intervals provide a full-scale sensitivity of 1 ppb, with a
detection limit of approximately .05 ppb. The availability of
this convenient and specific method should make it feasible
for air quality authorities to undertake meaningful surveys to
establish H2S04 levels which at present are unknown or in
serious doubt because of the limitations of existing methods.
25851
Nash, T.
LOW-VELOCITY GAS-LIQUTO EMPEVGER FOR THE CON-
TINUOUS ESTIMATION OF SULPHUR DIOXIDE AND
OTHER ATMOSPHERIC POLLUTANTS. J. Sci. Instr. vol.
38:480-483, Dec. 1961. 3 refs.
An impinger is described, based on the observation that a low-
velocity jet of air containing sulfur dioxide can transfer it very
efficiently to the surface of dilute hydrogen peroxide, then by
rapid micro-circulation to the underlying solution. Air is drawn
into the cell compartment through a filter and glass jet, blow-
ing vertically down onto 0.1 volume peroxide in the cell in
which SO2 is scrubbed from the air and converted to sulfuric
acid. The electrical conductivity of the solution in the cell is
measured through electrodes connected to a simple oscillator,
amplifier, and recorder. The vapor reaction, electrical circuit^
stock solution, jet characteristics, and time constant are
discussed. Calibration and performance are also described.
The instrument records SO2 in the range 0.01 to 10 ppm where
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C. MEASUREMENT METHODS 31
rapid changes in concentration can be expected but the accura- and no peroxide, it is possible to record carbon dioxide con-
ey required is not more than 1 in 20. Its advantage is that gas centration in the range normally encountered in air. One
absorption and measurement of conductivity are done in the modification of the instrument measures light absorption in-
same small cell, with the consequent gain in simplicity and stead of conductivity, permitting the use of colonmetnc re-
speed of response. By using 0.1 mM alkali in the reservoir, agents.
-------
32
D. AIR QUALITY MEASUREMENTS
05152
J. V. Kerrigan, and K. Snajberk
STUDIES ON SULFUR OXIDE POLLUTANTS IN THE AT-
MOSPHERE. California Univ., Berkeley, Sanitary Engineering
Research Lab. May 10, 1960. 82 pp.
The location of the laboratory in an area zoned for heavy in-
dustry and having a local air pollution problem, together with
the availability of an industrial sampling chamber as a source
of sulfur oxide gases, made experimental work particularly
feasible. The investigation was therefore designed to deter-
mine: (1) the comparative reliability of various instruments
used to sample and detect sulfur oxide particles and gases; (2)
the accuracy of various chemical methods of sulfate analysis
at low sulfate ion concentrations; and (3) the concentration of
certain sulfur oxide gases in the local atmosphere at the
Richmond Field Station. Pans of distilled water were set up in
the path of prevailing winds in such fashion that the winds
would pass over an adjacent sulfuric acid manufacturing plant
before entering the Field Station area. The pans were used to
measure the fallout of sulfuric acid mist droplets, while an
electro-static precipitator set adjacent to one of the pans mea-
sured the concentration of sulfuric acid mist in the air. The
validity of the electro-static precipitator results was confirmed
by comparison with a Greenburg-Smith impinger and with a
sintered glass filter by sampling a gas chamber containing a
mixture of sulfur dioxide and sulfuric acid mist under steady-
state conditions. To approximate the concentrations of sulfuric
acid mist under field conditions, samples fed to the instru-
ments were diluted 10 to 50-fold with air. Both a Kruger au-
tometer and a Thomas autometer were used to collect and
analyze for sulfur dioxide. The turbidimetric, the Fritz
titrimetric, the pH titration, and the acidimetric titration
methods of chemical analysis for sulfate were compared in the
course of the investigation.
11492
Polyak, V. E.
ATMOSPHERIC POLLUTION BY NITROGEN OXIDES IN
THE MANUFACTURE OF SULFURIC ACID BY THE
TOWER PROCESS. ((Zagryaznenie atmosfernogo vozdukha
okislami azota pri bashennom proizvodstve sernoi kisloty.))
Hyg. Sanit. (English translation of: Gigiena i bSsanit), 33(4-
6):266-267, April-June 1968. CFSTL TT 68-50449/2
An investigation of atmospheric pollution by nitrogen oxides
(tail gases from the plant for the manufacture of sulfuric acid
by the tower process) at various distances from the pollution
source was made. The gases are discharged into the at-
mosphere by a chimney 40 m tall. The daily discharge into the
atmosphere amounts to 4 tons of nitrogen oxides (expressed as
nitric acid), with a gaseous volume of 817 cu m. There are no
other discharges of nitrogen oxides on the factory premises or
elsewhere in the district. Air was sampled at a level of 1-1.5 m
from the ground, in the direct vicinity of the chimney, and at
distances of 500, 1,000, 3,000 and 6,000 m, the total number of
samples being 413. Measurements were made of the tempera-
ture, relative humidity and velocity of the air and of the
barometric pressure, wind direction, cloudiness, and the color
and movement of the visible 'tail' of the gas discharge.
Nitrogen oxides were detected and determined at the laborato-
ry in most samples (79-89.3%). In a considerable number of
samples the concentration of nitrogen oxides exceeded the
maximum permissible concentration, including some samples
taken at large distances from the discharge site (3,000 and
6,000 m). All minimum concentrations were either equal to or
lower than the maximum permissible concentration, but the
maximum concentrations exceeded this level. The mean con-
centrations of nitrogen oxides likewise exceeded the maximum
permissible concentration, being 2.45 mg/cu m at the distance
of 6,000 m, i.e., eight times the maximum permissible concen-
tration.
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33
E. ATMOSPHERIC INTERACTION
10751
Hoegstroem, Ulf
A STATISTICAL APPROACH TO THE AIR POLLUTION
PROBLEM OF CHIMNEY EMISSION. Atmos. Environ
2(3):251-271, May 1968.
A method is described that not only gives one single concen-
tration value but the expected concentration frequency dis-
tribution at an arbitrary point in the vicinity of the emitting
chimney. The concentration frequency distribution obtained
comprises the full range of meteorological conditions at a
given place. In making the principal mathematical formulation
of the method no assumptions whatsoever are needed about
the mechanism of dispersion. In the practical application on
the other hand, full use is made of the detailed knowledge of
the dispersion process. First a 'basic case' is treated, the chief
characteristics of which are: isolated stack, situated on a flat
surface of uniform roughness; sampling time about an hour.
The following information is found necessary for solving a
concrete problem of this kind. (1) plant data, viz. rate of emis-
sion, gas volume and temperature, chimney height and exit
diameter; (2) geographical site data, viz. roughness length; (3)
meteorological data, viz. wind direction frequencies and
statistics of 'dispersion categories' (stability and wind speed).
Applicable formulae are discussed and also how statistics of
'dispersion categories' can be obtained by evaluating data
from radiosonde stations. Certain deviations from the basic
case are also treated in some detail; limited mixing height, the
effect of large heat content on the dispersion parameters, the
effects of buildings and topography, ground level release and
sampling times other than an hour. A thorough test of the
described method is presented. Nine months statistics of 2-hr
SO2 concentration (2602 values) measured at a point situated
750 m from a sulphuric acid plant are compared with theoreti-
cally obtained statistics. The results strongly supports the
method presented.
21791
Katz, Morris
PHOTOCHEMICAL REACTIONS OF ATMOSPHERIC POL-
LUTANTS. Can. J. Chem. Eng., vol. 48:3-11, Feb. 1970. 44
refs. (Presented at the Canadian Chemical Engineering Con-
ference, 19th Edmonton, Alberta, Oct. 19-22, 1969.)
Photochemical reactions of atmospheric pollutants are
described. The most important primary photochemical process
is the dissociation of nitrogen dioxide into nitric and atomic
oxygen. Activation energy for most atmospheric reactions may
be supplied by absorption of ultraviolet and visible light by
molecules and atoms that act as absorbers. The formation of
free radicals from the photodissociation of aldehydes and
other compounds which absorb solar radiation represents an
important step in the series of reactions that lead to the
production of eye irritation, plant damage, and photochemical
smog. The meteorological and chemical circumstances which
lead to photochemical smog are explained. Quantum yields
from the photooxidation of sulfur dioxide are discussed, and
an experimental method is described. The effect of humidity,
nitrogen dioxide, light intensity, and unsaturated hydrocarbons
are included. The roles of sulfuric acid aerosols, singlet ox-
ygen, and ozone are analyzed.
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34
F. BASIC SCIENCE AND TECHNOLOGY
00530
W. O. Negherbon
SULFUR DIOXIDE, SULFUR TRIOXIDE, SULFURIC ACID
AND FLY ASH: THEIR NATURE AND THEIR ROLE IN AHt
POLLUTION. Hazleton Labs., Inc., Falls Church, Va. June
1966. 1218 pp.
This monograph discusses the following: (1) Historical con-
siderations; (2) Guidelines for the study of air pollution; (3)
Physical and chemical properties of SO2, SOS, and H2SO4; (4)
Meteorological considerations; (5) Anatomical and physiologi-
cal considerations; (6) Deposition and retention of aerosol par-
ticles in the respiratory tract; (7) The effects of SO2 and
H2SO4 on plants; (8) The effects of SO2, SOS, and H2SO4
mist on man and animals; (9) Fly ash origin, nature, and possi-
ble effects; and (10) Removal of pollutants from flue gases.
The bibliography includes 2264 references.
04626
D. R. Coughanowr and F. E. Krause
THE REACTION OF S02 AND 02 EM AQUEOUS SOLUTIONS
OF MNS04. Ind. Eng. Chem. Fundamentals 4, (1) 61-6, Feb.
1965.
An experimental investigation was made to determine the rate
of reaction of sulfur dioxide and oxygen in aqueous solution
containing manganous sulfate as a catalyst. The catalyst was
varied from 0 to 15 p.p.m. of MnSO4 in a batch method, and
from 100 to 10,000 p.p.m. in a flow method. The temperature
was 25 C. The reaction is zero order with respect to both sul-
fur dioxide and oxygen. The concentration of manganous
sulfate has a large effect on the rate of reaction; from 0 to 100
p.p.m. of manganous sulfate, the reaction rate constant, k, is
proportional to the square of the catalyst concentration, but
above 100 p.p.m., k increases less rapidly up to about 500
p.p.m., after which k increases very slowly with catalyst con-
centration. The reaction is easily inhibited by very small
amounts of contaminant.
10907T
Lunge, G. and E. Berl
NITROGEN OXIDES AND THE LEAD CHAMBER PROCESS.
H. BEHAVIOR OF A MIXTURE OF GASES, PRESUMABLY
NO + NO2, IN CONCENTRATED SULFURIC ACID AND
SODIUM HYDROXIDE 1/5 N. ((Untersuchungen ueber
Stickstoffoxyde und ueber den Bleikammerprozess. II. Verbal-
ten eines Gasgemisches von der ungefaehren Zusammenset-
zung NO + NO2 gegen konz. Schwefelsaeure und 1/5-n.
Natronlauge.)) Translated from German. Z. Angew. Chem.
(Weinheim), 19(19):857-869, May 1906.
The behavior of a gas mixture containing NO and NO2 in sul-
furic acid and sodium hydroxide was investigated with the
result that for analytical purposes sulfuric acid is the only ab-
sorption liquid for this gas mixture. Also the behavior of
nitrogen oxide in the presence of oxygen and water was stu-
died together with the kinetics of nitrogen oxide oxidation with
oxygen or air. The kinetic curves indicated that the reaction
2NO+O2=N2O4 takes place at a constant rate which indicates
that the oxidation takes place directly without formation of
N2O3 as an intermediate.
13652
Ovchinnikova, Ye. N. and O. K. Davmyan
OXIDATION OF SULFUR DIOXIDE ON ACTIVATED CAR-
BON BY THE LIQUID- CONTACT METHOD. (Ob okislenii
sernistoge angidrida na aktivirovannoni ugle zhidkostno-kon-
taktnym metodom). Text in Russian. Zh. Fiz. Khim.,
30(8): 1735-1738, 1956. 1 ref.
The oxidation of SO2 on the surface of activated carbon at
room temperature with formation of a definite quantity of ox-
idation product which can be removed with water in the form
of sulfuric acid was demonstrated. Above 220 C, the surface-
oxidized product reverts to SO2. As the quantity of water
sorbed by the carbon increases, the yield approaches a limit of
0.25 g H2SO4 per gram carbon. The rate of acid formation
decreases as the acid concentration increases and is directly
proportional to the square root of the product of the oxygen
and sulfur dioxide partial pressures.
13802
Lewis, W. K. and E. D. Ries
INFLUENCE OF REACTION RATE ON OPERATING CON-
DITIONS IN CONTACT SULFURIC ACID MANUFACTURE.
Ind. Eng. Chem., vol. 17:593-598, June 1925. 6 refs.
The data of Knietsch on the conversion of SO2 to S03 by
platinum at commercial operating temperatures demonstrates
that the catalytic activity of platinum rises rapidly with the
temperature to about 500 C, then goes through a maximum at
about 525 C, beyond which it greatly decreases. The reason
for this maximum is not clear and no experimental data are
available to confirm it. Operating variables under the control
of an engineer are the composition of the gas entering a con-
verter, operating temperature, and the amount, character, and
distribution of platinum used for a given amount of gas. Equa-
tions based on these conditions were derived to determine the
capacity and efficiency of a converter and the optimum tem-
perature at each stage of converter operation. They suggest
that a decided increase in converter efficiency can be obtained
by controlling the temperature of the gases. To achieve this,
converters must be modified to absorb the heat of reaction
and the sensible heat of the gases. Two types of converters
employing this principle are suggested. In both, gases reach
the bottom of the converter at about 400 C. The correct tem-
perature gradient for one converter is maintained by by-pass
valves. Gases are cooled by coils and contact masses. Gases
passing through the second converter are cooled and diluted
by auxiliary air valves. Adiabatic converters control the tem-
perature. The temperature in the first converter after reaction
can rise to 530 C without losing efficiency; the temperature in
the second to 550 C.
-------
F. BASIC SCIENCE AND TECHNOLOGY
35
13875
Pechkovskiy, V. V.
THERMOCHEMICAL DISSOCIATION OF MAGNESIUM
SULFATE. (0 tennokhimicheskom razlozhenii sul 'fata mag-
niya). Text in Russian. Zh. Prikl. Khim., 29(8):1137-1142, 1956.
5 refs.
The rate of thermochemical dissociation of magnesium sulfate
as affected by termperature, time, oxygen content of the gas
passing over the sulfate, and the presence of various metal ox-
ides was studied experimentally to determine the usefulness of
this material as a source for producing acid. Practical dissocia-
tion occurred at 950-1100 C. Of the additives tested (SiO2,
Fe203, CuO), ferric oxide and cupric oxide were found to
have a very significant accelerating influence on the dissocia-
tion reaction, this influence being always greatest in the
absence of oxygen (under nitrogen). The data presented will be
helpful in determining additives to be selected for use with this
process.
13940
Davtyan, 0. K. and E. N. Ovchinnikova
INVESTIGATION OF THE MECHANISM OF OXIDATION,
HYDROGENATION AND ELECTROCHEMICAL COM-
BUSTION ON SOLID CATALYSTS. I. OXIDATION OF SUL-
FUR DIOXIDE ON ACTIVATED CARBON AT 20 C IN THE
PRESENCE OF WATER VAPOR. (Issledovaniye mekhanizma
okisleniya, gidrirovaniya i elektrokhimicheskogo goreniya na
tverdykh katalizatorakh. i. Okisleniye sernistogo angidrida na
poverkhnosti aktivirovannogo uglya pir 20 C v prisutstvii
vodyanykh parov). Text in Russian. Zh. Fiz. Khim., 35(4): 713-
718,1961. 2 refs.
The low-temperature oxidation of sulfur dioxide on the surface
of activated carbon at 20 C was studied, and a method was
developed for determining the absorption and oxidation of
S02 when the oxidation product remains adsorbed on the sur-
face. It was found that in the presence of water vapor, the ox-
idation product is held on the surface in the form of sulfuric
acid. As the amount of adsorbed water vapor increases, the
quantity of sulfuric acid absorbed on the carbon reaches some
maximum determined by the partial pressure of oxygen in the
gaseous phase. Removal of the H2SO4 from the carbon
completely restores its activity.
14249
Calderbank, P. H.
CONTACT-PROCESS CONVERTER DESIGN. Chem. Eng.
Progr., 49(11): 585-590, Nov. 1953. 9 refs.
An equation was derived to express the rate of SO2 oxidation
with a vanadium oxide catalyst in a flow-type isothermal reac-
tor. The expression is applicable up to 100% conversion for a
variety of commercial vanadium catalysts and up to 59% con-
version under near-isothermal conditions and can be used to
calculate the weight of a catalyst required to produce a given
amount of conversion. The units used for the expression can
be converted into tons H2SO4 produced/tons catalyst/day, the
loading in tons multiplied by fractional conversion giving the
reaction rate in tons H2SO4 produced at the relevant tempera-
ture and mean partial pressure of SO2, O2, and SO3. Reaction
rate data from other sources are in broad agreement with the
proposed equation, which was applied to an evaluation of
adiabatic converters and converters with integral heat exchan-
gers. Reaction rates, optimum temperature distribution, and
the required amount of catalyst were determined. An adiabatic
reactor producing 50 tons H2S04 per day requires 14.7 tons of
catalyst for 96% conversion of a feed. A reactor with a heat
exchanger producing the same amount of H2SO4 requires 0.93
tons catalyst for 96% conversion. The calculated optimum
temperature distribution does not differ greatly from that ob-
tained in the converter with a heat exchanger.
14506
Hull, William Q., Frank Schon, and Hans Zirngibl
SULFURIC ACID FROM ANHYDRITE. Mod. Chem.
Processes, vol. 5: 123-133, 1958. 12 refs. (Also: Ind Eng
Chem., Aug. 1957.)
The chemistry of sulfate decomposition and differences in ce-
ment clinker production are discussed. The effect of decom-
position speed, dependence on temperature and additives, par-
ticle size, and granular size with gypsum residues from the
sulfate decomposition were investigated. In the industrial an-
hydrite sulfuric acid process, coke is used as a reducing agent
and enough aluminum-containing materials are added so that
Portland cement is produced per ton of acid. Dissociation of
the calcium sulfate consists of three stages; CaSO4 plus 2 C
yields CaS plus 2CO2; CaS plus 3CaSO4 yields 4CaO plus
4SO2 (the overall reduction process is 2CaSO4 plus C yields
2CaO plus CO2 plus 2SO2); and 3CaS plus CaSO4 yields
3CaO plus 2S2. The CaS and CaSO4 have, at each tempera-
ture, a definite decomposition pressure. Additives of clay or
similar materials raise the decomposition pressure and the tem-
perature in order to maintain the same decomposition rate.
Too much CaS and CaSO4 also lowers the decomposition rate.
As far as sulfur dioxide is concerned, this is the end of the
process. The rest involves making the cement clinker. A
further rise in temperature up to 1400 C completes the reaction
between the components and lime, formed during decomposi-
tion, to produce a good clinker. Besides an exact adjustment
of the proportions of the reduction coke to the anhydrite, the
proportions of the added materials to the CaO and to each
other must be carefully adjusted within determined limits so
that a good clinker results. Even more important, kiln opera-
tion must be carried out under steady conditions. Heat con-
sumption for clinker in the anhydrite sulfuric acid process as
compared with that of normal portland cement clinker must
also be considered. A typical plant and its contact process are
described. Production is inexpensive, and cement is sold at
market value. There was no difficulty in marketing surplus
acid.
