J JUl t_/ \JTI_j\J
FOR REMOVING SULFUR DIOXIDE
FROM FLUE GASES
FINAL PHASE I REPORT
UNDER CONTRACT PH 22-63-19
for
NEW PROCESS DEVELOPMENT SECTION
DIVISION OF PROCESS CONTROL ENGINEERING
ATIONAL AIR POLLUTION CONTROL ADMINISTRAT
PUBLIC HEALTH SERVICE
DEPARTMENT OF HEALTH, EDUCATION, AND WEL
March 1969
RESEARCH REPORT
ID
BATTELLE If] NORTHWEST
BATTEUE MEMORIAL INSTITUTE IIH PACIFIC NORTHWEST LABORATORY
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-------
APPLICABILITY OF ORGANIC LIQUIDS
TO THE DEVELOPMENT OF NEW PROCESSES
FOR REMOVING SULFUR DIOXIDE
FROM FLUE GASES
FINAL PHASE I REPORT
UNDER CONTRACT PH 22-63-19
for
NEW PROCESS DEVELOPMENT SECTION
DIVISION OF PROCESS CONTROL ENGINEERING
NATIONAL AIR POLLUTION CONTROL ADMINISTRATION
PUBLIC HEALTH SERVICE
U.S. DEPARTMENT OF HEALTH, EDUCATION, AND WELFARE
March 1969
BATTELLE MEMORIAL INSTITUTE
PACIFIC NORTHWEST LABORATORY
Richland, Washington 99352
Battelle is not engaged in research for advertising, sales promotion, or publicity,
and this report may not be reproduced in full or in part for such purposes.
-------
11
T ABLE OF CONTENTS
LIST OF TABLES
INTRODUCTION
SUMMARY AND CONCLUSIONS.
RECOMMENDATIONS
OBJECTIVE
SCOPE OF WORK.
DISCUSSION
Organic Liquids as Scrubbing Agents
Present Status
Reaction Mechanisms, Classes and Candidate Organics.
Symbols
Compilation of Equilibrium Data.
Correlation of Activity Coefficients with
Molecular Structure
Evaluation of Practical Utility of Liquids as
S02 Absorbents
Dissociation Pressures of Solid Adducts of
S02 and Organic Substances
Selection Criteria
Background Data
Availability and Cost
Physical and Chemical Properties
Conditions of Use
Potential Sulfur Bearing Products
Methods of Contacting Flue Gases with Scrubbing Agents.
Methods of Assuring Adequate Stack Plume Dispersion
Organic Regeneration.
Applicability of Organic Liquids
General Considerations
Properties of Organic Liquids
Effects of Flue Gas Temperature.
Oxidation and Degradation Effects.
Solvent Emission Considerations.
Solvent Availability.
BATTELLE-NORTHWEST
iv
1
3
5
5
6
7
7
7
8
9
9
10
12
13
13
13
14
15
15
15
17
18
19
22
23
25
27
31
33
36
-------
iii
Most Promising Organic Liquids for
Gas Scrubbing
Application to Smelter Gas.
Preliminary Economic Comparison
Economic Bases.
Adjustment of Alkalized Alumina Costs.
DMA Process Comparison
Data Necessary for Assessment of Engineering and
Potential of Promising Candidates
Proposed Future Program
References.
Flue
APPENDIX A
APPENDIX B
BATTELLE-NORTHWEST
Economic
. 38
. 40
. 41
. 41
. 47
. 50
. 52
. 53
. 54
.A-1
.B-1
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1
2
3
4
5
6
7
8
9
10
11
12
13
iv
LIST OF TABLES
Activity Coefficients at Infinite Dilution - Low Values
Activity Coefficients at Infinite Dilution - High Values
Sulfur Dioxide Capacitiers of Liquid When Partial Pressure
of S02 is 2. 3 Torr
,
Dissociation Pressures of S02-0rganic Adduct
Comparison of Organic Liquids Having Promising
S02 Solubilities
Solvent Evaporation and Solvent Recovery Requirements
Solvent Recovery Requirements for 40 lb/day Solvent
Emission
U. S. Production and Sales of Various Organic Liquids
Levelized Fixed Charges for Investor-Owned Utility
Wage Rates in Fossil-Fueled Power Plants
Adjusted Total Investment for Alkalized Alumina
Adjusted Annual Operating Cost for Alkalized Alumina
Approximate Chemical Costs of DMA Process for
Flue Gas
BAT TEL L E - NOR T 'H W EST
11
12
13
14
26
29
36
37
43
46
48
49
52
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1
PHASE I FINAL REPORT
APPLICABILITY OF ORGANIC LIQUIDS
TO THE DEVELOPMENT OF NEW PROCESSES
FOR REMOVING SULFUR DIOXIDE FROM FLUE GASES
INTRODU CTION
The two principal gaseous pollutants in urban and industrial atmo-
spheres are automobile exhausts and sulfur oxides. (1) Air pollution by
sulfur oxides, initially and mainly sulfur dioxide, is critical because of its
damaging effects on plant life, impairment of air clarity, damage to struc-
tural materials via corrosion of metals, and deterioration of Portland
cement, dimension stone, paper, leather and textiles. There is also, and
more alarmingly, a strong correlation between human death rates and periods
of heavy sulfur dioxide air pollution. These death rates are most significant
among individuals with histories of respiratory, heart and circulatory disease,
particularly infants and the elderly. (2)
The most prevalent source of sulfur dioxide air pollution is from the
stack gas from thermoelectric power plants. These plants burn coal and
petroleum fractions high in sulfur content. An increase in the amount of
these fossil fuels burned for power can be expected to continue in the future.
The critical dependence of the nation's total life and economy on a rapidly
growing supply of electric power demands that all fuel resources be utilized.
A large fraction of fossil fuel (coal) has a significant sulfur content.
The release of sulfur bearing waste gases also represents a loss of
an otherwise very useful raw material, sulfur. This loss exceeds the
amounts of. sulfur produced in the U.S. from the usual sources. As power
production increases, this source of air pollution will increase at even a
greater rate because of the need to use lower grade or more available fuels
of higher sulfur content. Other contributors to sulfur dioxide air pollution
are major sources in some localities, but their total contribution is far less
than that of the power plants. Smelters, petroleum refineries, pulp mills,
sulfuric acid manufacturing plants, and other chemical industries are classic
examples of such contributors.
BATTELLE-NORTHWEST
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2
There is no established technology today for assuring the efficient
removal of sulfur dioxide from power plant stack gases without either imposing
a severe economic burden on the industry or raising the pollution levels, for
instance, of waste water or in the disposal of additional solid wastes.
In recognition of the seriousness and magnitude of the sulfur dioxide
pollution problem, inherent in power plant stack gases, the National Air
Pollution Control Administration has initiated support of a number of studies
on the development of new processes for the removal of sulfur dioxide from
industrial waste gases, specifically coal burning, power plant, stack gases.
This report covers such a study made over the period of May 15 to
December 13, 1968, as Contract No. PH 22-68-19.
BATTELLE-NORTHWEST
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3
SUMMARY AND CONCLUSIONS
The technology for the removal of sulfur dioxide from smelter gases
by use of an organic liquid (dimethylaniline) is well established in the United
States. Two large plants have been operating for about 20 years, one in
California and one in Tennessee. No such technology, however, exists for
similar treatment of thermal power plant (coal or oil fired) stack gases.
The magnitude of the engineering and economic factors for power
plant stack gas treatment via organic liquids is enormously different from
smelter gas treatment in volumes and composition of the gases to be handled,
the effectiveness of SO 2 removal to meet allowable residual concentrations,
and the critical dependence on extremely efficient recovery of the organic
scrubbing agent.
Several prospective organic liquids have been noted. However, essen-
tial data which firmly suggest their applicability as suitable scrubbing agents
are lacking. The classes of organic scrubbing agents include hydrocarbons
(including olefins), esters, ethers, ketones, alcohols, amines, amides,
nitro and sulfo compounds. Some candidates are 2, 4--dimethylpyridine,
N ,N-dimethylaniline, triethanolamine, N ,N-dimethylacetamide, and
tetraethylene pentamine.
The most critical property of a candidate organic liquid sorbent which
establishes its suitability for removal of S02 from power plant stack gases
is its vapor pressure or volatility. In view of the enormous volumes of gas
to be processed, and even at relatively low temperature, a material generally
acceptable for its low vapor pressure could still be involved with intolerable
economic losses because of volatility.
The candidate organic liquids, from an engineering or process stand-
point, are sufficiently similar to enable the assessment of general applicability
by study of anyone on which the most data exist. Dimethylaniline and
triethanolamine are typical candidates even though dimethylaniline has far too
high a vapor pressure for power plant stack gas treatment.
BATTELLE-NORTHWEST
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4
Methods of contacting the gas with the scrubbing agent could be via
venturi, cyclone, spray or grid systems. The grid systems are strongly
preferred from the standpoints of cost and power requirements.
Thermal stripping is concluded to be the most acceptable method of
regeneration. Reagents employed to form displacement compounds wh ich,
in turn, must be treated chemically to recover the organic agent appear to
be too complex and costly. However, geographical considerations may
necessitate conversion of the sulfur concentrate (802) to a more marketable
form such as elemental sulfur.
Cooling of stack gas will be required for any organic scrubbing pro-
cess. If a visible steam plume is not tolerable, reheating will be required.
However, adequate plume dispersion could probably be achieved without a
major reheat requirement by increasing gas velocity in the stack.
The potential for increased pollution caused by injection of intolerable
amounts of unrecovered sorbent into the atmosphere must be resolved for
any organic scrubbing system. In addition, the potential operational hazards
of flammability and explosiveness must be factored into the choice of an
organic scrubbing agent.
From an optimistic viewpoint, given adequate equilibrium data with
minimum sorbent degradation and minimum autocatalytic oxidation of 802
to 803 in the system, a process economically competitive with other scrub-
bing processes could probably be achieved by the use of rather conventional
process equipment. Under such assumptions, problems of geography or
environment and marketability of the recovered sulfur bearing product would
be as important as the economy of the process in determining the choice of
process and scrubbing agent. However, the obtaining of unfavorable data
on sorbent degradation, 802 oxidation, or pollution aggravation by the
release of objectionable quantities of the sorbent to the environment might
require elimination of organic scrubbing as an applicable means in the
development of processes for the removal of 802 from flue gases.
BATTELLE-NORTHWEST
-------
r-- -
5
RECOMMENDA TIONS
In order to achieve a realistic appraisal of the applicability of
organic liquids as sorbents for S02 stack gases, experimental work in
accordance with the following outline is suggested:
. Develop necessary equilibrium data for representative sorbents
under flue gas compositions and conditions.
. Determine realistic vapor pressure and entrainment losses.
. Determine degradation or oxidation properties of representative
sorbents.
.
Determine the extent of autocatalytic oxidation of 502 to 503 in the
sorbent system.
Develop means for minimizing losses.
Establish, in reactions common to the proce ss, the role of the
following major gas constituents: oxygen, nitrogen, nitrogen oxide,
carbon dioxide, carbon monoxide, and sulfur trioxide.
Develop the regeneration process.
Establish the process flow sheet (material balance).
Scout the applicability of likely sorbents selected on the basis of
cost, availability, and desirable chemical, physical, and nonpollution
properties, and possibilities for integration with the overall power
plant function. Candidates might include polyethylene glycols, and
the related amines, crude carbohydrates, and crude petroleum
fractions (olefins).
.
.
.
.
.
.
In this phase of the study, a critical evaluation should be made of
the potential atmospheric pollution resulting from the use of organic
scrubbing agents for S02 removal from industrial waste gases.
OBJECTIVE
The objective of this phase of the study was to survey the literature
and, on the basis of findings, to assess the applicability of organic liquids
to the development of new processes for removing sulfur dioxide from
fossil fuel fired power plant stack gases.
BATTELLE-NORTHWEST
-------
.
-~-- ~---"- -.
6
SCOPE OF WORK
The literature search was made to establish the most promising
classes of liquid organic compounds for sulfur dioxide removal and recovery.
Individual compounds considered most promising were also identified.
The search also extended to the process engineering field to indicate
the preferred methods of contacting the sorbent with the flue gas and the
preferred technique of sorbent regeneration and recovery of sulfur values.
A preliminary assessment of the applicability of organic liquids for
cleaning both smelter effluent and power plant flue gases was made J and
conditions required to assure adequate effluent gas plume dispersion were
reviewed.
Economic factors important to the comparison of organic liquids as
scrubbing agents were reviewed, along with other means of sulfur dioxide
removal. A compilation of pertinent literature references reviewed in the
course of this study was completed and is attached as Appendix B to this
report.
Experimental laboratory work to provide data required for adequate
assessment of the engineering and economic potential of promising organic
liquids is suggested.
BATTELLE-NORTHWEST
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7
DISCUSSION
ORGANIC LIQUIDS AS SCRUBBING AGENTS
Present Status
No evidence indicating the use of organic liquids on any scale for
routinely removing the sulfur dioxide from power plant stack gases has been
established. However, two sulfide ore smelters in the United States have
been using dimethylaniline routinely on a large scale for about 20 years to
scrub sulfur dioxide from a portion of their stack gases. The American
Smelting and Refining Company plant at Selby, California (3) operates pri-
marily on lead ores. The Tennessee Copper Company plant at Copper Hill,
Tennessee, operates on both pyrite and copper ores. Both companies market
the recovered product as liquid sulfur dioxide. In addition, both companies
produce sulfuric acid from their stack gases.
In Germany, (3) xylidine (or toluidine) has been used as a scrubbing
agent in one copper smelter and in one Portland cement - - sulfuric acid --plant
(via reduction of gypsum).
There are references to similar or modified applications of these
organics to smelter stack gases in other countries, but the certainty of
current commercial scale operations on a routine basis was not established.
Although no evidence of organic scrubbing of power plant stack gases
has as yet been found, aqueous treatment has been applied in Europe. Air
pollution abatement action against power plant stack effluents is just begin-
ning in the United States. Controls thus far have been limited to specifying
the sulfur content of fuels which are being consumed.
The enormous differences between the engineering and economic
problems in the treatment of power plant stack gases, and problems in the
treatment of smelter or chemical plant off gases should be acknowledged
early in this study. Smelters generally release gases rich in sulfur dioxide
and measuring several percent by volume. On the other hand, sulfur dioxide
content in the effluent gases from the highest sulfur-type fuels burned by
power plants should not exceed a few tenths of one percent. Whereas smelters
or chemical plants may release gases at thousands of cubic feet per minute,
BATTELLE-NORTHWEST
-------
8
the larger power plants may release millions of cubic feet per minute. The
required dispersal of spent fumes from smelters via relatively small
volumes from tall stacks is more assured than for power plants. The require-
ments for removing sulfur dioxide from stack gases thus can be expected to
be more stringent for power plants than for smelters. The engineering,
economics, and chemistry of power plant stack gas treatment therefore
can not be viewed as simply a scale-up problem from smelter gas treatment
technology. Instead, major problems are inherent in the assurance of the
engineering performance of all of the processes and equipment, the guaran-
teed performance of the chemistry and kinetics of the process, and the
economic penalties of off- standard efficiency. In addition, many organic
agents which might be employed could introduce new pollution problems
requiring solution.
Reaction Mechanisms, Classes and Candidate Organics
The S02 molecule has an O-S-O angle of 120°, S-O bond length of
1.43 A, and dipole moment of 1.6 x 10-18 e.s.u. in the gas phase. (4) It is
thus a small and strongly polarized molecule with a high positive charge
density on the S atom not sterically protected by a surrounding shell of other
atoms.
These features determine much of the chemical behavior of S02 with
organic liquids. The exposed electrophilic S atom is attracted by nucleophilic
centers in organic molecules, and its small size allows the S02 molecule to
approach such centers closely if they are not sterically protected. Sulfur
dioxide thus forms adducts with organic compounds containing ° and N atoms
possessing lone pairs of electrons. Such compounds include alcohols, ethers,
aldehydes, ketones, esters, acid amides, and amines. Olefins and aromatic
compounds, because of the pi electron cloud on the benzene ring, also form
adducts with S02. The dissolution of S02 in liquids of these classes is due
to adduct formation and, in some cases, precipitates of solid adducts can be
obtained.
In systems containing H20 a,s well as amines, S02 may react by a
mechanism other than adduct formation, viz., by formation of sulfites:
BATTELLE-NORTHWEST
-------
9
2RNH + H ° + SO - 2RNH _3: + S032- + H+
2 2 2
The small size of the S02 molecule also enables it to play the role
of guest molecule in clathrate compounds. Hydroquinone, for instance, forms
hydrogen - bonded crystals with a cage-like structure in whose vacant spaces
S02 molecules can be trapped if they are present when the hydroquinone
crystals are growing by precipitation from solution.
Symbols
The symbols to be used in the subsequent treatment are collected
and defined here for reference:
A
Approximate activity coefficient of S02 in liquid at infinite dilution,
1. P
1m -
x
x- 0
f
Fugacity of S02 in equilibrium with liquid
Fugacity of S02 in standard state
Number of S02 molecules per organic molecule in adduct
Partial pressure of S02 in torr
Partial pressure of S02 in atm
Temperature, °C
Mass of S02 dissolved in mass 100 of solvent
Mole fraction of S02 in liquid
fO
n
r
P
t
w
x
. Compilation of Equilibrium Data
The abstracts collected in the literature search were scanned for
references to S02 partial pressures in equilibrium with solutions of S02
in organic liquids. Most of the information gathered in this way was compiled
in uniform format for easy comparison, and is contained in Appendix A.
Information not included in Appendix A was rejected because of incomplete
reporting of data, because the S02 partial pressures were far higher than
those of interest in the present study, or because the liquids were much
too volatile. Also, Appendix A does not contain data on mixed organic-
aqueous absorbents.
BATTELLE-NORTHWEST
-------
10
The quantity A defined in the preceding list of symbols is useful for
comparing the otherwise unwieldy collections of p-w-t data for different
liquids. It is a close approximation to the activity coefficient of S02 in solu-
tion at infinite dilution. The exact definition of this activity coefficient is
f/ xfo. If the standard state of S02 is chosen to be the ideal gas at unit fugacity,
the foregoing expression reduces to fix which, in turn, tends to Pix as P-o.
Values of A were determined by plotting Pix against x and extrapolating the
graphs to zero x.
Tables 1 and 2 show the values of A for compounds grouped according
to molecular structure. Values of A less than unity at room temperature are
listed in Table 1, those greater than unity in Table 2.
Correlation of Activity Coefficients with Molecular Structure
The smaller the value of A, the stronger is the affinity of a liquid
for S02' According to the meager published data, the types of compounds
listed in Table 1, particularly heterocyclic amines, show more promise as
S02 absorbents than do those in Table 2. However, the compounds listed in
Table 2 are too limited to allow the definite conclusion that their types do
not include good S02 absorbents.
It is interesting to examine the effect on A of replacing H atoms by
alkyl groups. For the series aniline, N - methylaniline N ,N -dimethylaniline,
for instance, the values of A at 25° are 0.41, 0.17, and 0.062. It is well
known in organic chemistry that an alkyl group entering a molecule increases
the electron density in the rest of a molecule by replacing hydrogen. The
progressive decrease in A for 0, 1, 2 methyl groups on the N atom supports
the view that the positively charged S atom of S02 is attracted by the nega-
tive charge on the N atom of the amine. For the series aniline,
N-ethylaniline, N,N-diethylaniline, the values of A at 25° are 0.41,0.29, and
0.8. The anomalously high value of A for N ,N-diethylaniline may be due
to partial steric blocking of the approach of S02 by the two ethyl groups. The
pairs of compounds N ,N - dimethylformamide, N, N -dimethylacetamide
(A = 0.43,0.11) and 2-methylpyridine, 2,4-dimethylpyridine (A = 0.08,0.05)
also show the expected effect of replacing H by CH3'
BATTELLE-NORTHWEST
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11
TABLE 1. Activity Coefficients at Infinite Dilution -
Low Values
Compound Type Compound t A
Substituted N ,N - Dimethylacetamide 25 O. 11
acid amide CH3CON(CH3)2 38 0.24
66 1.0
93 2.8
N ,N - Dimethylformamide 25 0.43
HCON(CH3)2 38 0.48
66 0.80
93 1. 46
Sulfoxide D imethy lsulfoxide 20 O. 104
(CH3)2S0
Ether Tetraethylene glycol dimethyl 25 0.18
ether 38 0.38
CH30C2H40C2H40C2H40C2H40CH3 66 1.4
93 3.5
Heterocyclic Quinoline r;o 25 0.07
amine 2-Methylpyridine o-CH3
30 0.08
N~
2, 4-Dimethylpyridine CH3 30 0.05
N
Aromatic Aniline Q-NH2 25 0.41
amine
N - MethYlanilin"BNHCH 3 25 0.17
N-Ethylaniline NHC2H5 25 0.29
N J N -Dimethylaniline 15 0.02480
Q N(CH3)2 20 0.03895
25 0.061
N,N-DiethYlanilineQ N(C2H5)2 40 0.186
25 0.8
1- Methylaniline O~~2 25 O. 4( 4)
2- Methylaniline Q-NH2 15 O. 17
25 O. 30
3
BATTELLE-NORTHWEST
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12
TABLE 2. Activity Coefficients at Infinite Dilution -
High Values
Compound Type Compound t A
Ketone 2-0ctanone CH3CO(CH2)5CH3 25 2.0
Ester Ethyllaurate CH3(CH2)10COOC2H5 25 2.7
Alcohol 1-Heptanol CH3(CH2)5CH20H 25 6.
Nitro compound Nitrobenzene 0 N02 25 3.
Aromatic Dicumylmethane (mixture of isomers) 25 1.7
hydrocarbon (CH3) 2CH 0 CH20 CH(CH3) 2 40 2.8
Ditolylmethane (mixture of isomers) 25 1.7
CH30 CH20CH3 40 2.3
The methyl group is only weakly electron donating in comparison with
the OH and NH2 groups. (5) If the foregoing interpretation of the effect on A
of introducing CH3 groups is correct, then the introduction of OH and NH2
groups should strongly increase the 802 affinity of nucleophilic centers in
organic molecules. This expectation is verified by results reported( 6) for
tetraethy lenepentamine, triethanolamine, pentahydroxyethy 1- die thy lenetri-
amine, and hexahydroxyethyl-triethylenetetramine. Triethanolamine, for
instance, with an A value of about 0.02 at 100°, indicates an enormously
higher affinity for 802 than do the c~mpounds in Table 1.
Evaluation of Practical Utility of Liquids as 802 Absorbents
A typical 802 content of 0.3% in boiler flue gas at 1 atm total pressure
corresponds to 2.3 torr. For smelter off-gas, 3% is a typical 802 content,
so that 90% removal of 802 from the gas would reduce the 802 partial pres-
sure to 2.3 torr. The value of w in equilibrium with p = 2.3 torr is thus a
rough practical measure of a liquid IS utility as an 802 absorbent. Liquids
with small values of A have been selected from Table 1 and listed in Table 3,
together with values of w in equilibrium with r = 2.3 torr at the temperatures
noted. These values of w were obtained from graphs P Ix against x, or r
against w. While these data provide a measure of an agent's capacity for
802 absorption, a much more rigorous engineering analysis of equilibrium
data between gas inlet and exit conditions would be necessary to assess
applicability of the agent for flue gas scrubbing.
BATTELLE-NORTHWEST
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13
TABLE 3. Sulfur Dioxide Capacities of Liquids When
Partial Pressure of S02 is 2.3 Torr
Compound t w
N ,N - Dimethylacetamide 25 1.8
Dimethylsulfoxide 20 2.4
Tetraethylene glycol dimethyl
ether 25 0.5
Quinoline 25 1.9
2 - Methylpyridine 30 2.5
2 , 4 - D imethy lpyrid ine 30 2.9
N -Methylaniline 25 1.1
N , N - D imethy Ian iline 25 2.5
Dissociation Pressures of Solid Adducts of S02 and Organic Substances
Table 4 shows the partial pressures of S02 in equilibrium with some
solid adducts with organic substances. The organic compounds marked with
asterisks are solid at room temperature. Their values of r are listed, but
their adducts could possibly be prepared by precipitation from solution in
organic liquids so that they fall within the scope of this study. Again, much
more data, particularly equilibrium data in the inlet and exit range of condi-
tions, are necessary to assess applicability of the agent for flue gas scrubbing.