14526
Postnikov, V. F., T. I. Kunin, and A. A. Astasheva
THE CONTACT CAPABILITY OF CHROMIC OXIDE FOR
THE OXTOATION OF SO2 TO SO3. (O kontaktiruyushchey
sposobnosti okisi khroma dlya okislaniya S02 v SO3). Text in
Russian. Zh. Prikl. Khim., 9(8):1373-1377, 1936. 10 refs.
The catalytic activity of chromic oxide in the oxidation of sul-
fur dioxide depends on the starting materials and the method
of preparation. Greatest activity was given by a chromic oxide
gel precipitated with ammonia on heating; chromic oxide gels
precipitated with sodium or potassium hydroxides had a much
lower contact property. Water vapor increases the activity of
pure chromic oxide, shifting the curve of contact in the
direction of higher temperatures in comparison with operation
in dry gas. Activation of the chromic oxide gel, precipitated by
ammonia, by the acetates of calcium, zinc, aluminum, and
nickel does not improve the contact properties of chromic ox-
ide. The activity of chromic oxide precipitated with sodium
hydroxide increases in the presence of activators but does not
attain the level of activity of pure chromic oxide precipitated
with ammonia.
-------
36
SULFURIC ACID MANUFACTURING
14538
Boreskov, G. K. and V. P. Pligunov
KINETICS OF THE CONTACT OXIDATION OF SO2.
(Kinetika kontaktnogo okisleniya SO2). Text in Russian. Zh.
Prikl. Khim., 6(5):785- 796, 1933. 14 refs.
An isothermal method was developed for the oxidation of SO2
in a flowing system. The effects of contact time, gas composi-
tion, and temperature on the oxidation rate of SO2 over the
vanadium catalyst 'BOV were studied. The applicability of
the Taylor Lenher formula was shown. The apparent heat of
activation was determined as 20,000 cal for high temperatures
and 55,000 cal for low temperatures. The point of inflection
was at 440 deg. The results were compared with those known
for a platinum catalyst. It was shown that for temperatures
higher than the point of inflection, the course of the reaction
on platinum and vanadium catalysts occurs almost identically.
Upon temperature decrease to the point of inflection, the rate
of oxidation on a vanadium catalyst falls rapidly in proportion
to the sharp increase in apparent heat of activation to 50,000
cal. In this temperature interval, the total rate of the process
determines the rate of freeing the catalyst surface from the
SO3 being formed. On the basis of these conclusions, the
practical use of vanadium catalysts is considered. Formulas
and diagrams are given, establishing the optimal curve of tem-
perature change along the layer of contact mass. This curve
provides for the maximum rate of the process, shows the time
of contact necessary for carrying out any part of the oxida-
tion, and also provides for finding the optimal composition of
the gas mixture giving maximum productivity under these con-
ditions.
14539
Adadurov, I. E., M. V. Apanasenko, L. M. Orlova, and A. I.
Ryabchenko
EFFECT OF THE COMPOSITION AND DISPOSITION OF
THE CONTACT MASS ON THE CATALYTIC ACTIVITY OF
CHROMIUM CATALYSTS. (Vliyaniye sostava i raspoloz-
heniya kontaktnoy massy na kataliticheskuyu aktivnost'
khromovykh katalizatorov). Text in Russian. Zh. Prikl. Khim.,
7(8):1356-1362, 1934. 3 refs.
In spite of their high quality, chromium-tin catalysts have the
disadvantage that the activating mixture requires unavailable
amounts of tin. Attempts to decrease the requirement of cata-
lytic material by applying it to a carrier have not yet led to
favorable results. Efforts to replace tin with other activators
have not produced any promising patents for industrial use.
Only aluminum oxide at temperatures beginning at 530 deg has
given a conversion close to the theoretical yield of approxi-
mately 90%. The maximum increase in the amount of sulfur
dioxide converted into sulfur trioxide per unit volume of con-
tact mass using a chromium-tin catalyst can be attained by
coordinating the reaction with its kinetics and by arranging the
contact material according to particle size in the contact ap-
paratus. Arranging the catalyst particles according to the
movement of the gas with the largest particles at the top of the
apparatus increases contact by 4-5%. The same kinetic princi-
ples applied to a two-stage contact process (loading the first
converter with a chromium mass activated with aluminum ox-
ide, operating at 550 deg, the second converter with a chromi-
um-tin catalyst, operating at 450 deg) resulted in a productivity
increased by 250%. Thus, it appears possible to operate a con-
tact process on a combination chromium catalyst.
14625
Davtyan, O. K., B. A. Manakin, and E. G. Misyuk
TEMPERATURE DEPENDENCE OF SULFURIC ACID FOR-
MATION RATE DURING CATALYTIC OXIDATION OF
SULFUR DIOXIDE ON ACTIVATED CARBON BY THE WET
CONTACT METHOD. (Temperaturnaya zavisimost' skorosti
obrazovaniya sernoy kisloty pri kataliticheskom okislenii
sernistogo angidrida na aktivirovannom ugle zhidkostno- kon-
taktnym metodom). Text in Russian. Nauchn. Ezhegodnik
Odessk. Gos. Univ., Khim. Fak., no. 2:113-115, 1961. 2 refs.
The formation of sulfuric acid was studied experimentally in a
laboratory percolating device in which an incoming SO2-02
mixture serves to lift the solvent so that it trickles over the
catalyst before returning to the solvent reservoir. The partial
pressures of the gas mixture were 200 and 400 mm Hg in two
series of experiments over 10 deg temperature intervals rang-
ing from 0 to 60 C. The temperature coefficient in all cases
varied from 1.2 to 1.3, i.e., within the range typical for a diffu-
sion process.
14626
Chzhi-tsayn, Syao, V. I. Smirnov, and I. T. Sryvalin
THERMODYNAMICS OF SULFATE ROASTING OF CON-
VERTER SLAGS IN A BOILING LAYER. (Termodinamika
protsessov sul'fatiziruyushchego obzhiga konverternykh
shlakov v kipyashchem sloye). Text in Russian. Tr. Ural'sk.
Politekhn. Inst., no. 98:67-71, 1960. 9 refs.
Data from the literature are used to make thermodynamic cal-
culations for reactions of elemental metals (nickel, cobalt,
copper, iron), metal sulfides, metal oxides, and metal oxide-
silicon dioxide complexes with sulfuric acid and sulfur dioxide
at 573-973 K. Isobaric potential is plotted for a number of
reactions. Reaction of metals with sulfuric acid is in the
sequence: cobalt, nickel, copper. Isobaric potentials for reac-
tions between metal sulfides and sulfuric acid are comparable
for iron, cobalt, and nickel but considerably higher for copper.
The reaction sequence for the sulfating of metal oxides is
found to be: cobalt, nickel, copper, iron. Sulfating of silicates
is characterized by much more negative isobaric potentials,
being nearly the same for iron, cobalt, and nickel. It may be
concluded that under similar conditions, oxides, metals, and
sulfides will sulfate more readily than will silicates, ferrites,
and aluminates. It is noted that the drop in isobaric potential
decreases with increasing temperature in the case of sulfur
dioxide but increases with sulfuric acid, the isobaric potential
plots intersecting at 450-500 C. Hence, sulfation with sulfuric
acid will predominate at practicable roasting temperatures
(600-700 C).
14641
Kapustinksy, A. F.
THERMODYNAMICAL THEORY OF SULPHURIC ACID
PROCESSES. Compt. Rend. Acad. Sci. URSS, 53(8):719-722,
1946. 16 refs.
The manufacture of sulfuric acid, regardless of the production
method and catalyst employed, is based on the equilibrium
reaction SO2 plus 1/2O2 yields SOS. With the aid of known
specific heats of gaseous reagents, equations for calculating
the free energy and heat of the reaction were derived from
previously determined equilibrium constants for the formation
of sulfur trioxide from sulfur dioxide and oxygen on a
platinum catalyst. Standard values of these thermodynamic
functions are shown and compared with those contained in the
literature. The absolute entropy of liquid sulfuric acid and its
heat of formation under standard conditions are given, as well
-------
F. BASIC SCIENCE AND TECHNOLOGY
37
as the absolute entropy of gaseous sulfur trioxide. The
proposed thennodynamic theory of the sulfuric acid process
makes it possible to represent as a single system, data con-
stituting the basis of all sulfuric acid production methods for
the oxidation of sulfur dioxide by oxygen.
14653
Kapustinskiy, A. F.
ON THE PHYSICOCHEMICAL THEORY OF OBTAINING
SULFURIC ACID BY THE CONTACT METHOD. (K fiziko-
khimicheskoy teorii kontaktnogo sposoba polucheniya semoy
kisloty). Text in Russian. Issled. Po Prikl. Khim., Akad. Nauk.
SSSR, Old. Khim. Nauk, Sb., 1955:22-38. 38 refs.
This study examines the formation of SO3 from SO2 and ox-
ygen, the thermodynamics of SO3 synthesis, and the
mechanisms of catalysis in this synthesis. The study of the dis-
sociation equilibrium of SO3 at high temperatures over
platinum using modern measuring techniques is described. A
rigorous thennodynamic analysis of available results, based on
classical thermodynamics, was made without any assumptions
or approximations and was found to be in agreement with
spectroscopic and calorimetric data. A structural-model ap-
proach is given to explain the catalytic action of platinum,
proceeding from a proposed deformation of the molecules dur-
ing adsorption, drawing on data from crystal chemistry and
new information regarding molecular structure.
14845
Streicher, J. S.
THE CATALYSIS OF SO2 TO SO3. Chem. Met. Eng.,
37(6):501-502, Aug. 1930.
The use of vanadium as a catalyzer in the sulfuric-acid process
is discussed as a substitute for platinum. At low flow rates
vanadium achieves the same conversions as platinum at given
temperatures. The problem with vanadium is reaching the high
rate at which the gases can be combined independently of the
percentage yield. The joint action of the two factors, highest
flow rates and highest conversions, is the decisive point of
every contact plant. The elimination of platinum and the sub-
stitution of vanadium compounds and other catalytic com-
pounds has an important economic aspect. In 1930, 1 kg of
platinum cost $1286 and 1 kg of vanadium cost $7. The amount
invested in platinum can be overlooked, considering that the
additional cost of patented apparatus, machinery, license fee,
and depreciation always offsets the investment. The high
return value of platinum is often in calculations. Moreover,
platinum does not cost 'two thousand times, as much as
vanadium', the true proportion of the cost of vanadium to
platinum in July 1930 was 1:184.
14871
Graf ton, Raymond William
PROCESS FOR THE TREATMENT OF GLAUBER'S SALT.
(Courtaulds Ltd., London) Brit. Pat. 801,527. 9p., Sept. 17,
1958. (Appl. Jan. 24, 1957, 6 claims).
A process is claimed relating to the treatment of Glauber's
salt, large quantities of which are obtained as a by-product in
the viscose rayon industry, in order to permit the recovery of
useful chemicals from the salt. To date, this salt has had little
market value. The process comprises dissolving the salt in
water, treating the solution with an ion-exchange resin to form
sulfuric acid and a sodium resin salt, and regenerating the
sodium resin salt by treatment with nitric acid. The reactions
involved in this process are RH + Na2SO4 yields NaR +
1/2H2SO4, and NaR + HN03 yields RH + NaNO3, R being
the cation exchange resin. The process is preferably effected
in a cyclic manner. The recovered solutions are sulfuric acid,
which can be used directly in the viscose rayon factory, and
sodium nitrate, which can be used as a fertilizer. In one cyclic
process of this invention, the ion-exchange resin is contained
in a number of reactors which are arranged on a turntable,
which moves the reactors in a cyclic manner so that each reac-
tor moves in turn through four fixed zones. In another cyclic
process, the reactors, instead of being arranged on a turntable,
are fixed, and a single rotary valve is provided which connects
the various reactors to the correct liquor feeding and
withdrawal points at the appropriate stages in the cyclic
process. The number of reactors in the various zones is deter-
mined by the particular reaction to be carried out and the
degree of conversion required, but in general from two to five
reactors in each zone seems to be sufficient for economic
operation. In addition, the speed of rotation of the turntable or
rotary valve and the rate of feed of the solutions supplied to
the reactors must be suitably correlated to allow for adequate
reaction times. Technical details of the process, a sample ex-
perimental apparatus, and pertinent diagrams are included.
15325
Suchkov, A. B., B. A. Borok, and Z. I. Morozova
THERMAL DECOMPOSITION OF A MIXTURE OF MnSO4
+ FeSO4 IN A FLOW OF STEAM. (O termicheskom razloz-
henii smesi MnS04 + FeSO4 v toke vodyanogo para). Text in
Russian. Zh. Prikl. Khim., vol. 32: 1618-1620, May-Aug. 1959.
8 refs.
It was established experimentally that the decomposition of
ferric sulfate in a flow of steam of 500 C yields high-quality
ferric oxide and regenerates a significant quantity of sulfuric
acid of 96% concentration. Decomposition of a mixture of fer-
ric sulfate and manganese sulfate in a flow of steam at 600 C
followed by washing of the solid product with water yields fer-
ric oxide free of manganese impurities.
15416
Suchkov, A. B., B. A. Borok, and Z. I. Morozova
THERMAL DECOMPOSITION OF CERTAIN SULFATES IN
A FLOW OF STEAM. (O termicheskom razlozhenii nekoto-
rykh sul'fatov v toke vodyanogo para). Text in Russian. Zh.
Prikl. Khim., vol. 32: 1616-1618, May-Aug. 1959. 2 refs.
Thermal decomposition at 200-1000 C in steam was studied
using sulfates of lithium, sodium, potassium, copper, berylli-
um, magnesium, calcium, aluminum, titanium, chromium,
manganese, iron, cobalt, and tin. It was demonstrated that
decomposition of certain sulfates under these conditions is an
effective process for obtaining sulfuric acid and corresponding
oxides and that it proceeds at much lower temperatures than
ordinary thermal decomposition. A bond-theory explanation is
given for differences in decomposition temperatures among
these sulfates.
16292
Kozhevnikova, N. V. and D. G. Tracer
PETROGRAPfflC AND X-RAY EXAMINATION OF HtON
OXIDE CATALYST FOR THE PRODUCTION OF SULFURIC
ACID. (Petrograficheskoye i rentgenograficheskoye iss-
ledovaniye okisno-zheleznogo katalizatora dlya proizvodstva
sernoy kisloty). Text in Russian. Zh. Prikl. Khim., 39(6):1272-
1275, 1966. 6 refs.
Iron oxide catalysts undergo partial sulfatization by the action
of sulfur dioxide and sulfur trioxide at 675-750 C. Roasting the
catalyst at 1000 C leads to the formation of nonactive minerals
-------
38
SULFURIC ACID MANUFACTURING
of the iron orthoclase type (aegirite) and solid solutions of iron
oxide with quartz. Long-term (100 hrs) treatment of the
catalyst at high temperatures with insufficient oxygen causes
gradual accumulation of solid solutions of iron oxides with sil-
ica, which subsequently leads to a reduction in catalytic activi-
ty. X-ray data for catalysts prior to and after high-temperature
treatment and after roasting are tabulated.
16377
Rzayev, P. B., V. A. Royter, and G. P. Korneychuk
KINETICS OF SULFURIC ACID CATALYSIS ON BARIUM-
ALUMINUM-VANApIUM CATALYSTS. (O kinetike ser-
nokislotnogo kataliza na bariyevo- alyumovanadiyevykh
katalizatorakh). Text in Russian. Ukr. Khim. Zh., 26(2):161-
167, 1960. 5 refs.
The kinetics of sulfur dioxide oxidation on barium-aluminum-
vanadium catalysts were studied and found to conform to an
equation derived elsewhere by G. K. Boreskov. The heat of
activation was 23 kcal/mole and pertained to an internal-
kinetic regime which was not distorted by the effect of
macrofactors. Even with small catalyst grains (1.5-2.0 mm
diameter), conversion factors below 70%, and temperatures
above 500 C, an internal diffusion retardation occurred which
reduced the measured heat of activation. The activity of the
catalyst remained practically constant with significant dif-
ferences in the degree of reduction of vanadium oxides in the
catalyst. Possible causes for overestimation of the heat of ac-
tivation by the diaphragm method were discussed.
20274
Collins, Conrad G., Jr.
A REVIEW OF SULPHUR FLAME TECHNOLOGY. (PART
2). Sulphur Inst. J., 6(l):18-22, Spring 1970. 52 refs. Part I.
Ibid, Winter 1969-70.
The encounter and reaction of sulfur dioxide with an oxygen
atom appears to be the predominant mechanism for sulfur
trioxide formation according to most studies of stack gases
and the hydrogen sulfide flame. The mechanism can be impor-
tant only in flames with high temperature (1200 C) zones for
the formation of atomic oxygen, as at lower temperatures, the
slow homogeneous reaction between S02 and molecular ox-
ygen appears to be a two body collision reaction. Catalytic ac-
tion of nitric oxide for oxidizing SO2 to 803 is questioned in
lower temperature regions where SO2 would react only with
molecular oxygen, but if high temperatures prevail, such that
the oxygen atom concentration is appreciable, the catalytic ef-
fect of NO may be established. Experimental work with
hydrogen chloride added to the flame (nucleophilic partner)
yielded 38% SO3, and HC1 was viewed as a stabilizing medium
for SO3. Different sulfur oxide species have been detected
spectroscopically at a variety of conditions, from low tempera-
ture to the high temperature of shock waves.
21068
Lasiewicz, Krystyna, Aleksandra Pudliszak-Dziewanowska,
and Juliusz Wesolowski
POROUS STRUCTURE OF VANADIUM CATALYSTS FOR
SO2 OXIDATION. (Struktura porowata katalizatorow
wanadowych do utleniania SO2). Text in Polish. Przemysl
Chem., 43(3):140-143, 1969. 2 refs.
Vanadium catalysts used to oxidize sulfur dioxide in the manu-
facture of sulfuric acid were studied in terms of their pore
structure. The preferred catalyst had pores with a radius larger
than 5,000 A. When 90% of the pores exceeded 1,000 A, the
activity of the catalyst was fairly high, while lowest activity
was assigned to those with a majority of pores below 1,000 A.
For pores ranging in their radius from 75 to 75,000 A, the
specific volume was 0.12-0.65 sq cm/g. The range of specific
surface was 2.4-6.3 sq m/g.
22098
Honti, Georges
OPTTMALIZATION OF A SULFURIC ACID PLANT WITH
THE AID OF A COMPUTER. (OptimaKzation d'une usine
d'acid suBurique a 1'aide d'un ordinateur ekctronique). Text in
French. Ann. Genie Chun., 1967:206-214, 1967. 28 refs.
A computer program to optimalize industrial plant capabilities
is presented. The program is of a general nature and can be
adapted to every process and every actual factory. The in-
dividual blocks are also universally applicable and can be
adapted to actual conditions and data. In the case of calcula-
tions relating to a sulfuric acid factory, the only problem is
that of the catalytic converter, and the corresponding op-
timalization program is drawn up. A simplified version, used
for checking purposes without optimalization, enables the ac-
tivity of the catalyst to be checked as a function of the data
relating to temperature, concentration, and linear velocity
measured in the converter. Working with industrial and labora-
tory measurements, this program can be used to check the
validity of a large number of kinetic equations. The results of
some of these calculations are described. (Author abstract
modified)
22154
Stopperka, K. and V. Neumann
INFRARED SPECTROSCOPIC INVESTIGATIONS OF THE
LIQUID SYSTEMS SO3-H2O AND SO3-D20. 5. THE TEM-
PERATURE-DEPENDENT EQUILIBRIA IN THE LIQUID
SYSTEM H2SO4-SO3. (Infrarotspecktroskopische Unter-
suchung an den fluessigen Systemen SO3-H2O und SO3-D2O.
5. Ueber die temperaturabhaengigen Gleichgewichte im flues-
sigen System H2SO4-SO3). Text in German. Z. Anorg. Allgem.
Chem., 374(2):113- 124, May 1970. 11 refs.
During investigations of the stability of sulfuric-acid mists, the
necessity arose to obtain accurate data on the temperature-de-
penden equilibria of the liquid system sulfuric acid-sulfur
trioxide. An infrared absorption spectrographic study was car-
ried out of H2SO4-SO3 solutions with O to 100% SOS in incre-
ments of 10% (except for one step with 5% SOS). Tempera-
tures increased from 20 C by 10 deg increments up to and in-
cluding the respective boiling points. To withstand the chemi-
cal attack of the solutions at the test temperatures, a special
cuvette was designed in which the solution to be analyzed was
placed in an annular container surrounded by a heating mantle
with a thermostatic temperature control. This, in turn is sur-
rounded by and communicates with a hollow, 2.5 micron thick
(at 20 C), 25 mm diameter space bounded by two 1 mm thick,
25 mm diameter discs of pure silicon and assembled by a very
ingenious method. Sets of infrared absorption spectra of
H2SO4-SO3 solutions with 0.5, 40, 50, 80, and 100% SOS are
presented graphically. Their correction with the aid of data ob-
tained by a compensation cuvette, as well as their interpreta-
tion, are discussed at some length. The information provided
by the spectra is presented tabularly, confirming and supple-
menting previous findings.
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39
G. EFFECTS-HUMAN HEALTH
11379
Bustueva, K. A.
TOXICITY OF SULFUR OXIDES INHALATION IN
CHRONIC CONTINOUS EXPERIMENT. In: Biological Effect
and Hygienic Significance of Atmospheric Pollutants, Book
1/9, V. A. Ryazanov and M. S. Gol'dberg (eds.), Translated
from Russian by B. S. Levine, U. S. S. R. Literature on Air
Pollution and Related Occupational Diseases, Vol. 16, pp. 82-
98, 1968. ((15)) refs. CFSTI: PB 179141
Prolonged uninterrupted inhalation of air containing a mixture
of SO2 and sulfuric acid aerosol affected the organism in a
synergistic (additive) manner. In this connection sanitary
evaluation of the simultaneous presence of SO2 and of sulfuric
acid aerosol in atmospheric air of inhabited areas should be
quided by a general formula which is based on the principle of
simple addition. A formula is proposed as a guide in evaluating
the sanitary condition of atmospheric air of populated air of
populated areas which contained SO2 gas and sulfuric acid
aerosol simultaneously.
16774
Amdur, Mary O.
TOXICOLOGIC APPRAISAL OF PARTICULATE MATTER,
OXIDES OF SULFUR, AND SULFURIC ACID. J. Air Pollution
Control Assoc., 19(9):638-646, Sept. 1969. 62 refs.
An examination of the available lexicological literature in-
dicates that sulfur dioxide itself would be properly classified
as a mild respiratory irritant, the main portion of which is ab-
sorbed in the upper respiratory tract. The literature further in-
dicates that sulfuric acid and irritant sulfates, to the extent
that the latter have been examined, are more potent irritants
than SO2. The irritant potency of these substances is affected
by particle size and by relative humidity, which factors are
probably interrelated. There is evidence, based on animal ex-
periments of one investigator, indicating that the presence of
particulate matter capable of oxidizing S02 to H2SO4 caused
a three to fourfold potentiation of the irritant response. The
aerosols causing this potentiation were soluble salts of ferrous
iron, manganese, and vanadium all of which would become
droplets upon inhalation. Insoluble aerosols such as carbon,
iron oxide fume, triphenylphosphate, or fly ash did not cause
a potentiation of the irritant of sulfur dioxide even when used
at higher concentrations. The concentrations of SO2 used in
these various experiments were in some cases as low as 0.16
ppm. The catalytic aerosols were used at concentrations of 0.7
to 1 mg/m3 which is above any reported levels of these metals
in urban air. If the S02 present as an air pollutant remained
unaltered until removed by dilution, there would be no
evidence in the lexicological literature suggesting thai it would
be likely to have any effects on man al prevailing levels. Slu-
dies of almospheric chemislry have shown thai SO2 does nol
remain unaltered in the atmosphere, but is converted to
H2SO4. Such a conversion increases ils irritanl potency. On
this basis, ihe lexicological literature combined with the litera-
ture of atmospheric chemistry suggest thai sulfur dioxide
levels be conlrolled in terms of Ihe potential formation of irri-
tant particles. Therefore control measures should be, as far as
feasible, aimed at bolh SO2 and particulate material and not
against either alone. This article is followed by a discussion by
J. Wesley Clayton, Jr. (Author's Abslracl Modified)
17623
Bushlueva, K. A.
EXPERIMENTAL STUDIES ON THE EFFECT OF LOW OX-
DDES OF SULFUR CONCENTRATIONS ON THE ANIMAL
ORGANISM. In: Limils of Allowable Concenlralions of Al-
mospheric Pollulants. V. A. Ryazanov (ed.), Book 5, Washing-
ton, D. C., U. S. Public Heallh Service, March 1962, p. 92-103.
7 refs. (Translated by B. S. Levine.)
Sevenly-eighl guinea pigs approximately one monlh old and
weighing belween 150 and 250 g were divided into groups of
four and exposed for 120 continuous hours to low concenlra-
lions of sulfuric acid aerosol and sulfur dioxide, individually
and in combination. A continuous 120 hr exposure to 3 mg/cu
m of SO2 and 1 mg/cu m of sulfuric acid aerosol produced
pathomorphological changes in the lungs and upper respiralory
passages and brought aboul Ihe appearance of sclerosis two to
three months after exposure discontinuation. Similar changes
were observed in the lungs and upper respiratory tracts in
animals exposed to the combined effects of sulfur dioxide and
sulfuric acid aerosol in concentrations reduced cor-
respondingly to 1.0 mg/cu m and 0.5 mg/cu m. Changes in lung
histamine contenl were observed and suggesl the possible role
of this subslance in Ihe palhogenesis and clinical sympto-
matology frequently witnessed during London smogs. Dala ob-
tained in the investigation, support the contention of other in-
vestigators thai SO2 is the leading agent in the London smog
formation.
22594
Bushtueva, K. A.
NEW STUDffiS ON THE EFFECT OF SULFUR DIOXIDE
AND OF SULFURIC ACID AEROSOL ON REFLEX ACTIVI-
TY OF MAN. In: Limils of Allowable Concentrations of At-
mospheric Pollutanls. Book 5, V. A. Ryazanov (ed.), p. 86-92.
Translated from Russian. B. S. Levine, March 1962. 2 refs.
Data on the threshold reflex activity of simultaneously present
sulfur dioxide and sulfuric acid aerosol were gathered by a
direcl continuous recording of Ihe effecl of inhalation of Ihe
gases on Ihe cerebral cortex. Onsel of electrical activity
desynchronizalion, or alpha-rhylhm suppression, was laken as
Ihe index of positive response. Sulfur dioxide broughl aboul a
well-defined desynchronizalion al 0.9 mg/cu m concenlration.
When combined wilh lighl, sulfur dioxide stimulated the
developmenl of conditioned reflexes. In such inslances,
desynchronizalion effecl were even more pronounced. The
maximum sulfur dioxide concenlration eliciting conditioned
reflexes was 0.6 mg/cu m. In olher experimenls, lesl subjecls
inhaled sulfur dioxide in sublhreshold concentrations, with
light Ihe conditioned stimulator. After 19 associated applica-
tions, ihe reflex manifested ilself even in Ihe absence of sulfur
dioxide, indicating that sulfur dioxide continues to stimulate
reflex activity despite the extinction of Ihe primary visible
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40
SULFURIC ACID MANUFACTURING
reaction. Incidental application of sulfuric aerosol in
subthreshold concentrations elicited no electrical cerebral ac-
tivity changes in the form of desynchronization. Where 0.63
mg/cu m, or threshold concentrations, were used,
desynchronization lasting only 1-2 seconds was observed.
However, when a 0.4 mg/cu m subthreshold concentration was
used as a conditioned stimulator, with light the conditioned
reflex reinforcing agent, a fully conditioned reflex eventually
developed. This suggests that subthreshold odor perception
concentrations of sulfuric acid aerosol can be used in
establishing changes in cortical activity as recorded on an elec-
troencephalogram.
23930
Clayton, J. Wesley, Jr.
BIOLOGICAL EFFECTS OF SULFUR DIOXIDE AND FLY
ASH. Edison Elec. Inst. Bull., 38(7):222-225, July-Aug. 1970.
(Presented at the Edison Electric Institute, 38th Annual Con-
vention, Boston, Mass., June 2, 1970.)
Experiments were undertaken to determine the biological ef-
fects on monkeys and guinea pigs of several concentrations of
sulfur dioxide, sulfuric acid mist, and fly ash, as well as mix-
tures of these materials. In all of the measurements employed
to assess lung performance, no adverse effects were discerned
when guinea pigs inhaled 0.1, 1.0, or 5.0 ppm of SO2 in fil-
tered air. In fact, as shown by carbon monoxide uptake, the
guinea pigs breathing 5.0 ppm SO2 showed a greater ability to
effect the diffusion of oxygen and carbon dioxide across lung
membranes than all the animals including the controls. When
the investigation was terminated after one year, the guinea
pigs exposed to 5.0 ppm evidenced a reduction in the
prevalence and severity of the lung changes which are the nor-
mal accompaniment of age in these animals. A slight increase
in the size of the liver cells was observed, as well as an in-
crease in liver cell vacuoles. Sulfur dioxide concentrations of
0.1, 0.5, and 1.0 ppm imposed no detriment on monkeys as in-
dicated by body weight, lung function, blood studies,
biochemical measurements, or microscopic examination of tis-
sues. However, an accidental overexposure of 200 to 1000
ppm SO2 for about 60 minutes was responsible for a deteriora-
tion of lung function and an apparently lowered oxygen-carry-
ing ability of the blood. Studies on fly ash participates in
which monkeys were exposed to 0.1 or 0.5 mg/cu m indicated
no adverse effects of the 18-month exposure.
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41
I. EFFECTS-MATERIALS
20820
COMMUNITY AIR QUALITY GUIDES: SULFUR COM-
POUNDS. Am. Ind. Hyg. Assoc. J., 31(2):253-260, March-April
1970. 26 refs.
The major sulfur compounds detected in the atmosphere are
sulfur dioxide, sulfur trioxide, sulfuric acid, sulfates, and
hydrogen sulfide. The chief effects of SO2 are eye and
respiratory tract irritation, and increased pulmonary resistance.
At concentrations of 87 mg/cu m for 2.75 hours, SO3 proved
fatal to guinea pigs. Hydrogen sulfide is a respiratory and eye
irritant at low concentrations, and at high concentrations can
cause respiratory paralysis. It is believed that sulfur com-
pounds produce a more severe effect when they are adsorbed
on a particle small enough to penetrate the lung. Sulfur oxides
and hydrogen sulfide can also damage vegetation. Materials
such as metals, paper, leather, textiles, paint, and ceramics are
also damaged by sulfur compounds. It is suggested that the
sulfur oxide concentration in the air kept as low as possible to
prevent damage to vegetation, deterioration of materials, and
to avoid the presumed adverse health effects. Methods for
sampling sulfur compounds and their physical and chemical
properties are also included.
24160
Maeda, Seiichiro, Hiromi Hasegawa, and Hiroya Watanabe
A NEW METHOD OF TREATMENT OF SULFUR DIOXIDE
ABSORBING SOLUTION. (Aryusangasu kyushueki no shori
hoho). Text in Japanese. (Steel Manufacturing Chemical Indus-
tries (Japan)), Japan. Pat. Sho 37-9451 3p., July 27, 1962.
(Appl. Sept 3, 1960, claims not given).
The dilute sulfur dioxide discharged from sulfuric acid plants
or ore refineries is removed by absorption in ammonium
sulfite solution. The concentrated solution of sulfur dioxide
thus formed is added to sulfuric acid and regenerated. In this
process of recovering sulfur dioxide, ammonium sulfate is also
recovered. Normally, minute amounts of ammonium
thiosulfate and ammonium polythionite are contained in the
solution, causing corrosion of the container. The present in-
vention is concerned with abating the corrosion. After
establishing that corrosion was primarily caused by the two
ammonium salts, it was found that the rate of decomposition
of the salts was a function of acid concentration, temperature,
and time. The decomposition is a one-molecular reaction that
decreases corrosion when these three factors are satisfied.
Container corrosion was almost completely negligible when an
ammonium sulfite-SO2 solution was heated with excess sul-
furic acid, so the potassium dichromate consumption was
below 0.002 mol/1. In a sulfuric acid manufacturing factory,
the sulfur dioxide absorbing solution contained 7-9% ammonia
and 25-33% free sulfuric acid. The result of a corrosion test
showed 10-15 g/sq m/nr. When the solution was kept at 90 C
for 3 hours and at an acid concentration of 10 N, ammonium
thiosulfate and ammonium polythionite were reduced below
0.0004 mol/1 in terms of potassium dichromate consumption.
As a result, corrosion was reduced to 1.2-1.5 g/sq m/nr, which
was negligible.
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42
J. EFFECTS-ECONOMIC
11791
A STUDY OF PROCESS COSTS AND ECONOMICS OF
PYRTTE-COAL UTILIZATION. Little (Arthur D.) Inc., Cam-
bridge, Mass, and Dorr- Oliver, Inc., Stamford, Conn., Con-
tract PH 86-27-258, 251p., March 1968. CFSTI: PB 182303
The economics of utilizing iron pyrite (FeS2) from coal
beneficiation were investigated; the prices that might be paid
coal operators for low-sulfur coal and an acceptable grade of
pyrite feed material for use in sulfuric acid manufacture were
determined. The net financial benefits to operators are esti-
mated at $1.16 to $1.57 per ton of coal processed. A premium
of $1.10-$1.20 per ton of coal should be paid by nonutility
users and by utilities subject to stringent air pollution abate-
ment restrictions. Of this amount, approximately $0.30
represents the net value of the coal to a user; the balance
represents the premium connected with achieving lower sulfur
content in the stack gas and reduced sulfur dioxide pollution
of the atmosphere. It is emphasized that considerable tonnages
of pyrite-bearing coal must be processed to support a 1500-
ton-per-day sulfuric acid plant. Assuming a feed stream con-
taining 85% pyrite, a requirement of 1550 pounds of feed per
ton of 98% acid produced, an original sulfur content of 4%,
and a coal yield of 90%, 5.1 million tons/yr of coal will have to
be beneficiated to yield 1% sulfur-content coal. Investment
and operating costs have been calculated for every combina-
tion of the three major variables associated with sulfuric acid
production: plant capacity, feed composition, and plant type.
The results show manufacturing costs to be $5.51 to $25.40 per
ton of acid and plant investment, $3.7 to $35.5 million.
17203
Dels, Heinriche
AIR POLLUTION PROBLEMS IN WEST GERMANY AND
THE ROLE OF INDUSTRY. (Luftforurensningsproblemer i
Vest-Tyskland industriens innsats). Text in Norwegian. Tek.
Ukeblad (Oslo), 116(45): 1245-1247, Dec. 1969.
West Germany has been occupied in the last decade with
reducing emissions of dust and smoke. Effectiveness of dust
filters has increased threefold, and filtration is more economi-
cal. The dust content can now be reduced to 150 mg/cu m for
an emission rate of 100,000 cu m/hr. In 1950, the dust output
from the West German cement industry was 3.5% of the
clinker produced; in 1967, it was 0.15%. Dust output from the
manufacture of calcium carbide was reduced to 3 mg/cu m of
exhaust gases. Attention now centers on reducing sulfur diox-
ide emissions. An electric power plant in Essen absorbs it with
a new type of activated carbon, recovering the SO2 for the
manufacture of H2SO4, the cost per 1000 kWh being about 1
DM (25 cents), and this can be further reduced. Government
standards now limit the sulfur content of fuel oils to 1.8%.
About 20% of the total SO2 emission in West Germany comes
from sulfuric acid plants. A new 'double contact' process can
reduce S02 emissions of such a plant from 17 to 3 kg per ton
of H2SO4 produced. Nitrogen oxides emitted from nitric acid
plants have been reduced by 50% with special absorption
equipment. New legislation sets a maximum average of 2
mg/cu m for fluorine emissions, or 5 mg for short intervals.
Readings as high as 2.7 mg have been recorded above the
Ruhr from January 1, 1966, to December 31, 1968. During that
period, industry in North Rhine-Westphalia invested
4,000,000,000 DM on air pollution problems related to existent
operations and about 275,000,000 DM on those related to new
ones. Exhaust purification for the 2-year period cost
3,000,000,000 DM, plus an additional 30,000,000 for research
this in comparison with a gross national product of
300,000,000,000 DM per year. The total amount spent by in-
dustry is small compared with the damage caused, which
amounts to 50 DM per capita per year, or 3,000,000,000 for
the entire republic, not including losses due to sickness or
sanitation problems.
21206
Schwartz, Irvin
ENVIRONMENTAL CONTROL. Chem. Week, 106(24):79-86,
June 17, 1970.
Methods and costs of air pollution control are reviewed with
emphasis on the efforts of the chemical processing industry.
The magnitude of the task is shown by Public Health Service
estimates of the amount of pollutants poured into the at-
mosphere each year: particulates, 15 million tons; sulfur ox-
ides, 30 million tons; hydrocarbons, 24 million tons; carbon
monoxide, 87 million tons; nitrous oxides, 17 million tons.
Within the chemical processing industry, the percentage of
capital outlay for air pollution control equipment is expected
to remain constant, but the kind of equipment is expected to
change. Expenditures for particulate controls account for more
than one-third of industry expenditures. Gaseous emission
controls, currently less than 2% of sales, is expected to jump
to 40% following development of Federal gaseous emission
criteria. The Health, Education, and Welfare Dept. guidelines
for air quality criteria issued to date are listed. The cost of
compliance with the HEW 'suggestions' are estimated. For the
sulfuric acid industry, this estimate is $26-39 million capital ex-
penditure and $1.5-2.8 million/year operating cost. For the
phosphate fertilizer industry, the estimates are $3.1-6.7 million
and $1.3-2.7 million. The four basic means of collecting par-
ticulates, fabric filter, electrostatic precipitator, cyclones, and
scrubber are described, along with their capabilities and cost.
The three basic systems for gaseous emission control,
scrubbing, adsorption, and incineration are similarly treated.