Selection Criteria
The following paragraphs highlight selection criteria which are
reviewed in greater detail later on.
Background Data
It is concluded from data presented in the preceding section that not
nearly enough information is available to make a firm selection of a candidate
organic scrubbing agent. However, the available data do provide a starting
point in indicating appreciable capability of certain agents or classes of
organics for sulfur dioxide absorption, and that many form rather loosely
bound compounds or adducts from which the S02 can probably be released
by heating or steam stripping.
BATTELLE-NORTHWEST
-------
14
TABLE 4. Dissociation Pressures of S03-0rganic Adduct
Compound
Aniline 0 NH 2
1- Methylaniline 0
n t r Ref
---
1 25 43.0 7
1 25 48.2 8
1 25 323 8
1 20 11 8
1 25 45 8
1/2 25 4.0 8
1 25 17.0
2 50 19.0 8
2 25 6.0 8
2-Methylaniline 0
CH3
3-MethYlaniline>:,CH3-0 -NH2
Quinoline 00
N NH2 NH2
1,2-Diaminobenzene>:'O
1,4-Diaminobenzene>:' H2N 0 NH2
4,41- Diaminobiphenyl>:'
H2N ~ NH2
Hydroquinone>:' t HO-O -OH
NH2
CH3
NH2
Unknown
25
3.8
9
>:'Solid at room temperature.
tS02 adduct is a clathrate.
A vailability and Cost
Any extensive program of S02 removal from power plant flue gases
might require several major additional production facilities to supply suffi-
cient amounts of any organic material approved for use. It is even doubtful
that adequate raw material supplies of rp.any agents could be provided in the
. event of a concentrated demand by a substantial fraction of the power industry.
Coupled with this limitation is the obvious cost disadvantage. With
few exceptions, most pure organics are costly. Most pure organics except
for a few low molecular weight alcohols, the ketones, crude carbohydrates, ,
fats, and crude petroleum fractions range well above 10 and even 20 cents a
pound, with many well above a dollar a pound even in tank car quantities.
The inventory requirements in such materials alone could range into millions
BATTELLE-NORTHWEST
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15
of dollars of investment. It is also unlikely that the production of any non-
volatile pure organic, involving the introduction of special groups such as
hydroxyl, amine, sulfur, or combinations of these, can ever be inexpensive
regardless of production levels. These conclusions point to the requirement
for a low cost material and for extremely low process losses.
Physical and Chemical Properties
An organic suitable for S02 scrubbing, aside from having good sorbent
capacity for S02' must be extremely stable chemically in the environment of
use. It must no degrade readily to nonreusable forms or form stable S02
complexes. In addition, if it is a liquid, it must stay as a liquid and not form
solid intermediates. For reasons of economy and in order to simplify its
recovery and reuse, its vapor pressure must be very low.
In addition to these physical and chemical property requirements, the
organic agent must form adducts or compounds with S02 that are easily decom-
posed to yield the sulfur product in concentrated form and to yield regenerated
organic at very high recoveries.
Conditions of Use
It is rather obvious that the selected organic agent should be compatible
with the conditions under which it is to be used. The flue gas will contain
oxygen, carbon dioxide, and carbon monoxide, as well as sulfur dioxide,
sulfur trioxide, and nitrogen oxides as reactive components. Any of these
could contribute to the irreversible degradation of the organic. Organics
which could form explosive mixtures in a flue gas composition are, obviously,
eliminated. Finally, in considering contributions of the organic agent or its
degradation products to the overall pollution situation, any specific regula-
tions applicable to the geographical area of use must be known.
POTENTIAL SULFUR BEARING PRODUCTS
There appear to be four saleable sulfur bearing products
from power plant flue gases via organic scrubbing:
Sulfur Dioxide
Sulfur
recoverable
Sulfuric Acid
Ammonium Sulfate
BATTELLE-NORTHWEST
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16
Geography as related to markets is probably the major factor in
determining what product should be produced. Sulfur dioxide, although the
easiest and probably the cheapest sulfur bearing product obtainable via
organic scrubbing, has limited use at present prices. Sulfuric acid, perhaps
the most useful product, is already quite inexpensive from usual sources,
and thus cannot tolerate appreciable shipping costs from the producing plant
to the customer. Elemental sulfur may be regarded as the preferred product.
It is a solid of high purity and very stable under the simplest storage condi-
tions, (usually outdoors unprotected from weather). Potential markets for
sulfur, because of economical bulk handling in open railroad cars and barges,
are not limited by shipping costs. Ammonium sulfate, an important material
marketed worldwide as a bulk commodity, could be produced for sale as a
fertilizer. Ammonia, however, would be required as an additional and costly
raw material. The sulfate ion under some soil conditions is beneficial. In
the form of ammonium sulfate, however, it serves principally as the means
of providing a stable, solid, readily handled form of ammonia nitrogen.
Other ions such as nitrate could also be used and, in many situations, with
greater advantage. Thus ammonium sulfate is probably a desirable means of
disposing of S02 but only under special circumstances which could limit its
marketability.
Of the four potential products, elemental sulfur would be the most
marketable and sulfur dioxide the easiest to produce.
The equivalent daily outputs and value (at current prices) of each of
these potential products recoverable (at 90% yield) from the flue gas (0.30/0
S02) from a 1400 MWe power plant would be about as follows:
800 tons S02 @ $75/ton = $60, OOO/day
400 tons sulfur $37/ton = $14, 800/day
1200 tons sulfuric acid $35/ton = $42, OOO/day
1650 tons ammonium sulfate $23/ton = $38, OOO/day
Elemental sulfur while representing the lowest value per day, is
probably the only one of these potential products readily marketed from almost
any location. A market for S02 at current prices and current high output
BATTELLE-NORTHWEST
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17
does not seem possible. This product would have to be priced (on a delivered
basis) at appreciably less than half the present price to make it competitive
with elemental sulfur for sulfuric acid manufacture. Sulfuric acid would
have to be priced to allow for shipping costs to make it competitive. Since
two-thirds of the value of ammonium sulfate is represented by the ammonia
content (at $60/ton), this product has the least value as an outlet for
recovered sulfur.
The sulfur- bearing products marketable from a power plant flue gas
treatment process thus can not be readily determined and will require a
more detailed analysis.
METHODS OF CONTACTING FLUE GASES WITH SCRUBBING AGENTS
The major characteristic of any process for scrubbing power plant
stack gases is the capability for handling high amounts of gas. Compared to
normal petroleum and chemical industries, the contact required may be
relatively incomplete. Major potential costs entailed in the scrubbing
process itself include:
. Interest on the inventory of organic liquids required in the process.
. Organic losses resulting from degradation and volatility.
. Interest, depreciation, and maintenance on the scrubbing facility.
. Cost of operating pumps and fans.
The most economic methods of contacting would most likely be via
various types of grid towers. Their higher power requirements limit con-
sideration of Venturi and cyclone scrubbers. Performance data on the use
of devices for scrubbing industrial boiler stack gases already exist. The
pulp industry uses these and similar devices as "direct contact evaporators"
where they concentrate an aqueous organic (black liquor) and, if operated
correctly, scrub hydrogen sulfide out of the stack gas.
Aside from the volume of the flue gas to be handled, nothing particu-
larly unique can be seen in the engineering of the flue gas contacting
process.
BATTELLE-NORTHWEST
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18
METHODS OF ASSURING ADEQUATE STACK PLUME DISPERSION
Regardless of the method finally used to remove sulfur dioxide from
power plant stack gases, the stripped gases must be released in a non-
objectionable manner. Therefore, the plume itself must be adequately dis-
persed, i. e., mixed with environmental air, before contacting the ground.
No foreseeable method of treatment could produce an effluent gas heavier
than air. The worst conceivable case could produce a plume at 125 of
saturated with a density equivalent to that of dry air at 120 of. Under these
conditions, the plume would necessarily still rise. Use of a higher stack
might be necessary in order to compensate for the loss of buoyancy, but the
added height would not be more than about 5 stack diameters in the most
severe cases.
The plume itself could cause a problem, however. Should the plume
be discharged while saturated with water, a dense fog obscuring visibility
and constituting a hazard to modern high speed travel, both surface and air,
could result. Several methods for avoiding this problem seem to exist and
a competitive evaluation of the alternatives would seem to be in order,
possibly as a separate program.
Gas must be exhausted from the stack at a temperature substantially
above its dew point to prevent the formation of dense fog. Possibilities
include:
.
Cooling the gas leaving the power plant through a second economiser
before scrubbing the sulfur dioxide from it. The heat 50 collected
could be used to reheat the scrubbed (therefore adiabatically saturated)
gas prior to its release.
Cooling the gas leaving the power plant before it enters the scrubbing
system by using ambient air on the cool side of the economiser. The
heated ambient air could then be mixed with the scrubbed stack gas
.
.
prior to its release.
Cooling the gas as described in the method immediately preceding,
except that the heated ambient air and the scrubbed gas would be
released in two concentric stacks with the heated ambient air in
the annulus.
BATTELLE-NORTHWEST
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19
. Dehydration of the stack gas prior to release, e. g., by scrubbing
with a hydro scopic liquid such as concentrated sulfuric acid.
. Reheating by direct flame.
8, Reheating with steam coils using bleed steam from the turbines.
Other possibilities probably also exist. Of those methods listed, the first
four would actually reduce the amount o'f water vapor released. The first
three would reduce water vapor by lowering the temperature of the gas
entering the adiabatic saturation (and scrubbing) section, while the fourth
would remove water from the treated gas. Any of these operations, by
reducing the amount of water to be dispersed, probably possess an inherent
advantage over the last two. The relative merit of the alternatives, in order
of preference, would appear to be the first, third or second, sixth or fourth,
and fifth. However, some of these met~.o?s..might be inexpensive and adequate
in warm or dry areas of the country, ..while others would be more desirable
in cool or damp areas. Some stuQy of the effects of atmospheric conditions
on plume dispersion has been done. However, little has been done to charac-
terize the effect of plume modifications. Work in this area is needed and
will be useful to all industry regardless of the methods chosen to remove
S02 from power plant stack gases.
"
ORGANIC REGENERATION
There appears to be no possibility that the organic-sulfur dioxide
combination produced from the stack gas scrubbing process might be salable
as a valuable chemical. Thus, the organic must be recovered in a form
suitable for reuse. Even a material available at a price as low as 59/lb
(e. g., raw sugar) would be too expensive to use on a "once through" basis.
Both the efficiency of recovery required and the cost of recovery allowed will
vary with the costs of the rest of the process and the cost of the compound
used. Heat, chemicals, or electricity are possible "ingredients" required
by the recovery process.
Use of heat is potentially the cheapest means of recovery. Steam at
509 per million Btu's is approximately the cost of generation. Turbine bleed
steam should be available at lower cost such as:
Steam at 150 psig (365 OF) = 259/106 Btu's
Steam at atmospheric pressure = 159/106 Btu's
BATTELLE-NORTHWEST
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20
Most organic liquids amenable to regeneration by heat would be
regenerated by volatilizing a mixture of water and sulfur dioxide away from
the organic, essentially a process of steam-stripping the organic. This
could be done in a fractionation tower such as used in petroleum refineries
to remove substantially all organic in the overhead and obtain the desired
organic to water ratio in the regenerated liquid leaving the bottom of the
tower. This approach would also serve to remove any volatile products
produced by decomposition of the organic. These decomposition products
could be forced out with the 802 and water leaving the top of the fractionating
tower, although their removal as a liquid" side stream" should also be
possible in most cases.
The organic may undergo some decomposition in both the scrubbing
and regeneration sections. The decomposition products may constitute Qr
may form volatile or nonvolatile materials or, more likely, both. They
must, therefore, be removed. The volatiles will be treated as described in
the foregoing if heat is used for regeneration. One obvious method of remov-
ing the nonvolatiles (tars) would be to evaporate a portion of one of the organic
streams in an "agitated thin film evaporator" such as is used to evaporate
paraffin from still bottoms in the petroleum industry. The vapor stream
from this still could be passed into 'a fractionating column for removal of
volatiles not automatically removed at some other part of the process. The
decomposition products are presumed to be of no value and could be disposed
of by burning along with the usual fuel.
The use of electricity to regenerate the organic is conceivable for
some cases. The practical difficulties and the state of the art, however,
mitigate against serious consideration of such processing. The state of the
art is not generally well developed except for a few specific products. The
application of electrical energy to chemical reactions is neither cheap nor
efficient. The reduction of aluminum may be taken as an example. The
power theoretically required is 2.3 kW-hr/lb, but operating plants actually
required 10 kW-hr/lb. The cost of applying the 10 kW-hr/lb power is about
1 c; /kW - hr plus the cost of the power itself.
BATTELLE-NORTHWEST
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21
The use of chemicals to regenerate the organic liquid is impaired by
the low value of the sulfur which must be removed and the high cost of any
reagents required. Although sulfur has increased in price lately and further
increases are possible in the future, it is still a cheap, large volume, bulk
material. For this reason, recovery of sulfur a's a salable salt, a sulfate for
instance, is limited to salts of very cheap cations, e. g., sodium or, possibly,
ammonium. The advantage gained from sale of a more expensive salt would
be more than offset by the cost of the cation required, regardless of form,
and the expenses associated with losses and interest on inventory.
The use of sodium as a cation would be limited to regions having a
good market for sodium sulfite, or sulfate and a plentiful cheap supply of
some sodium salt of a cheap and basic anion, probably sodium carbonate
(soda ash).
The major markets for sodium sulfate are the Kraft pulp industry,
located in Washington, Oregon, Maine, and the south-eastern coastal states,
and the synthetic detergent industry. The Kraft industry uses it as a makeup
chemical and it could accept a crude sulfate-sulfite mixture. Unfortunately,
the entire country uses only about 5000 tons per day. This market could be
filled by the sulfur recovered from 4000 MW of coal fired electric power
production. The synthetic detergent market, perhaps smaller in size,
requires a clean, high quality sodium sulfate. The existence of adequate
suppliers of high quality by-product sodium sulfate from a number of other
industries does not indicate a strong possibility for beneficial disposal of
recovered sulfur dioxide by this means.
Ammonium sulfate is also a possible product, although the ammonia
in the product would be more valuable than the sulfur. Assuming the cost of
ammonia can be borne and losses of ammonia minimized, the major problem
would lie in producing a product capable of competing in the fertilizer market.
Most of the sulfur, removable from the stack gas as a sulfite, would be
converted completely to sulfate because the sulfite ion is poisonous to plants.
If this difficulty could be overcome, the ammonium sulfate could be used as
fertilizer in a world -wide market. Unfortunately, the high cost of the ammonia
BATTELLE-NORTHWEST
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22
required for such production and the trend toward higher nitrogen concentra-
tions in fertilizers mitigate against the economic production of this compound
as the product.
Calcium sulfate (gypsum) from a chemical regeneration step is
another product of very limited value. The "chemical" pu rchased would
probably be calcium carbonate (limestone) and it would probably be used
"as is", although it might be advantageous to convert it to quicklime or
slaked lime before use. The calcium sulfite -sulfate mixture could probably
not be sold. It is insoluble, however, and could probably be disposed of by
dumping or used as land fill.
In summary, regeneration of the organic in a form suitable for reuse
1S mandatory and a heating process appears to be the best approach. In most
cases the use of heat would recover the sulfur in a form amenable to conver-
sion into elemental sulfur (or sulfuric acid, where there is a market). This
approach is necessary because only the market for elemental sulfur appears
large enough to accept the amount produced in the event a major fraction of
the country's power industry were to convert to a sulfur recovery scheme.
Elemental sulfur is also the easiest and cheapest material to transport and
store.
If heat cannot be used, the use of limestone, with or without burning
to quicklime, appears the only solution. The "product", mixed calcium
sulfite- sulfate, would have to be dumped. Other materials could and might
be used in specific instances. However, the market for sodium sulfate, for
example, is small in respect to the total amount potentially available. The
production of ammonium sulfate (fertilizer) of suitable quality involves major
economic problems in use of large quantities of a costly raw material
(ammonia) which must subsequently be marketed at a price permitting the
recovery of raw material and processing costs.
APPLICABILITY OF ORGANIC LIQUIDS
The applicability of organic liquids to the removal of S02 from flue
gases is explored in the following subsections. The use of organic liquids
BATTELLE-NORTHWEST
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IL_- --
23
in general and the suitability of specific organic liquids are discussed in
detail. Primary emphasis .is on the use of organic liquids to remove S02
from the flue gases from fossil-fired power plants. The last .subsection is
devoted to S02 removal from smelter gases.
General Considerations
As discussed in earlier sections of this report, many organic liquids
have the ability to remove S02 from flue gases. However, other physical
properties and characteristics of organic liquids must be considered before
applicability can be established. For example, most organic liquids have
appreciable vapor pressures at desirable operating temperatures. Since
most organic liquids are fairly costly, evaporation losses and recovery
requirements must be considered. Also, many potential organic liquids are
extremely toxic and odorous and these features make evaporation losses and
recovery requirements even more important in determining the applicability
of individual organic liquids. Other important considerations include the
S02 loading, viscosity, oxidation or degradation losses, type of by-product,
cost, and availability. Unfortunately, information on many of these items
is not available for many organic liquids. However, available data on poten-
tial organic liquids are compared in subsequent subsections.
As has been stated earlier in this report, no process using an organic
liquid to remove S02 from the flue gases from power plants was found during
the course of this study. Two processes using organic liquids have been used
to remove S02 from smelter and chemical processing gases. One process
using anhydrous N, N -dimethylaniline (DMA) was developed by the American
Smelting and Refining Company and is currently in use in this country. (10-12)
The other process is called the Lurgi Sulphidine process and was developed
and used in Germany. (10-11) The Lurgi process employs a suspension of
xylidine or toludine in water. Neither process has ever been commercially
used at the dilute S02 concentrations occurring in power plant flue gases. The
dimethylaniline process operates on a smelter gas containing 4 to 6% S02' and
the exit gas is discharged to the atmosphere at only about O. 05% SO 2' In both
processes, a cold aqueous solution of dilute H2S04 is used to recover organic
BATTELLE-NORTHWEST
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24
vapors from the gases leaving the absorption towers. In both processes,
the organic absorbent is regenerated by steam stripping. S02 is the recovered
product. Either process may be applicable to removal of S02 from power
plant flue gases. However, flue gas cooling and equipment for recovery of
organic vapors from the flue gas would be required. Also, the literature on
both processes refers to an autocatalytic oxid.ation of S02' especially at low
concentrations. This phenomenon must be the subject of extensive laboratory
investigation in any study of the applicability of these and other organic
scrubbing agents.
A major example of the use of organic liquids to treat flue gases is
the commerical recovery of C02 from combustion gases by the use of
aqueous ethanolamine solutions. This process was developed in the early
1930's by the Girdler Corporation and is called the Girbotol process. (13-14)
. .
Currently, monoethanolamine is used in preference to either diethanolamine
or triethanolamine, primarily because of its higher absorption capacity for
C02' One objection to the use of ethanolamine solutions is their corrosive-
ness due to their oxidation to glycine and oxalic acid. (13) lVIonoethanolamine
is much less susceptible to oxidation than the di- and tri-compounds. Also,
data from existing plants indicate that monoethanolamine suffers degradation
losses as a result of irreversible reactions with C02' (15) Study of the C02
degradation reactions shows no likelihood of similar reactions with
triethanolamine. Other problems associated with the Girbotol process
include fouling of solutions by sludge, foaming, and thiosulfate accumulation
m solutions. (14)
The main purpose of mentioning the Girbotol process at this time is
its importance in indicating potential problems for S02 absorption from com-
bustion gases by organic liquids. For example, C02 is present in much
greater quantities than S02 in combustion gases. The C02 could interfere
with S02 absorption in some organic liquids and will absorb simultaneously
with S02 in most organic liquids. Thus, the by-product could be contaminated
with C02 or carbonates. Some organic liquids will suffer degradation losses
from C02' S02' or oxides of nitrogen. Oxidation losses will also occur
because of the oxygen in the combustion gases. Experimental data on C02
interference and on oxidation and degradation losses will be very important.
in assessing the potential of organic liquids.
BATTELLE-NORTHWEST
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25
Properties of Organic Liquids
Costs and various other characteristics of potential organic liquids
are compared in Table 5. These items are important in comparing potential
organic liquids and assessing the potential of each. Many of the probable
reasons for the use of N, N -dimethylaniline (DMA) today for removing 502
from smelter gases are readily apparent. DMA has a lower cost than most
other liquids in the table, has a reasonably high 502 capacity (at smelter
. gas concentrations), and can be easily regenerated. The vapor pressure of
DMA is reasonably low at the temperatures of 20 to 25°C employed in
smelter gas treatment, and a salable product (502) is recovered. A similar
inspection of the tabulated information shows why xylidine and toluidine have
been studied extensively and used in the Lurgi process.
The tabulated information can also be used to make a preliminary
assessment of potential organic liquids for 502 absorption from combustion
gases. Inspection of the vapor pressure data in Table 5 shows why
triethanolamine (TEA) and tetraethylenepentamine (TEPA) have received.
considerable attention as potential organic liquids for high temperature
absorption of 502 from combustion gases. (16) The low vapor pressure at
high temperatures results in less evaporation of organic liquid during the
absorption step, and in reduced requirements for recovery of organic vapors.
However, other items in the tables, such as lack of a regeneration process
and cost of TEPA indicate the need for much more experimental information
before an accurate assessment of the potential of these two organics can be
made.
In the absence of conclusive experimental data on the performance of
organic liquids in combustion gases, many organic liquids exhibiting obviously
poorer features or properties than DMA can be tentatively eliminated. DMA
is a logical IIbase point ", both because of the extensive information available
and its use on smelter gases. Thus, many of the organic liquids in Table 5
. .
can be tentatively classified as less promising than DMA by inspection of the
boiling point, vapor pressure at various temperatures, cost, and 502
solubility.
BATTELLE-NORTHWEST
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TABLE 5.
Comparison of Organic Liquids Having Promising S02 Solubilities
Approximate
S02 Solubility, (1) Vapor
Cost, Boilin& Pressure at
Compound g /1 OOg solvent $/lb Point, C 25°C, mm Hg
N, N -Dimethylaniline 2.5 0.22 194 0.6
N - M ethylaniline 1.1 0.70 196 0.4
N, N-Dimethylacetamide 1.8 0.40 166 0.9
Dimethylsulfoxide 2.4 (20°C) 0.33 100 (d.) 0.6
Quinoline 1.9 0.50 237 1 (60 "C)
2- Methylpyridine 2.5 (30°C) (4) 128.8 11
2,4-Dimethylpyridine 2.9 (30°C) (4) 159 3
T et raethy leneglycold imethy 1 ethe r 0.5 1. 35 275.3 0.015
Xylidine (mixed 0, m, p) ~7 (20 °CP) 0.44 ~220 0.35
Toluidine (0-) 0.4 0.22 -200
Triethanolamine N = 21.45(3) 0.22 360 0.042
A = 42.9(3)
T etraethy lenepentamine N = 86(3) 0.60 333 1 (1510C)
A=I72
I. S02 solubility at 25 "C unless specified and at S02 partial pressure of 2.3 mm Hg in flue gas.
2. S02 solubility in I: 1 xylidine:water mixture.
3. Maximum solubility at equilibrium; N = neutral salt (amine: 002 = 2: 1); A = acid salt (amine:002 = 1: 1>.
4. Cost probably greater than pyridine. Refined pyridine (2° cut) costs 0.55/lb.
5. Viscosity without water dilution of triethanolamine.
6. Not fully defined but probably heat.
7. According to scouting experiments, regeneration by distillation with H2S04 or by precipitation with
lime slurry may be chemically feasible when S02 is absorbed at room temperature.
Approximate
Viscosity, Regeneration
centipoise Process
1.28 (25°C) Heat
(6)
(6)
(6)
(6)
(6)
(6)
4.05 (200C) (6)
Heat
10.5 (100 0C)(5) (7)
Not developed I\J
en
Not developed
-------
27
The tabulation of viscosity data in Table 5 can also aid in preliminary
screening of potential liquids . Viscosity is an important property of the
liquid phase in gas absorption. As the viscosity of the liquid. phase increases,
absorption efficiency tends to decrease because the greater viscosity means
lower liquid diffusion coefficients and greater resistance to transfer in the
liquid. Thus, higher viscosity tends to indicate more expensive gas absorp-
tion equipment and a greater hold-up of liquid absorbent in the equipment.