By-product recovery is evaluated as a means of reducing the
effective cost of air pollution control. In contradiction to the
National Research Council-National Academy of Engineering's
statement 'commercially proven technology for control of sul-
fur oxides from combustion processes does not exist', half-a-
dozen sulfur oxide-sulfuric acid conversion processes are
listed.
21308
Ferguson, F. A., K. T. Semrau, and D. R. Monti
SO2 FROM SMELTERS: BY-PRODUCT MARKETS A
POWERFUL LURE. Environ. Sci. Technol., 4(7):562-568 July
1970.
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J. EFFECTS-ECONOMIC
43
The non-ferrous smelting industries currently recover less than
one quarter of the sulfur in the ores treated by the 26 smelters
west of the Mississippi. The rest, almost 1.6 million long tons
of sulfur a year, is being emitted as sulfur oxides. Pollution
control could be advanced significantly if smelters could make
and market any of the following by-products: elemental sulfur,
sulfuric acid, liquid sulfur dioxide, and ammonium sulfate (or
bisulfite). The results of an analysis of the potential market are
reported. The total market for liquid sulfur dioxide in the
western United States is so small that no market or producc-
tion data was developed. The 1970 cost of producin elemental
sulfur at the smelter (45-100 dollars per ton) provides little op-
portunity to complete with Frasch mine produced products at
10-30 dollars. Sulfuric acid with its smelter-produced cost of 4-
25 dollars per ton can complete as long as transportation costs
are held to a minimum. This requires that the market be within
a few hundred miles of the smelter. Even with this stipulation,
the total market including potential growth through 1975 could
absorb only 40% of the potentially producible sulfuric acid.
Emission reductions of 60-65% could be obtained. Together
with the current and potential market for ammonium sulfate,
an emission reduction of 65-70% is possible.
22397
SULFUR THAT GETS AWAY. Chem. Week, 98(21):26-28,
May 21, 1966.
Several processes under development for recovering sulfur
now emitted in stack gases are noted; this potential resource is
related to a present shortage of sulfur for industrial use in the
U. S. and other areas. A major cause of the shortage is the in-
creasing demand due to new foreign and domestic capacity for
sulfuric acid and fertilizer. Sulfuric acid producers are hardest
hit by the shortage. U. S. governments efforts to discourage
rising sulfur prices are outlined. Drilling of offshore sulfur
deposits is receiving increasing attention, and a worldwide
search for more sulfur from a variety of sources is underway.
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44
K. STANDARDS AND CRITERIA
06349
AMBIENT Am QUALITY OBJECTIVES - PART 500 (STATU-
TORY AUTHORITY: PUBLIC HEALTH LAW. 1271, 1276).
New York State Air Pollution Control Board, Albany, Dec. 11,
1964, 11 pp.
Ambient air quality objectives are tabulated for various pollu-
tants. The objectives vary according to subregions which are
determined by land use. Included is a list of references for the
sampling and analytical methods employed in the measurement
of particulates, sulfur dioxide, hydrogen disulfide, fluorides,
beryllium, oxidants, carbon monoxide, and sulfuric acid mist.
19750
Pennsylvania State Dept. of Health, Harrisburg, Air Pollution
Commission
PENNSYLVANIA AMBIENT AIR QUALITY STANDARDS.
6p., Oct. 20, 1969. 10 refs.
Annual, 30-day, 24-hr and/or 1-hr air quality standards are
given for 12 pollutants (suspended and settled particulates,
lead beryllium, sulfates as H2SO4, sulfuric acid mist, fluorides
as HF, sulfur dioxide, nitrogen dioxide, oxidants, hydrogen
sulfide, and carbon monoxide) in accordance with the require-
ments of the Pennsylvania Air Pollution Control Act of 1960.
These standards, which will be reviewed at least once a year,
are for single-point measurements; they represent minimum,
and not necessarily desirable quality. The 24-hr standard for
SO2 is 0.10 ppm; for suspended particulates, 195 micro-
grams/cu m. An antidegradation policy is stated to the effect
that where present air quality is significantly higher than the
established standards, the difference will be conserved, based
on a long range forecast of probable land and air uses in areas
of high air quality. Sampling and analytical procedures to be
employed for measuring ambient levels are specified for each
of the 12 pollutants.
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45
L. LEGAL AND ADMINISTRATIVE
05407
T. Toyama
AIR POLLUTION AND HEALTH IMPEDIMENT. Japan J.
Ind. Health (Tokyo) 8, (3) 45-8, Mar. 1966. Jap. (Presented at
the 39th Annual Meeting, Japan Society of Industrial
Medicine, Ube, Japan, Apr. 7-9, 1966.)
The 39th Annual Meeting of the Japan Society of Industrial
Medicine was held on April 7-9, 1966 in Ube, Yamaguchi-ken,
Japan. The theme of one of the symposia was planning pro-
grams for air pollution control in which air pollution and
health impairment and the engineering and practice of air pol-
lution control were discussed. The main health impairments
covered deal with effects of pollution on the respiratory
system and acute diseases resulting therefrom. Prior to World
War II there were no legal problems in pollution control but
by 1963, it was necessary to establish laws covering soot and
dust control. City planning and building restriction ordinances
have come into effect. Dust and soot fall have decreased by
one-sixth in the past sixteen years. Millions of dollars have
been paid by factories and industries for the establishment of
dust collectors and SO2 counter-measures. Waste gas disposal
in nitric and sulfuric acid plants has been brought under con-
trol since 1964. Re-use of the waste gases has played an im-
portant role in the economic feasibility of air cleaning.
10998
Putnam, B. and M. Manderson
IRON PURITES FROM HIGH SULFUR COALS. Chem. Eng.
Progr. 64(9):60-65, Sept. 1968.
The major sources of SO2 emission are coal fired power
generation facilities, followed by other industrial facilities and
space heating. It also appears that power plants will become
increasingly important potential contributors of SO2 emissions.
Therefore, reduction of emissions from coal fired power
generation facilities is of principal concern. The National
Center for Air Pollution Control authorized two commercial
firms to investigate the economics of utilizing iron pyrite
(FeS2) obtained from coal beneficiation, such as in sulfuric
acid manufacture. The evaluation includes technical, market-
ing, and economic considerations and emphasizes the three
major coal producing regions in the U. S. believed to have sig-
nificant quantities of pyrite associated with the coal: central
Pennsylvania, southern Illinois, and northeast Ohio.
11242
M. C. Manderson
SULFUR OUTLOOK INTO THE EARLY 1970'S. Preprint,
Arthur D. Little, Inc., Cambridge, Mass., ((28))p., 1968.
(Presented at the 61st Annual Meeting, American Institute of
Chemical Engineers, Symposium on Sulfur, Sulfuric Acid and
the Future, Part I, Los Angeles, Calif., Dec. 1-5, 1968, Paper
5-A.)
In 1967, the United States consumed 9.3 million long tons of
sulfur equivalent. Ninety percent of the total amount of sulfur
consumed was in the form sulfuric acid. The major end uses
of sulfuric acid were used in producing nitrogenous and
phosphatic fertilizers. The Free World increase in sulfur con-
sumption has been higher than that of the United States since
1950, 51% per year compared with 3.6% per year. Over the
next seven years Free World consumption is expected to grow
at 5% per year, from the 1967 level to 36 million long tons to
39 million long tons. About 5.5 million long tons of new sulfur
capacity will emerge outside the United Sates over the next 2
1/2 years. Sulfur production in U. S. will grow from the 1967
level of 9.3 million long tons to 14.1 million long tons by 1970
and to 15.8 million long tons by 1975. The amounts of sulfur
from lower cost sources will be adequate to meet U.S. needs
by 1970, including net exports of one million tons per year. It
is believed that sulfur prices will seek lower levels which are
more in line with mimimum return requirements.
24033
Damon, W. A.
THE CONTROL OF NOXIOUS GASES AND FUMES
DISCHARGED FROM INDUSTRIAL UNDERTAKINGS.
World Health Organization, Copenhagen (Denmark), Regional
Office for Europe, Proc. Conf. Public Health Aspects Air Pol-
lution Europe, Milan, Italy, 1957, p. 103-130. 26 refs. (Nov. 6-
14.)
The greatest contribution to air pollution arises from the com-
bustion of fuel for domestic and industrial purposes and from
motor traffic. Its damaging effects include injury to plants,
deterioration of property, and possible or proven hazards to
the health of humans and animals. British air pollution legisla-
tion is embodied mainly in three Acts of Parliament: the Alkali
etc. Works Regulation Acts, first enacted in 1863; the Public
Health Acts, 1936; and the Clean Air Act, 1956. Evolution of
the chemical industry has caused a variety of changed and
new pollutants. Fluorine compounds can be washed in alkaline
solutions, followed by electrical precipitation. The escape of
SO2 from the exits of sulfuric acid plants depend on the effi-
ciency with which the the process is conducted. In four stage
contact plants burning brimstone, recourse to scrubbing the
exit gas with either soda or ammonia may be necessary. Power
stations remove SO2 from waste fuel gases by scrubbing with
slightly alkaline water. Sulfur dioxide arising from the roasting
of copper as in the production of iron oxides is normally ab-
sorbed by passage through towers packed with limestone.
Hydrogen chloride may be recovered at a useful strength by
arranging a counter current series of absorbers. Hydrogen sul-
fide may be scrubbed with caustic soda to produce sodium sul-
fide; it may be absorbed by passage through hydrated iron
oxide which can be regenerated to produce spent oxide con-
taining up to 50% sulfur; or it can be stripped out by means of
a solvent and regenerated in concentrated form for treatment
in a Claus Kiln. Gases containing chlorine may be scrubbed
with an alkaline solution or by contact with milk of lime;
passage through a tower packed with scrap iron is also effec-
tive. Nitrogen peroxide may be recovered in the form of nitric
acid by water washing; but for every three molecules of
nitrogen peroxide thus absorbed there is evolution of one
molecule of nitric oxide which must be reoxidized to nitrogen
peroxide.
-------
46
SULFURIC ACID MANUFACTURING
25520
Wright, G. A.
ENVIRONMENTAL POLLUTION. J. New Zealand Inst.
Chem., 34(5): 171-179, Oct. 1970.
A condensed account of four speeches which were presented
at a symposium on Environmental Pollution in Auckland, May
12, 1970 are given, together with a brief summary of the
discussion. The concern today with total quality of our sur-
roundings is not merely with pollution of water by sewage,
toxicants, nutrients and other unwanted materials, nor with air
pollution by industrial and other gaseous or smoky garbage
escaping into the atmosphere; the world is becoming con-
cerned also about noise and heat pollution and the general
man-made changes in our surroundings which frequently bring
deterioration in living. Air pollution legislation in New Zealand
requires scheduled chemical processes to employ the 'best
practicable means' to control the discharge of pollution to the
atmosphere, but there have been criticisms of the effective-
ness of such legislation when compared with, for example,
legislation that specifies emission standards. In New Zealand,
animal dropping from nearly sixty-million sheep, from eight-
and-a-half million cattle, and from over half a million pigs will
be spread on the ground for a long time to come and much of
this will be washed by rain into the waters. There must be a
tripartite compromise between the natural desire of the public
to enjoy an unpolluted atmosphere; the legitimate aspirations
of industry to avoid unremunerative expense; and national
health and global rights, requirements and interests. To take
one particular example to illustrate improvements in technolo-
gy, mention is made of a contact sulfuric acid plant with the
Chatelier principle having been applied to it.
-------
47
N. GENERAL
04845
H. C. Wohlers
SULFUR OXIDES AS AIR POLLUTANTS. Preprint. 1965.
Air pollution by sulfur oxides, SO2 in particular, is reviewed
in its various aspects. Health effects of SO2 include respirato-
ry ailments which can occur to a greater or lesser degree, de-
pending upon concentration of the gas in the air and the
susceptibilities of those effected. Air concentrations of less
than 0.3 ppm are considered harmless to vegetation; the ef-
fects of higher concentrations result from the interaction of
such factors as time and environment with concentration. The
corrosive effects of SO2 and H2SO4 aerosols in urban areas
are particularly noticeable in materials deterioration. H2SO4
aerosols play a part in visibility reduction in urban air. Based
upon an estimate of 390,000,000 tons of sulfur per year
deposited as sulfate in rain, 30% of the sulfur emissions are
considered to be man-made. Precipitation is the most efficient
process by which sulfur is removed from the air. Guidelines
for better control of this problem are suggested.
-------
AUTHOR INDEX
49
ADACHI N »B-23264
ADADUROV I E 'F-14539
AMDUR M 0 *G-16774
AMELIN A G 'B-19682, B-24256
ANGHEL P B-15739
ANON 'B-11146
APAKHOV I A B-23070
APANASENKO M V F-14539
ARGENBRIGHT L P *B-21309
ARKHIPOV, A S 'B-06282
ASANO T *B-24673
ASTASHEVA A A F-14526
AVDEYEVA I V B-23070
AVERBUKH T D 'B-23070
AVY, A P 'B-03129
B
BACON R F *B-19886
BAKINA N P B-23070
BARTON S C 'C-22645, 'C-25445
BASARGIN, N N 'C-09295
BEIGHTON, J 'B-07925
BENCOWITZ I B-19886
BERL, E F-10907
BERLY E M *B-24110
BILLINGS, C E *B-07552
BLINOVA N P B-23070
BONDARCHUK T P B-16291
BOONE, R E C-00482, *C-01819
BORESKOV G K 'B-16480, 'F-14538
BOROK B A F-15325, F-15416
BOYTSOV, A N B-06282
BRICE, R M C-01819
BRINDUE L B-15739
BRINK J A JR *B-25717, *B-26095,
C-23771
BRINK, J A JR 'B-00587, 'B-11235
BROOMHEAD F B-25643
BROWDER T J JR *B-24103
BULICKA M *B-13206
BURBA A A B-23070
BURGESS W D 'B-19606
BURGGRABE W F B-26095
BURGGRABE, WF B-00587, B-11235
BUSHTUEVA K A *G-17623, *G-22594
BUSHTUEVA, K A *G-11379
CADA V B-25768
CALDERBANK P H *F-14249
CARES, JW »C-11140
CHZHI TSAYN S 'F-14626
CLAUS, K E B-09559
CLAUSS N W 'B-23556
CLAYTON J W JR 'G-23930
COLLINS C G JR 'F-20274
CONNOR J M *B-17053
COTHAM, R L 'B-05514
COUGHANOWR, D R 'F-04626
CRAWFORD H L A-21221
CRIDER, W L 'C-00381
CUFFE, S T *B-02355
CUNNINGHAM G H 'A-13596
D
DAMON W A 'L-24033
DAVMYAN 0 K F-13652
DAVTYAN O K *F-13940, 'F-14625
DEAN, C M B-02355
DOERR K H B-19228, B-24628
DONOVAN J R *B-25133
DRECHSEL H *B-19228, *B-24628
DUBOIS L *C-15745
DUFF, G M C-09369
DUKES, R R *B-11238
EMICKE K *B-13337
FAIRS G L *B-24695
FARKAS, M D B-11238
FARRAR G L *B-24246
PELS M 'A-21221
FERGUSON F A 'J-21308
FIRST M W B-24110
FITT T C B-15991
FLEMING E P *B-15991
FOHL J B-21703
FRANZ M 'B-25491
FULTON C H 'A-25605
FURKERT H 'B-20670
GANZ S N 'A-13403, 'B-19370
GARBATO C 'B-17887
GIBSON, F W 'A-10749
GLOWIAK B *B-25468
GOSTOMCZYK A B-25468
GRAFTON R W 'F-14871
GREEN, W D 'C-09633
GREENWELL, L E B-00587, B-11235
GRIM H B-24628
GRIMM H B-19228
GRODZOVSKIY M K 'B-19943
GUYOT G B-11629, 'B-13728, 'B-14030
GUYOT, G L *B-09913
H
HAJEK J B-13206
HAMMOND R 'B-22943
HARA H *B-19486
HASEGAWA H 1-24160
HASHIMOTO S B-23264
HAYASHI, M 'C-03035
HEILINGOETTER R 'C-24970
HENSINGER, C E 'B-09559
HERZOG G *B-14660
HISHINUMA Y B-20777
HOEGSTROEM, U 'E-10751
HONTI G 'F-22098
HSUEH L B-26254
HULL W Q 'F-14506
IRELAND F E
IRELAND, F E
'A-23044
•A-12633
J
JACKSON A B-19469
JAGER L B-17810
JEPHSON A C A-13596
JUTZE, G A C-00482
K
KANGUN I 'C-17700
KAPUSTINKSY A F 'F-14641
KAPUSTINSKTY A F *F-14653
KATZ M 'E-21791
KERRIGAN, J V 'C-01387, *D-05152
KIMURA M B-23264
KLIMECEK R B-17810, B-25491
KOHEN, E S 'C-03852
KORNEYCHUK G P F-16377
KOSHI, S C-03035
KOSINKSI K C-20595
KOSSOVSKII, E O 'B-04067
KOTO K *B-15846
KOZHEVNIKOVA N V 'F-16292
KRAUSE, F E F-04626
KROUSE, M B-05079
KUNIN T I B-19856, F-14526
KURKER, C JR B-07552
KUZNETSOV I E B-19370
KUZNETSOV I Y A-13403
LARRAT P *C-21415
LASIEWICZ K 'F-21068
LASTOCHKIN Y V 'B-16291
LEHLE W W 'B-13667
LEIKIN L I B-19370
LEITHE, W 'B-07535
LESOKHIN I G B-16291
LEWIS W K 'A-13841,'F-13802
LEYKIN L I A-13403
LINDAU L 'A-18305
LOUISE J C-21415
LUNGE, G *F-10907
M
MAEDA S '1-24160
MANAKIN B A F-14625
MANAKIN, G A B-08181
MANDERSON, M L-10998
MANDERSON, M C 'L-11242
MAYDUROVA O V B-23070
-------
50
SULFURIC ACID MANUFACTURING
MAZIARKA S C-20595
MCADIE H G C-22645, C-25445
MEINHOLD, T F *B-03945
MISIAKIEWICZ Z C-20595
MISYUK E G F-14625
MOELLER, W *B-09126
MONKMAN J L C-15745
MONTI D R J-21308
MORASH, N *B-05079
MOROZOVA Z I F-15325, F-15416
MUKHLENOV I P B-16289, B-16290,
B-16291, B-20024
N
NAGIBIN V D *B-23939
NAKAZONO T 'B-25742
NASH T "C-25851
NEGHERBON, W O 'F-00530
NEUMANN V F-22154
NILSSON F 'B-25275
O
O KEEFFE A E *C-12596
DELS H *J-17203
OLEINIKOVA, N K C-09295
OLEVINSKIY M I B-14568
ORLOVA L M F-14539
OSMUL KEVICH V A B-24256
OVCHINNIKOVA E N F-13940
OVCHINNIKOVA Y N 'F-13652
PATTON W F "C-23771
PECHKOVSKIY V V *F-13875
PERRINE R L 'B-26254
PETERSSON S *B-24451
PETROVSKIY V A B-24256
PIATTIL A-23972
PLIGUNOV V P F-14538
PODMOLIK J B-13206
POL YAK, V E *D-11492
POPOVICI N *B-15739
POPPELE E W B-24833
POSTINIKOV V F *B-19856
POSTNIKOV V F *F-14526
POTOP P B-15739
PREBLE B B-21309
PUDLISZAK DZIEWANOWSKA A
F-21068
PUTNAM, B *L-10998
QUITTER V *B-25370
R
RAUSCHER J A B-26095
REHME, K A C-09033, C-11089
REMIREZR 'B-16718
RIES E D A-13841, F-13802
RMMER L G B-16480
ROESNER G *B-17889
ROLLKH *B-19033
ROMOVACEKJ 'B-21703
ROSENDAHL F *B-24594
ROYTER V A F-16377
RUDLING B B-25275
RUMYANTSEVA Y S B-16291
RYABCHENKO A I F-14539
RZAYEV P B *F-16377
S
SAFIULLIN N S *B-14568
SAKABE, H C-03035
SCARINGELLI, F P *C-00482, *C-09033,
*C-11089
SCHEIDEL, C F *B-11250
SCHON F F-14506
SCHWARTZ I "J-21206
SEMRAU K T J-21308
SHLIFER V A A-13403, B-19370
SIEDLEWSKIJ *B-13880
SILVERMAN L B-24110
SILVERMAN, L *B-05567, B-07552
SKRIVANEK J *B-25768
SMIRNOV V I F-14626
SMYSLOV N I *B-14386
SNAJBERK, K C-01387, D-05152
SNOWBALL A F *B-22055
SNOWBALL, A F *A-04946
SORDELLI, D *B-01125
SRBEK J *B-17810
SRYVALIN I T F-14626
STAROSEL SKII, Y I B-08181
STASTNY, E P *B-00800
STEINKE I *C-14735
STOPPERKA K *F-22154
STOPPERKA, K 'B-02985
STREICHER J S *F-14845
STRUSINSKY A C-20595
STUBER P J B-25133
SUCHKOV A B 'F-15325, *F-15416
SYKES W 'B-25643
TAKAHASHI A *C-21056
TAKEUCfflT *B-19592
TAMM O M *B-16447
TAMURA Z *B-20777
TANAKA T B-19592
TAYLOR HD *C-19384
TEICHMAN T C-15745
TESKE, W *B-11058
TEWORTE W M *A-25178
THOMAS R S C-15745
THOMPSON A P 'A-13850
TOYAMA, T *L-05407
TRABER D G B-16289, B-16290, B-20024,
F-16292
TSUDO K *B-19644
UBL, Z "C-09983
UHI K *C-14486
u
V
VARLAMOV, M L *B-08181
VASIL EVA E M B-16447
VOLKOVA E I B-16480
VOSSELLER, W P B-05079
W
WAKEFIELD, R E B-09559
WATANABE H 1-24160
WEISSENBERGER G *A-23972
WESOLOWSKIJ F-21068
WILSON, H N *C-09369
WINKLER, K B-09126
WOHLERS, H C *N-04845
WOLFGANG, H *B-11906
WOOLLAM J P V *B-19469
WRIGHT G A 'L-25520
WYSZYNSKAH *C-20595
YASHKE YE V *B-24256
YESELEV I M *B-16289, *B-16290,
*B-20024
YORK 0 H *B-24833
ZANON, D B-01125
ZIRNGIBL H F-14506
ZWILLINGJP *B-11629
-------
SUBJECT INDEX
51
ABATEMENT A-21221, B-11906, L-25520
ABSORPTION A-02235, A-13403, A-18305,
A-25178, B-00587, B-01125, B-03945,
B-07535, B-07J52, B-08181, B-09126,
B-09913, B-11235, B-13667, B-14568,
B-16718, B-17889, B-19370, B-19383,
B-19593, B-22055, B-24110, B-24833,
B-25133, C-09633, E-21791, F-00530,
F-10907, F-13940, J-17203, L-24033
ABSORPTION (GENERAL) A-12751,
A-12823, A-23972, A-25605, B-07535,
B-09913, B-11250, B-11629, B-11906,
B-13206, B-13672, B-14030, B-15739,
B-15879, B-15991, B-17053, B-17810,
B-17889, B-19228, B-19469, B-19592,
B-19606, B-19644, B-19856, B-19886,
B-20670, B-21824, B-24103, B-24451,
B-24594, B-24628, B-24673, B-24695,
B-25275, B-25468, B-25742, B-25768,
F-13652, 1-24160, J-17203, L-24033
ACETONE C-22645
ACETYLENES B-03129, B-07925
ACID SMUTS A-23044, B-21824, B-24833,
C-24970
ACIDS A-02235, A-04946, A-10749,
A-12633, A-12751, A-12823, A-13403,
A-13596, A-13841, A-13850, A-15517,
A-18305, A-21221, A-23044, A-25178,
A-25605, B-00587, B-00800, B-01125,
B-02355, B-02985, B-03129, B-03945,
B-04067, B-05079, B-05514, B-05567,
B-06247, B-06282, B-07535, B-07552,
B-07925, B-08181, B-09126, B-09559,
B-09913, B-11058, B-11146, B-11235,
B-11238, B-11250, B-11629, B-11906,
B-13206, B-13337, B-13667, B-13672,
B-13728, B-13806, B-13880, B-14030,
B-14386, B-14533, B-14568, B-15739,
B-15846, B-15879, B-15991, B-16289,
B-16290, B-16291, B-16447, B-16480,
B-16718, B-17053, B-17810, B-17887,
B-17889, B-19033, B-19228, B-19370,
B-19383, B-19486, B-19592, B-19593,
B-19594, B-19595, B-19606, B-19644,
B-19682, B-19856, B-19943, B-20024,
B-20248, B-20416, B-20670, B-20777,
B-21309, B-21703, B-21824, B-22055,
B-22182, B-22943, B-23048, B-23070,
B-23264, B-23556, B-23939, B-24103,
B-24110, B-24246, B-24256, B-24451,
B-24594, B-24628, B-24673, B-24695,
B-24833, B-25133, B-25275, B-25370,
B-25468, B-25491, B-25643, B-25717,
B-25742, B-25768, B-26095, B-26254,
C-00040, C-00381, C-00482, C-01387,
C-01819, C-03035, C-03852, C-09033,
C-09295, C-09369, C-09633, C-09983,
C-11089, C-11140, C-12596, C-14486,
C-14735, C-15745, C-19384, C-20595,
C-21056, C-21415, C-22645, C-23771,
C-24970, C-25445, C-25851, D-05152,
D-11492, E-I0751, E-21791. F-00530,
F-04626, F-10907, F-13652, F-13802,
F-13875, F-13940, F-14249, F-14506,
F-14625, F-14626, F-14641, F-14653,
F-14845, F-14871, F-15325, F-15416,
F-16292, F-16377, F-20274, F-21068,
F-22098, F-22154, G-11379, G-16774,
G-17623, G-22594, G-23930, 1-20820,
1-24160, J-11791, J-17203, J-21206,
J-21308, J-22397, K-06349, K-19750,
L-05407, L-10998, L-11242, L-24033,
L-25520, N-04845
ACROLEIN C-09369
ACUTE 1-20820
ADMINISTRATION A-04946, B-03129,
B-20248, C-01819, L-05407
ADSORPTION A-13403, B-01125, B-13880,
B-14533, B-15846, B-19593, B-22182,
C-03852, F-13940, J-21206
ADSORPTION (GENERAL) B-14660,
B-20777, B-21824, B-22182, F-13652
AEROSOL GENERATORS C-00482
AEROSOLS B-05079, B-05567, B-06282,
B-14568, B-24110, C-00040, C-00381,
C-00482, C-01819, C-09033, C-09633,
C-09983, C-11089, C-22645, C-25445,
E-21791, F-00530, G-11379, G-16774,
G-17623, G-22594, N-04845
AFRICA F-00530, L-11242
AFTERBURNERS B-07535, B-07925,
B-23070, J-21206
AIR POLLUTION EPISODES F-00530,
G-16774
AIR QUALITY CRITERIA G-16774
AIR QUALITY MEASUREMENT
PROGRAMS C-01819
AIR QUALITY MEASUREMENTS
A-04946, C-00040, C-01819, C-20595,
D-05152, D-11492, F-00530, G-16774,
L-05407, N-04845
AIR QUALITY STANDARDS B-03129,
D-11492, G-11379, K-06349, K-19750
ALCOHOLS B-24594, C-09369, C-09983,
C-22645
ALDEHYDES C-09369, C-09983, E-21791
ALIPHATIC HYDROCARBONS B-03129,
B-07925, C-09369, C-12596
ALKALINE ADDITIVES A-12751,
A-12823, A-13403, A-23044, A-25605,
B-14660, B-20248, B-24594, B-25491,
F-00530, L-24033
ALKALIZED ALUMINA (ADSORPTION)
F-00530
ALLERGIES F-00530
ALTITUDE E-10751, E-21791, N-04845
ALUMINUM B-03129, B-07925, B-20248,
B-25643
ALUMINUM COMPOUNDS A-25178,
B-07925, B-20248, B-23070, B-24110,
F-16377
ALUMINUM OXIDES B-20248, B-23070,
F-14539
ALVEOLI F-00530
AMIDES B-24594
AMINES B-01125, B-15879, B-15991
AMMONIA A-18305, B-13667, B-15739,
B-19370, B-24594, C-09369, C-09983,
C-24970
AMMONIUM CHLORIDE C-23771
AMMONIUM COMPOUNDS A-04946,
A-18305, B-07552, B-13667, B-15739,
B-17889, B-19370, B-19383, B-19592,
B-19606, B-24110, B-24594, C-09033,
C-09369, C-09983, C-23771, C-24970,
1-24160, J-21308
ANALYTICAL METHODS B-02355,
B-19594, B-19595, B-20248, C-00040,
C-00381, C-00482, C-03852, C-09033,
C-09295, C-09369, C-09633, C-09983,
C-11089, C-11140, C-12596, C-14486,
C-14735, C-15745, C-17700, C-19384,
C-20595, C-21415, C-24970, C-25445,
C-25851, D-05152, F-00530, F-16292,
G-11379, 1-20820, K-06349
ANIMALS C-00381, F-00530, G-11379,
G-16774, G-17623, G-23930, 1-20820
ANNUAL K-19750
AROMATIC HYDROCARBONS B-07925,
B-11058, B-15879, B-15991, C-09983,
C-20595
ARSENIC COMPOUNDS B-11238, C-09983
ASBESTOS B-26254
ASHES B-07535, B-07925
ASIA B-15846, B-19486, B-19592, B-19644,
B-20416, B-20777, B-23264, B-24673,
B-25742, C-03035, C-14486, C-21056,
F-00530, 1-24160, L-05407, L-11242
ASTHMA F-00530
ATMOSPHERIC MOVEMENTS A-04946,
C-01387, D-11492, E-10751
AUTOMATIC METHODS C-01819,
C-25445
AUTOMOBILES B-07535
AUTOMOTIVE EMISSIONS B-07535,
C-00381, C-09369, C-09633, F-00530
AZO DYE C-09295
B
BAG FILTERS A-10749, A-25605, B-07925,
B-23556
BARIUM COMPOUNDS B-23070, C-11140,
F-16377
BASIC OXYGEN FURNACES B-07925,
B-26254
BENZENES B-07925, C-20595
BERYLLIOSIS B-00587, B-00800, B-02355,
C-00381, C-00482, C-01387, C-01819,
C-03035, C-03852
BERYLLIUM K-06349
BERYLLIUM COMPOUNDS K-06349,
K-19750
BIOCLIMATOLOGY F-00530
BIOMEDICAL TECHNIQUES AND
MEASUREMENT B-04067, F-00530,
G-11379
BLAST FURNACES A-10749, B-23939,
B-25643
BLOOD CELLS G-11379
BODY CONSTITUENTS AND PARTS
F-00530, G-11379, L-05407
BODY FLUIDS G-11379
BODY PROCESSES AND FUNCTIONS
F-00530, G-11379
-------
52
SULRJRIC ACID MANUFACTURING
BOILERS B-07535, B-07925, B-19469,
B-19886, B-20777, B-25468, B-25643,
F-20274
BORON COMPOUNDS C-09369
BREATHING G-11379
BRONCHITIS F-00530, G-11379
BRONCHOCONSTRICTION G-16774
BUBBLE TOWERS B-07925, B-15991
BUDGETS B-20248
BUILDINGS E-10751
BUTANES C-09369
BY-PRODUCT RECOVERY A-12751,
A-12823, A-13850, A-18305, A-23972,
A-25178, B-09559, B-09913, B-11146,
B-11238, B-11250, B-11629, B-11906,
B-13337, B-13672, B-13728, B-14030,
B-14533, B-15739, B-17053, B-17810,
B-17887, B-19370, B-19383, B-19469,
B-19592, B-19595, B-19886, B-20416,
B-20670, B-20777, B-21309, B-22055,
B-23048, B-23939, B-24103, B-24246,
B-24451, B-24594, B-24628, B-24673,
B-25133, B-25275, B-25491, F-14871,
1-24160, J-11791, J-17203, J-21206,
J-21308, J-22397, L-10998, L-11242,
L-24033
CADMIUM COMPOUNDS A-13596
CALCIUM COMPOUNDS B-11058,
B-19644, B-23048, B-25742, C-24970,
F-14506
CALCIUM SULFATES B-19644, B-23048,
F-14506
CALIBRATION METHODS C-00381,
C-00482, C-03852, C-25851
CALIFORNIA B-07535, C-0%33, D-05152
CANADA A-04946, B-19606, B-22055,
C-00381, C-00482, C-01819, C-03035,
C-15745, C-22645, C-25445, E-21791,
F-00530, F-14249, L-11242
CARBIDES B-11058
CARBON DIOXIDE B-11235, C-09369,
C-24970, C-25851
CARBON DISULFIDE B-07925, B-23070,
C-09983, C-20595
CARBON MONOXIDE B-24594, C-09369,
C-09983, C-12596, J-21206, K-06349,
K-19750
CARBONATES B-15879, B-20248, B-25768
CARBONYLS C-09369
CARCINOGENS B-01125, C-00381,
C-01387, C-01819, C-03852, F-00530
CASCADE SAMPLERS C-03035, C-09633,
C-23771
CATALYSIS A-13850, A-23972, B-01125,
B-09126, B-16289, B-16290, B-16291,
B-16480, B-16718, B-17887, B-19486,
B-20024, B-22055, B-23070, C-11089,
F-04626, F-13802, F-14249, F-14526,
F-14539, F-14845, F-16292, F-16377,
F-21068
CATALYSTS A-13850, A-23972, B-09126,
B-16289, B-16290, B-16291, B-17887,
B-20024, B-23070, F-04626, F-14249,
F-14845, F-21068
CATALYTIC ACTIVITY B-16480, B-19486,
B-20024, C-11089, F-04626, F-13802,
F-14526, F-14539, F-16292, F-16377,
F-21068
CATALYTIC AFTERBURNERS B-07535,
B-07925, B-23070
CATALYTIC OXIDATION A-13841,
B-01125, B-09913, B-11629, B-13206,
B-13672, B-13806, B-13880, B-14030,
B-16289, B-16290, B-16291, B-16480,
B-17887, B-19228, B-19486, B-19886,
B-19943, B-20024, B-20670, B-24103,
B-24628, C-09033, F-13652, F-13802,
F-13940, F-14249, F-14526, F-14538,
F-14539, F-14625, F-14641, F-14653,
F-16292, F-16377, F-20274, F-21068,
J-21206
CELLS F-00530, G-11379, G-23930
CEMENTS A-21221, B-07535, B-25643,
F-14506, J-17203
CENTRIFUGAL SEPARATORS A-13596,
B-04067, B-17889, C-23771, J-21206
CERAMICS B-07925
CHAMBER PROCESSING A-02235,
B-07925, B-11906, B-14533, B-14568,
B-25643, C-00040, C-17700