For expensive organic liquids, increased liquid hold -up can be important.
The high viscosity of tetraethylene glycol dimethyl ether is an additional
drawback along with high cost and relatively low S02 solubility. In some
cases, such as TEA, the high viscosity must be reduced by diluting the
organic liquid with water or other low viscosity diluent. Dilution is most
applicable to liquids with a high S02 solubility.
Effects of Flue Gas Temperature
A major reason for considering organic liquids has been the hope of
developing a regenerative absorption process that does not require cooling of
the flue gases. Elimination of stack gas cooling has been considered desirable
(1) to avoid reheating the exit gas for improved buoyancy, and (2) to eliminate
the water plume that could result from an aqueous scrubbing process. Unfor-
tunately, most organic liquids exhibit appreciable vapor pres sures at flue
gas temperatures, and organic vapors are swept from the absorption equip-
ment with the exit gas. These vapors must be recovered by other additional
scrubbing processes because the cost or toxicity of the organic vapors would
most likely be intolerable. Thus, the use of organic liquids probably will
not eliminate the need for aqueous scrubbing of the flue gas. The ASARCO
dimethylaniline process, the Lurgi process, and the Girbotol process all
employ aqueous scrubbing to recover organic vapors from the exit gases.
The amount of organic vapor carried from the S02 absorption step is
shown as a function of operating temperature in Table 6 for several organic
liquids. The recovery efficiency required to reduce organic losses to
O. 1 mill/kW - hr are also shown along with the amount of organic discharged
after the organic recovery step. This information clearly show s the enormous
BATTELLE-NORTHWEST
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28
quantity of organic vapor that must be recovered from high-temperature
flue gas, and also shows the extremely high recovery efficiency that must
be attained for most organic liquids in order to avoid major economic
penalties. Values in Table 6 were calculated assuming a flue gas flow rate
.6
of 2.3 x 10 sefm from a 1400 MW power plant and a system pressure of
e
1 atm. The exit gas was also assumed to be. saturated with organic vapor
at equilibrium liquid temperatures of 77 and 200 "F at the gas - exit end of
the 802 scrubber.
Of the organic liquids examined, evaporative losses and recovery
requirements are lowest for TEA but recovery of TEA is still required at
high temperature (200 OF). Recovery will probably be desirable if TEA is
used at room temperature even though evaporative losses are fairly low.
As shown in data presented earlier in this report, the flue gas
temperature affects the solubility of 802 in organic liquids that do not form
a stable adduct with 802 at the temperature in question. As the temperature
increases, the solubility of 802 in the organic liquid rapidly decreases.
Unfortunately, little information is available on 802 solubility as a function
of temperature. Available equilibrium data for several organic liquids are
shown in Figure 1 as a function of temperature. These data show the
equilibrium solubility when the 802 partial pressure is 2 ~ 3 mm Hg in the
gas phase. The rapid decrease in 802 solubility at high temperature is
clearly shown. In practical terms, this reduced solubility means much
larger quantities of organic liquid and larger scrubbing equipment are
required at higher temperatures. For example, from Figure 1 the
solubility of 802 is 0.0011 mole 802/mole of N, N-dimethylacetamide at a
temperature of 200 of. Assuming this temperature and 802 loading for: the
exit liquid, the minimum possible liquid rate can be calculated from .the
inlet gas composition, gas flow rate, and degree of 802 removal. This
minimum liquid rate is calculated to be 10.6 x 106 gal/hr assuming an inlet
gas flow rate of 2.3 x 106 sefm, an inlet 802 concentration of 0.3 vol%,
and a 90% removal of 802. In gas absorption, the actual liquor rate is
usually greater than the minimum rate by 25 to 100%. However, the
theoretical minimum liquid rate is convenient to use for a preliminary
screening of potential solvents. The calculated minimum liquid rate is
BATTELLE-NORTHWEST
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TABLE 6.
Solvent Evaporation and Solvent Recovery Requirements
Solvent Loss Equal
Evaporation from Efficiency Required in the to O. 1 mill/kW -hI',
Organic Liquid Scrubber, 1000 lb/da~ Organic Recovery Section(3) lb/day(1)
77 °F(2) 200 °F(2 n"F 200 "F
-
N, N -Dimethylaniline 872 41,600 98.2 99.96 15, 270
N - Methylaniline 514 31,500 99.0 99.98 4,800
N, N-Dimethylacetamide 950 51,800 99.1 99.98 8,400
Quinoline 9,790 99.93 6,720
T et raethy lene glycol-
dimethylether 40 1,540 93.8 99.8 .2, 490
Xylidine(4) I:\.:)
492 78,400 98.4 99.99 7,640 CD
T . th 1.' (5) 2 34.8 None 56. 1 15, 270
rle ano amIne
1. For 1400 MW Power Plant.
e
2. Temperatures represent equilibrium liquid temperature at gas-exit end of S02
3. Required efficiency for O. 1 mill/kW -hI' solvent loss.
4. 1: 1 xylidine:water mixture.
5. 20 wt% TEA in water.
scrubber.
-------
O. 1
0.09
0.08
.... 0.07
c:
a;
>
'0
U)
a;
.....
o
E 0.06
--
N
o
(fJ
U)
a;
.'5'
E 0.05
.2
.....
E
;;j
.....
o
(fJ
N O. 04
o
(fJ
0.03
0.02
O. 01
o
30
502 Partial Pressure in Gas = 2. 3 mm Hg
N, N-Dimethylaniline
N, N -Dimethylacetamide
60
80
160
180
100
120
140
Temperature, 0 F
FIGURE 1.
S02 Solubility as a Function of Temperature
200
-------
31
impractical because of the large organic inventory and equipment required
to accommodate such flows. Since most organic liquids follow the capacity
trends in Figure 1, organic liquids that form stable adducts with S02 at
high temperatures will probably be the only ones exhibiting adequate S02
capacities at high temperature.
Flue gas temperatures will also affect the degradation of the organic
liquid in the scrubbing system. Degradation and the formation of corrosive
degradation products will increase as temperatures are increased in the
scrubbing and regeneration equipment. Degradation of organic liquids is so
important that it is discussed separately in the following subsection.
Oxidation and Degradation Effects
Degradation of the organic liquid can result from oxidation, thermal
decomposition at high temperature, or irreversible reactions with con-
stituents of the flue gas. Unfortunately, little information is available on the
rate of degradation of organic liquids at typical conditions for flue gas
scrubbing. However, many organic compounds have an increased tendency
to react with oxygen as the temperature is increased.
Available information on the oxidative degradation of monoethanolamine
(MEA) in C02 scrubbers and solvent regenerators under conditions of
nuclear submarine service provides some insight into the situation. (17) In
this work, oxidative degradation of MEA was studied as a function of
temperature under a variety of conditions. Experimental results showed
that, in air containing 10/0 C02' oxidative degradation increased as temperature
increased. Trace metal contaminants, such as copper, iron '. nickel, and
chromium, were found to catalyze the reaction. At 131°F, tetrasodium-
ethylenedinitrilotetraacetate (EDTA) was found to inhibit oxidation satis-
factorily even in the presence of catalytic metals. At 208 of with trace
metals present, both EDT A and the monosodium salt of N, N -diethanologlycine
(VFS) were needed for stabilization. Inhibitors were not effective at 280
and 300 of with only limited amounts of oxygen present. On: the basis of
these results, exposure of MEA solutions to temperatures of 280 of or
above in scrubber equipment is feasible only if oxygen can be removed
BATTELLE-NORTHWEST
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32
before exposure. Unfortunately, the limited amount of oxygen was not
defined, but the inference of severe oxidation at high temperatures in the
presence of oxygen is quite clear.
The experimental data on oxidative degradation of MEA are interest-
ing to consider in terms of the large inventory or organic required for 802
rem.oval from the flue gases of a large power plant. From the experih1ental
data, the MEA oxidation rate at 208 of, when no inhibitors or trace metals
are present, is calculated to be 0.0002 lb MEA oxidized/hr/lb of MEA
inventory. At this oxidation rate, an annual loss of 350, 000 to 1,3 00, 000 lb
would be sustained by MEA inventories of 400, 000 to 1,500, 000 lb,
respectively, if oxidizing conditions are encountered only half the time.
These degradation rates are not directly applicable to TEA or other organic
liquids used at high temperatures, but the potential magnitude of losses
emphasizes the importance of laboratory experiments on oxidation rates
and inhibitor requirements. Oxidation experiments on TEA are especially
important since the literature states that TEA is much more susceptible
than MEA to oxidation in combustion gases. (13)
Organic loss is not the only difficulty resulting from oxidative
degradation. Organic degradation products are frequently corrosive to
equipment, and these corrosive materials and trace metals from equipment
corrosion must be removed from the organic liquid. In most cases,
continuous distillation of a portion of the organic liquid will probably be
required in addition to normal regeneration. Distillation is used to purify
the ethanolamines when they are used to recover C02 from combustion gases.
The distillation step not only increases equipment and operating costs but
also provides another source of organic loss. These losses will occur as a
result of organic solubility and entrainment when the residues from the still
are discarded.
Degradation of MEA by C02 is an example of organic loss caused by
irreversible reaction with one of the constituents of flue gas. MEA losses
by C02 degradation have been reported by plants using MEA to remove C02
from hydrogen. (15) These losses are reported to be about 21 lb MEAl
100, 000 scf of C02 treated. For a 1400 MWe power plant, this degradation
BAT TEL.L E - NOR T H W EST
-------
33
I
I .
I
6
loss would mean a MEA loss of about 30 x 10 Ib/ yr at a plant factor of 80%.
This loss alone would eliminate MEA as a candidate for removing S02 from
flue gas. Ins pection of the degradation reactions for MEA show s that
similar reactions will probably not occur with TEA; however, the magnitude
of the MEA losses emphasizes the need for laboratory experiments on
possible irreversible reactions between promising organic liquids and
constituents in the flue gas. In this regard, further experimental work is
needed on the irreversible reaction between S02 and any of the promising
amines before their applicability can be established with certainty.
Solvent Emission Considerations
The control of solvent emissions is just starting to receive national
attention, (18) with detailed surveys of solvent emission having been
completed for the Los Angeles and San Francisco areas. Similar surveys
have been underway in New York and Chicago but the results are not known.
The Air Pollution Control Districts of Los Angeles County and the San
Francisco Bay Area have been actively working for many years with the
problems relating to solvent emissions. These efforts resulted in the
passage of Rule 66 and 66.2 in Los Angeles in July, 1966, and in the
passage of Rule 3 effective in the Bay Area in January, 1967. (19)
From an air pollution standpoint, the emission of organic vapors into
the atmosphere is objectionable because of the photochemical reactions that
can occur. Under the influence of sunlight, organic vapors react with
oxygen ozone and nitric oxide to form ozone, aerosol particles (smog), and
eye irritants such as aldehydes. Practically all organic vapors participate
in these reactions, but some compounds are much more reactive than
others.
The approach taken by Los Angeles and San Francisco to control
solvent emissions has been to divide organic solvents into two classes based
on susceptibility to photochemical smog-forming reactions. Although Rule 66
is very complex some basic provisions are briefly described in part as
follows:
a. A person shall not discharge more than 15 pounds of organic
materials into the atmosphere in anyone day from any article,
machine, equipment or other contrivance in which any organic solvent
BATTELLE-NORTHWEST
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34
or any material containing organic solvent comes into contact with
flame or is baked, heat-cured or heat-polymerized, in the presence
of oxygen, unless all organic materials discharged from such
article, machine, equipment or other contrivance have been reduced
either by at least 85 percent overall or to not more than 15 pounds
in anyone day.
b. A person shall not discharge more than 40 pounds of organic
material into the atmosphere in anyone day from any article,
machine, equipment or other contrivance used under conditions
other than described in section (a) for employing, applying, evaporat-
ing or drying any photochemically reactive solvent or material
containing such solvent, unless all organic materials discharged from
such article, machine, equipment or othe r contrivance have been
reduced either by at least 85 percent overall or to not more than
40 pounds in anyone day.
c.
For the purposes of this rule, a photochemically reactive solvent
is any solvent with an aggregate of more than 20 percent of its total
volume composed of the chemical compounds classified below, or
which exceeds any of the following individual percentage composition
limitations, referred to the total volume of solvent:
e. A combination of hydrocarbons, alcohols, aldehydes, esters,
esters or ketones having an olefinic or cyclo-olefinic type of
unsaturation: 5 percent;
e
A combination of aromatic compounds with eight or more carbon
atoms to tne molecule except etyhlbenzene: 8 percent;
e A combination of ethylbenzene, ketones having branched hydro-
carbon structures, trichloroethylene or toluene: 20 percent.
Wh.2n2ver any organic solvent or any constituent of an organic solvent
may be classified from its chemical structure into more than one of the
groups of organic compounds, it shall be considered as.a member of the
most reactive chemical group; that is, that group having the least allowable
percent of the total volume of solvents.
BATTELLE-NORTHWEST
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35
Rule 66.2 applies to the disposal and evaporation of solvents.
rule is as follows:
This
"A person shall not during anyone day dispose of a total of more
than 1-1/2 gallons of any photochemically reactive solvent or of any
material containing more than 1- 1/2 gallons of any such photo-
chemically reactive solvent by any means which will permit the
evaporation of such solvent into the atmosphere. "
Presumably, all organic solvents are photochemically reactive to
some extent, so the differentiation between exempt and nonexempt solvents
is a matter of judgement. The probable actions of other pollution
authorities on adoption of solvent emission controls and on the concept of
exempt and n.onexempt.solvents is not clear. In many cases, initial regula-
tions will probably differentiate between solvents, but as the volume of
organic vapors in the atmosphere increases, more and more solvents will
probably have to be removed from exempt lists. Use of exempt solvents
may be only an interim step in the advance toward more effective air
pollution control.
The effect of solvent emission regulations on the use of organic
liquids to remove 802 from flue gases is not known. Also, the degree of
solvent removal that will represent compliance to the regulations is not
clear. According to the Los Angeles regulations, DMA appears to be non-
exempt from emission controls while TEA appears to be exempt. Table 7
shows the recovery efficiency required at several temperatures for recovery
of DMA or TEA vapors from flue gas leaving the 802 scrubber if a solvent
emission rate of only 40 lb/ day is desired. Values in Table 7 were
calculated by assuming a flue gas flow rate of 2.3 x 106 sefm and a
saturation of the exit gas with organic vapor at an equilibrium liquid tempera-
ture of 77 and 200 of. Anhydrous DMA and a 20 wt% TEA -water solution
were also assumed.
BATTELLE-NORTHWEST
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, -
36
TABLE 7. Solvent Recovery Requirements for 40 lb/day Solvent Emission(a)
Temp, of
Evaporation from Scrubber,
1000 lb/Day
Required Recovery
Efficiency, 0/0
77
200
DMA
872
41, 600
TEA
--
2
34.8
DMA
99.995
99.9999
TEA
--
98.1
99.88
a.
From a 1400 MW power plant.
e
The tabulated values show the spectacular difference between
recovery requirements for DMA and TEA. This difference occurs because
DMA has a higher vapor pressure than TEA. The table also shows that
solvent removal requires much higher scrubber efficiencies than S02
removal. With the possible exception of TEA at 77 of, the recovery
efficiencies are obviously impractical for large scrubbers because the use
of organic liquids for S02 removal could eliminate one pollution problem and
create another.
Solvent Availability
Commercial availability is another point of comparison between
organic liquids. Because of the large quantities of flue gas being treated,
large inventories of organic liquid will be required. These inventories
could range from 0.5 to 2 million pounds or more for large power plants of
1000 to 1400 MW .
e
Some organic liquids are produced in much lower quantities or are
available in much lower quantities from raw materials than others. The raw
materials for most organic chemicals are coal, crude petroleum, natural
gas, and certain other natural materials such as vegetable oils, fats, rosin,
and grains. Crude organic chemicals are derived from coal by thermal
decomposition, from petroleum or natural gas by catalytic cracking and by
distillation or absorption, and from other natural sources by steps such as
fermentation. Production of these crude organic chemicals is the first step
in the manufacture of synthetic organic chemicals. From the crude chemi-
cals' intermediate chemicals are obtained by synthesis or refining and are
BATTELLE-NORTHWEST
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37
then converted to finished chemical products. Usually, more than half the
total production of intermediates is used to produce other compounds.
Many of the cyclic compounds listed earlier in Table 1 are classified as
cyclic intermediates by the organic chemical industry. For example,
over 500/0 of the N, N -dimethylaniline production is used in the production
of other chemicals.
Table 8 show s U . S. production and sales of various potential organic
liquids. (20,21) The differences between production and sales generally
represent the amount used in the manufacture of other chemicals and
finished products.
TABLE 8. U.S. Production and Sales of Various Organic Liquids(a)
Organic Liquid
Production,
1000 lb
N, N -dimethylaniline
Quinoline
Pyridine (2° cut)
Pyridine Crude Bases
Triethanolamine
(dry basis)
10,855
637
5,503
464,000 (gal)
48,130
65,521
Diethanolamine
a. Production and sales in 1964.
Sales,
1000 lb
4,901
519
46,839
49,043
The low production of some organic liquids shows the importance of
determining availability of any specific organic liquid under consideration.
The availability problem is illustrated by the low production of pyridine
crudes, most of which are derived as by-products from coal- coking
processes. Thus, pyridine and pyridine- base compounds may not have the
necessary availability at acceptable prices if demand far exceeds the amount
available from the coal-coking processes. Also, since the low. production
rate makes the use of quinoline questionable, further study of the price-
demand supply situation is needed for other promising organic liquids.
BATTELLE-NORTHWEST
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38
Most Promising Organic Liquids for Flue Gas Scrubbing
In the preceding subsections, the characteristics of potential organic
liquids have been reviewed along with their effects in determining the
suitability of an organic liquid for S02 removal from flue gas. These same
properties can be used to provide a preliminary judgement of the applica-
bility of organic liquids at various operating conditions.
When the applicability of organic liquids at various operating
conditions is considered, it would be desirable to use organic liquids at low
temperatures because of the detrimental effect of high temperatures on
volatility or solvent emission potential, on S02 capacity, and on degradation
potential. Presently, all of the organic liquids discussed in the previous
subsections have one or more potentially severe difficulties at flue gas
temperatures.
DMA was chosen here as a base-point for a preliminary screening of
I potential organic liquids. Only known properties or characteristic s can be
compared, and any unknown properties of DMA in flue gas service are
assumed to be no worse than the other liquids being screened.
Dimethylacetamide, 2, 4-dimethylpyridine, and 2-methylpyridine
appear to be less promising than DMA because they are more expensive,
more volatile, and have 802 solubilities comparable to or less than DMA.
Quinoline and N - methylaniline appear less promising because of lower S02
solubility and higher cost. Pyridine derivatives and quinoline are also
questionable because, without intolerable price increases, large quantities
are not expected to be available. Dimethylsulfoxide costs more than DMA
and has a low decomposition temperature. Tetraethyleneglycoldimethylether
is five times more expensive, is more viscous, and has a much lower 802
solubility than DMA. Also, according to sales literature, this ether (like
other ethers) undergoes autoxidation to form peroxides with light, heat, and
oxygen promoting the reaction. Even. though it has a much lower vapor
pressure than DMA, requirements for vapor recovery from flue gas are
still quite high because of the high cost and high molecular weight.
A clear- cut comparison of xylidine, toluidine and DMA cannot be
made with the available data. Both DMA and xylidine have certain
BATTELLE-NO~THWEST
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39
advantages. Essentially, anhydrous DMA is used to absorb 802; whereas,
xylidine is used in a mixture of 50% -xylidine in water, which has a higher
802 solubility than DMA at the low 802 concentrations of flue gas. Although
xylidine has a slightly lower vapor pressure than DMA, this is not an
advantage at high temperatures beca~se of steam distillation effects.
However, xylidine costs twice as much as DMA, and the solubility of DMA
sulfate in water is much greater than that of xylidine sulfate. Therefore,
the DMA sulfate concentration can be much greater than the xylidine sulfate
concentration in the weak sulfuric acid solution used in the solvent recovery
scrubbers, which results in a much lower water load on the regenerator.
During the absorption of 802 with either DMA or xylidine, the auto-
catalytic oxidation of 802 to 803 occurs. The amount of oxidation which is
greater in a xylidine-water system, increases rapidly as the 802 concentra-
tion in the flue gas decreases. The greater autocatalytic oxidation and
lower solubility of xylidine sulfate results in the need for more careful
control of operating conditions when xylidine is used. Also, large amounts
of water must be recycled to the regenerator to keep xylidine sulfate from
precipitating and clogging the system. Experimental data on autocatalytic
oxidation of 802 to 803 at flue gas conditions is needed to make a more
precise comparison.
Toluidine could be more promising than xylidine because of the lower
cost; however, 802 solubility in toluidine is much lower and the vapor
pressure of toluidine is higher. Other definitive data at flue gas conditions
are lacking.
A definitive comparison between TEA and DMA cannot be made at the
present state of experimental data. Although the prices .of TEA and DMA
are the same, TEA apparently has a greater availability. Also, TEA has a
higher 802 capacity and a much lower vapor pressure. TEA may be an
exempt solvent; whereas, DMA apparently is a nonexempt solvent when
applied to existing solvent emission regulations. Because TEA is used in a
water solution, 802 removal with an aqueous TEA solution could result in a
steam plume. The lower vapor pressure of TEA results in much less
evaporation of solvent during the 802 absorption step and reduced requirements
BATT ELL E - N 0 RT H \'II EST
-------
40
for recovery of organic vapors. TEA is a much more promising solvent
than DMA when only these evaporation losses and solvent recovery require-
ments are considered. Unfortunately, a complete process is not yet
available for TEA, nor is a regeneration step developed. However, scouting
laboratory experiments have indicated that regeneration may be chemically
feasible by distillation with H2S04 or by precipitation with lime slurry. (16)
Also, existing data indicate a problem with irreversible reactions between
S02 and TEA, particularly at flue gas temperatures. Qualitative information
on the use of ethanolamines to recover C02 from combustion gases indicates
a potential oxidation problem for TEA. Experimental data are needed on
these items before a definitive judgement on TEA can be made.
TEPA is in much the same category as TEA. TEPA has the
advantage of a lower vapor pressure than TEA. However, the lack of a
regeneration process and the cost indicate the need for more experimental
data before an accurate assessment of TEPA can be made.
-',
From the foregoing comparisons, DMA, xylidine, and TEA'" appear
to be the most promising of the organic liquids for which data are available.
However, the extremely high scrubber efficiencies required for recovery of
solvent vapors makes the use of DMA and xylidine very questionable. The
comparisons also show some of the properties needed by any promising
organic liquid for purposes of theoretical S02 solubility. Such promising, .
though untested, organic liquids should have a cost comparable to or not
much greater than DMA, xylidine, or TEA. Also, the vapor pressure must
be lower than DMA. Viscosity should be considered.
Application to Smelter Gas
Organic liquids are highly applicable to removal of S02 from smelter
gases. The DMA scrubbing process is now used at two locations in the U . S.
to remove and recover S02 from smelter gases while the Lurgi Sulphidine
process is used in Europe. The lower gas flow rates from smelters may
-',
','
In view of data presented in Reference (16) (which was issued in the
course of this present study) TEA itself is not a likely candidate. TEA
must therefore be considered throughout this present report as a member
of a class of compounds in which likely candidates may be developed.
BATTELLE-NORTHWEST
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41
allow more flexibility in determining alternative solvents; however, present
solvent emission regulations indicate the desirability of low vapor pressure.
These regulations also indicate the potential advantages of replacing
apparently nonexempt DMA with an exempt organic liquid.
TEA is promising for application to smelter gas if a satisfactory
process can be developed. TEA may be an exempt solvent and the low
evaporation from the S02 scrubber could result in reductions in capital and
operating costs. In continued studies on this program, sorbents [other than
TEA which does not appear clearly suitable .in view of data presented in
Reference (16) ] which involve simpler and more economical processing
than DMA for smelter gases could very likely be identified. Interest here
may emphasize the development of a process based on an exempt
solvent. (19)
PRELIMINARY ECONOMIC COMPARISON
Since no developed processes using organic liquids for S02 removal
from power plant flue gases were found during the study, a detailed economic
analysis cannot be made at this time. Experimental data are lacking for
determination of realistic chemical flow sheets (material balances) and
equipment requirements. However, the DMA process for smelter gas is
well developed, and a preliminary comparison between some known features
of this process in flue gas service and the alkalized alumina process can
be made. To make the comparison, published economic information on the
alkalized alumina process(22} was adjusted to reflect inflation and recently
published economic bases for utilities. The adjustments mostly represent
the economic bases proposed for the detailed Phase III study rather than
any major disagreement with the published costs. The following subsections
present the economic bases, adjustment of the costs for the alkalized alumina
process J and a preliminary comparison with some known features of the
DMA process.
Economic Bases
As in the economic study of the alkalized alumina process, the
economic bases used for adjustment purposes apply to an investor-owned
BATTELLE-NORTHWEST
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42
utility. Statistics published by the Federal Power Commission in 1964
showed that 76% of the generating capacity was investor-owned, 10% was
publicly-owned (nonfederal), 13% was Federal-owned, and 1% was
cooperative-owned. (23) Based on the,se percentages, fixed charges and
other economic bases should be representative of an investor-owned electric
t'l"t (24-26)
u 1 1 y.
For investor-owned utilities, the return on investment is the average
cost of mone.y to the utility and is a composite of interest on debt (bonds),
and earnings on equity (stock). The debt / equity ratio varies appreciably;
but a 50/50 debt-equity ratio is not uncommon. The range of 40/60 to
60/40 probably includes most companies. Interest rates vary with the
financial conditions of the country and the risk associated with investing in
a particular company. In addition, the utilities use a variety of techn iques
to determine fixed charges, and they do not all incorporate the same
components in their fixed charges. These different techniques do not result
in grossly different fixed charges but do cause a rearrangement of tne
magnitude of some of the components.
Table 9 presents a tabulation of the fixed charges used in this study.
This table presents fixed charges for an investor-owned utility for both the
depreciating plant and the nondepreciating assets. The fixed charges for
nondepreciating assets, such as land and working capital, differ primarily
because they do not have the depreciation component; this J in turn, changes
the magnitude of the income taxes. Although fixed charges on the
depreciable plant are shown for three different plant lives to show the
importance of this factor, a 30 year life is used in this study, with an
assumed debt / equity ratio of 50/50. The bond interest and earnings on
equity are assumed to be 5 and 8.5%, respectively J to give a composite
rate of return of 6. 75%. This return is in the upper range usually allowed
for this regulated industry by utility rate commissions. A higher bond
interest, similar to current interest rates, was not used because the current
interest on utility bonds may only be a short-term peak. However J as bond
interest goes' up, earnings on equity decrease, or debt/ equity ratio is
reduced so that the composite rate of return remains essentially unchanged.
BATTELLE-NORTHWEST
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TABLE 9. Levelized Fixed Charges for Investor-Owned Utility
CD
»
-I
-I
111
r
r
111
I
Z
o
~
-I
I
Component
Return on Investment(a)
Depreciation (Sinking Fund)(b)
Federal Income Taxes(c)
Other Taxes(d)
Property Insurance
Interim Replacements
Total (rounded)
Fixed Charge Rates, % of Initial Investment
Depreciating Plant
10 yr life 30 yr life 45 yr life
Nondepreciating
Assets(a)
6.75 6.15 6.75
7.32 1. 11 0.38
1. 07 1. 49 1. 79
2.0 2.0 2.0
0.25 0.25 0.25
0.35 0.35 0.35
17.7 12.0 11.5
6.75
3.92
2.0
12.7
~
eN
a. Primarily for land and working capital. If used for nondepreciating catalysts
or chemicals add 0.25% for property insurance.
b. Constant debt/equity ratio of 50/50 assumed. Bond interest at 5%/yr; equity
earnings at 8.5%/yr.
c. Plant life as specified in each column. Zero salvage value.
d. Federal income tax rate of 48% is assumed. SYD accelerated depreciation
credit and 3% investment tax credit for first year are included. Tax life
equal to book life. .. . ... .
e. Does not include gross revenue tax.
~
111
U1
-I
-------
44
With the composite rate of return remaining constant, a slight shift in debt I
equity ratio or rearrangement between bond interest and equity earnings will
have only a slight effect on levelized fixed charges.
In the actual "book accounting' of a utility, investment in a dePr:eciable
plant is almost universally recovered over the book life by straight line
depreciation. The net investment declines linearly, and the fixed charges--
as a percent of initial investment- -decline from year to year because the
required return on investment is only charged against the undepreciated
investment. Therefore, for engineering economy studies of utility alternatives,
a "levelized" fixed charge value- -as a percent of initial investment- -is
commonly used. This levelized fixed charge accounts for not only the year-
by-year changes but for also the time value of money (present worth). A
standard technique for calculating the levelized annual return plus deprecia-
tion is to use the required return on investment in conjunction with a sinking
fund factor for depreciation. (24,27) This technique is used in Table 9.
Another method is to use straight line depreciation and a "levelized"
return on investment. This levelized return is a present-worth average of
the year-to-year return (on undepreciated investment) computed as a
percent of initial investment. The methods are equivalent in terms of the
sum of return plus depreciation, but the method used in Table 9 is more
commonly used.
A levelized federal income tax on equity earnings is used in
Table 9. This levelized tax, as a percent of initial investment, is calculated
by use of the equity portion of the levelized return on investment. The
sum-of-years-digits (SYD) method of calculating accelerated depreciation
for tax purposes was used in determining the income tax in Table 9. Either
the SYD or the double-declining-balance method has been used by investor-
owned utilities 'since 1954. The federal income tax rate is as sumed to be
48% since the future of the surtax is uncertain. The federal investment tax
credit of 3% on the first year has also been included.
There are a variety of other taxes, besides federal income taxes,
that are encountered by utilities, with local property taxes the most
important. Some states have income taxes and franchise taxes and there
BATTELLE-NORTHWEST
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45
are also gross revenue or gross receipts taxes; however, since gross
revenue taxes must also be added to operating costs in economic studies,
they are commonly added to the total annual expense rather than individually
to the annual fixed charges and operating costs. The total of other taxes,
as a percent of initial investment, can range from less than 2 to over 4%,
depending upon the location. Economic studies of various utility alternatives
usually use 2 to 3% for other taxes. (24) From these studies and other
tabulated costs(23, 26) encountered by utilities, 2% is used in Table 9 for
other taxes.
A value of 0.25% is used for insurance in Table 9 and is commonly
used in economic studies of utility alternatives. (24)
A value of 0.35% is used for interim replacements. This charge
represents large expenditures for replacing major equipment components
where failure of such equipment would impair the integrity of the asset
during its life. As used here, this charge does not affect normal maintenance
costs. Some utilities do not include this component in their fixed charges
because of the excellent performance of modern fossil-fired power plants.
Interim replacement is routinely used as a component of fixed charges in
economic studies of chemical processing plants and seems appropriate here
for the chemical processing equipment for S02 removal, . especially since
fixed charges equivalent to a 30-year book and tax life are assumed.
A depreciation time of 30 years is assumed for several reasons. The
utility industry routinely uses 30 to 35 years for fossil-fired plants, and the
same book life is commonly used for all parts of the depreciating plant.
When a short book life is used by the chemical processing industry and a
short tax life, such as 10 years, is allowed by the IRS, the short lives are
usually in recognition of rapid obsolescence of the product and/or process
in an extremely competitive industry. Such recognition mayor may not
occur in this instance. Electricity will not become obsolete, and
obsolescence (if any) of a process for treating a waste stream may not be
overly significant to utilities whose allowable return on investment and
electricity rates are carefully controlled by regulatory agencies. However,
a short tax life or special tax credits may be allowed to reduce the burden
of pollution treatment on electricity rate structures.
BATTELLE-NORTHWEST
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46
A shorter book life, such as 10 years, could result in fixed charges
that are difficult to absorb in the electricity rate structure. In actuality J
the book and tax life will be established by the utilities after negotiations with
the Internal Revenue Service, Federal Power Commission, and State Public
Utility Commissions. In any event, a 30-year book life for equipment should
be used only in conjunction with the interim replacement component in the
fixed charges to provide for major equipment replacements resulting from
failures or process improvements.
For purposes of this preliminary study J the alkalized alumina
catalyst was capitalized and added to the plant investment as was done in the
published evaluation of the alkalized alumina process. For a precise detailed
comparison of alternative processes, inclusion of the initial cost of
expensive catalysts or chemicals in the plant investment may not be proper.
For example, a recoverable platinum catalyst will probably be a nondepreciat-
ing asset like land or working capital. Other catalysts or chemicals can
have a salvage value or a shorter life than the plant investment. Since any
of these conditions will alter the fixed charges, the conditions and fixed
charges must be determined individually for each case.
The direct labor rates used in this study were developed by escalation
of tabulated wage rates from a study in 1966 on fossil-fueled. plant costs. (24)
Escalation was arbitrarily taken as 80/0, or 40/0 / yr for 2 years. Salary rates
for some personnel categories are summarized in Table 10.
TABLE 10. Wage Rates in Fossil-Fueled Power Plants
Per sonnel
Plant Superintendent
Shift Supervisor
Control Room Operator
Equipment Operator
Utility Man
Relief
Mechanic
Electrician
Reference 1966
Salary, $ / yr
$15, 600
9,000
8; 000
7,200
6,660
5,200
7, 280
7,280
Escalated 1968
Salary, $/yr
$16,800
9, 700
8, 600
7,780
7, 190
5,600
7,860
7,860
BATTELLE-NORTHWEST
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47
A payroll burden of 30%, also listed in the 1966 study of fossil-fueled
plant costs, was used in this study..
Interest during construction was taken as 6. 75% of the cost of the gas
scrubbing equipment, assuming installation along with a new power plant.
Prior to the recent surge in interest rates, interest during construction has
usually been calculated by utilities on the basis of 5 or 6% interest, with pay-
ment assumed during construction. The interest during construction is
assumed to apply to the total construction cost for 45% of the design and con-
struction period. The 45% is a standard factor in engineering economy studies
and is based on the classical sigmoid curve for construction costs. Design
and construction time is generally taken as 3 to 4 years. The 6. 750/0 used in
this study was calculated by assuming an interest rate of 50/0/yr and a design
and construction period of 3 years. A higher interest rate, similar to the
current prime interest rate, was not used because the current rates may
only be short-term peak rates.
For purposes of this study, working capital was not added to the plant
investment but was handled separately. Annual costs for working capital
were calculated from the levelized fixed charges in Table 9 for a nondepre-
ciating asset. This method of handling fixed charges on working capital is
generally used by the utilities.
A plant capacity factor of 90%, used in the published study of the
alkalized alumina process, was used in this study for simplification, but
this value is probably slightly high. Detailed studies of new fossil-fired
plants indicate that the average lifetime capacity factor is likely to be only
60 to 70% because such plants will be part of the baseload portion of the
system for only the first 10 to 15 years of life. (24) For evaluation purposes,
an average lifetime capacity factor of 80% is commonly used.
Adiustment of Alkalized Alumina Costs
Adjustments of the published costs were primarily made by escalatirig
the total plant cost by 8%, or 4% /yr for two years, and by incorporating the
economic bases described in the preceding subsection. The published plant
cost was assumed to contain the usual indirect construction costs, start-up
BATTELLE-NORTHWEST
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48
costs, and contingency factor. The study assumed 0.2 vol% S02 in the inlet
gas. Costs were not adjusted for this factor (S02 concentration) because
details were lacking on the effect. Labat requirements and various percent-
ages for labor and maintenance supervision, operating supplies, maintenance
materials, spare parts, and indirect cost were not changed. Unit costs for
coal, power, heat, and water were not changed, but alkalized alumina costs
were escalated by 8%. The published construction costs were estimated on
the basis of an addition to an existing plant. Some savings would probably
occur if the unit was a part of a completely new plant; however, no adjust-
ment was included in this study. The various categories of working capital
were not changed, and the gross revenue tax was not added to the annual
operating cost.
The adjusted total investment and annual operating cost are shown in
Tables 11 and 12, respectively. These estimated costs are for a unit capable
of removing 90% of the S02 from 87.3 x 106 scfh in an 800 MWe power plant
operating at an operating efficiency of 900/0.
TABLE 11. Adjusted Total Investment for Alkalized Alumina
Item
Cost, $
Total Construction Cost
Initial Catalyst Cost
$8,000,000
369,000
Total Plant
Interest During Construction
$8,369,000
565, 000
Subtotal for Depreciation
$8,934,000
642,000
Working Capital
Total Investment
$9, 576,000
($12/kW)
BATTELLE-NORTHWEST
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49 '
TABLE 12., Adjusted Annual Operating Cost
for Alkalized Alumina
Item
Cost, $/yr
Direct Cost:
Raw Materials and Utilities:
Absorbent Makeup
Coal for Producer Gas
$
973,800
475, 200
90, 300
435, 500
26,000
-311, 100
Power
Heat
Water
Credit (Heat)
Direct Labor:
Operating
Su pervi sian
98, 500
14,800
Plant Maintenance:
Maintenance Personnel
180,000
'36,000
75,000
99,000
'58, 000
$2, 251, 000
231,000
86,000
1, 149, 000
$3,717,000
(0.59 mills/kvV-hr)
Supervision
Material
Payroll Overhead
Operating Supplies
Total Direct Cost
Indirect Cost
Working Capital Charges
Fixed Charges on Plant
Total annual cost
BATTELLE-NORTHWEST
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5G
The adjusted total investment, including total plant cost, interest
. .
during construction, and working capital, is $9,576,000 or $12/kW. The
adjusted operating cost is $3,717, OOO/yr or O. 59 mill/kW-hr.
DMA Process Comparison
The DMA process has never been used for S02 removal from power
plant flue gases so a precise definition of both the flow sheet and equipment
requirements cannot be made. The chemical process will be nearly identical
for S02 removal from either flue gas or smelter gas. Since essentially all
chemical costs for the DMA process result from DMA losses or recovery of
DMA vapors from the exit gas from the S02 scrubber, chemical costs can be
readily developed for the use of DMA to remove S02 from flue gas. In view
of the enormous quantities of DMA evaporated into flue gas, considerable
insight on the applicability of the DMA process (and related processes) can.
be gained by comparing the annual chemical costs for the DMA process with
the annual operating costs for the alkalized alumina process.
In the removal of S02 from smelter gas by DMA, the absorption tower
is divided into three separate sections. Flue gas enters the bottom of the
absorption tower and S02 is removed in the bottom section by counter-current
contact with DMA. The flue gas containing some S02 and SMA leaves the
bottom section and passes upward through the middle section where it is
scrubbed with an aqueous 6% Na2C03 solution. The Na2C03 reacts with the
residual S02 in the smelter gas as shown by the following reaction:
Na2C03 + S02 --> Na2S03 + C02
The gas leaves the middle section and passes through the top section where
the gas is scrubbed with an aqueous 100/0 H2S04 solution to recover the DMA
vapors. The acid reacts with the DMA base to form DMA sulfate which is
. .
soluble in the scrubber water. The H2S04 flow is adjusted so the acid is
nearly saturated with DMA when it leaves the tower. The smelter gas leaves
the top of the ~ower with only small amounts of wasted S02 and DMA.
The aqueous effluent from the middle section and top section flow to a
collecting tank and are mixed. DMA is liberated as a result of the following
reaction:
(DMAH) 2S0 4 + Na2S03 --> 2DMA + Na2S04 + S02 + H20
BATTELLE-NORTHWEST
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51
The mixture is then pumped to a gravity separator where DMA is removed
and returned to the main supply. Part of the DMA remains dissolved in the
water as DMA sulfite. The water, containing DMA sulfite and Na2S04'
first goes to the stripper water tank and then to the top tray of the regenera-
tor wher.e it is boiled vigorously. Any DMA sulfite dissolved in water i.s
broken down into DMA and S02 which are carried by steam into the stripper
and recovered. The aqueous Na2S04 effluent from the regenerator is dis-
carded to waste.
Some process changes would be required for DMA treatment of flue
gas from a power plant. Because of the low S02 content and the large gas
flow rate, there would not be enough residual S02 in the exit gas from the
S02 scrubber to convert the necessary amount of Na2C03 to Na2S03' Thus,
an aqueous Na2C03 solution would probably have to be added to the receiver
for the aqueous solution of DMA sulfate from the DMA recovery scrubber.
The C02 would be removed and discharged to the stack with the exit flue gas.
Should the use of Na2C03 in this manner prove unsatisfactory, more expen-
sive Na2S03 would have to be used to react with DMA sulfate in the receiver.
Alternatively, Na2C03 and the aqueous solution of DMA sulfate could be
added to the regenerator. The Na2C03 would react with freed S02 to form
Na2S03 which would then react with the DMA sulfate to form DMA, Na2S04'
and S02' However, use of the regenerator for the reaction is unsatisfactory
because the recovered S02 would be contaminated with C02'
The use of H2S04 and Na2C03 is carefully balanced to the amount of
DMA vapor in the exit gas from the S02 scrubber. Therefore, the stoichio-
metric amounts of Na2C03 and H2S04 required in the preceding reactions
are a fairly good approximation of chemical requirements for recovery of
DMA vapor. For a system handling 87. 3 x 106 scfh of flue gas from an
800 MWe power plant, D.MA evaporation from the 802 scrubber is calculated
to be 181. 3 x 106 lb /yr at an operating efficiency of 90%. This value was
calculated by assuming the exit gas is saturated with vapor at an equilibrium
DMA temperature of 77 of. Assuming a fairly optimistic 98% recovery
efficiency in the large scrubbers, DMA recovery is 177.7 x 106 lb/yr and the
DMA loss to the stack is 3. 6 x 106 lb /yr. On the basis of stoichiometric
amounts of Na2C03 and H2804' chemical costs are summarized in Table 13.
Should Na2S03 be required instead of Na2C03' costs would be higher.
BATTELLE-NORTHWEST
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52
TABLE 13.
Chemical
DMA
H2S0 4
Na2C03
Unit
Cost, $/lb
O. 22
0.017
0.016
Approximate Chemical Costs of DMA Process
for Flue Gas(a) .
Annual
Consumption,
1 b / yr
6
3. 6 x 10
6
71.85x10
6
77.7x10
Annual
Cost, $
792,000
1, 222,000
1, 243,000
Cost,
mills/kW -hr
O. 125
O. 193
O. 197
Total
3,257,000
O. 51
(a) For 800 MW power plant.
e
Comparison of these chemical costs with the total annual costs for
the alkalized alumina process clearly shows the poor competitive position
of the DMA process. The DMA process will not be competitive with the
alkalized alumina process unless the degradation of alkalized alumina, the
cost of al!<.alized alumina, and other estimated cost factors turn out to be
significantly higher.
The chemical costs also show that further experimental work on
organic liquids should be limited to liquids with vapor pressures much
lower than DMA.
DATA NECESSARY FOR ASSESSMENT OF ENGINEERING AND ECONOMIC
POTENTIAL OF PROMISING CANDIDATES
On the basis of vapor pressure losses tabulated in the previous
section, few candidates hold much promise as applicable sorbents. The
recovery of the volatilized sorbent- -taking dimethylaniline as the example--
will involve large daily tonnages of sulfuric acid and soda ash equivalent
to the DMA recovered. The resulting dilute sodium sulfate must then also
be disposed of without further contributing to environmental pollution. This
can be done only by recovery as solids for sale as low valued salt cake.
Extensive study should therefore be directed at other candidates of a class
in which triethanolamine (TEA) is an example. Data required include the
following:
. Determine degradation or oxidation properties of representative
sorbents of the class of which TEA is an example.
BATTELLE-NORTHWEST
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53
.
Determine the kinetic s of autocatalytic oxidation of 802 to 803 in
the sorbent system.
Determine realistic vapor pressure and entrainment losses.
Evaluate economical means of minimizing losses.
Establish the conditions for an acceptable regeneration process.
Develop necessary equilibrium data for representative sorbents
under flue gas composition and conditions.
Establish the process flow sheet and material balance.
Scout the applicability of additional likely sorbents selected on the
basis of cost) availability, and desirable chemical, physical, and
nonpollution properties and possibilities for integration with the over-
all power plant function. Candidates might include other .fatty amines,
polyethylene glycols and amine derivatives, crude carbohydrates and
crude petroleum factions (heavy olefins),
On this phase of the study, a critical evaluation should be made of
the potential atmospheric p()llution resulting from the use of likely
liquid organic scrubbing agents for removal of S02 from industrial
waste gases.
.
.
.
.
.
.
.
PROPOSED FUTURE PROGRAM
A program should be initiated to provide the data obtainable by doing
the work outlined above. It is recommended that work on the first three
items and the fifth be studied initially to be certain of the applicability of any
specified agent. This program could place considerable emphasis on the
selection of sorbents which can be expected to be classed as exempt under
existing control regulations. (19) Attention should be placed on the prospects
for developing such an absorbent to replace DMA in smelter off -gas
processing.
BATTELLE-NORTHWEST
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54
REFERENCES
1. Ludwig, J. H. and Spaite, P. W.
CONTROL OF SULFUR OXIDES POLLUTION: THE CHALLENGE TO
THE CHEMICAL ENGINEER.
A. 1. CH. E, Detroit, Michigan.
(December 4-8, 1966)
2. u. S. Department of Health, Education and Welfare.
AIR QUALITY CRITERIA FOR SULFUR OXIDES.
Public Health Service Publication NQ. 1619 (March 1967)
3. Cole, R. J.
THE REMOVAL OF SULPHUR GASES FROM SMELTER FUMES.
Report by Ontario Research Foundation, Toronto, Canada (1947)
4. Weast, R. C., ed. (Chemical Rubber Company, Cleveland)
HANDBOOK OF CHEMISTRY AND PHYSICS.
48th edition, pp. F-148, E-65. (1967)
5. Fieser, L. F. and M.
ADV ANCED ORGANIC CHEMISTRY
Chapter 17, Reinhold, New York (1961)
6. Arthur D. Little, Inc.
THIRD MONTHLY PROGRESS REPORT ON CONTRACT PH 86-68-57
Table I (1968)
7. Hill, Arthur E.
REACTION OF AMINES WITH SULFUR DIOXIDE.
1. ANILINE AND SULFUR DIOXIDE.
J. Am. Chern. Soc. 53, 2598-2608 (1931)
CA 25, 4482
8. Hill, Arthur E., and Fitzgerald, Thomas B.
COMPOUNDS OF SULFUR DIOXIDE WITH VARIOUS AMINES.
J. Am. Chern. Soc. 57, 250-4 (1935)
CA 29, 1689
9. Wynne-Jones, W. F. K., and Anderson,. A. R.
THE THERMODYNAMIC CONDITIONS FOR THE FORMATION AND THE
EXISTENCE OF CLATHRATE COMPOUNDS.
Compt. Rend. Reunion Ann. Avec. Comm. Thermodynam.,
Union Intern. Phys. (Paris) 1952
DA 48, 34
10. Fleming, E. P. and Fitt, T. C.
LIQUJD SULFUR DIOXIDE FROM WASTE SMELTER GASES.
Ind. Eng. Chern., vol. 42, no. 11, p. 2253 (November 1950)
11. Cole, R. J. (Ontario Research Foundation, Toronto, Canada)
THE REMOVAL OF SULFUR GASES FROM SMELTER FUMES.
1947
12. Anon.
HI-PURITY LIQUID S02
Chern. Eng., p. 274. (April 1953)
BATTELLE-NORTHWEST
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55
13. Shreve, R. N.
THE CHEMICAL PROCESS INDUSTRIES.
McGraw-Hill Book Company, Inc., New York,
(1956)
14. Updegrass, N. C. and Reed, R. M.
TWENTY -FIVE YEARS OF PROGRESS IN GAS PURIFICATION.
Petroleum Eng., vol. 26, pt. 3, p. C- 57 (September 1954)
15. Berlie, E. M., Estep, J. W., and Ronicker, F. J.
PREVENTING MEA DEGRADATION.