CHARCOAL B-11250, B-13880, B-14533,
B-15846, B-19592, F-00530, F-13652,
F-13940
CHEMICAL COMPOSITION A-04946,
C-00040, C-20595
CHEMICAL METHODS C-00040, C-09033,
C-09633, C-09983, C-12596, C-14735,
C-15745, C-17700, C-20595, C-21415,
C-24970, D-05152, G-11379
CHEMICAL PROCESSING A-02235,
A-04946, A-10749, A-12633, A-13403,
A-13841, A-13850, A-15517, A-18305,
A-21221, A-23044, A-23972, B-00587,
B-00800, B-01125, B-02355, B-02985,
B-03129, B-03945, B-04067, B-05079,
B-06247, B-06282, B-07535, B-07925,
B-08181, B-09126, B-11058, B-11235,
B-11238, B-11250, B-11906, B-13206,
B-13667, B-13672, B-13728, B-13806,
B-14030, B-14386, B-14533, B-14568,
B-14660, B-15846, B-16289, B-16290,
B-16291, B-16447, B-16718, B-17053,
B-17810, B-19033, B-19370, B-19383,
B-19469, B-19486, B-19593, B-19595,
B-19644, B-19682, B-19856, B-19886,
B-20248, B-20416, B-20670, B-21824,
B-22055, B-22943, B-23556, B-23939,
B-24246, B-24673, B-24695, B-24833,
B-25133, B-25370, B-25468, B-25643,
B-26254, C-00040, C-01387, C-03852,
C-09295, C-17700, C-23771, D-05152,
D-11492, E-10751, F-13802, F-14249,
F-14506, F-14526, F-14538, F-14539,
F-14641, F-14653, F-22098, 1-20820,
1-24160, J-11791, J-17203, J-21206,
L-05407, L-10998, L-11242, L-24033,
L-25520
CHEMICAL REACTIONS A-02235,
A-10749, A-12751, A-12823, B-01125,
B-09126, B-11906, B-15739, B-19886,
B-23556, B-24673, C-09033, C-0%33,
E-21791, F-04626, F-10907, F-13875,
F-14506, F-15325, F-15416
CHLORIDES B-11238, C-09369, L-24033
CHLORINE A-18305, B-01125, B-03129,
C-09369, C-09983, C-24970, L-24033
CHLORINE COMPOUNDS B-00587,
B-11238, B-21703, C-09369, C-20595,
L-24033
CHROMATOGRAPHY B-19595, C-12596
CHROMIUM COMPOUNDS F-14539
CHROMIUM OXIDES F-14526
CHRONIC F-00530, G-11379, 1-20820,
N-04845
CILIA F-00530
CINDERS B-06282
CIRCULATORY SYSTEM G-11379
CLEAN AIR ACT B-07925, F-00530
COAL A-12633, A-23044, B-07535,
B-07925, B-11250, F-00530, 1-20820,
J-11791, L-10998
COAL PREPARATION A-15517, B-15846,
B-20248, J-11791, L-10998
COBALT COMPOUNDS F-14626
COFFEE-MAKING B-26254
COKE A-23044, B-07925, B-22055,
B-22182, F-00530
COLLECTORS A-13596, A-25605, B-00587,
B-00800, B-04067, B-17889, B-19886,
B-20777, B-22943, C-09033, C-23771,
J-21206, L-05407
COLORIMETRY C-00040, C-00381,
C-03852, C-09033, C-09295, C-09983,
C-11089, C-14735, C-20595, C-25445,
C-25851, D-05152, 1-20820
COMBUSTION A-23044, B-09126
COMBUSTION AIR A-10749, B-23939
COMBUSTION GASES A-04946, A-12751,
A-12823, A-15517, A-23044, A-23972,
A-25605, B-00800, B-01125, B-03945,
B-05567, B-07925, B-11058, B-11250,
B-11629, B-11906, B-13337, B-13672,
B-14568, B-14660, B-15739, B-15879,
B-15991, B-16718, B-17053, B-19033,
B-19228, B-19370, B-19469, B-19592,
B-19606, B-19644, B-19856, B-19886,
B-19943, B-20777, B-21309, B-21824,
B-22943, B-23070, B-23264, B-23939,
B-24103, B-24110, B-24246, B-24451,
B-24594, B-24628, B-24673, B-24833,
B-25133, B-25275, B-25491, B-25742,
B-25768, C-11140, C-14735, C-17700,
E-10751, F-20274, 1-20820, J-21206,
J-22397, L-10998, L-24033, N-04845
COMBUSTION PRODUCTS A-04946,
A-12751, A-12823, A-15517, A-23044,
A-23972, A-25605, B-00800, B-01125,
B-03945, B-05567, B-06282, B-07535,
B-07925, B-11058, B-11250, B-11629,
B-11906, B-13337, B-13672, B-14568,
B-14660, B-15739, B-15879, B-15991,
B-16718, B-17053, B-19033, B-19228,
B-19370, B-19469, B-19592, B-19606,
B-19644, B-19856, B-19886, B-19943,
B-20777, B-21309, B-21824, B-22943,
B-23070, B-23264, B-23939, B-24103,
B-24110, B-24246, B-24451, B-24594,
B-24628, B-24673, B-24833, B-25133,
B-25275, B-25491, B-25742, B-25768,
C-11140, C-14735, C-17700, E-10751,
F-20274, 1-20820, J-21206, J-22397,
L-10998, L-24033, N-04845
COMMERCIAL AREAS K-06349
COMMERCIAL EQUIPMENT B-01125
COMMERCIAL FIRMS L-24033
COMPRESSED GASES B-00587
COMPUTER PROGRAMS F-22098
CONDENSATION B-19606, B-19682,
B-24110, C-19384
CONDENSATION (ATMOSPHERIC)
D-05152
CONSTRUCTION MATERIALS A-21221,
B-07535, B-25643, F-14506, J-17203
CONTACT PROCESSING A-02235,
A-10749, A-12633, A-13841, A-18305,
A-23972, B-07925, B-09126, B-11058,
B-11906, B-13667, B-13728, B-13806,
B-14386, B-14660, B-16289, B-16290,
B-16291, B-16718, B-19469, B-19486,
B-19682, B-19856, B-19886, B-21824,
B-22055, B-24695, B-25133, B-25643,
C-00040, C-09295, F-14249, F-14526,
F-14538, F-14539, F-14653, L-24033
CONTINUOUS AIR MONITORING
PROGRAM (CAMP) C-01819
-------
SUBJECT INDEX
53
CONTINUOUS MONITORING B-07925,
B-20248, C-01819, C-125%, C-21056,
C-21415, C-25851, D-05152, G-11379
CONTROL EQUIPMENT A-02235,
A-04946, A-10749, A-12751, A-12823,
A-I3403, A-13596, A-23044, A-25605,
B-00587, B-00800, B-01125, B-02355,
B-02985, B-03129, B-03945, B-04067,
B-05079, B-05514, B-05567, B-06247,
B-07535, B-07552, B-07925, B-08181,
B-09559, B-11058, B-11235, B-11238,
B-11629, B-13337, B-13667, B-14568,
B-15879, B-15991, B-17889, B-19033,
B-19383, B-19469, B-19644, B-1%82,
B-19886, B-20248, B-20777, B-22055,
B-22943, B-23070, B-23264, B-23556,
B-23939, B-24110, B-24256, B-24594,
B-24673, B-24695, B-24833, B-25370,
B-25643, B-25717, B-25768, B-26095,
B-26254, C-00040, C-01387, C-09033,
C-11089, C-22645, C-23771, C-25851,
D-05152, F-00530, J-17203, J-21206,
L-05407, L-24033
CONTROL METHODS A-02235, A-04946,
A-10749, A-12751, A-12823, A-13403,
A-13841, A-13850, A-15517, A-18305,
A-23044, A-23972, A-25178, A-25605,
B-00587, B-00800, B-01125, B-02355,
B-02985, B-03129, B-03945, B-04067,
B-06282, B-07535, B-07552, B-07925,
B-08181, B-09126, B-09559, B-09913,
B-11058, B-11146, B-11235, B-11238,
B-11250, B-11629, B-11906, B-13206,
B-13337, B-13667, B-13672, B-13728,
B-13806, B-13880, B-14030, B-14386,
B-14533, B-14568, B-14660, B-15739,
B-15846, B-15879, B-15991, B-16289,
B-16290, B-16291, B-16447, B-16480,
B-16718, B-17053, B-17810, B-17887,
B-17889, B-19033, B-19228, B-19370,
B-19383, B-19469, B-19486, B-19592,
B-19593, B-19595, B-19606, B-19644,
B-19856, B-19886, B-19943, B-20024,
B-20248, B-20416, B-20670, B-20777,
B-21309, B-21703, B-21824, B-22055,
B-22182, B-22943, B-23048, B-23070,
B-23264, B-23939, B-24103, B-24110,
B-24246, B-24451, B-24594, B-24628,
B-24673, B-24695, B-24833, B-25133,
B-25275, B-25468, B-25491, B-25643,
B-25717, B-25742, B-25768, B-26254,
C-03852, C-09033, C-09633, E-21791,
F-00530, F-10907, F-13652, F-13802,
F-13940, F-14249, F-14526, F-14538,
F-14539, F-14625, F-14641, F-14653,
F-14871, F-16292, F-16377, F-20274,
F-21068, 1-24160, J-11791, J-17203,
J-21206, J-21308, J-22397, L-05407,
L-10998, L-11242, L-24033
CONTROL PROGRAMS A-04946, B-03129,
B-20248, L-05407
CONTROLLED ATMOSPHERES C-00381
COOLING B-19606, B-22055
COPPER B-07925, B-11146, B-11906,
B-21309, B-23939, B-25275, C-09033,
C-11089
COPPER COMPOUNDS A-12751, A-12823,
B-07925, C-09033, C-11089, F-14626
CORONA B-05514, B-23264
CORROSION B-00800, B-02985, B-03945,
B-22055, C-03035, 1-20820, I-24I60,
N-04845
COSTS A-12751, A-12823, A-13850,
A-15517, A-18305, A-2122I, A-25178,
B-01125, B-05079, B-05514, B-07552,
B-11238, B-11250, B-16718, B-17053,
B-21309, B-21824, B-23048, B-23556,
B-25133, F-14845, J-11791, J-17203,
J-21206, J-21308, L-10998
CRACKING 1-20820
CRITERIA A-12823, G-16774
CRYSTAL STRUCTURE F-14653
CUPOLAS B-07925
CYANIDES C-09369
CZECHOSLOVAKIA B-13206, B-17810,
B-21703, B-25491, B-25768, C-00381,
C-00482, C-01387, C-03852, C-09983,
F-00530
D
DATA ANALYSIS C-01387
DATA HANDLING SYSTEMS C-01387,
F-22098
DECOMPOSITION B-15739, B-23556,
C-09033, F-14506, F-15325, F-15416
DELAWARE B-02985
DENSITY B-24256, B-24673, C-21056
DESIGN CRITERIA A-10749, A-25605,
B-00800, B-07925, B-11146, B-11238,
B-13337, B-17053, B-17887, B-19606,
B-19644, B-20777, B-21703, B-21824,
B-24695, B-25370, B-25643, B-25717,
B-26095, C-25851, F-14249
DESULFURIZATION OF FUELS A-15517,
A-23044, B-15846, B-20248, B-21703,
F-00530, J-11791, L-10998
DIFFUSION C-15745, E-10751
DIFFUSION MODELS E-10751
DIGESTIVE SYSTEM G-11379, G-23930
DIOLEFINS B-07925
DISCOLORATION 1-20820
DISPERSION A-15517, B-01125, C-15745,
D-11492, E-10751, F-00530
DISSOCIATION E-21791, F-13875, F-14506
DIURNAL G-11379, K-19750
DOMESTIC HEATING B-07535, F-00530
DONORA F-00530
DROPLETS B-24110, C-00381, C-09633
DRYING B-25491
DUST FALL A-04946, F-00530, L-05407
DUSTS B-04067, B-05079, B-06282,
B-07535, B-07925, B-11058, B-11906,
B-17889, B-20777, B-22943, B-24110,
B-25643, B-26254, C-09983, C-20595,
C-23771, J-17203, L-05407
ECONOMIC LOSSES J-11791, J-17203,
J-22397
ELECTRIC CHARGE B-05514, B-25468
ELECTRIC FURNACES B-07925
ELECTRIC POWER PRODUCTION
A-15517, A-21221, A-23044, B-07925,
B-11238, B-11250, B-11906, B-14660,
B-24673, E-10751, J-17203, L-10998,
L-11242, L-24033
ELECTRICAL MEASUREMENT DEVICES
C-00381, G-22594
ELECTRICAL PROPERTIES B-05514,
B-23264, B-25468, B-25643
ELECTROCHEMICAL METHODS
C-09983, C-12596, C-14735, C-15745,
C-21415, G-11379
ELECTROCONDUCnvrTY ANALYZERS
C-01819, C-125%, C-21056, C-25851,
D-05152
ELECTROLYSIS B-25491
ELECTROSTATIC PRECIPITATORS
A-10749, A-13596, A-25605, B-00587,
B-00800, B-02985, B-05514, B-07535,
B-07925, B-09559, B-11235, B-11238,
B-17889, B-19033, B-19886, B-20248,
B-22943, B-23264, B-23939, B-24256,
B-25370, B-25643, C-00040, C-01387,
D-05152, J-21206, L-24033
EMISSION STANDARDS B-03129,
B-16718, L-25520
EMISSIVTTY F-00530
EMPHYSEMA G-11379
ENGINE EXHAUSTS B-07535, C-00381,
C-09369, C-09633, F-00530
ENZYMES F-00530, G-11379
EPIDEMIOLOGY F-00530
ESTERS B-05079, B-25742
ETHYLENE B-07925
EUROPE A-02235, A-13403, A-18305,
A-23972, A-25178, B-00587, B-00800,
B-02985, B-03129, B-03945, B-04067,
B-07535, B-07925, B-08181, B-09126,
B-09913, B-11058, B-11629, B-11906,
B-13206, B-13337, B-13728, B-13880,
B-14030, B-14386, B-14568, B-14660,
B-15739, B-16289, B-16290, B-16291,
B-16447, B-16480, B-17810, B-17887,
B-17889, B-19228, B-19469, B-1%82,
B-19856, B-19943, B-20024, B-20670,
B-21703, B-22182, B-23070, B-23939,
B-24256, B-24451, B-24594, B-24628,
B-24695, B-25275, B-25370, B-25468,
B-25491, B-25643, B-25768, C-00381,
C-00482, C-01387, C-03852, C-09295,
C-09983, C-14735, C-17700, C-19384,
C-20595, C-21415, C-24970, C-25851,
E-10751, F-00530, F-04626, F-10907,
F-13652, F-13875, F-13940, F-14526,
F-14538, F-14539, F-14625, F-14626,
F-14641, F-14653, F-14871, F-15325,
F-15416, F-16292, F-16377, F-21068,
F-22098, F-22154, G-11379, G-17623,
G-22594, J-17203, L-11242, L-24033
EXHAUST SYSTEMS A-135%, B-04067,
B-22055
EXPERIMENTAL EQUIPMENT B-05079
EXPERIMENTAL METHODS C-01387,
C-09983
EXPOSURE CHAMBERS C-00381,
G-16774
EYE IRRITATION E-21791, 1-20820
EYES 1-20820
FALLOUT C-01387
FANS (BLOWERS) A-13596, B-04067,
B-22055
FARMS F-00530, K-06349
FEASIBILITY STUDIES A-21221, L-10998
FEDERAL GOVERNMENTS B-07925
FERTILIZER MANUFACTURING
A-21221, B-15739, F-14871, J-21206
FERTILIZING A-04946, B-03129, B-11058,
L-11242
FIELD TESTS C-03852
FILTER FABRICS B-05567, B-20248,
B-24110, B-24256, B-24695, B-25717,
B-26095, B-26254, C-09033, C-11089,
C-22645
FILTERS A-10749, A-13403, A-25605,
B-05079, B-05567, B-06247, B-07552,
B-07925, B-13667, B-14568, B-19682,
B-20248, B-22943, B-23556, B-24110,
B-24256, B-24695, B-25717, B-26095,
B-26254, C-09033, C-11089, C-22645,
C-23771, D-05152, J-17203, J-21206
FIRING METHODS A-10749, B-07925,
B-23939
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54
SULFURIC ACID MANUFACTURING
FLAME AFTERBURNERS B-07925
FLAME IONIZATION DETECTOR
C-12596
FLARES B-07925
FLOW RATES A-12751, A-25605, B-00587,
B-05079, B-05514, B-08181, B-23070,
B-23264, B-24110, B-24256, B-25768,
C-00381, C-00482
FLUID FLOW A-12751, A-25605, B-00587,
B-05079, B-05514, B-08181, B-23070,
B-23264, B-24110, B-24256, B-25768,
C-00381, C-00482
FLUORESCENCE C-11140, C-12596
FLUORIDES B-01125, B-07552, B-11058,
B-11238, B-26254, K-06349
FLUORINE A-18305, B-03129, C-09369,
C-09983, C-24970, K-06349, L-24033
FLUORINE COMPOUNDS A-25178,
B-01125, B-07552, B-07925, B-11058,
B-11238, B-26254, C-09369, C-20595,
K-06349
FLY ASH B-05567, B-07552, B-07925,
B-19606, B-25643, F-00530, G-23930
FOG D-05152
FOOD AND FEED OPERATIONS B-26254
FORESTS F-00530
FORMALDEHYDES C-09369, C-09983
FORMIC ACID B-25742
FRANCE B-09913, B-11629, B-13728,
B-14030, C-21415
FREE RADICALS E-21791
FUEL GASES B-07925, B-11629, B-19886
FUEL OILS A-12633, A-23044, B-07925,
B-11250, F-00530
FUELS A-12633, A-15517, A-23044,
B-07535, B-07925, B-11250, B-11629,
B-19886, B-22055, B-22182, F-00530,
1-20820, J-11791, L-10998
FUMES A-25605, B-01125, B-03129,
B-07552, B-07925, B-19383, B-21824
FUMIGATION F-00530
FURNACES A-10749, A-23044, B-05567,
B-06282, B-07535, B-07925, B-19606,
B-19886, B-23939, B-25643, B-26254
G
GAS CHROMATOGRAPHY C-12596
GAS SAMPLING B-20248, C-24970
GASES A-04946, B-00587, B-00800,
B-03945, B-05514, B-09913, B-11238,
B-15879, B-15991, B-19682, B-22182,
B-24110, B-25768, C-09633
GASIFICATION (SYNTHESIS) B-15846
GASOLINES F-00530
GERMANY A-23972, A-25178, B-02985,
B-07535, B-09126, B-11058, B-11906,
B-13337, B-14660, B-17889, B-19228,
B-20670, B-22182, B-24594, B-24628,
B-25370, C-03852, C-14735, C-24970,
F-00530, F-10907, F-22154, J-17203
GLASS FABRICS B-24110, B-24256,
B-25717, B-26095, B-26254, C-09033,
C-11089, C-22645
GOVERNMENTS B-07925, K-06349,
K-19750, L-24033
GRAVITY SETTLING B-25717
GREAT BRITAIN B-07535, B-07925,
B-13337, B-19469, B-24695, B-25643,
C-19384, C-25851, E-10751, F-14871,
L-24033
GROUND LEVEL E-10751
GUINEA PIGS G-17623, G-23930, 1-20820
H
HALOGEN GASES A-18305, B-01125,
B-03129, C-09369, C-09633, C-09983,
C-24970, K-06349, L-24033
HEALTH IMPAIRMENT B-04067, F-00530,
L-05407, N-04845
HEALTH STATISTICS F-00530
HEART G-11379
HEAT CAPACITY F-00530
HEAT TRANSFER B-19606, B-22055,
B-24103, B-24628, C-09033
HEMATOLOGY F-00530
HI-VOL SAMPLERS C-01819, C-09033,
C-11089, C-15745
HOURLY K-19750
HUMANS F-00530, G-16774, G-22594,
1-20820
HUMIDITY C-00482, C-09633, D-05152,
D-11492, E-21791, G-16774
HYDROCARBONS B-00587, B-03129,
B-07925, B-11058, B-11235, B-15879,
B-15991, C-09369, C-09983, C-12596,
C-20595, E-21791, J-21206
HYDROCHLORIC ACID A-18305, B-07552,
B-11058, B-22943, B-26254, C-03035,
C-14486, C-24970, F-20274, L-24033
HYDROFLUORIC ACID B-01125, B-05567,