Chem. Eng. Prog., vol. 61, no. 4, p. 82 (April 1965)
16. Beutner, H. P., Niesson, W. R., Haley, H. E., and Emerson, W. S.
FEASIBILITY OF A REGENERATIVE HIGH TEMPERATURE AMINE
ABSORPTION PROCESS FOR THE CONTROL OF SULFUR DIOXIDE
EMISSIONS FROM STACK GASES.
A. D. Little, Inc., New York (August 1968)
17. Blachly, C. H. and Ravner, H.
ST ABILIZATION OF MONOETHANOLAMINE SOLUTIONS IN CARBON
DIOXIDE SCRUBBERS.
J. Chem. Eng. Data, vol. 11, no. 3, p. 401 (July 1966)
18. Cooper, J. C.
"Control of Solvent Emissions, "
NEW DEVELOPMENTS IN AIR POLLUTION CONTROL, PROCEEDINGS
MECAR SYMPOSIUM NEW YORK, OCTOBER 23, 1967.
Metropolitan Engineers Council on Air Resources, New York (1967)
19. Anon.
A COMPILATION OF SELECTED AIR POLLUTION EMISSION CONTROL
REGULATIONS AND ORDINANCES.
Public Health Serivce, U. S. Dept. of Health, Education and Welfare,
Revised Edition, Washington (1968)
20. Anon.
SYNTHETIC ORGANIC CHEMICALS, U. S. PRODUCTION AND SALES,
1964.
T C Publication 167.
U. S. Tariff Commission, Washington (1965)
21. Manufacturing Chemists Assoc., Inc., Washington.
CHEMICAL STATISTICS HANDBOOK.
6th ed., (1966)
22. Katell, S.
REMOVING SULFUR DIOXIDE FROM FLUE GASES.
Chem. Eng. Progr., vol. 62, no. 10, p. 67 (October 1966)
23. Federal Power Commission, Washington, D. C.
NATIONAL POWER SURVEY.
October, 1964
24. Newbold, H. L. R. (Jackson & Moreland, Boston, Mass.).
COSTS OF LARGE FOSSIL FUEL FIRED POWER PLANTS.
J&M No. 636A, July 15, 1966
2nd ed., pp. 131-132
BATTELLE-NORTHWEST
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56
25. Geller, L., Hogerton, J. F., and Stoller, S. M.
ANALYZING POWER COSTS FOR NUCLEAR PLANTS.
Nucleonics, vol. 22, no. 7, p. 64 (July 1964)
26. Anon.
14th STEAM ST ATION COST SURVEY.
Electrical World, vol. 164, no. 16, pp. 103-18 (October 18, 1965)
27. Thuesen, H. F., and Fabrucky, W. G.
ENGINEERING ECONOMY.
3rd Ed. Prentice-Hall, Inc., Englewood Cliffs, N. J. (1964)
28. Gel'perin, N. 1., Others.
ABSORPTION OF SULFUR DIOXIDE AND CARBON DISULFIDE IN
HYDROCARBONS OF THE DIPHENYLMETHANE SERIES.
Zhur, Priklad. Khirn. 31,.1323-32 (1958)
J. Applied Chern. USSR 31, 1309-17 (1958) - English Trans.
29. Balej, Jan, and Regner, Albert.
THE SYSTEM SULFUR DIOXIDE-DIMETHYLANILINE.
1. ABSORPTION ISOTHERMS.
Collection Czech. Chern. Cornrnuns. 21, 1545-52 (1956)
(in German)
II. HEATS OF SOLUTION,
Ibid. 1553-9
CA 51, 11831
30. Vian, A., Andres, A. Soler, and Fernandez, C. Iriarte.
ST ABILITY AND HEATS OF FORMATION IN PYRIDINES-S02
SYSTEMS OF INDUSTRIAL INTEREST.
Quirn. Ind. (Bilbao) 13(2), 47-53(1966) (Span. )
CA 66 1991
31. Albright, Lyle F., Shannon, Paul T., Yu, Sun-Nien, and
Chueh, Ping Lin.
SOLUBILITY OF SULFUR DIOXIDE IN POLAR ORGANIC SOL VENTS.
Chern. Eng. Progr., Syrnp. Ser. 59(44), 66-74 (1963)
CA 59, 3363
32. Srnedslund, Tor H.
DIMETHYL SULFOXIDE AS SOL VENT FOR SULFUR DIOXIDE.
Finska Kernistsarnfundets Medd. 59, 40-3 (1950)
CA 46, 4329
BATTELLE-NORTHWEST
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APPENDICES
BATTELLE-NORTHWEST
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A-I
APPENDIX A
Published solubilities of 802 in organic liquids are listed in
Table A-I. Entries are in alphabetical order of compound names.
tion of symbols are found on page 9.
Defini -
Where the original articles give tables of experimental results for
solubility as a function of pressure, these data are usually listed with change
of units to achieve uniformity. For a few compounds, only graphs are
published, with the values tabulated below having been read from the graphs.
. .
Reference 28 reports measured solubilities for different temperatures at
fixed pressures. These results have been plotted and the graphs used to
find solubilities at 25 and 40° for different pressures.
The values of A for N, N-dimethylaniline are taken to be the recipro-
cals of the K values reported on page 1552 of Reference 29.
For N, N -dimethylacetamide' and N, N -dimethylformamide, the total
pressures given in Reference 30 have been corrected by subtracting the
vapor pressures of the pure liquids.
BATTELLE-NORTH W EST
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TABLE A-I. Solubilities of S02 in Organic Liquids
Compound t w r P x Pix A Hef
Aniline 25 3.77 17. 5 O. 0230 O. 052 O. 44( 2) o. 40(7) 7
7.57 37.0 0.0487 0.099 O. 49(2)
Diamylmethane 25 O. 26 12. (9) 0.017 0.010(1) 1. 6(8) 1. 6(8) 28
(mixture of isomer s) 1. 09 53. 8 0.0708 0.041(3) 1. 71
3.11 160 O. 21 o. 109(1) 1. 93
6.80 439 O. 5775 0.211(3) 2.73
ro 40 O. 64(3) 53.8 0.0708 0.0247 2. 87 2. 7(6)
:>. 1. 93 160 O. 21 O. 070(6) 2. 97
-I
-I 4. 13 439 O. 5775 0.139(9) 4. 12(8)
rr1 N, N -Diethylaniline 25 8. 7(6) 119. 3 O. 1570 O. 169 O. 92(9) O. 8(0) 8
r 17.6(0) 247.5 O. 3257 O. 291 1. 11(9)
r 26. 4(8) 391. 6 0.5153 O. 382 1. 34(9)
rr1
I 34. 4(6) 528.0 0.6947 O. 445 1. 56(1)
43. 3(5) 678.0 0.8921 O. 502 1. 77(7) :r>
z I
o. 05(7) ~
o 2, 4-Dimethylpyridine 30 5. 8 4 0.005 0.088 0.05 30
::0 11. 1 13 0.017 O. 157 o. 10(9)
-I 17.7 25 0.033 0.228 O. 14(5)
I
:E 40 5. 8 8 0.011 0.088 O. 12(5)
rr1 11. 1 26 0.034 O. 157 o. 21(7)
(J) 50 5. 8 16 0.021 O. 088 0.24
-I
N, N-Dimethylacetamide 25 8.6 14. (6) 0.019(2) 0.105 o. 18(3) o. 11(0) 31
14. 7 44. (6) 0.058(7) O. 166 o. 35( 4)
31. 1 94. (2) 0.123(9) O. 297 o. 41(7)
47.2 185.(3) 0.263(4) O. 391 o. 67(4)
38 8. 6 28. (3) 0.037 O. 105 0.35(4) o. 23(6)
14. 7 68. (6) 0.090 0.166 0.54(4)
31. 1 168.(4) O. 222 O. 297 0.74(6)
47. 2 310. (6) 0.409 O. 391 1. 04( 5)
-------
Compound t w r P x Pix A Ref
N, N -dimethylacetamide 66 8. 6 91. (5) O. 120 O. 105 1. 15 o. 9(8)
14. 7 179. (4) O. 236 O. 166 1. 42
30.6 448. (8) O. 591 O. 294 2.01
46. 8 854. (7) 1. 125 0.389 2.89
93 8. 6 253 O. 333 O. 105 3. 17 2. 7(5)
14.7 453 O. 596 O. 166 3. 59
30.2 109. (2) 1. 43(7) O. 291 4. 94
30. 5 111(7) 1. 47(0) O. 293 5.02
m 45.6 1 91( 4) 2. 51(8) O. 383 6. 57
» N, N -Dimethylaniline 15 11.83 5. 27 0.02480 29
~ 20. 68 12. 30
~ 22.05 14. 19
IT! 24. 86 21. 51
r 32. 91 30.30
r 40.23 48.70
IT!
I 45. 20 63.4
z 47.47 78. 6 ::r>
48.37 83.6 I
o . CN
JJ 50.61 95.0
~ 54.39 121.0
I 60. 79 169. 5
~ 65. 70 220. 5
IT! 20 16.02 12. 25 0.03895
(f) 16.50 13. 25
~ 22.41 21. 23
26.83 28. 08
30. 86 39. 90
31. 06 42. 20
43.82 89.0
50. 43 137. 3
51. 96 150. 0
60. 52 235. 5
-------
Compound t w r P x Pix A Ref
-
N, N -Dimet.hylaniline 25 11.89 13. 10 0.0617
12. 16 13. 78
19. 17 25.72
27.49 48. 0
27.70 49. 7
29.71 56.0
37. 37 89. 2
41. 87 119. 5
47.36 162. 0
m 54. 34 232. 5
> 40 3.72 8.98 O. 1862
-I 4.81 13. 30
-I 8.43 25.80
rt1
r 11. 73 36.30
r 12.40 39. 10
rt1 13. 00 43.00
I 17.45 58. 5 :P
z 22.84 93.5 I
>I>-
o 24. 35 103. 95
::0 30.92 154. 9
-I 31. 57 158.0
I 38. 12 246.0
< N, N - Dimethylformamide 25 19.2 68. (4) 0.090 O. 180 O. 50(O} O. 43 31
rt1 60. 1 2 3( 4} o. 30(8} O. 407 0.75(7)
(j) 146. (7) 99(4} 1. 30(8) O. 626 2. 08( 9)
-I
348 199(2} . 2. 62(l} O. 799 3. 28(0)
38 19. 2 89. (2) O. 177 O. 180 0.65(0} 0.48
60. 1 38(0} o. 50(0} 0.407 1. 22(9}
146. (l) 149(2} 1. 96(3} O. 625 3. 14( 1)
346 301(7} 3. 97(0) . 0.798 4.97(5}
-------
Compound t w r P x Pix A Ref
N, N -Dimethylformamide 66 19. 2 212 O. 279 O. 180 1. 55 O. 80
59. 9 108( 3) 1. 42( 5) 0.406 3. 51
143. (0) 328(1) 4.31(8) O. 620 6. 96
336 633(6) 8. 33(8) O. 793 10. 5(1)
93 19. 2 493 0.649 O. 180 3. 6(1) 1. 4( 6)
58. 7 233(2) 3. 06( 9) 0.401 7. 6(5)
136. (5) 6 40 (1) 8. 42 (4) O. 609 13.8(3)
324 118 40 15.58 O. 787 19.8(0)
(jJ Dimethylsulfoxide 20 5. 2 5. 2 0.0068 0.059 O. 115 O. 104 32
:I> 17. 1 21 0.028 O. 173 O. 162
.-1 38. 1 71 0.093 O. 317 O. 293
-I
[T1 Ditolylmethane 25 O. 32 12.(9) 0.017 0.009(7) 1. 7(5) 1. 7(0) 28
r 1. 39 53. 8 0.0708 0.040(9) 1. 73
r 4. 19 160 O. 21 0.113(8) 1. 85
[T1 9. 42 439 O. 5775 O. 224(0) 2.58
40 0.81 53. 8 0.0708 o. 29(7) 2.3(2) ;p
z I
2. 64 160 O. 21 0.74(8) 2.81 c..,.
o
;u 5.58 439 O. 5775 O. 146(0) 3. 96
-I N -Ethylaniline 25 9.62 45. 0 0.0592 0.154 0.384 O. 29 8
I 19.08 99.5 O. 1309 O. 265 O. 494
< 28.33 171. 0 O. 2250 0.349 0.645
fTI 37.32 263.0 O. 3461 O. 414 0.836
(f) 49. 99 376. 5 O. 4954 0.465 1.065
-j 54.29 508. 5 0.6691 O. 507 1. 320
62. 53 653. 5 0.8599 O. 542 1. 587
Ethyllaurate 25 23. 2 1090 1. 44 O. 453 3. 1(7) 2.7 31
49. 4 1860 2. 45 0.638 3.84
146 2580 3. 40 O. 839 4. 06
154 2630 3. 46 0.846 4.09
1-Heptanol 25 33. 4 1530 2.01 O. 377 5. 33 6. (4) 3
92. 5 2260 2. 97. 0.626 4.74
271 2610 3. 54 O. 831 4. 26
-------
Compound t w r P x PIx A Ref
-
1- Methy laniline 25 1. 26 7.0 0.0092 0.0206 o. 44(7) O. 4( 4) 8
2. 93 15. 5 0.0204 O. 467 o. 43(7)
4. 42 28. 5 0.0375 O. 0688 O. 545
6. 22 40. 5 0.0533 0.0942 O. 566
2-Methylaniline 15 9. 0 23. 0 0.0303 O. 131 O. 231 O. 17(2) 8
19. 2 58.0 0.0763 0.243 O. 314
25 8. 6 40. 5 0.0533 O. 126 O. 423 O. 29(6)
19. 4 121. 5 O. 1599 O. 245 0.653
(jJ 29.0 226. 5 O. 2980 O. 327 0.911
» N - Methylaniline 25 7.4 17.5 0.0230 O. 110 0.204 O. 16(5) 8
-I 15. 4 40.0 O. 526 O. 205 O. 257
-I
fT1 23.7 70. 5 0.0928 0.284 0.326
r 31. 4 112.4 0.1479 O. 344 O. 430
r 39. 0 164. 1 0.2159 0.395 O. 547
fT1 46.2 235.0 O. 3092 O. 436 O. 709
I 53. 6 327.0 O. 4303 0.473 O. 910 ~.
z 60.4 434. 0 O. 5711 O. 502 1. 138 I
0)
o 66. 7 550. 5 O. 7243 O. 527 1. 374
:u 2-Methylpyridine 30 5.8 0.007 0.077 0.09 0.08 30
-I 5
I 11. 1 13 0.017 O. 139 O. 12
< 17.7 23 0.030 O. 204 O. 15
fT1 Nitrobenzene 25 28. 8 990 1. 30 O. 371 3. 5( 1) 3. (2) 31
(J) 64. 4 1620 2.13 O. 569 3.7(5)
-I 260 2470 3.25 O. 842 3. 8(6)
262 2550 3.35 O. 843 3. 9(7)
2 -Octanone 25 33. 6 850 1. 12 0.402 2.7(9) 1. 9(7) 31
77.7 1520 2.01 O. 609 3. 3(0)
292 2590 3. 40 O. 854 3. 9(9)
Quinoline 25 7.2 14.3 0.0188 O. 127 0.148 0.06(5) 8
11. 0 34. 2 0.0450 O. 182 0.247
-------
Compound t w r P x PIx A Ref
Tetraethylene glycol 25 6. 4 32 0.042 O. 157 o. 26( 4) o. 18(3) 31
dimethyl ether 9. 8 65 0.085 O. 253 O. 336
16. 3 119 O. 157 O. 361 O. 433
27.0 212 O. 279 O. 484 O. 576
58. 8 626 0.823 0.671 1. 22(7)
38 6. 4 64 0.084 O. 157 o. 53(3) 0.37(5)
9. 8 116 O. 153 O. 253 O. 60(5)
16. 1 212 O. 279 O. 359 o. 77(7)
OJ 26. 9 381 O. 502 0.483 1. 03(8)
:I> 66 6. 4 184 O. 242 O. 157 1. 54 1. 4( 2)
~ 9. 7 336 O. 442 O. 252 1. 75(5)
~ 16. 1 623 O. 819 0.358 2. 28(9)
fTl 27.0 1140 1. 50 0.484 3. 09( 3)
r
r 93 6. 4 448 O. 589 O. 157 3. 7(5) 3. 5(0)
fTl 9.7 819 1. 077 O. 251 4. 2( 9)
I 15.9 1480 1. 95 O. 355 5. 4(9) ;p
z 26. 2 2560 3.37 O. 476 7. 0(8) I
o -J
;u
~
I
~
fTl
(f)
.~
-------
B-1
APPENDIX B
1.
Conard.
Albertson, Noel F., and Fernelius, W.
ADDITION COMPOUNDS OF S02.
J. Am. Chern. Soc. 65, 1687-90 (1943)
CA 37, 6577
2.
Albright, Lyle F., Shannon,Paul T., Yu, Sun- Nien, and
Chueh, Ping Lin. . .
SOL UBILITY OF SULFUR DIOXIDE IN POLAR ORGANIC
SOLVENTS. .
Chern. Eng. Progr., Symp. Ser. 59(44), 66-74 (1963) .
CA 59, 3363
3.
Allison, S. A., and Barrer, R. M.
CLATHRATION BY PHENOL AND QUINOL.
PART 1. EQUILIBRIA. .
Trans. Faraday Soc. 64(2), 557 - 65 (1968)
4.
Anon.
HIGH-PURITY LIQUID SULFUR DIOXIDE FROM ROASTER
GASES. .
Chern. Eng. 60, No.4, 274-7 (1953)
CA 47, 4659
5.
Anon. .
RECOVERY OF SULFUR FROM SPENT OXIDE.
Gas World 57, 497 .
CA 7, 547
6.
Anon.
THE SULFIDINE PROCESS FOR RECOVERING SULFUR
DIOXIDE. . . . ..
Ind. Eng. Chern. ,News Ed. 14, 105 (March 1936)
CA 36, 6497. .. .
7.
. .
Asinger, Friedrich, Schmidt, Walter, and Ebeneder, Franz.
PRODUCTS OF THE SIMULTANEOUS ACTION OF SULFUR
DIOXIDE AND CHLORINE ON ALIPHATIC HYDROCARBONS IN
ULTRAVIOLET LIGHT. 1. . PRODUCTS OF THE. SIMULTANEOUS
ACTION OF SULFUR DIOXIDE AND CHLORINE ON PROPANE IN
CARBON TETRACHLORIDE SOLUTION. .
Ber. 75B, 34- 41 (1942) .
CA 39, 3251
8ATTELLE-NCRTH~EST
-------
10.
11.
12.
13.
14.
B-2
8.
Asinger, Friedrich.
PRODUCTS OF THE COMBINED ACTION OF S02 AND Cl ON
ALIPHATIC HYDROCARBONS IN ULTRAVIOLET LIGHT.
IV. PRODUCTS OF THE COMBINED ACTION OF S02 AND
Cl ON DODECANE.
Ber. 77B, 191-4 (1944)
CA 37, 3048 .
9.
Avdeeva, A. J., andPitelina, N. P.
SOLUBILITY OF SULFUR-CONTAINING GASES IN OILS.
Khim. Prom. 1947, .No. 2, 19'-21
CA 41, 5775
Backer, H. J., and Strating, J.
CYCLIC SULFONES DERIVED FROM BUT ADIENES.
Rec. Trav. Chim. 53, 525-43 (1934)
CA 28, 4697
Backer, H. J., St ratirig , J., and Huisman,L. H. H.
ADDITION OF SULFUR DIOXIDE TO 1, I' BICYCLOHEXENYL.
FORMATION OF DERIVATIVES OF DIBENZOTHIOPHENE
SULFONE. .
Rec. Trav. Chim. 60, 381-90 (1941)
CA 36, 89
Balej, Jan, and Regner, Albert.
THE SYSTEM SULFUR DIOXIDE-DIMETHYLANILINE.
1. ABSORPTION ISOTHERMS.
Collection Czech. Chern. Communs. 21, 1545-52 (1956)
(in German)
II. HEATS OF SOLUTION.
Ibid. 1553- 9
CA 51, 11831
Barwasser, J., and Roesner, G.
OBTAINING SULFUR DIOXIDE FROM INDUSTRIAL GASES.
Reichsant Wirtschaftsausbau, Chern. Ber. Pruf. -Nr. 93
(PB52008), 135-48 (1940) (Pub. 1941)
CA 41, 6374 (1947)
Baume, G., and Pamfil, G.
FUSIBILITY CURVES OF GASEOUS MIXTURES, COMPOUNDS
OF HYDROGEN CHLORIDE AND SULFUR DIOXIDE WITH
METHYL ALCOHOL.
Compt. Rend., 152, 1095-7
CA 5, 2769
EAT TEL L E - NOR T H \V EST
-------
15.
16. .
17.
18.
19.
20.
21.
22.
B-3
Baume, G.
VOLATILE SYSTEMS. FUSIBILITY CURVES OF THE SYSTEMS
FORMED BY METHYL OXIDE WITH HYDROCHLORIC ACID
,
WITH SULFUR DIOXIDE AND WITH METHYL CHLORIDE.
J. Chim. Phys. 12, 216-24 (1914); 9, 245 (1911)
Compt. Rend. 148, 1322 (1909) .
CA 9, 547
Baume, G., and Pamfil, G. P.
VOLATILE SYSTEMS. FUSIBILITY CURVES OF SYSTEMS
FORMED BY HYDROCHLORIC ACID AND SULFUR DIOXIDE
WITH METHYL ALCOHOL. MECHANISM OF ESTER
FORMA TION. . .
J. Chim. Phys. 12, 256-69 (1914)
CA 9, 547 .
Bhatnagar, Vijay Mohan (Punjab Univ. ,Chandigarh, India)..
CLATHRATE COMPOUNDS OF QUINOL. .
DeL Sci. J. (N. Delhi), Suppl.. 13(4), 57-66 (1963) Eng. )
CA 67, 121180 .
Bianconi, A., and Bianchi, A. .
THE CHEMICAL REACTION BETWEEN SULFUROUS ACID
AND COMPOUNDS OF AN ALDEHYDIC OR KETONIC NATURE.
Ann. Chim. Applicata 22, 291- 316 (1932)
CA 26, 6025 .
Bienstock, D., Others.
SULFUR DIOXIDE - ITS CHEMISTRY AND REMOVAL FROM
INDUSTRIAL WASTE GASES .
U. S. Bureau of MineS Info. Circular 7836 (1958)
TN 1. U56 #7836
Binns, Frederick W., and Lurie, Joseph M.
SULFUR DIOXIDE ADDITION DERIVATIVE OF NITROSO-
i3 - N APHTOL.
U. S. 1,822,122, Sept. 8
CA 25, 5901
Blohm, C. L.
PROCESSING SULFUR BEARING GASES.
Petroleum Eng. 24, C68-74 (April 1952)
Eng. Index 1952 .
Boeseken, J., and Muller, H. D. .
PRECISE DETERMINATION OF VERY SMALL QUANTITIES OF
GASES CONTAINING SULFUR (HYDROGEN SULFIDE, SULFUR
DIOXIDE AND CARBON DISULFIDE) IN THE ATMOSPHERE.
WHEN THEY ARE PRESENT SIMULTANEOUSLY.
Rec. Trav. Chim. 50, 1117-24 (1931)
CA 26, 1212
BATTELLE-NORTHWEST
-------
B-4
23.
Brehmer, T. E., and Nirkko, P.
SULFUR DIOXIDE AND DIMETHYLANILINE. .
Finska Kemistsamfundets Medd. 65, 19-24 (1956) (in Swedish)
CA 50, 13566 .
Brehmer, T.' E., and Ruuskanen, p, (Tek. Hogskolan,
Helsingfors) .'
THERMODYNAMIC PROPERTIES OF SOME SOL VENTS USED
IN ABSORPTION-TECHNIQUE REFRIGERATION.
Finska Kemistsamfundets Medd. 60, 20-34 (1951)
CA 46, 10838
24.
25.
Bright, J. Russell, and Jasper, Joseph j. .
MOLECULAR SURFACE ENERGY OF SULFUR DIOXIDE
ADDITION COMPOUNDS. I. .
J. Am. Chern. Soc. 63, 3486-8 (1941)
CA 36, 947 .
Bright, J. Russell, arid Jasper, Joseph J.
MOLECULAR SURFACE ENERGY OF SULFUR DIOXIDE
ADDITION COMPOUNDS. II.
J. Am. Chern. Soc. 65, 1262-3 (1943); d. CA 36, 947
CA 37, 4944
26.
27.
Bright, J. Russell, and Fernelius, W. Conard.
TEMPERATURE-CONCENTRATION EQUILIBRIA IN THE
SYSTEM DIMETHYLANILINE-SULFUR DIOXIDE.
J. Am. Chern. Soc. 65, 637- 9 (1943)
CA37, 3326
28.
Briner, E., and Cardoso, E.
THE COMPRESSIBILITY AND VAPOR PRESSURE OF MIXTURES
OF METHYL OXIDE AND SULPHUR DIOXIDE.
Compt. Rend., 144911'-13 (1907)
CA1, 1818
Burg, A. B.
THE BEHAVIOR OF Me3N, Me:lNSO~, and Me3NO TOWARD S02'
J. Am. Chern. Soc. 65, 1629-3'5 (19Zl3)
CA 37, 5641
de Carli, F. -
ADDITION PRODUCTS OF SULFUR DIOXIDE AND AROMA TIC
HYDROCARBONS.
. Alli Accad. Lincei (6) 4,460- 6 (192 S)
CA21,738
29.
30.
31.
de Carli, F.
ADDITION PRODUCTS OF SULFUR DIOXIDE AND AROMA TIC
HYDROCARBONS. II.
Alli Accad. Lincei (6) 4, 523-30 (1926)
CA 21, 1449
BAT TEL L E - N aRT H WEST
-------
34.
35.
36.
37.
38.
39.
B""S'
32.
Christian, Sherril D., and Grundnes, Just. (Univ. Oslo, Norway).
CHARGE- TRANSFER COMPLEX BETWEEN SULFUR DIOXIDE.
AND TRIMETHYLAMINE IN THE GAS PHASE AND IN HEPTANE.
Nature 214 (5093), 1111-12 (1967)(Eng.); cf. Burg, CA 37; 5641 .
CA 67, 69057 .
33.
Collin, F. C. .
PURIFICATION OF GASES FROM METALLURGICAL PLANTS
AND RECUPERATION OF SULFUR DIOXIDE.
Tids. Kjerni, Bergvesen Met. 1, 112-17 (1941)
CA 36, 5738
Cupr, Vaclav.
THE ABSORPTION OF HYDROGEN CHLORIDE AND SULFUR
DIOXIDE IN SULFURIC ACID AND ACETIC ACID.
Spisy Vydavane Prirodovedeckou Fakulton Masarykovy Univ.
1926, No. 68, 5-17
CA 20, 3781
Cupr, Vaclav. .
THE ABSORPTION OF HYDROCHLORIC ACID GAS AND SULFUR
DIOXIDE IN SULFURIC AND ACETIC ACIDS.
Rec. Trav. Chirn. 47, 55-72 (1928)
CA 22, 1262
Dodgson, John W.
REDUCTION OF SUBSTITUTED p~BENZOQUINONES BY
SULFUR DIOXIDE ALONE AND IN THE PRESENCE OF ALKALI.
J. Chern. Soc. 1930, 2498- 2502; d. CA 9, 206
CA 25, 691
Dokladalova, J., and Stankova, 0., (Univ. Olornouc, Czech.)'.
THE SCHIFF REACTIONS WITH THE USE OF COMPLEXED
SULFUR DIOXIDE.
Mikrochirn. Ada 1968 (1), 219-27(Ger.)
CA 68, 56442
Dunken, H., and Winde, H.
INTERACTIONS OF SULFUR DIOXIDE WITH POLAR.
COMPOUNDS. EFFECTS OBSERVED IN THE UV ABSORPTION
SPECTRUM. .
Z. Phys. Chern. (Frankfurt am Main) 56(5-6), 303-8 (1967)(Ger. ) .
CA-68, 86647 .
Ebel, C..
DIE FABRIKATION VON SCHUHCREME UND BOHNERWACHS.
BAND 45 OF "MONOGRAPHIEN UBER CHEMISCH-TECHNISCHE
FABRIKATIONSMETHODEN: "
Berlin, Hirschwalksche Buchhandlung. 168 pp.
CA 24, 3864
BATTELLE-NORTf-'WEST
-------
40.
41.
42.
43.
44.
45.
46.
47.
B-6
Emelin, V. P., Zolotarev, E. K., and Yudin, A; M.
KINETICS OF ABSORPTION OF SULFUR TRIOXIDE IN THE
SULFONATION OF NITROBENZENE BY GASEOUS S03'
Khim. Prom. 1965(1), 30-1 (Russ.)
CA 62, 8961
"
Ephraim, Fritz, and Piotrowski, H.
ACTION OF SULFUR AND COMPOUNDS CONTAINING SULFUR
ON HYDRAZINE. .
Ber. 44, 386- 94
CA 5, 1880
Feigl, F, and Feigl, E. .
THE TERNARY COMPOUNDS OF SULFUR DIOXIDE WITH
KETONES AND AMINES.
Z. Anorg. Allgem. Chern.
CA 26, 1576
Fernelius, W. Conard, Audrieth, Ludwig F, Bailar, John C., Jr.
Booth, Harold S., Johnson, Warren C., Kirk, Raymond C. ,
Schumb, Walter C., and Scott; Janet D. .
INORGANIC SYNTHESIS.
Inorg. Syntheses II, 294 pp. (1946) - 48
CA 40, 7025
Ferroni, Enzo, and Cocchi, Marco. (Univ. F1orence)
EPITAXY OF CLA THRA TES.
Ann. Chim. (Rome) 48, 630-6 (1958); d. CA 52, 14301d
CA 53, 16633
Fleming, E. P., and Fitt, T. C.
LIQUID SULFUR DIOXIDE FROM WASTE SMELTER GASES.
USE OF DIMETHYLANILINE AS ABSORBENT.
Ind. Eng. Chern. 42, 2253- 58 (1950)
Fluck, Ekkehard, and Binder, Herbert. (Univ. Heidelberg, Ger.
NUCLEAR MAGNETIC RESONANCE OF PHOSPHORUS .
COMPOUNDS. XVI. REACTIONS OF PHOSPHORUS(III)
COMPOUNDS WITH SULFUR DIOXIDE.
Z. Anorg. AUg. Chern. 354(3-4), 139-48 (1967)(Ger.)
CA68, 25326
Foote. H. W., and Fleischer, Joseph.
EQUILIBRIUM IN SYSTEMS COMPOSED OF SULFUR DIOXIDE
AND CERTAIN ORGANIC COMPOUNDS. .
J. Am. Chern. Soc. 56, 870-3 (1934); d. CA 25, 3551; 26, 5822
. CA 28, 3290 .
BATTELLE-NORTHWEST
-------
48.
49.
50.
51.
52.
53.
54.
55.
56.
B-7
Frederick, D. S., Cogan, H. D., and Marvel, C. S.
REACTION BETWEEN SULFUR DIOXIDE AND OLEFINS.
CYCLOHEXENE.' ,
J. Am. Chern. Soc. 56, 1815-19 (1934)
CA 28, 6118
Gel'perin, N. I., Others.
ABSORPTION OF SULFUR DIOXIDE AND CARBON DISULFIDE
IN HYDROCARBONS OF THE DIPHENYLMETHANE SERIES.
Zhur. Priklad. Khirn. 31, 1323- 32 (1958)
J. Applied Chern. USSR 31, 1309-17(1958) - English Trans.
Gerhards, Erich, and Dirscherl, Wilhelm. (Univ. Bonn, Ger.).
REACTION OF S03 WITH CYCLOHEXANE; PREPARATION OF
A POL YENEDIHYDROXYDISULFONIC ACID.
Ann. 642, 71-82 (1961)
CA 55, 71094
Gilbert, E. E.
REACTIONS OF SULFUR TRIOXIDE AND OF ITS ADDUCTS
WITH ORGANIC COMPOUNDS.
Chern. Res. 62, 549-89 (1962)
Gilford, Martin, and Gordon, Saul.
THERMOANAL YTICAL GI ARACTERIZATION OF SEVERAL
QUINOL CLA THRA TE COMPOUNDS.
U. S. Dept. Com., Office Tech. Serv., P B Rept. 145, 517,
23 pp. (1960)
CA 57, 380
Goliath, Marit, and Lindgren, Bengt O. (Forest Prods. Res.
Lab., Stockholm)
MECHANISM OF REDUCTION OF SULFUR DIOXIDE BY
FORMIC ACID.
Ada. Chern. Scand. 16, 570- 4 (1962)(in English)
CA 51, 5558
Gomes, A., and Joullie, M. M. .
CYCLOADDITION OF KETENE AND IMINES TO SULFUR
DIOXIDE.. .
Chern. Cornrnun. 1967(18), 935-6(Eng. )
CA 68, 21875
Good, A., and Thynne, J. C. J. (Univ. Edinburgh, Scot.)
REACTION OF FREE RADICALS WITH SULFUR DIOXIDE.
I. METHYL RADICALS.
Trans. Faraday Soc. 63(11) ,2708 -19 (1967) (Eng. )
C A 68, 122 19 and 1 2220
Guiselin, A. L. C. ,
USE OF MINERAL OILS AS SOLVENTS FOR SULFUR DIOXIDE.
Mat. Grasses, 6, 3144-5 ,
CA 7, 4048
8~TTELLE-NORTHWES,T
-------
B-8
57.
Guss, L. S., and Kolthoff, 1. lVI.
THE BEHA VIOR OF S02 AS AN ACID IN MeOH.
J. Am. Chem. Soc. 66,1484-8 (1944)
'CA38,6165 .
58.
Guyot, J., and Simon, L. J.
ACTION OF SULFURIC ANHYDRIDE AND OLEUM ON METHYL
ALCOHOL. PREPARATION OF DIMETHYL SULFATE.
Compt. Rend. 169, 795-7 (1919); cf. CA 14, 403
CA 14, 539
59.
Hamill, Wm. H. .
EQUILIBRIA IN SOLUTIONS.
Proc. Indiana Acad. Sci. 51,
CA 37, 22
165-6 (1941)(Pub. 1942)
60.
Hampson, N. H.
ECONOMIC ELIMINATION OF AIR POLLUTION THROUGH
RECOVERY OF PRODUCTS IN POLYESTER GAS SCRUBBERS.
Alle. Papier-Rundschau No. 21, 1392, 1394, 1396 (1965)
CA 66, 31834 .
61.
Hexter, R. M., and Goldfarb, T. D.
INFRARED SPECTRA OF QUINOL CLATHRATECOMPOUNDS.
J. Inorg. & Nuclear Chem. 4, 171-8 (1957)
CA 51, 12660 .
62.
Hill, Arthur E. .
REACTION OF AMINES WITH SULFUR DIOXIDE.
1. ANILINE AND SULFUR DIOXIDE.
J. Am. Chern. Soc. 53, 2598-2608 (1931)
CA 25, 4482
63.
Hill, Arthur E., and Fitzgerald, Thomas B. .
. COMPOUNDS OF SULFUR DIOXIDE WITH VARIOUS AMINES.
J. Am. Ci1(~m. Soc. 57, 250-4 (1935)
CA 29, 1689
64.
Hjrd, S. A., and Lloyd, L. L.
THE ACTION OF SULFUR DIOXIDE UPON OILS
J. Soc. Chern. Ind., 31, 316-9
CA 6, 1688 .
65.
Hoffman, Kenneth R., and VanderWerf, Calvin A. ..
ADDITION COMPOUNDS' OF SULFUR DIOXIDE WITH PYRIDINE
AND THE PICOLINES. . .'.
J. Am. Chern. Soc.' 68, 997-1000 (1946)
CA 40, 5433
BATTELLE-NORTHWEST
-------
72.
B-9
66.
Horiuchi, Juro.
THE SOLUBILITY OF GAS AND THE COEFFICIENT OF
DILATATION BY ABSORPTION. II. '
Bull. Inst. Phys. Chern. Research (Tokyo) 9, 697 -73'0 (1930>
CA 25, 3543 '
67.
Horiuchi, Juro. '
THE SOLUBILITY OF GAS AND THE COEFFICIENT OF
DILATATION BY ABSORPTION. III.
Bull. Inst. Phys. Chern. Res. (Tokyo) 10, 374-401
CA 25, 5609
68.
Hunt, Madison, and Marvel,C. S.
REACTION BETWEEN SULFUR DIOXIDE AND OLEFINS.
II. PROPYLENE.
J. Am. Chern. Soc. 57, 1691-6 (1935); d. CA 28, 6118
CA 29, 7276 '
69.
Ingles, D. L. (C. S. 1. R. 0., Div. Food Preservation,
North Ryde, Australia)
SOME NOVEL ADDUCTS OF SULFUR DIOXIDE WITH
CARBONYLS AND AMINO ACIDS.
Chern. Ind. (London) 1967(35) 1492-3(Eng.)
CA 68, 96115
70.
Ipatieff, V. N., and Monroe, G. S.
DETERMINATION OF SOLUBILITIES OF GASES AT HIGH,
TEMPERATURES AND HIGH PRESSURES BY THE ROTATING
BOMB. '
Ind. Eng. Chern., Anal. Ed. 14, 166-71 (1942)
CA 36, 2196
71.
Ishikawa, Fusao, Mitsui, Saburo, and Murooka, Toyosaku.
EQUILIBRIUM IN THE SYSTEM CONSISTING OF CAMPHOR
AND SULFUR DIOXIDE.
, Sci. Repts. Tohoku Irnp. Univ., 1st Ser. 23, 852-70 (1935)
Bull. Inst. Phys. Chern. Res. (Tokyo) 13, 684-96 (1934)
, CA 29, 4245
Ivanov, Trifon., (Inst. Technol Super. Ind. Alirnentaires,
Plovdiv, Bulg.).
OXIDATION OF GRAPE MUST. II. A COMPARATIVE STUDY
OF SULFUR DIOXIDE AND BENTONITE RN AS INACTIV A TORS
OF GRAPE MUST POL YPHENOLOXIDASE. ' '
Ann. Techno!. Agr. 16(2), 81-8 (1967}(Fr.); d. CA 67; 72433g
. CA 68, 28446
BAT TEL L E -,N 0 R T H W EST
-------
I
,78.
B-10
73.
Jasper, Joseph J., and Bright, J. Russell.
MOLECULAR SURF ACE ENERGY OF S02 ADDITION
COMPOUNDS. III. .
J. Arn. Chern. Soc. 66, 105-6 (1944); cf. CA 37, 4944
CA 38, 1157
74.
Jeffrey, G. A.', and McMullan, R. K.
THE CLATHRATE HYDRATES
Prog. in Inorg. Chern. 8, 43-108 (1967)
CA 68, 56004
75.
Johnstone, H. F.
RECOVERY OF SULFUR DIOXIDE FROM WASTE GASES.
EQUILIBRIUM PARTIAL VAPOR PRESSURES OVER SOLUTIONS'
OF THE AMMONIA-SULFUR DIOXIDE-WATER SYSTEM.
Ind. Eng. Chern. 27, 587-93 (1935)
CA 29, 4137 .
76.
Johnstone, H. F., Read, H. J., and Blankrneyer, H. C.
RECOVERY OF SULFUR DIOXIDE FROM WASTE GASES.
EQUILIBRIUM VAPOR PRESSURES OVER SULFITE- BISULFITE
SOL UTIONS. ' . '
Ind. Eng. Chern. 30, 101-9 (1938)
CA 32, 1874
77.
Kalaushin, A. E., Leont'eva, L. S., Frurnkina, A. Kh, and
Kas'yan, D. T.
PROCESS OF RENDERING HARMLESS SULFUR WASTE GASES
UNDER FOAM CONDITIONS. '
Neftepererab. Neftekhirn. 1967(9), 30-2(Russ.)
CA 68, 51692 .
Kangun, 1.
THE DETERMINATION OF SULFUR DIOXIDE IN THE PRESENC'E
OF OXIDES OF NITROGEN IN THE CHAMBER AND TOWER
GASES.
J. Chern. Ind. (Moscow) 1934, No.5, 33-5
CA 28, 5365
79.
Katz, M., and Cole, R. J.
RECOVERY OF SULFUR COMPOUNDS FROM ATMOSPHERIC
CONTAMINANTS. . ,
Ind. Eng. Chern. 42, 2258-69 (Nov. 1950)
80.
Kerp, W., and Wohler, P.
CONTRIBUTION TO THE KNOWLEDGE OF COMBINED
SULPHUROUS ACID. '
Arb. Kais. Gesundheitsarnt., 32, 120- 43
, CA 4, 380
BATTELLE-NORTHWEST
-------
B-ll
81.
Konopator, A. P., and Strom, L. D.
PRODUCTION OF SULFUR FROM HYDROGEN SULFIDE OF
REFINERY GASES. .
Neftepererab. Neftekhim. 1967(2), 25-9 (Russian)
CA 67, 13550 .. .
82.
Kulcsar, Geza J., Makkay-Beke, Clara, and Vodnar, loan.
THE SYSTEM S02-ANILINE. 1. ABSORPTION ISOTHERMS.
Studia Univ. Babes-Bolyai l,No. 2, 163-71 (1960)
CA 56, 5795 .
83.
Kulcsar, Geza J., Vodnar, loan, and Santa, Stefan.
THE SYSTEM S02-ANILINE.. . .
II. DETERMINATION OF THE HEAT OF ABSORPTION
. Studia Univ. Babes-Bolyai Ser. I, No.2, 155-8 (1961)
d. CA 56, 5795b .
CA 57, 10578
84.
Kulcsar, Geza J., and Lengyel-Szabo, Gyorgyi. (Univ. Babes-
Bolyai, Cluj, Romania) .
THE SYSTEM SULFUR DIOXIDE-ANILINE.
III. ABSORPTION ISOTHERMS IN AQUEOUS SOLUTION.
Studia Univ. Babes- Bolyai, Ser. Chemia 9(1), 77 - 83 (1964)
cf. CA 57, 10578c
C A 61, 1 5403
85.
Lecher, Z., and Hardy, W. B.
COMPOUNDS OF TRIALKYLAMINE OXIDES WITH SULFUR
DIOXIDE AND TRIOXIDE. II. .
J. Am. Chem. Soc. 70, 3789- 92 (1948)
CA 43, 2574
86.
Lepouse, Hector. . .
THE ACTION OF SULFURIC ACID AND SULFURIC ANHYDRIDE
ON ACETYLENE DICHLORIDE.
Bull. Soc. Chim. Belg. 34, 133-42 (1925)
CA 19, 2323
87.
Lloyd, Stewart J.
SOME SOLUBILITY MEASUREMENTS.
J. Phys. Chem. 22, 300-3 (1918)
CA 12, 1433
88.
Locket, Geo. H.
MOLECULAR ASSOCIATION OF AROMATIC HYDROC ARBONS
WITH THIONYL CHLORIDE, SULFURYL CHLORIDE AND
SULFUR DIOXIDE.
J. Chem. Soc. 1932, 1501-12
CA 26, 403 .
BAT TEL L E - NOR. T H \V EST
-------
89.
90.
91.
92.
93.
94.
95.
96.
97.
B-12
MacFarlane, Walter, and Wright, Robert.
SOL UBILITY OF VAPORS IN GASES.
J. Chern. Soc. 1934, 207-10
CA 28, 3952
Makrauczy, Jozsef, and Mohai, Bela.
GAS ABSORPTION STUDIES. XI. ACID-BASE EQUILIBRIUMS.
1. ABSORPTION OF SULFUR DIOXIDE IN POTASSIUM,
AMMONIUM, AND BARIUM HYDROXIDE SOLUTIONS.
Veszpremi Vegyip. Egyet. Kozlemeny. 6, 173-82 (1962);
cf. CA 57, 4505b
CA 58, 6252
Marks, G. W., and Ambrose, P. M. ..
DIETHYLENETRIAMINE AND OTHER AMINES AS AGENTS
FOR THE RECOVERY OF SULFUR DIOXIDE. .
U. S. Bur. Mines, Rept. Investigations No. 3339, 41-6 (1937)
CA 31, 6422
Mazzetti, C., and de Carli, F.
ADDITION PRODUCTS OF SULFUR DIOXIDE WITH BEN ZENE.
Gazz. Chim. Ital. 56, 34-6 (1926) .
CA 20, 1984
Michael, Arthur, and Weiner, Nathan.
MECHANISM OF THE SULFONATION PROCESS.
J. Am. Chern. Soc. 58, 294-8 (1936)
CA 30, 2922
Mousseron, Max.
ALICYCLIC S DERIVATIVES.
Compt. Rend. 216, 812-14 (1943); d.
CA 38, 4568
CA 38, 3623
Mousseron, Max., and Granger, Robert.
VI. THE ORGANOMAGNESIUM COMPOUNDS.
Bull. Soc. Chim. 1946, pp. 251-56
CA 40, 6430
Naulmann, A. .
REACTIONS IN NON-AQUEOUS SOLUTIONS.
VI. IN ACETONITRILE.
Giessen. Ber., 47, 247-56; d. CA 4, 1851
. CA 8, 1373
Nelson, H. W., and Lyons, C. J.
SOURCES AND CONTROL OF SULFUR-BEARING POLLUTANTS.
J. Air Pollution Control Assoc. 7(3), 187-93 (Nov. 1957)
8 A T TEL L E - t, 0 R T H \'v' E S. T
-------
100.
101.
102.
103.
104.
105.
B-13
98.
Overberger, C. G., and Moore, J. A.
COPOL YMERIZA TION OF BENZYL VINYL SULFIDE WITH
SULFUR DIOXIDE.
Chern. Ind. (London) 1968(1), 24 (Eng. )
CA 68, 50095
99.
Palin, D. E., and Powell, H. M.
THE STRUCTURE OF MOLECULAR COMPOUNDS.
PART III. STRUCTURE OF ADDITION COMPLEXES OF QUINOL
WITH CERTAIN VOLA TILE COMPOUNDS.
J. Chern. Soc. 1947, 208-21 (1947)
Progress in Inorganic Chern. Vol. 8 p. 103
Pasteur, Felix.
SOME PROPERTIES OF FENCHONE.
Bull. Sci. Pharrnacol. 38, 279-81 (1931)
CA 25, 4164
Paul, Ram Chand, Ahluwalia, S. C., and Pahil, Sarvinder Singh.
(Univ. Panjab, Chandigarh).
THERMOCHEMICAL STUDIES IN DIMETHYLFORMAMIDE.
1. HEATS OF SOLUTION AND NEUTRALIZATION OF
LEWIS ACIDS.
Indian J. Chern. 3(7), 300-4 (1965)(Eng.)
Paul, Ram Chand, Narula, Saraj Parkash, and Mayer, Prabha.
(Panjab Univ., Chandigarh).
CONDUCTOMETRIC STUDIES OF MIXTURES OF SULFUR
TRIOXIDE WI TH ORGANIC ESTERS.
Bull. Nat. Inst. Sci. India No. 29, 209-13 (1965)(Eng. )
CA67,119429 .
Paul, Ram Chand, and Bains, M. S.
(Panjab Univ., Chandigarh, India).
COORDINA TION CHEMISTRY OF SULFUR TRIOXIDE WITH
OXYGEN BASES.
Proc. Int. Conf. Coord. Chern., 8th. Vienna 1964, 366-9 (Eng. );
cf. CA 63, 10986c, 15118c .
CA 67, 81740
Pfeifer, Gyula. (Nehezvegyipari Kutato Int., Veszprern, Hung.)
ABSORPTION OF S02 IN DIMETHYIFORMAMIDE (DMF).
Magy. Kern. Folyoiral 69, No.3, 138-41 (1963)
CA 59, 33638
Pipik, O. G:'
A NEW METHOD FOR DETERMINING THE REACTIVITY OF
ORGANIC SUBSTANCES.
Azerbaidzhanskoe Neftyanoe Khozyaislvo 1936, No. 12, 60-8
CA 32, 4515
SATTELLE-NORTHWEST.
-------
106.
107.
108.
109.
110.
111.
112.
113.
114.
B-14
Pond, Wrn. F.
DETERMINATION OF THE QUANTITY OF SULFUR DIOXIDE
ABSORBED BY A LIQUID.