B-07552, B-11058, B-22943, B-24110,
B-26254, C-24970, K-19750, L-24033
HYDROGEN C-00381, C-21415, C-25851
HYDROGEN SULFIDE B-00800, B-07925,
B-11058, B-11629, B-14030, B-17889,
B-19033, B-19886, B-22943, B-23048,
B-23070, B-24594, B-26254, C-00040,
C-03852, C-09369, C-09983, C-20595,
1-20820, K-06349, K-19750, L-24033,
N-04845
HYDROXIDES B-22182, B-25468, B-25491,
C-24970
I
IMPINGERS B-22943, C-09033, C-25851,
D-05152
INCINERATION B-09913, B-20248
INDUSTRIAL AREAS A-18305, C-01387,
D-05152, D-11492, K-06349
INDUSTRIAL EMISSION SOURCES
A-02235, A-04946, A-10749, A-12633,
A-12751, A-12823, A-13403, A-13596,
A-13841, A-13850, A-15517, A-18305,
A-21221, A-23044, A-23972, A-25178,
A-25605, B-00587, B-00800, B-01125,
B-02355, B-02985, B-03129, B-03945,
B-04067, B-05079, B-05567, B-06247,
B-06282, B-07535, B-07925, B-08181,
B-09126, B-09559, B-09913, B-11058,
B-11146, B-11235, B-11238, B-11250,
B-11906, B-13206, B-13667, B-13672,
B-13728, B-13806, B-14030, B-14386,
B-14533, B-14568, B-14660, B-15739,
B-15846, B-16289, B-16290, B-16291,
B-16447, B-16718, B-17053, B-17810,
B-19033, B-19370, B-19383, B-19469,
B-19486, B-19593, B-19595, B-19644,
B-19682, B-19856, B-19886, B-20248,
B-20416, B-20670, B-21309, B-21824,
B-22055, B-22943, B-23556, B-23939,
B-24246, B-24451, B-24673, B-24695,
B-24833, B-25133, B-25275, B-25370,
B-25468, B-25643, B-26254, C-00040,
C-01387, C-03852, C-09295, C-17700,
C-23771, D-05152, D-11492, E-10751,
F-00530, F-13802, F-14249, F-14506,
F-14526, F-14538, F-14539, F-14641,
F-14653, F-14871, F-22098, 1-20820,
1-24160, J-11791, J-17203, J-21206,
J-21308, L-05407, L-10998, L-11242,
L-24033, L-25520, N-04845
INFRARED SPECTROMETRY F-22154
INORGANIC ACIDS A-02235, A-04946,
A-10749, A-12633, A-12751, A-12823,
A-13403, A-13596, A-13841, A-13850,
A-15517, A-18305, A-21221, A-23044,
A-25178, A-25605, B-00587, B-00800,
B-01125, B-02355, B-02985, B-03129,
B-03945, B-04067, B-05079, B-05514,
B-05567, B-06247, B-06282, B-07535,
B-07552, B-07925, B-08181, B-09126,
B-09559, B-09913, B-11058, B-11146,
B-11235, B-11238, B-11250, B-11629,
B-11906, B-13206, B-13337, B-13667,
B-13672, B-13728, B-13806, B-13880,
B-14030, B-14386, B-14533, B-14568,
B-15739, B-15846, B-15879, B-15991,
B-16289, B-16290, B-16291, B-16447,
B-16480, B-16718, B-17053, B-17810,
B-17887, B-17889, B-19033, B-19228,
B-19370, B-19383, B-19486, B-19592,
B-19593, B-19594, B-19595, B-19606,
B-19644, B-19682, B-19856, B-19943,
B-20024, B-20248, B-20416, B-20670,
B-20777, B-21309, B-21703, B-21824,
B-22055, B-22182, B-22943, B-23048,
B-23070, B-23264, B-23556, B-23939,
B-24103, B-24110, B-24246, B-24256,
B-24451, B-24594, B-24628, B-24673,
B-24695, B-24833, B-25133, B-25275,
B-25370, B-25468, B-25491, B-25643,
B-25717, B-25742, B-25768, B-26095,
B-26254, C-00040, C-00381, C-00482,
C-01387, C-01819, C-03035, C-03852,
C-09033, C-09295, C-09369, C-09633,
C-09983, C-11089, C-11140, C-12596,
C-14486, C-14735, C-15745, C-19384,
C-20595, C-21056, C-21415, C-22645,
C-23771, C-24970, C-25445, C-25851,
D-05152, D-11492, E-10751, E-21791,
F-00530, F-04626, F-10907, F-13652,
F-13802, F-13875, F-13940, F-14249,
F-14506, F-14625, F-14626, F-14641,
F-14653, F-14845, F-14871, F-15325,
F-15416, F-16292, F-16377, F-20274,
F-21068, F-22098, F-22154, G-11379,
G-16774, G-17623, G-22594, G-23930,
1-20820, 1-24160, J-11791, J-17203,
J-21206, J-21308, J-22397, K-06349,
K-19750, L-05407, L-10998, L-11242,
L-24033, L-25520, N-04845
INSTRUMENTATION C-00381, C-00482,
C-01819, C-09633, C-25851, D-05152,
F-00530
INTERNAL COMBUSTION ENGINES
B-07535
INTERNATIONAL F-00530
INVERSION A-04946, B-07535, E-21791,
F-00530
IODIDES C-03852, C-09633
IODIMETRIC METHODS C-00040,
C-17700, C-20595
IODINE COMPOUNDS C-03852, C-09633
IONIZATION B-05514
IONS C-09633
IRON A-04946, B-05567, B-07925, B-20248,
C-03035
IRON COMPOUNDS A-04946, B-04067,
B-07925, B-20024, B-24594, F-14626
F-15325, G-16774, J-11791, L-10998
IRON OXIDES B-07552, B-07925, B-16289
B-16290, B-16291, B-20024, F-13875
F-15325, F-16292
-------
SUBJECT INDEX
55
ITALY B-17887
JAPAN B-15846, B-19486, B-19592,
B-19644, B-20416, B-20777, B-23264,
B-24673, B-25742, C-03035, C-14486,
C-21056, F-00530, 1-24160, L-05407
K
KEROSENE F-00530
KETONES A-23972, C-09369, C-22645
KILNS B-06282, B-07535, B-07925
KRAFT PULPING A-15517, B-03129,
B-20248, B-25643, B-26254
LABORATORY ANIMALS C-00381,
F-00530, G-11379, G-16774, G-17623,
G-23930, 1-20820
LABORATORY FACILITIES C-09983
LARYNX F-00530
LEAD A-04946, A-10749, B-02985,
B-11238, B-21309, B-25275, C-09983
LEAD COMPOUNDS A-04946, A-10749,
A-12751, A-12823, B-11238, B-25370,
C-09983, K-19750
LEAVES F-00530
LEGAL ASPECTS A-21221, A-25605,
B-03129, B-07925, B-24833, F-00530,
K-06349, K-19750, L-05407, L-24033,
L-25520
LEGISLATION B-03129, B-07925, F-00530,
K-06349, L-05407, L-24033, L-25520
LEUKOCYTES G-11379
LIGHT RADIATION B-07535, E-21791
LIMESTONE A-21221, B-19644
LIQUIDS B-05079, B-07552, B-11235,
B-19856, B-20777, B-23264, B-23556,
B-25717, C-01387, C-09633, D-05152,
F-10907, F-13652, F-22154
LITIGATION A-25605
LIVER G-11379, G-23930
LONDON B-07535
LOS ANGELES B-07535, C-09633
LOWER ATMOSPHERE E-21791
LUNGS F-00530, G-11379, G-17623
LYMPHOCYTES G-11379
M
MAGNESIUM COMPOUNDS F-13875
MAINTENANCE B-25643
MANGANESE COMPOUNDS B-19943,
B-24673, C-09983, F-04626, F-15325,
G-16774
MANGANESE DIOXIDE (JAPANESE)
B-20416
MANGANESE SULFATES B-19943,
F-04626
MASS SPECTROMETRY C-125%
MATERIALS DETERIORATION B-00800,
B-02985, B-03945, B-22055, C-03035,
1-20820, 1-24160, N-04845
MATHEMATICAL ANALYSES A-13841,
B-055I4, B-25768, E-10751, F-00530,
F-14249
MATHEMATICAL MODELING B-25768,
E-10751
MAXIMUM ALLOWABLE
CONCENTRATION B-03129,
D-11492, G-11379, K-06349, K-19750
MEASUREMENT METHODS B-07925,
B-20248, C-00381, C-01387, C-01819,
C-03035, C-03852, C-09033, C-09633,
C-09983, C-11140, C-12596, C-21056,
C-21415, C-25445, C-25851, D-05152,
F-00530, G-11379
MEETINGS L-05407
MEMBRANE FILTERS C-25445
MERCAPTANS B-07925, B-26254
MERCURY B-11238
MERCURY COMPOUNDS A-23972,
B-11238, B-21703, C-09369, C-23771
METABOLISM G-11379
METAL COMPOUNDS A-04946, A-10749,
A-12751, A-12823, A-13596, A-18305,
A-23972, A-25178, B-04067, B-05079,
B-07925, B-09126, B-09559, B-11058,
B-11238, B-15879, B-15991, B-16480,
B-17810, B-19486, B-19644, B-19943,
B-20024, B-20248, B-21703, B-22182,
B-23048, B-23070, B-23264, B-24110,
B-24594, B-24673, B-25370, B-25491,
B-25742, C-03035, C-03852, C-09033,
C-09369, C-09983, C-11089, C-11140,
C-23771, C-24970, F-04626, F-10907,
F-13875, F-14506, F-14538, F-14539,
F-14626, F-14871, F-15325, F-16377,
F-21068, G-16774, J-11791, K-06349,
K-19750, L-10998
METAL FABRICATING AND FINISHING
A-15517, B-07925, B-20248, B-25643,
B-26254
METALS A-04946, A-10749, A-13841,
A-13850, B-02985, B-03129, B-05567,
B-07925, B-09559, B-11146, B-11238,
B-11906, B-20248, B-21309, B-23939,
B-25275, B-25643, C-03035, C-09033,
C-09983, C-11089, F-13802, F-14538,
F-14845, K-06349
METEOROLOGY A-04946, B-07535,
C-00482, C-01387, C-09369, C-09633,
D-05152, D-11492, E-10751, E-21791,
F-00530, G-16774, N-04845
METHANES C-12596
MICE 1-20820
MICROSCOPY C-03035, C-09633
MIDDLE ATMOSPHERE N-04845
MINERAL PROCESSING A-04946,
A-13596, A-21221, B-04067, B-07925,
B-16447, B-25643, B-26254, C-03852,
F-00530, J-17203
MINERAL PRODUCTS A-21221, B-07552,
B-19644, B-23048, B-26254
MINING A-04946, B-26254
MISSOURI B-00587, C-00482, F-00530
MISTS A-13403, B-00587, B-00800,
B-02355, B-02985, B-03945, B-05079,
B-05514, B-05567, B-06247, B-07552,
B-07925, B-11058, B-11235, B-11238,
B-13667, B-17889, B-19370, B-19594,
B-19682, B-23556, B-24110, B-24256,
B-24695, B-24833, B-25370, B-25717,
B-26095, C-00040, C-01387, C-03035,
C-09295, C-11089, C-11140, C-12596,
C-14486, C-23771, D-05152, F-00530,
F-22154, G-23930
MONITORING B-07925, B-20248, C-00381,
C-01387, C-01819, C-12596, C-21056,
C-21415, C-25851, D-05152, G-11379
MONTHLY K-19750
MORBIDITY F-00530
MORTALITY F-00530, 1-20820
N
NAPHTHALENES B-11058
NASHVILLE F-00530
NATURAL GAS B-11629, B-19886
NERVOUS SYSTEM G-11379, G-22594
NEW YORK STATE K-06349
NICKEL B-11146
NICKEL COMPOUNDS C-09369, F-14626
NITRATES B-23070, C-09369, C-23771,
E-21791, F-14871
NITRIC ACID A-18305, B-00587, B-01125,
B-03129, B-07535, B-07552, B-07925,
B-11058, B-14533, B-14568, B-26254,
C-23771, J-17203, L-05407, L-11242
NITRIC OXIDE (NO) B-01125, B-07535,
B-11058, C-00040, C-00381, C-09369,
E-21791, F-10907, F-20274
NITROGEN B-21703, C-11089
NITROGEN DIOXIDE (NO2) B-00800,
B-01125, B-07552, B-11058, C-00040,
C-00381, C-09369, C-09983, C-14486,
C-24970, E-21791, F-10907, K-19750
NITROGEN OXIDES A-13403, B-00800,
B-01125, B-02355, B-07535, B-07552,
B-07925, B-08181, B-11058, B-14533,
B-19370, B-19593, C-00040, C-00381,
C-09369, C-09983, C-14486, C-17700,
C-24970, D-11492, E-21791, F-10907,
F-20274, J-17203, J-21206, K-19750,
L-24033
NITROUS ACID C-24970
NON-INDUSTRIAL EMISSION SOURCES
A-04946, A-15517, B-00800, B-03129,
B-07535, B-11058, B-11238, B-26254,
F-00530, L-11242, L-25520, N-04845
NON-URBAN AREAS B-11906, F-00530,
K-06349
o
OCCUPATIONAL HEALTH B-04067
ODOR COUNTERACTION B-07535
ODORS B-03129, B-26254, G-22594,
K-06349
OIL BURNERS A-23044
OLEFINS B-03129, B-07925
OPEN HEARTH FURNACES B-05567,
B-26254
OPERATING CRITERIA A-12823
OPERATING VARIABLES A-12823,
B-19644, B-20416, B-21309, B-21824,
B-24103, B-24256, B-25643, F-22098
ORGANIC ACIDS B-25742
ORGANIC NITROGEN COMPOUNDS
B-01125, B-15879, B-15991, B-19856,
B-24594
ORGANIC SULFUR COMPOUNDS
B-07925, B-24594, B-26254
ORLON B-05079
OWENS JET DUST COUNTERS C-03035
OXJDANTS C-09633, E-21791, K-06349,
K-19750
OXIDATION A-10749, B-09126, B-11906,
E-21791, F-04626, F-10907
OXIDES A-02235, A-04946, A-10749,
A-12633, A-12823, A-13403, A-13596,
A-13841, A-13850, A-18305, A-23972,
A-25605, B-00800, B-01125, B-02355,
B-05079, B-05567, B-06282, B-07535,
B-07552, B-07925, B-08181, B-09126,
B-09559, B-09913, B-11058, B-11235,
B-11238, B-11250, B-11906, B-13206,
B-13337, B-13667, B-13880, B-14533,
B-15846, B-16289, B-16290, B-16291,
B-16480, B-16718, B-17887, B-19370,
B-19383, B-19486, B-19593, B-19594,
B-19595, B-20024, B-20248, B-21703,
B-22055, B-23070, B-24594, B-24628,
-------
56
SULFURIC ACID MANUFACTURING
B-24673, B-25370, B-25491, B-26254,
C-00040, C-00381, C-00482, C-01819,
C-03852, C-09033, C-09295, C-09369,
C-09983, C-11089, C-11140, C-12596,
C-14486, C-14735, C-17700, C-19384,
C-20595, C-21056, C-21415, C-24970,
C-25851, D-05152, D-11492, E-21791,
F-00530, F-04626, F-10907, F-13802,
F-13875, F-13940, F-14249, F-14526,
F-14538, F-14539, F-14625, F-14626,
F-14641, F-14653, F-14845, F-15325,
F-16292, F-16377, F-20274, F-21068,
F-22154, G-11379, G-16774, G-17623,
G-22594, G-23930, 1-20820, J-17203,
J-21206, J-21308, K-06349, K-19750,
L-05407, L-24033, N-04845
OXYGEN A-13596, B-09126, B-13880,
B-22055, E-21791, F-04626, F-10907,
F-13875
OXYGEN LANCING B-07535
OZONE B-00800, B-19943, C-09369,
C-12596, C-20595, E-21791
PACKED TOWERS B-08181, B-15879,
B-22055, B-24110, L-24033
PAPER MANUFACTURING A-15517,
B-03129, B-16447
PARTICLE COUNTERS C-03035
PARTICLE GROWTH D-05152
PARTICLE SHAPE G-16774
PARTICLE SIZE B-00587, B-00800,
B-05514, B-07552, B-22943, B-24110,
B-24256, B-24695, B-24833, B-25643,
B-26095, C-00482, C-01387, C-03035,
C-09033, C-09633, C-23771, D-05152,
G-16774
PARTICULATE CLASSIFIERS B-00587,
B-00800, B-05514, B-07552, B-22943,
B-24110, B-24256, B-24695, B-24833,
B-25643, B-26095, C-00482, C-01387,
C-03035, C-09033, C-09633, C-23771,
D-05152, F-00530, G-16774
PARTICULATE SAMPLING B-20248,
C-00482, C-09033, C-23771, C-25445
PARTICULATES A-04946, A-13403,
A-25605, B-00587, B-00800, B-01125,
B-02355, B-02985, B-03129, B-03945,
B-04067, B-05079, B-05514, B-05567,
B-06247, B-06282, B-07535, B-07552,
B-07925, B-11058, B-11235, B-11238,
B-11906, B-13667, B-14568, B-15879,
B-15991, B-17889, B-19370, B-19383,
B-19594, B-19606, B-19682, B-20777,
B-21824, B-22943, B-23556, B-24110,
B-24256, B-24695, B-24833, B-25370,
B-25643, B-25717, B-26095, B-26254,
C-00040, C-00381, C-00482, C-01387,
C-01819, C-03035, C-09033, C-09295,
C-09633, C-09983, C-11089, C-11140,
C-12596, C-14486, C-20595, C-22645,
C-23771, C-25445, D-05152, E-21791,
F-00530, F-22154, G-11379, G-16774,
G-17623, G-22594, G-23930, 1-20820,
J-17203, J-21206, K-06349, K-19750,
L-05407, L-24033, N-04845
PATHOLOGICAL TECHNIQUES G-11379,
G-23930
PENELEC (CONTACT PROCESS) A-18305
PENNSYLVANIA F-00530, K-19750
PEROXIDES C-09369, C-21056, C-21415,
C-25851
PEROXYACETYL NITRATE E-21791
PEROXYACYL NITRATES E-21791
PESTICIDES F-00530
PETER SPENCE PROCESS (CLAUS)
B-09913, B-24246, L-24033
PETROLEUM PRODUCTION B-00800,
B-07925
PETROLEUM REFINING A-15517,
B-07925, B-19033, B-24673, 1-20820,
L-10998, L-11242
PH B-19469, B-19644, B-25491, C-09033,
C-09633, D-05152
PHENOLS C-09983
PHOSPHATES A-04946, B-03129, C-23771,
L-11242
PHOSPHINE C-09369
PHOSPHORIC ACID A-18305, B-00587,
B-07552, B-09559, B-11058, B-25717,
B-26095, C-14486, C-23771
PHOSPHORUS COMPOUNDS A-04946,
B-03129, B-11058, C-09369, C-23771,
L-11242
PHOTOCHEMICAL REACTIONS E-21791
PHOTOMETRIC METHODS C-12596,
C-25851
PHOTOSYNTHESIS F-00530
PHYSICAL STATES A-04946, B-00587,
B-00800, B-03945, B-05079, B-05514,
B-07552, B-09913, B-11235, B-11238,
B-13728, B-14533, B-14568, B-15879,
B-15991, B-19682, B-19856, B-20777,
B-22182, B-23264, B-23556, B-24110,
B-25717, B-25768, C-01387, C-09633,
D-05152, F-10907, F-13652, F-15325,
F-15416, F-22154, G-11379
PHYTOTOXICANTS F-00530, N-04845
PILOT PLANTS B-23070, B-23556, B-25468
PLANNING AND ZONING A-21221,
L-05407
PLANS AND PROGRAMS A-04946,
B-03129, B-20248, C-01819, L-05407
PLANT DAMAGE A-25605, C-24970,
E-21791, F-00530, 1-20820, L-24033,
N-04845
PLANT GROWTH F-00530
PLANTS (BOTANY) C-24970, F-00530,
N-04845
PLASTICS B-03129
PLATINUM A-13841, A-13850, F-13802,
F-14538, F-14845
PLUME BEHAVIOR D-11492, E-10751,
F-00530
PNEUMOCONIOSIS B-04067
PNEUMONIA G-11379
POINT SOURCES E-10751
POLAROGRAPHIC METHODS C-09983,
C-15745
POLYNUCLEAR COMPOUNDS B-11058
PORTABLE C-23771