Chernist- Analyst 18, No.4, 10-11 (1929)
CA 23, 5357
Postnikov, V. F., and.Astasheva, A. A.
THE ABSORPTION OF SULFUR DIOXIDE BY XYLIDINE.
J. Chern. Ind. USSR 17(3), 14-19 (1940)
CA 34, 6777
Postnikov, V. F., and Kunin, T. 1.
EXTRACTION OF SULFUR DIOXIDE FROM THE WASTE
GASES OF CONTACT SULFURIC ACID PLANTS.
Trans. Inst. Chern. Tech. Ivanovo (USSR) No.2, 56-70 (1939)
CA 33, 8927
Powell, H. M. .
THE STRUCTURE OF MOLECULAR COMPOUNDS.
PART IV. CLATHRATE COMPOUNDS.
J. Chern. Soc. 1948, 61-73 (1948)
Pupezin, Jovan; Ribnikar, Slobodan; Knezevic, Zivojin; and
Dokic, Vidosava.
LIQUID- VAPOR EQUILIBRIUM AND THERMODYNAMIC
PROPERTIES OF THE SYSTEM SULFUR DIOXIDE +
DIMETHYL ETHER. .
Bull. Boris Kidric Inst. Nucl. Sci. 17 (4), 297-309 (1966)(Eng. )
CA 67, 47783
Ragirnov, F. M., Kaiaushin, A. E., Leont 'eva, L. S.,
Frumkina, A. Kh., and Kas 'yan, D. T.
REMOVING SULFUR DIOXIDE IN FOAM MIXING CHAMBERS.
Azerb. NeiL Khoz. 44 (8), 38-40 (1965) (Russ.)
CA 64, 4835 .
. Reid, W. S.
CONCENTRATION OF THE SULFUR DIOXIDE CONTENT OF
DWIGHT-LLOYD SINTERING- MACHINE GAS BY
RECIRCULA TION. .
J. Metals 1(4), Trans.' 261-6 (1949)
CA 43, 3753
Renzanigo, F. . .'
ANALYTICAL DETERMINATION OF SMOKE POLLUTANTS
FROM COMBUSTION IN DOMESTIC HEATING UNITS.
Riv. Cornbust. 21(10), 506-20 (1967)(Ital).
CA 68, 81176 .
Ries, E. D., and Clark, 1. E. .
ANALYSIS OF SULFUR DIOXIDE IN THE PRESENCE OF
EXCESS AIR. .
Ind. Eng. Chern. 18, 747 (1926)
CA 20, 2800
BATTELLE-NORTHWEST
-------
115.
;1.16.
117.
118.
119.
120.
121.
122.
B-15
Riezebos, Gerrit; van Dorp, David A., and Schweigl, Othrnar F.
N-SUBSTITUTED AMINOALKANESULFONIC ACIDS FOR
DETERGENTS.
U. S. 3, 346, 628 (C1. 260-501), Oct. 10, 1967
CA 67, 116576
Ringstorff, G. W.
ROLE OF METHANE AND OTHER FACTORS IN CONTROLLING
EMISSIONS FROM STEELMAKING PROCESSES.
Met. Soc. AIME-Open Hearth Proc. 46, 438-56 (1963)
Eng. Index 1966, p. 61
Roberson, A. H., and Marks, G. W.
FIXATION OF SULFUR FROM SMELTER SMOKE. PARTIAL
PRESSURES OF SULFUR DIOXIDE OVER SOLUTIONS OF
SULFUR DIOXIDE IN MIXTURES OF WATER AND VARIOUS
ALIPHATIC AMINES.
U. S. Bur. Mines, Rept. Investigations 3415, 45 pp. (1938)
CA 33, 9499
Roesner, G.
THE SULFIDIN METHOD, A NEW METHOD OF UTILIZATION
OF GASES CONTAINING SULFUR DIOXIDE.
Metallu. Erz 34, 5-11 (1937)
CA 31, 1964
Rotariu, George J., Hoskins, Elizabeth L., and
Hattori, Donald M.
DEVELOPMENT OF KRYPTON-85 CLATHRATE ANALYTICAL
TECHNIQUES TO MEASURE OXIDATION-REDUCTION
PRODUCTS IN THE LIQUID STATE.
U. S. At. Energy Comm. TI D-17223, 98 pp. (1962)
CA 60, 1106
Rothenfusser, S.
DETECTION AND DETERMINATION OF SULFUR DIOXIDE.
Z. Untersuch, Lebensm, 58, 98-109 (1929)
CA 24, 1056
Ryden, L. L., and Marvel, C. S.
REACTION BETWEEN SULFUR DIOXIDE AND OLEFINS.
III. HIGHER OLEFINS AND SOME LIMITATIONS OF THE
REAC TION.
J. Am. Chern. Soc. 57, 2311-14 (1935); cf. CA 29, 7276
CA 30, 75
Ryden, L. L., and Marvel, C. S.
POLYSULFONES FROM ACETYLENES AND SULFUR DIOXIDE.
J. Am. Chern. Soc. 58, 2047 - 50 (1936); d. CA 30, 75
CA 30, 8184
BATTELLE-NORTHWEST
-------
r-----~..
123.
124.
125.
126.
127.
128.
129.
130.
131.
B-16
Ryss, 1. G., and Bogdanova, L. P.
SYNTHESIS AND HYDROLYSIS KINETICS OF 8-PICOLINE
SULFUR TRIOXIDE COMPLEX.
Zh. Neorg. Khim. 12(8), 2091-3 (1967) (Russ.)
CA 68, 12092
Schaafsma, A.
THE DISTRIBUTION OF SULFUR DIOXIDE BETWEEN WATER
AND GASOLINE.
Chern. Weekblad 35, 821-3 (1938)
CA 33, 2007
Schmidt- Nickels, Wilhelm.
THE ACTION OF SULFUR DIOXIDE ON THE BALOMAGNESYL
DERIVATIVES OF THE CARBINOLS.
Be r . 62 B, 91 7 - 9 (1929)
CA 23, 5180
Schumacher, H. J., and Stauff, J.
REACTIONS OF HYDROCARBONS WITH SULFURYL CHLORIDE
AND SULFUR DIOXIDE-CHLORINE MIXTURES.
Die Chemie 53, 341- 5 (1942)
CA 37, 5366
Seyer, W. F., and Cornett, W. F.
THE SYSTEM SULFUR DIOXIDE-DECALIN.
Ind. Eng. Chern. 29, 91-2 (1937)
CA 31, 3367
Seyer, W. F., and Gallaugher, A. F.
THE SYSTEM SULFUR DIOXIDE AND NORMAL OCTANE.
Trans. Roy. Soc. Can. 20, 343-5 (1926); d. CA 20, 2607
CA 21, 2572
Seyer, W. F., and Todd, E.
CRITICAL SOLUTION TEMPERATURES OF SYSTEMS OF
SULFUR DIOXIDE AND NORMAL PARAFFINS.
Ind. Eng. Chern. 23, 325-7 (1931)
CA 25, 2040
Seyer, W. F., Martin, K., and Hodnett, L.
SYSTEMS OF SULFUR DIOXIDE AND THE ISOMERIC XYLENES.
J. Am. Chern. Soc. 59, 362- 3 (1937); cf. CA 30, 5863
CA 31, 2502
Shibler, B. K., and Hovey, M. W. .
PROCESSES FOR RECOVERING SULFUR FROM SECONDARY
SOURCE MATERIALS.
U. S. Bureau of Mines Info. Circ. 8076 (1962)
TN 1. U56 #8076
BATTELLE-NORTHWEST
-------
132.
133.
134.
135.
136.
137.
138.
139.
140.
B-17
Slavik, Ivan. (Slovakian Acad. Sci., Bratislava).
THE DECOMPOSITION OF SULFUR DIOXIDE UNDER SULFITE
COOKING CONDITIONS.
Svensk Papperslidn. 64, 427 - 37 (1951) (in German)
CA 55, 21581
Smith, WalterT., Jr., and Chen, Wen-Yean.
PREPARATION OF PHENYL N-SULFINYLHYDRAZINES USING
DIMETHYLFORMAMIDE-SULFUR DIOXIDE REAGENT.
Trans. Ky. Acad Sci. 27(1-2), 37-8 (1966)(Eng.)
CA 68, 869512
Smedslund, Tor H.
DIMETHYL SULFOXIDE AS SOL VENT FOR SULFUR DIOXIDE.
Finska Kemistsamfundets Medd. 59, 40-3 (1950)
CA 46, 4329
Sokol'skii, G. A., and Kuunyants, 1. L.
REACTION OF SULFUR TRIOXIDE WITH
POL YCHLOROETHYLENES.
Izv. Akad. Nauk SSSR, Ser. Khim. 1965(9),
CA 64, 578
1655-7 (Russ. )
Sorokin, V. A., and Puzitzkii, K. V.
REACTIONS BETWEEN BUTADIENE AND SULFUR DIOXIDE.
Sintet. Kauchuk 1933, No.6, 12-16
CA 28, 3339.
Squire, J. M., and Waters, William A.
ADDITION OF PHENYL RADICALS TO SULFUR DIOXIDE.
J. Chern. Soc. 1962, 2068-9
CA 57, 8834
Sackelberg, M. V., Hoverath, A., and Scheringer, Ch.
THE STRUCTURE OF CLA THRA TE COMPOUNDS OF PHENOL.
Z. Elektrochem. 62, 123-30 (1958)
CA 52, 10683
Staudinger, H., and Ritzenthaler, B.
HIGHLY POLYMERIZED COMPOUNDS.
CIV. THE ADDITION OF SULFUR DIOXIDE TO ETHYLENE
DERIVATIVES.
Ber. 68B, 455-71 (1935); cf. CA 29, 766
CA 29, 3976
Stratford, H. W.
SULFONA TION WITH SULFUR TRIOXIDE.
U. S. 3, 056, 831 (CL 260-505), Oct. 2, 1962
CA 58, 1291
BATTELLE-NORTHWEST
-------
141.
142.
143.
144.
145.
146.
147.
148.
149.
B-18
Stutzer, A.
DETERMINATION OF SULFUROUS ACID IN WASTE LYES OF
THE SULFITE CELLULOSE FACTORIES.
Chem. -Ztg., 34, 1167-8
CA 5, 1335
Suter, C. M., Evans, P. B., and Kiefer, James M.
DIOXANE SULFOTRIOXIDE. A NEW SULFATING AND
SULFONATING AGENT.
J. Am. Chern. Soc. 60, 538 -40 (1938)
CA 32, 3405
Suzuki, Hiroyuki., .
PARTITION OF SULFUR DIOXIDE BETWEEN WATER AND
SOME SOLVENTS IMMISCIBLE WITH WATER.
Bull. Inst. Phys. Chem. Research (Tokyo) 19, 1360-3 (1940)
CA 35, 1292
Swisher, E. M.
S02-ACETONE AS A HOUSEHOLD FUMIGANT (FOR INSECTS>'
J. Econ. Entomol. 37, 694-7 (1944)
CA 39, 568
Thomas, T. L., and Clark, E. L.
MOLECULAR SIEVES REDUCE ECONOMIC,
PROCESS PROBLEMS.
Oil Gas J. 65(12) 112-15 (1967)(Eng.)
CA 67, 4525
OPERATIONAL
Timberlake, C. F., and Bridle, P.
FLA VYLIUM SALTS, ANTHOCY ANIDINS, AND ANTHOCY ANINS.
II. REACTIONS WITH SULFUR DIOXIDE.
J. Sci. Food Agr. 18(10), 479-85 (1967)(Eng. )
CA 68, 28494
Troitzkii, M., and Rassolenko, L.
DECOMPOSITION OF SODIUM PHENOLATE WITH SULFUR
DIOXIDE.
Org. Chem. Ind. (USSR) 1, 272- 6 (1936)
CA 30, 6347
Ujhidy, Aurel; Babos, Barnabas; and Farady, Laszlo.
(Ungar, Akad. Wiss., Veszprem, Hung.).
SULFONA TION OF DODECYLBENZENE WITH SULFUR
TRIOXIDE-AIR MIXTURE IN A THIN-LAYER REACTOR.
Chem. Tech. (Berlin) 18(11), 652-4 (1966)(Ger. )
CA 67, 18557
Vasil'ev, A. M.
THE PROBABLE COMPOSITION OF THE EUTECTIC S OF
SOME VOLA TILE SUBST ANC ES.
J. Russ. Phys. -Chem. Soc. 49, 432-41 (1917)
CA 18, 1418
BATTELLE-NORTHWEST
-------
150.
151.
152.
153.
154.
155.
156.
B-19
Vian, A., Andres, A. Soler, and Fernandez, C. Iriarte.
STABILITY AND REA TS OF FORMATION IN PYRIDINES- S02
SYSTEMS OF INDUSTRIAL INTEREST.
Quim. Ind. (Bilbao) 13(2), 47-53(1966)(Span.)
CA 66 19991
Weidmann, H., and Roesner, G.
PROCESS FOR THE MANUFACTURE OF PURE SULFUR
DIOXIDE.
Ind. Eng. Chern. News Ed. 14, 105 (1936)
Metallges. Periodic Rev. No. 11, 7-13 (1936)
CA 30, 3595
Weissenberger, G., and Hadwiger, H.
THE ABSORPTION OF SULFUR DIOXIDE IN ORGANIC LIQUIDS.
Z. Angew. Chern. 40, 734-6 (1927)
CA 21 3052
Weissenberger, G., and Piatti, L.
OBTAINING SULFUR DIOXIDE FROM WASTE GASES WITH
THE AID OF CYCLIC KETONES.
Chern. -Ztg. 53, 245-7, 266-7 (1929).
CA 23, 3282
Whiting, R. P., Others
ON MECHANISM OF SULPHUR DIOXIDE ABSORPTION IN
AQUEOUS MEDIA.
Tappi 36(4), 172-5 (April 1953)
Eng. Index 1953 p. 1069
Wynne-Jones, W. F. K., and Anderson, A. R.
THE THERMODYNAMIC CONDIT IONS FOR THE FORMATION
AND THE EXISTENCE OF CLATHRATE COMPOUNDS.
Compt. Rend. Reunion Ann. Avec. Comm. Thermodynam.,
Union Intern. Phys. (Paris) 1952
CA 48, 34
Yushkevich, J. F., Karzhavin, V. A., Avdeeva, A. V., and
Nikol'skaya, Yu. P.
THE PREPARATION OF SULFUR FROM SULFUR DIOXIDE.
VIII. THE REACTION OF SULFUR DIOXIDE WITH
HYDROCARBONS.
J. Chern. Ind. (Moscow) 1934, No.2, 33-7; d. CA 28, 1474
CA 28, 3844
BATTELLE-NORTHWEST
-------
B-20
157. Agren, Per.
RECOVERY OF SULFUR FROM GASES CONTAINING SULFUR DIOXIDE.
Svensk Papperstidn. 39, 470-82(1936).-
CA 31: 27563 (1937)
158. Anon.
LIQUID SULPHUR FROM COLESHILL ALKAZID PLANT.
Indus Chemist v 40 n 1 Jan 1964,p. 9-12.
Eng. Index 1964, p. 2064
159. Anon.
PILOT PLANT ABSORBS SULFUR IN STATION STACK GASES.
Elec World v 168 n 15 Oct 9 1967, p.29-30.
Eng. Index Mi 68 p. 93
130. Anon.
POLLUTION CONTROL-AND BYPRODUCT SULFUR TOO.
Eng. and Mining J. 169: 91-100 (June 1968)
161. Anon.
PROGRESS IN DEVELOPMENT OF PROCESSES FOR LIQUID REMOVAL
OF HYDROGEN SULPHIDE.
Gas World v 158 n 4140-4141 Dec 21-28 1963,p. 822, 826-7, 829-31.
Eng. Index 1964,p.720
162. AVCO Space Systems Division
REMOVAL OF S02 FROM FLUE GAS. FINAL REPORT.
PB 177, 492 (Nov. 1, 1967)
163. Benny, J. C.
SULFUR DIOXIDE RECOVERY.
Pulp Paper Mag. Can. 46, 598(1945).
CA 39: 44834 (L)
164. Biryukova, L. V., Ovcharenko, V. G., Mironov, A. M.,
Karabaev, A. A.
ISPYT AN IE FORSUNOK I RAZBRYZGIV AYUSHCHIKH USTROISTV,
PRIMENY AEMYKH DL Y A OROSHENIY A V ABSORBERAKH.
Khimicheskaya Promyshlennost n 6 June 1963, p. 64-8.
Eng. Index 1964,p. 2
1 '15. Blomen, T.
ROSENBLAD SYSTEM FOR RECOVERY OF HEAT AND SULFUR
DIOXIDE IN THE CHEMICAL WOOD-PULP INDUSTRY.
Tech. Assoc. Papers 20, 346-8(June, 1937); Paper Trade J. 105,
No. 13, 52-4.
CA 31: 89197 (L)
136. Bloomfield, B. D.
CONTROL OF GASEOUS POLLUTANTS.
Heating, Piping, Air Condo 40 (1), 195-206 (Jan.
APCA ABS June 68, No. 9813
1968).
BATTELLE-NORTHWEST
-------
B-21
1;(. Bloomfield, B. D.
COSTS, EFFICIENCIES, AND UNSOLVED PROBLEMS OF AIR
POLLUTION CONTROL EQUIPMENT.
Air Pollution Control Assn-J v 17 n 1 Jan 1967, p. 28-32.
Eng. Index July 67, p. 5
168. Bondarenko, 1. P., and Zemskaya, E. Kh.
INFLUENCE OF TEMPERATURE ON PERFORMANCE OF ARSENIC-
SODA SULPHUR REMOVAL PLANT.
Coke and Chern USSR (English translation of Koks 1 Khimiya) n 6 1965,
p.53-4.
139. Brief, R. S., and Oiestad, A.
IMPINGEMENT BAFFLE PLATE SCRUBBER FOR FLUE GAS.
Air Pollution Control Assn-J v 14 n 9 Sept 1964, p. 372-7.
Eng. Index 1965, p. 803
170. Broman, C. U., and Iseli, R. R. .
THE CONTROL OF OPEN HEARTH STACK EMISSIONS WITH VENTURI
TYPE SCRUBBERS.
Industrial Heating June 1968, p. 1085-96
171. Chashchin, 1. P. (Poly tech. Inst., Tomsk).
EFFECT OF FIN HEIGHT AND SPACING ON HEAT TRANSFER AND
HYDRAULIC RESISTANCE OF A HEAT EXCHANGER.
Izv. Vysshikh Uchebn. Zavedenii, Khim, i Khim. Tekhnol. 8(4),
674 - 9(1965)(R uss).
CA 64: 3070g
172. Chedd, G.
FERTILIZER FROM FLUE GASES?
New Scientist (London) 36 (569), 281-3 (Nov.
. APCA 1968, No. 9591
1967) .
173. Chute, A. E.
LARGE SULPHUR RECOVERY UNITS.
European Chern. News Large Plant Supplement (London) 21-3
(Sept. 30,1966).
APCA 1967, No. 7947
174. Coykendall, J. W., Spencer, E. F., and York, O. H.
NEW HIGH-EFFICIENCY MIST COLLECTOR.
J. Air Poll. Control Assoc. 18 (5), 315-18 (May 1968).
APCA ABS June 68, No. 9815
175. Csathy, D.
EVALUATING BOILER DESIGNS FOR PROCESS-HEAT RECOVERY.
Chern Eng v 74n 12 June 5 1967, p. 117 -24.
Eng. Index 1961', p. 26
173. Davies, G. A., Ponter, A. B., and Craine, K.
DIFFUSION OF CARBON DIOXIDE IN ORGANIC LIQUIDS.
Can J Chern Eng v 45 n 6 Dec 1967, p. 372-6.
Eng. Index April 68, p. 62-3
BATTELLE-NORTHWEST
-------
B-22
177. Dillon, G. B., and Harris, I. J.
DETERMINATION OF MASS TRANSFER COEFFICIENTS AND INTER-
FACIAL AREAS IN GAS-LIQUID CONTACTING SYSTEMS.
Can J Chern Eng v 44 n 6 Dec 1966, p. 307-12.
Eng. Index July 1967, p. 29
178. Donovan, J. R., and Stuber P. J.
SULFURIC ACID PRODUCTION FROM ORE ROASTER GASES.
J of Metals v 19 n 11 November 1967, p. 45-50.
Eng. Index March 1968, p. 263
179. Douglas, H. R., Snider, 1. W. A., and Tomlinson, II, G. H.
TURBULENT CONTACT ABSORBER.
Chern Eng Progress v 59 n 12 December 1963, p. 85-9.
Eng. Index 1964, p. 2
180. Eckert, J. S., Foote, E. H., Rollison, L. R., and Walter,
ABSORPTION PROCESS UTILIZING PACKED TOWERS.
Indus and Eng Chern v 59 n 2 February 1967, p. 41-7.
Eng. Index June 1967, p. 1
L. F.
181. Field, J. H., Kurtzrock, R. C., and McCrea,
HOW TO PREVENT S02 EMISSION.
Chern. Eng. 74 (13), 158-60 (June 19, 1967).
APCA 1967 No. 8671
D. H.
182. Field, J. H., Benson, H. E., Johnson, G. E., Tosh, J. S., and
Forney, A. J.
PILOT-PLANT STUDIES OF HOT-CARBONATE PROCESS FOR
REMOVING CARBON DIOXIDE AND .HYDROGEN SULFIDE.
U S Bur Mines-Bul 597 1962, 44 p.
Eng. Index 1962, p. 504
183. Francis, Wilfred.
REMOV AL OF SULFUR COMPOUNDS FROM INDUSTRIAL GASES.
Engineering 172, 180-2(1951).
CA 46: 1708
184. Frankenberg, T. T.
REMOV AL OF SULFUR FROM FUELS AND PRODUCTS OF
COMBUSTION.
ASME-Paper 64-WA/APC-2 for meeting Nov 29-Dec 4 1964, 12 p.
Eng. Index 1965, p. 45
185. Fuchs, O.
NEW DEVELOPMENTS IN GAS-SCRUBBING PROCESSES.
Gas-u. Wasserfach 80, 18-24(1937).
CA 31: 19855 (L)
BATTELLE-NORTHWEST
-------
B-23
1 8 :) . Fuquay, J. J.
METEOROLOGICAL FACTORS IN THE APPRAISAL AND CONTROL
OF ACUTE EXPOSURES TO STACK EFFLUENTS.
Second U. N. International Conference on Peaceful Uses of Atomic
Energy, 18: 272 -79. (1958).
187. DEVELOPMENT OF TWO-PHASE CONTACTOR WITHOUT PRESSURE
DROP.
B. GAL-OR. A. 1. Ch. E. J v 12 n 3 May 1966, p. 604-5.
Eng. Index 1966, p.356
188. Galeano, S. F., and Harding, C. 1.
SULFUR DIOXIDE REMOVAL AND RECOVERY FROM PULP MILL
POWER PLANTS.
Air Pollution Control Assn -J v 17 n 8 Aug 1967, p. 536-9.
Eng. Index January 1968, p. 7
189. Ganz, S. N., and Kuznetsov, 1. E.
DESIGN OF OPEN EQUAL-FLOW TOWERS WITH CENTRIFUGAL
SPRAYERS.
Int Chern Eng v 5 n 4 Oct 1965, p. 653-6.
Eng. Index 1966, p. 386
190. Ganz, S. N., Kuznetsov, I. E., and Lokshin, M. A.
DETERMINATION OF SIZE OF HOLLOW SCRUBBERS FOR REMOVING
HYDROGEN SULPHIDE FROM COKE-OVEN GAS.
Coke and Chern USSR (English translation of Koks i Khimiya) n 9 1964,
p. 46-8.
Eng. Index 1965, p. 387
191. Grenier, P.
SOLVENT COUNTER-DIFFUSION IN GAS ABSORPTION.
Can J Chern Eng v 44 n 4 August 1966, p. 213-16.
Eng. Index April 1967, p. 1
192. Guentheroth, H.
NEUERE ERFAHRUNGEN MIT VENTURI-SCRUBBERN FUER DIE
FEINSTREINIGUNG VON GASEN 1M KOKEREIBETRIEB.
Deutsche Gesellschaft fuer Chernisches Apparatewesen-DECHEMA
Monographien v 48 n 835-858 1963, p.329-45.