POTASSIUM COMPOUNDS B-22182
POTENTIOMETRIC METHODS C-12596,
C-14735
POWER SOURCES B-07535
PRECIPITATION C-09369, N-04845
PRESSURE B-00587, B-08181, B-11058,
B-23556, B-24110, B-25768, D-11492
PRIMARY METALLURGICAL
PROCESSING A-04946, A-10749,
A-12751, A-12823, A-15517, A-21221,
A-25178, A-25605, B-05567, B-07925,
B-09559, B-11146, B-13672, B-19469,
B-20248, B-21309, B-23939, B-24451,
B-24673, B-25275, B-26254, 1-20820,
1-24160, J-21308, L-10998, L-11242,
L-24033
PRIMATES G-23930
PROCESS MODIFICATION A-10749,
B-06282, B-07925, B-09126, B-11058,
B-11906, B-13728, B-16718, B-21824,
B-23939, B-25491
PROTEINS G-11379
PULMONARY FUNCTION F-00530,
G-16774, G-23930, 1-20820
PULMONARY RESISTANCE G-16774,
1-20820
QUINOLINES B-19856
R
RABBITS 1-20820
RADIOACTIVE RADIATION C-01387,
C-11140, K-06349
RADIOGRAPHY F-16292
RADON C-09369
RATS G-11379
REACTION KINETICS A-13841, B-16290,
B-16480, B-19486, B-19943, B-20024,
B-25133, E-21791, F-04626, F-10907,
F-13652, F-14538, F-16377
REACTION MECHANISMS B-13880,
E-21791, F-04626, F-20274
RECREATION AREAS K-06349
REDUCTION A-10749, A-12751, A-12823,
B-01125, B-19886, B-24673, F-14506
REGULATIONS B-03129, B-24833,
K-19750
REINLUFT PROCESS (ADSORPTION)
B-14660
RESEARCH METHODOLOGIES F-00530
RESIDENTIAL AREAS K-06349
RESPIRATORY DISEASES B-04067,
F-00530, G-11379, G-16774, L-05407,
N-04845
RESPIRATORY FUNCTIONS F-00530,
G-11379, G-16774, G-23930, 1-20820
RESPIRATORY SYSTEM F-00530,
G-11379, G-17623, 1-20820, L-05407
SAMPLERS B-00800, B-22943, C-00040,
C-00482, C-01819, C-03035, C-09033,
C-09633, C-09983, C-11089, C-15745,
C-23771, C-25445, C-25851, D-05152
SAMPLING METHODS B-00800, B-02355,
B-20248, B-22943, C-00040, C-00482,
C-01819, C-03035, C-09033, C-09633,
C-09983, C-11089, C-15745, C-19384,
C-22645, C-23771, C-24970, C-25445,
C-25851, D-05152
SAMPLING PROBES C-00040
SCREEN FILTERS B-24110
SCRUBBERS A-04946, A-12751, A-12823,
A-23044, B-00587, B-00800, B-01125,
B-05079, B-07535, B-07925, B-08181,
B-11058, B-11629, B-13337, B-13667,
B-14568, B-15879, B-15991, B-17889,
B-19383, B-19469, B-19644, B-20248,
B-22055, B-22943, B-23556, B-24110,
B-24594, B-24673, B-24695, B-24833,
B-25768, C-25851, F-00530, J-21206,
L-24033
SEASONAL B-11250
SEDIMENTATION B-25717, F-00530
SETTLING CHAMBERS A-25605
SETTLING PARTICLES A-13403, B-04067,
B-05079, B-06282, B-07535, B-07925,
B-11058, B-11906, B-17889, B-20777,
B-22943, B-24110, B-25643, B-26254,
C-00040, C-09983, C-20595, C-23771,
J-17203, K-06349, K-19750, L-05407
SEWAGE B-11238
SILICON COMPOUNDS B-07552, B-24695
C-09983
-------
SUBJECT INDEX
57
SILICON DIOXIDE C-09983, F-13875,
F-14626
SILICOSIS B-04067
SINTERING A-04946, A-10749
SKIN F-00530
SLAUGHTERHOUSES B-26254
SLUDGE B-11238
SMOG B-07535, E-21791, F-00530,
G-17623, 1-20820
SMOKES A-25605, B-07535, B-07925,
B-15879, B-15991, J-17203, K-06349
SMOKING F-00530
SOCIAL ATTITUDES F-00530
SOCIO-ECONOMIC FACTORS A-25178,
L-25520
SODIUM CARBONATE B-15991, B-23264
SODIUM COMPOUNDS A-18305, B-15879,
B-15991, B-22182, B-23264, B-25491,
B-25742, C-03035, C-03852, F-10907,
F-14871
SODIUM HYDROXIDE A-18305, B-22182,
B-25491, C-03035, F-10907
SOILING 1-20820
SOILING INDEX F-00530
SOLAR RADIATION B-07535, E-21791
SOLID WASTE DISPOSAL A-15517,
B-26254
SOOT C-09983, L-05407
SOOT FALL L-05407
SOURCE SAMPLING B-02355, C-00040
S02 REMOVAL (COMBUSTION
PRODUCTS) A-12751, A-12823,
A-13403, A-15517, A-18305, A-23044,
A-23972, A-25605, B-07535, B-09913,
B-11058, B-11250, B-11629, B-11906,
B-13206, B-13337, B-13672, B-13806,
B-14030, B-14660, B-15739, B-15879,
B-15991, B-17053, B-17810, B-17889,
B-19033, B-19228, B-19469, B-19592,
B-19595, B-19606, B-19644, B-19856,
B-19886, B-19943, B-20248, B-20416,
B-20670, B-20777, B-21309, B-21824,
B-22182, B-22943, B-23070, B-23264,
B-23939, B-24103, B-24246, B-24451,
B-24594, B-24628, B-24673, B-24695,
B-25133, B-25275, B-25468, B-25491,
B-25742, B-25768, F-00530, F-13652,
1-24160, J-17203, J-21206, L-24033
SPECTROMETRY B-20248, C-l 1140,
C-12596, F-20274, F-22154
SPECTROPHOTOMETRY C-00381,
C-09033, C-09295, C-11089, C-125%,
C-20595
SPOT TESTS C-14486
SPRAY TOWERS B-14568, B-22055
SPRAYS A-13403, C-00040
ST LOUIS B-00587, C-00482, F-00530
STABILITY (ATMOSPHERIC) A-04946,
B-07535, E-10751, E-21791, F-00530
STACK GASES A-04946, A-12751,
A-12823, A-15517, A-23044, A-25605,
B-00800, B-OI125, B-03945, B-07925,
B-11250, B-11629, B-11906, B-14568,
B-14660, B-15739, B-16718, B-17053,
B-19370, B-19469, B-19592, B-19606,
B-19644, B-19856, B-19886, B-22943,
B-23070, B-23264, B-24110, B-24246,
B-24451, B-24628, B-24673, B-24833,
B-25133, B-25275, C-14735, C-17700,
E-10751, F-20274, J-21206, J-22397,
N-04845
STACK SAMPLING B-02355, C-00040
STACKS A-04946, A-23044, A-25605,
B-00800, B-02355, B-03945, B-07925,
B-17053, B-21824, C-00040, D-05152,
E-10751, F-20274
STANDARDS B-03129, B-16718, D-l 1492,
G-I1379, K-06349, K-19750, L-25520
STATE GOVERNMENTS K-06349,
K-19750
STATISTICAL ANALYSES E-10751
STEAM B-09913, B-14533, B-15879,
B-15991, F-15325, F-15416
STEAM PLANTS B-07925, B-11238,
B-14660, E-10751
STEEL A-04946, B-05567, B-07925,
B-20248
SULFATES B-00800, B-01125, B-17889,
B-19592, B-19606, B-25491, C-09033,
C-09369, C-0%33, C-11140, C-15745,
D-05152, F-04626, F-15325, F-15416,
G-16774, 1-20820, 1-24160, K-19750,
N-04845
SULFIDES A-04946, A-10749, B-00800,
B-04067, B-07925, B-09559, B-11058,
B-11629, B-14030, B-17889, B-19033,
B-19886, B-22943, B-23048, B-23070,
B-24594, B-26254, C-00040, C-03852,
C-09369, C-09983, C-20595, F-14626,
1-20820, J-11791, K-06349, K-19750,
L-24033, N-04845
SULFITES B-19383, B-19644, B-25491
SULFUR COMPOUNDS A-04946, A-10749,
A-25178, B-00800, B-01125, B-04067,
B-07925, B-09126, B-09559, B-09913,
B-11058, B-11146, B-11235, B-11238,
B-11629, B-11906, B-14030, B-17887,
B-17889, B-19033, B-19383, B-19592,
B-19606, B-19644, B-19886, B-22943,
B-23048, B-23070, B-24246, B-24594,
B-25491, B-26254, C-00040, C-03852,
C-09033, C-09369, C-09633, C-09983,
C-11140, C-15745, C-20595, D-05152,
F-04626, F-10907, F-14626, F-15325,
F-15416, G-16774, 1-20820, 1-24160,
J-11791, J-21308, J-22397, K-06349,
K-19750, L-10998, L-11242, L-24033,
N-04845
SULFUR DIOXIDE A-02235, A-04946,
A-10749, A-12823, A-13403, A-13596,
A-13841, A-23972, B-00800, B-01125,
B-02355, B-05567, B-06282, B-07535,
B-07552, B-07925, B-09126, B-09559,
B-09913, B-11058, B-11238, B-11250,
B-11906, B-13206, B-13337, B-13667,
B-13880, B-15846, B-16289, B-16290,
B-16291, B-16480, B-16718, B-17887,
B-19383, B-19486, B-20024, B-21703,
B-22055, B-25370, C-00040, C-00381,
C-00482, C-01819, C-03852, C-09033,
C-09369, C-09983, C-11089, C-11140,
C-125%, C-14486, C-14735, C-17700,
C-20595, C-21056, C-21415, C-24970,
C-25851, D-05152, E-21791, F-00530,
F-04626, F-13802, F-13940, F-14249,
F-14526, F-14538, F-14539, F-14625,
F-14626, F-14641, F-14653, F-14845,
F-16292, F-16377, F-21068, G-16774,
G-17623, G-22594, G-23930, 1-20820,
J-21308, K-06349, K-19750, L-05407,
N-04845
SULFUR OXIDES A-02235, A-04946,
A-10749, A-12633, A-12823, A-13403,
A-13596, A-13841, A-18305, A-23972,
A-25605, B-00800, B-01125, B-02355,
B-05567, B-06282, B-07535, B-07552,
B-07925, B-09126, B-09559, B-09913,
B-11058, B-11235, B-11238, B-11250,
B-11906, B-13206, B-13337, B-13667,
B-13880, B-14533, B-15846, B-16289,
B-16290, B-16291, B-16480, B-16718,
B-17887, B-19370, B-19383, B-19486,
B-19594, B-19595, B-20024, B-21703,
B-22055, B-24628, B-25370, B-25491,
B-26254, C-00040, C-00381, C-00482,
C-01819, C-03852, C-09033, C-09295,
C-09369, C-09983, C-11089, C-11140,
C-125%, C-14486, C-14735, C-17700,
C-19384, C-20595, C-21056, C-21415,
C-24970, C-25851, D-05152, E-21791,
F-00530, F-04626, F-13802, F-13940,
F-14249, F-14526, F-14538, F-14539,
F-14625, F-14626, F-14641, F-14653,
F-14845, F-16292, F-16377, F-20274,
F-21068, F-22154, G-11379, G-16774,
G-17623, G-22594, G-23930, 1-20820,
J-21206, J-21308, K-06349, K-19750,
L-05407, L-24033, N-04845
SULFUR OXIDES CONTROL A-02235,
A-04946, A-12751, A-12823, A-13403,
A-15517, A-18305, A-23044, A-23972,
A-25178, A-25605, B-00800, B-02355,
B-02985, B-07535, B-09559, B-09913,
B-11058, B-11250, B-11629, B-11906,
B-13206, B-13337, B-13672, B-13806,
B-14030, B-14386, B-14660, B-15739,
B-15846, B-15879, B-15991, B-17053,
B-17810, B-17887, B-17889, B-19033,
B-19228, B-19469, B-19592, B-19595,
B-19606, B-19644, B-19856, B-19886,
B-19943, B-20248, B-20416, B-20670,
B-20777, B-21309, B-21703, B-21824,
B-22182, B-22943, B-23070, B-23264,
B-23939, B-24103, B-24246, B-24451,
B-24594, B-24628, B-24673, B-24695,
B-25133, B-25275, B-25468, B-25491,
B-25742, B-25768, F-00530, F-13652,
1-24160, J-11791, J-17203, J-21206,
L-10998, L-24033
SULFUR TRIOXJDE A-02235, A-13841,
A-25605, B-00800, B-01125, B-06282,
B-07535, B-07552, B-09126, B-09913,
B-11058, B-11235, B-11238, B-11250,
B-11906, B-13667, B-16718, B-17887,
B-19594, B-19595, B-22055, B-24628,
B-25370, B-25491, C-00040, C-00482,
C-09033, C-09295, C-09369, C-11089,
C-11140, C-125%, C-14735, C-19384,
C-20595, C-24970, F-00530, F-04626,
F-13802, F-14526, F-14538, F-14539,
F-14653, F-14845, F-16292, F-21068,
F-22154, G-16774, 1-20820
SULFURIC ACID A-02235, A-04946,
A-10749, A-12633, A-12751, A-12823,
A-13403, A-135%, A-13841, A-13850,
A-15517, A-18305, A-21221, A-23044,
A-25178, A-25605, B-00587, B-00800,
B-01125, B-02355, B-02985, B-03129,
B-03945, B-04067, B-05079, B-05514,
B-05567, B-06247, B-06282, B-07535,
B-07552, B-07925, B-08181, B-09126,
B-09559, B-09913, B-11058, B-11146,
B-11235, B-11238, B-11250, B-11629,
B-11906, B-13206, B-13337, B-13667,
B-13672, B-13728, B-13806, B-13880,
B-14030, B-14386, B-14533, B-14568,
B-15739, B-15846, B-15879, B-15991,
B-16289, B-16290, B-16291, B-16447,
B-16480, B-16718, B-17053, B-17810,
B-17887, B-17889, B-19033, B-19228,
B-19370, B-19383, B-19486, B-19592,
B-19593, B-19594, B-19595, B-19606,
B-19644, B-19682, B-19856, B-19943,
B-20024, B-20248, B-20416, B-20670,
B-20777, B-21309, B-21703, B-21824,
B-22055, B-22182, B-22943, B-23048,
B-23070, B-23264, B-23556, B-23939,
B-24103, B-24110, B-24246, B-24256,
B-24451, B-24594, B-24628, B-24673,
B-24695, B-24833, B-25133, B-25275,
B-25370, B-25468, B-25491, B-25643,
-------
58
SULFURIC ACID MANUFACTURING
B-25717, B-25742, B-25768, B-26095,
B-26254, C-00040, C-00381, C-00482,
C-01387, C-01819, C-03035, C-03852,
C-09033, C-09295, C-09369, C-09633,
C-09983, C-11089, C-11140, C-12596,
C-14486, C-14735, C-15745, C-19384,
C-20595, C-21056, C-21415, C-22645,
C-23771, C-24970, C-25445, C-25851,
D-05152, D-11492, E-10751, E-21791,
F-00530, F-04626, F-10907, F-13652,
F-13802, F-13875, F-13940, F-14249,
F-14506, F-14625, F-14626, F-14641,
F-14653, F-14845, F-14871, F-15325,
F-15416, F-16292, F-16377, F-20274,
F-21068, F-22098, F-22154, G-11379,
G-16774, G-17623, G-22594, G-23930,
1-20820, 1-24160, J-11791, J-17203,
J-21206, J-21308, J-22397, K-06349,
K-19750, L-05407, L-10998, L-11242,
L-25520, N-04845
SUPERSATURATION B-19682
SURFACE COATINGS C-03035
SURFACE PROPERTIES F-21068
SUSPENDED PARTICULATES A-13403,
A-25605, B-00587, B-00800, B-01125,
B-02355, B-02985, B-03129, B-03945,
B-05079, B-05514, B-05567, B-06247,
B-07535, B-07552, B-07925, B-11058,
B-11235, B-11238, B-11906, B-13667,
B-15879, B-15991, B-17889, B-19370,
B-19383, B-19594, B-19606, B-19682,
B-21824, B-23556, B-24110, B-24256,
B-24695, B-24833, B-25370, B-25643,
B-25717, B-26095, C-00040, C-00381,
C-01387, C-03035, C-09295, C-09633,
C-11089, C-11140, C-12596, C-14486,
C-23771, D-05152, E-21791, F-00530,
F-22154, G-17623, G-23930, 1-20820,
J-17203, K-06349, K-19750
SWEDEN A-02235, A-18305, B-00587,
B-00800, B-03945, B-24451, B-25275,
C-00381, C-00482, E-10751, F-00530,
F-04626
SYNERGISM G-11379, G-16774
SYNTHETIC FIBERS B-03129, B-05079,
B-24695
TECHNICAL SOCIETIES L-05407
TEMPERATURE B-07552, B-09126,
B-11058, B-11238, B-19886, B-22055,
B-22182, B-23070, B-25468, B-25742,
C-00482, C-09033, F-13802, F-13875,
F-16292, F-20274, F-22154
TEMPERATURE (ATMOSPHERIC)
D-11492
TENNESSEE F-00530
TESTING FACILITIES C-00381, C-09983,
F-00530, G-16774
TEXTILE MANUFACTURING B-11058,
F-14871, L-24033
TEXTILES B-03129, B-05079, B-05567,
B-07552, B-24695
THERMODYNAMICS B-16480, B-20024,
F-13802, F-13875, F-14626, F-14641,
F-14653
THRESHOLDS G-22594, 1-20820
TIN COMPOUNDS F-14539
TISSUES F-00530
TITANIUM COMPOUNDS B-05079
TOLUENES B-07925
TOPOGRAPHIC INTERACTIONS E-10751
TOXIC TOLERANCES C-24970, F-00530
TOXICITY G-11379, G-16774, 1-20820
TRACHEA F-00530, G-11379
TRANSPORTATION A-21221, B-07535,
F-00530, L-24033
TREATED FABRICS B-24695
TREATMENT AND AIDS F-16292
TREES C-24970, F-00530
TURBIDIMETRY D-05152
TURBULENCE (ATMOSPHERIC) F-00530
U
ULTRAVIOLET RADIATION E-21791
UNITED STATES B-09126, F-00530
URBAN AREAS A-18305, B-16447,
C-01387, C-01819, C-09633, D-05152,
D-11492, K-06349
URINALYSIS F-00530, G-11379
USSR A-13403, B-04067, B-08181, B-14386,
B-14568, B-16289, B-16290, B-16291,
B-16447, B-16480, B-19682, B-19856,
B-19943, B-20024, B-23070, B-23939,
B-24256, C-09295, C-17700, F-13652,
F-13875, F-13940, F-14526, F-14538,
F-14539, F-14625, F-14626, F-14641,
F-14653, F-15325, F-15416, F-16292,
F-16377, G-11379, G-17623, G-22594
VALLEYS F-00530
VANADIUM F-14845
VANADIUM COMPOUNDS B-09126,
B-16480, B-19486, B-23070, F-14538,
F-16377, F-21068
VAPORS B-09913, B-11235, B-13728,
B-14533, B-14568, B-15879, B-15991,
B-19682, F-15325, F-15416, G-11379
VEHICLES B-07535, L-24033
VENTILATION B-04067, B-06282
VENTURI SCRUBBERS B-01125, B-08181,
B-25768
VISIBILITY F-00530, N-04845
VISIBLE RADIATION E-21791
VOLTAGE B-23264
w
WASHOUT N-04845
WATER B-05079, B-07552, B-11235,
B-19856, B-20777, B-23264, B-23556,
C-01387, D-05152, F-10907, F-13652
WATER POLLUTION L-25520
WEST AND GAEKE METHOD C-00381,
C-14735, 1-20820
WET CYCLONES B-22943
WETTING B-05079
WINDS A-04946, C-01387, D-11492,
E-10751
WOOLS B-05567, B-07552
X
X-RAYS C-11140
XYLENES B-07925
YOKOHAMA F-00530
ZINC A-04946, B-09559, B-11906, B-21309
ZINC COMPOUNDS A-04946, A-12751,
A-12823, A-13596, A-25178,
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