Eng. Index 1965, p. 858
193. Haley, H. E.
S02 REMOVAL PROCESS PROMISES CLEANER AIR.
Elec. World 167 (20), 71-5 (May 15, 1967).
194. Hamberg, Marvin. (Atlantic Refining Co., Philadelphia, Pa.).
USER LOOKS AT BRAZED ALUMINUM PLATE-FIN EXCHANGER.
Proc. Am. Petrol. Inst. Sect. III 43, 180-94(1963).
CA 61: 12964f
BATTELLE-NORTHWEST
-------
B-24
195. Hangebrauck, R. P., and Spaite, P. W.
STATUS REPORT ON CONTROLLING OXIDES OF SULFUR.
Air Pollution Control Assn-J v 18 n 1 January 1968, p. 5-8.
Eng. Index April 1968, p. 4
19'). Hanhart, J., Kramers, H., and Westerterp, K. R.
RESIDENCE TIME DISTRIBUTION OF GAS IN AGITATED GAS-
LIQUID CONTACTOR.
Chern Eng Science v 18 n 8 August 1963, p. 503 -9.
Eng. Index 1963, p. 277
197. Harris, E. R., and Beiser, F. R.
CLEANING SINTER PLANT GAS WITH VENTURI SCRUBBER.
Air Pollution Control Assn-J v 15 n 2 February 1965, p. 46-9.
Eng. Index 1965, p. 803 .
"
~
198. Hartmann, F., and Roeck. G.
ABSORPTIONSVERSUCHE MIT CINEM BLASENW ASCHER.
Chemic -Ingenieur~Technik v 37 n 3 March 1965, p. 214-18.
Eng. Index 1966, p.2
199. Hellstrom, Arne G.
USE OF ABSORPTION TOWERS FOR RECOVERY OF PRESSURE
RELIEF GASES.
Pulp Paper Maj2;. Can. 47, No.3, 119-22(1946).
CA 40: 4516g- (L)
200. Hensinger, C. E., Wakefield, R, E., and Claus,
TURNING POLLUTION GASES INTO PROFITS.
Eng. Mining J. 169 (2), 131-5 (February 1968f
APCA ABS June 1968, No. 9823
K. E.
201. Hollis, O. L.
SEPARATION OF GASEOUS MIXTURES USING POROUS
POLY AROMATIC POLYMER BEADS.
Analytical Chern v 38 n 2 February 1966, p. 309-16.
Eng. Index'1966, p.3
202. Jameson, G. J.
SOME OPERATING CHARACTERISTICS OF RES0NANT BUBBLE
CONTACTOR.
Instn Chern Engrs-Trans v 44 n 3 1966, p. T91-8.
Eng. Index 1966, p. 3
203.
Johnstone, H. F., and Roberts, M. H.
DEPOSITION OF AEROSOL PARTICLES FROM MOVING GAS
STREAMS.
Industrial and Engineering Chemistry, 41 (11): 2417-23 (1949).
CA 44: 2674e. -
BATTELLE-NORTHWEST
-------
B-25
204.
Johnstone, Ii. F., and Silcox, H. E.
GAS ABSORPTION AND HUMIDIFICATION IN CYCLONE SPRAY
TOWERS.
Industrial and Engineering Chemistry, 39 (7): 808 (1947).
CA 41: 49718. . -
205. Johnstone, H. F., and Singh, A. D.
RECOVER Y OF SULFUR DIOXIDE FROM WASTE GASES.
Industrial and Engineering Chemistry, 29 (3): 286-97 (1937).
CA 31: 37434. -
208. Johswich, F.
SULFUR REMOVAL FROM FLUE GASES-IMPORTANCE AND
POSSIBILITIES. .
Brennstoff Waermekraft 14, No.3, 105 -15(1962).
CA 57: 3745
207. J ohswich, F.
UEBER DEN DERZEITIGEN STAND DER ABGASENTSCHWEFELUNG.
Brennstoff-Waerme-Kraft v 17 n 5 May 1965, p. 238-45; see also
English translation in Combustion v 37 n 4 October 1965, p. 18-26.
Eng. Index 1965, p. 803
208. Jones, W. P.
DEVELOPMENT OF THE VENTURI SCRUBBER.
Industrial and Engineering Chemistry, 41 (11): 2424-7 (1949).
CA 44: 1762f -
209. Jordan, W. von.
VENTURI- UND RADIALSTROM-WAESCHER ZUR KUEHLUNG UND
REINIGUNG VON NUTZ- UND ABGASEN.
Stahl u Eisen v 86 n 7 April 7 1966, p. 399-406.
Eng. Index 1966, p. 1081
210. Katell, S., and Plants, K. D.
HERE'S WHAT 802 REMOVAL COSTS.
Hydrocarbon Processing v 46 n 7 July 1967,
Eng. Index December 1967, p.7
p. 161-4.
211. Katell, S.
REMOVING SULFUR DIOXIDE FROM FLUE GASES.
Chern Eng Progress v 62 n 10 October 1966, p. 67 -73.
Eng Index April 1967, p. 79
BATTELLE-NORTHWEST
-------
B-26
212. Khanin, 1. M., Yakovlev, V.!., and Kartsynel, M. B.
SPRAY -TYPE BENZOLE SCR UBBER WITH RADIALLY - SLOTTED
GAS DISTRIBUTORS.
Coke and Chern USSR (English translation of Koks i Khimiya) n 1 1965,
p. 30-5.
Eng. Index 1965, p. 858
213. Kielback, A. W.
DEVELOPMENT OF FLOATING-BED SCRUBBERS.
Chern Eng Progress Symposium Ser v 57 n 35 1961, p.
Eng. Index 1962, p. 504
51- 4.
214. Kim; J. C., and Molstad, M. C.
FIGURE OPTIMUM ABSORPTION DESIGN.
Hydrocarbon Processing v 45 n 12 December
Eng. Index September 1967, p. 1
1966, p. 107-8.
215. Klimecek, R.. Skrivanek, J., and Bettelheim, J.
BEITRAG Z UR ENTSCHWEFEL UNG VON RAUCHGASEN.
Staub-Reinhaltung der Luft v 26 n 6 June 1966, p. 235-8.
Eng. Index July 1967, p. 29
BATTELLE-NORTHWEST
-------
B-27
216. Kochergin, N. A., Kaganskii, 1. M., Shul'ts, E. Z.
PRIMENENIE KOLONN S DYRCHA TRYMI PROV AL' NYMI T ARELI
-------
B-28
224. Morton, F., King, P. J., McLaughlin, A.
HELICAL-COIL DISTILLATION COLUMNS.
Instn Chern Engrs-Trans v 42 n 8 1964 P. T285-T304.
Eng. Index, 1965, p. 551
225. Nakai, Y. and Yokogawa, T.
THE STUDY OF MULTI-PURPOSE GAS ABSORBER BY WET PROCESS.
[Chern. Ind.] Kagaku Kogyo (Tokyo) 18 (12), 1228-35 (Dec. 1967).
2203. Nevins, J. W.
FINNED TUBE EXCHANGERS SOLVE WIDE VARIETY OF HEAT
TRANSFER PROBLEMS.
Power v 109 n 7 July 1965 p. 62-5.
Eng. Index, 1965, p. 992
227. Nicklin, T., Holland, B. H.
FURTHER DEVELOPMENTS IN STRETFORD PROCESS.
Gas World v 158 n 4125 Sept. 7, 1963, p. 273-8.
Eng. Index, 1964, p. 720
228. Nicklin, T., Brunner, E.
HOW STRETFORD PROCESS IS WORKING.
Petroleum Refiner v 40 n 12 Dec. 1961, p. 141- 6.
Eng. Index, 1962, p. 504
229. Nicklin, T., Holland, B. H.
REMOVAL OF HYDROGEN SULPHIDE FROM COKE OVEN
GAS BY STRETFORD PROCESS.
Deutsche Gesellschaft fuer Chernisches Apparatewesen-DECHEMA
Monographien v 48 n 835-858 1963, p. 243-71.
Eng. Index, 1965, p. 858
230. O'Brien, N. G. and Turner, R. L. (E. 1. du Pont de Nernours & Co.,
Wilmington, Del.).
FIN THERMAL EFFICIENCY DURING SIMULTANEOUS HEAT- AND
MASS-TRANSFER.
A.LCh.E. (Am. Inst. Chern. Engrs.) J. 11(3), 546-8(1965)(Eng).
CA 63: 5257c
231. Oldshue, J. Y.
MIXING
Indus & Eng Chern v 59 n 11 Nov.
Eng. Index, April 1968, p. 32
1967, p. 58-70.
232. Ostergaard, K., Theisen, P. 1.
EFFECT OF PARTICLE SIZE AND BED HEIGHT ON EXPANSION
OF MIXED PHASE (GAS-LIQUID) FLUIDIZED BEDS.
Chern Eng Science v 21 n 5 May 1966, p. 413-17.
Eng. Index, Feb. 1967, p. 31
BATTELLE-NORTHWEST
-------
B-29
233. Otsubo, S., Sanuki, Y., Yamamoto, T., Nakazono, 1., Haruta, M.
OPERATION OF NEWLY INSTALLED LURGI VENTURION TYPE
BLAST FURNACE GAS PRECIPITATOR.
Yawata Tech Report n 249 Dec. 1964, p. 5524-31.
Eng. Index, 1965, p. 858
234. Pasternak, R. .
NEUE VERFAHREN DER H2S- AND C02-ENTFERNUNG AUS GASEN.
Gas- u Wasserfach v 103 n 17 Apr. 27, 1962, p. 417-18.
Eng. Index, 1962, p. 504
235. Plit, 1. G.
ABSORBTSIY A DVUOKISI UGLERODA RASTVOROM
MONOETANOLAMINA V SKRUBBERE S PUL'VERIZATSIONNO-
FORSUNOCHNOI TARELKOI.
Khimicheskaya Promyshlennost n 5 May 1963, p. 57-61.
Eng. Index, 1964, p. 1
23'3. Plit, 1. G.
PUL'VER IZATSIONNYI SKRUBBER-DEKARBONIZATOR.
Khimicheskaya Promyshlennost n 8 Aug. 1964, p. 61-4.
Eng. Index, 1966, p. 1081
237. Plumley, A. L., et al.
REMOVAL OF S02 AND DUST FROM STACK GASES.
Proc. American Power ConL Vol. 29: 592-614 (1967)
TJ5. A55 (1967)
238. Pollock, W. A., Tomany, J. P. and Frieling,
FLUE-GAS SCRUBBER.
Mech Eng. 89 (8), 21-5 (Aug. 1967).
PCA 1967, No. 8683
G. G.
239. Pollock, W. A., Frieling, G., Tomany, J. P.
REMOVAL OF SULFUR DIOXIDE AND FLY ASH FROM COAL
BURNING POWER PLANT FLUE GASES.
ASME-Paper 66-WA/CD-4 for meeting Nov. 27-Dec. 1, 1966,8 p.
Eng. Index April 1967, p. 79
240. Porter, K. E.
EFFECT OF CONTACT-TIME DISTRIBUTION ON GAS ABSORPTION
WITH CHEMICAL REACTION.
Instn Chern Engrs-Trans v 44 n 1 1966 p. T25-36.
Eng. Index 1966, p. 2
BATTELLE-NORTHWEST
-------
B-30
241. Pozin, M. E., Tarat, E. Ya., Tereshchenko, L. Ya., Orekhov, 1. J.
ABSORBTSIYA SEROVODORODA MYSH'YAKOVO-SODOVYM
RASTVOROM PRI TURBULENTONOM (PENNOM) REZHIME.
Zhurnal Prikladnoi Khirnil v 39 n 8 Aug. 1966, p. 1712-19; see also
English translation in J Applied Chern of USSR v 39 n 8 Aug. 1966,
p. 1601-7.
Eng. Index, Oct. 1967, p. '89
Roesner, Gerhard
UTILIZATION OF INDUSTRIAL GASES AND 'V ASTE GASES BY THE
LURGI PROCESSES.
Metallges. Periodic Rev. No. 13, 22-30 (1938).
CA 32: 51047
242.
243. Rosenblad, C. v.
HEAT AND SULFUR DIOXIDE RECOVERY (IN SULFITE MILLS)
WITH AND WITHOUT HEAT EXCHANGERS.
Zellstoff u. Papier 19, 205-9(1939).
CA 33: 65911 (L)
244.
Rosenblad, C. .
RECOVERY OF HEAT AND SULFUR DIOXIDE GAS IN THE SULFITE-
PULP INDUSTRY WITH OR WITHOUT HEAT EXCHANGERS.
Paper Trade J. 8106, No. 26, 78-81(1938).
CA 32: 8135 (L)
245. Ross, T. K., Coombe, A. J.,
GAS ABSORPTION IN MULTIPLE LIQUID-JET CONTACTOR.
Instn Chern Engrs-Trans v 44 n 5 1966 p. T160-5.
Eng. Index, Jan. 1967, p. 93
c:::.
243. Ruckenstein, E., Srnigelschi, O.
THERMAL THEORY AND PLATE EFFICIENCY.
Can J Chern Eng v 45 n 6 Dec. 1967, p. 334-40.
Eng. Index, April 1968, p. 47
Ryason, P. R., Harkins, J.
STUDIES ON NEW METHOD OF SIMULTANEOUSLY REMOVING
SULFUR DIOXIDE AND OXIDES OF NITROGEN FROM COMBUSTION
GASES.
Air Pollution Control Assn-J v 17 n 12 Dec. 1967, p. 796-9.
Eng. Index, March 1968, p. 93
247.
248. Rylek, M., Standart, G.
HYDRAULICS OF SLEVE TRAYS.
Int Chern Eng v 4 n 4 Oct. 1964, p.
Eng. Index, 1965, p. 551
249. Shah, 1. S.
NEW EVAPORATOR-SCRUBBER SYSTEMS IMPROVE KRAFT
RECOVERY PROCESS.
Paper Trade J. 152 (12), 58-64 (Mar. 18, 1968).
APCA June 1968, No.9832
711-47.
BATTELLE-NORTHWEST
-------
B-31
250.
Sharma, M. M.
KINETICS OF REACTIONS OF CARBONYL SULPHIDE AND CARBON
DIOXIDE WITH AMINES AND CAT AL YSIS BY BROENSTED BASES
OF HYDROLYSIS OF COSo
Faraday Soc-Trans v 61 n 508 April 1965, p. 681-8.
Eng. Index, 1966, p. 2
251. Shibler, B. K., Hovey, M. W.
PROCESSES FOR RECOVERING SULFUR FROM SECONDARY
SOURCE MATERIALS.
U.S. Bur Mines-Information Cir 8076 1962, 62 p.
Eng. Index, 1962, p. 1375
252. Shnyakin, A. 1., Ermolaev, V. N.
K VOPROSU 0 TEKHNOLOGII OCHISTKI DOMENNOGO GAZA I
KONSTRUKTSII SKRUBBEROV.
Stal n 2 Feb. 1963, p. 176-8; see also English translation in Stal in
English n 2 Feb. 1963, p. 152-4.
Eng. Index, 1963, p. 786
253. Slesser, C. G. M., Highet, J.
TRANSFER UNIT MODEL OF SLURRIED BED REACTOR.
Brit Chern Eng v 11 n 4 April 1966, p. 247-52.
Eng. Index, Feb. 1967, p. 31
254. Slobodyanik, 1. P.
TESTS ON RING-SHAPED JET PLATE.
Chern & Technology of Fuels & Oils (English translation of Khimiya i
Tekhnologiya Topliv i Masel) n 1 Jan. 1966, p. 43- 6.
Eng. Index, Oct. 1967, p. 54
255. Smith, E. C., Gunter, A. Y., Victory, S. P.,
Corp., Houston, Tex.).
FIN TUBE PERFORMANCE.
Chern. Eng. Progr. 62(7), 57 - 67(19 66)(Eng).
CA 65: 10155b
Jr. (Hudson Eng.
25f1. Squires, A. M.
AIR POLLUTION: THE CONTROL OF S02_FROM POWER STACKS.
PART II. THE REMOVAL OF S02 FROM STACK GASES.
Chern. Eng. 74 (24), 133-40 (Nov. 20, 1967).
APCA ABS 1968, No. 9260
257. Srinivasan, P. R., Gururaja, J., Ramachandran, A.
ISOTHERMAL PRESSURE DROP ALONG TRANSVERSE,
HELICAL & INCLINED FINS IN CIRCULAR ANNULI.
Indian J Technology v 3 n 4 April 1965, p. 103-10.
Eng. Index, 1965, p. 992
TRANSVERSE
BATTELLE-NORTHWEST
-------
B-32
258. Potter, O. E., Sinclair, R. J., Stephens, G. K.
GAS EXCHANGE BETWEEN BUBBLES AND DENSE PHASE IN
FLUIDISED BED.
Powder Technology v 1 n 3 Oct. 1967, p. 157 - 66.
Eng. Index, April 1968, p. 32
259. Swartz, J. N.
SULFITE BLOW HEAT AND GAS RECOVERY.
Pulp Paper Mag. Can. 44, 139-42(1943)
CA 37: 21736 (L)
230. Tarat, E. Ya., Bogatykh, S. A.
OPERATION OF FOAM APPARATUS AT ELEVATED GAS PRESSURES.
Chem & Petroleum Eng (English translation of Khimicheskoe i
Neftyanoe Mashinostroenie) n 4 April 1965, p. 278 -81.
Eng. Index, 1966, p. 3
281. Terres, Ernst, Buscher, Hanna, and Matroff, Georg.
THE REACTIONS INVOLVED AND THE REACTION VELOCITIES
FOR THE REGENERATION OF THE SCRUBBING SOLUTIONS IN
THE METAL THIONA TE PROCESSES FOR PURIFYING COAL
GAS FROM AMMONIA AND HYDROGEN SULFIDE. A MANGANESE
SULFATE PROCESS.
Brennstoff-Chem. 35, 144-51(1954); ef. ivid. 65-74,119-20.
2.')2. Thomas, B. E.
OPERATING STRETFORD PURIFICATION PLANT.
Gas J v 317 n 5243 March 11, 1964, p. 283-5; see also Gas World v
159 n 4157 April 18, 1964, p. 520-2.
Eng. Index, 1964, p. 720
283. Thomas, M. 0., Hill, G. R., and Abersold, J. N.
DISPERSION OF GASES FROM TALL STACKS.
Industrial and Engineering Chemistry, .11(11): 2709 (1949).
CA 44: 2144e
2134. Timberlake, R. C.
FLUORINE SCRUBBER.
Southern Eng. 85 (6), 62-4 (June 1967).
APCA 1968, No. 9616
2')5. Todd, W. G., Van Winkle, M.
ENTRAINMENT AND PRESSURE DROP 'l/ITH JET TRAYS IN
AIR-WATER SYSTEM.
Indus & Eng Chem -Process Design & Development v 6 n 1 Jan.
p. 95-1 Ol.
Eng. Index, July 1967, p. 25
1967,
BATTELLE-NORTHWEST
-------
B-33
266. Towell, G. D., Strand, C. P., Ackerman, G. H.
MIXING AND MASS TRANSFER IN LARGE DIAMETER BUBBLE
COLUMNS.
A.1. Ch. E. -Inst Chern Engrs-1 O. Mixing-Theory Related to
Practice-Paper 10.10 for meeting London, June 13-17 1965,
p. 91-100.
Eng. Index, 1966, p. 3
237. Vlcek, V., Vavra, V., Stary, M.
OPTIMIZATION OF CONDITIONS FOR FOAM-PHASE ABSORPTION
OF SULFUR TRIOXIDE.
Int Chern Eng v 2 n 2 April 1962, p. 216-20.
Eng. Index, 1962, p. 1376
238. \rlalker, A. B., Hall, R. M.
OPERATING EXPERIENCE 'VITH A FLOODED DISC SCRUBBER-
A NE'N VARIABLE THROAT ORIFICE CONT ACTOR.
J. Air Poll. Control Assoc. 18 (5), 319-23 (May 1968).
APCA: June 1968, No. 9837
289. Wallis, E.
RECOVERY OF SULPHUR IN MARKETABLE FORM FROM FLUE
GASES.
Brit Chern Eng v 7 n 11 Nov. 1962, p. 833-6.
Eng. Index, 1963,p. 740
270. 'N eissbach, H.
KOELNER FRUEHJAHRSMESSE 1966-ALLGASGERAETE AUF
BREITER FRONT.
Gas- u Wasserfach v 107 n 21 May 27, 1966, p. 586-92; see also
English summary in Gas J v 327 n 5367 Aug. 17, 1955, p. 171.
Eng. Index, Oct. 1967, p. 89
271. Westerterp, K. R.
DESIGN OF AGITATORS FOR GAS-LIQUID CONTACTING.
Chern Eng Science v 18 n 8 Aug. 1963, p. 495-502.
Eng. Index, 1963, p. 277
272.
Calvert, S., Workman, W. L.
MASS TRANSFER IN SUPPORTED FROTHS.
A.1.Ch.E. J v 12 n 5 Sept. 1966, p. 867-76.
Eng. Index, June 1967, p. 33
BATTELLE-NORTHWEST
-------
B-34
273. Zalogin, N. G. and Sernlyanskii, G. I.
THE REDUCTION OF THE SIZE OF SCRUBBERS AND THE SAVING
OF ELECTRICAL ENERGY IN THE REMOVAL OF S OXIDES FROM
FLUE GAS BY THE LIME METHOD.
Izvest. Vsesoyuz. Teplotekh. Inst. 14, No.2, 19 - 23 (1941); .
Chern. Zentr. 1943, I, 1128.
CA 38: 41196 (L)
274.
Zinov'eva, A. P., Bashkirova, S. G.
EFFICIENCY OF CONTACT BETWEEN HETEROGENEOUS PHASES
AND DEGREE OF CHEMICAL CONVERSION IN FLUIDIZED BED.
Chern & Technology of Fuels & Oils (English translation of
Khirniya i Tekhnologiya Topliv i Masel) n 2 Feb. 1967, p. 77 -81.
Eng. Index, March 1968, p. 35
BATTELLE-NORTHWEST
-------
275.
276.
277.
278.
279.
280.
281.
282.
B-35
PATENTS
Austrian 174,896 (May 11, 1953)
RECOVERY OF CARBON DIOXIDE AND SULFUR DIOXIDE
FROM COMBUSTION GASES.
Bodoni & Co., G. m. b. H. (Desider Bodoni, inventor)
CA47,7750 .
Belg. 670,775 (Apri112, 1966)
U. S. Appl. Oct. 13, 1964, and Jan. 25, 1965
NEW SOL VENT ELECTROLYTE SYSTEMS FOR ELECTRO-
CHEMICAL CELLS.
American Cyanamid Co. (Arthur K. Hoffmann)
CA 67, 25473
Brit., 2,719 (Feb. 6, 1908)
FOR OBTAINING S FROM S02 AND H2S.
14 Hauptstrasse, Zehlendorf, Ger. (Walther Feld)
CA 3, 1330
Brit., 11,635 (May 11, 1914) .
ADDITION PRODUCTS OF OLEFIN HYDROCARBONS WITH
SULFUR DIOXIDE.
(F. E. Mathews, and H. M. Elder)
CA 9, 2971
Brit., 107,589 (June 26,1917)
SULFUR DIOXIDE.
(M. Kaltenbach)
CA 11, 2948
Brit., 159, 337 (Dec.
SULFUR DIOXIDE.
(P. Pascal)
CA 15, 2161
Brit., 267, 071 (March 5, 1926)
MULTIPLE-EFFECT EVAPORATING APPARATUS FOR
RECOVERY OF SULFUR DIOXIDE USED IN LIQUID FORM
FOR REFINING HYDROCARBON OILS.
Allgemeine Ges. Fur Chemische Industrie
CA 22, 865
2, 1919)
Brit., 371,888 (Apr. 29, 1932)
SULFUR DIOXIDE.
John S. Dunn and Imperial Chemical Industries Ltd.
CA 27, 3787
BATTELLE-NORTHWEST
-------
283.
284.
285.
286.
287.
288.
289.
290.
291.
292.
B-36
Brit., 400.998 (Nov. 6, 1933)
SULFUR DIOXIDE
Daniel Tyrer and Imperial Chemical Industries Ltd.
CA 28, 2135 .
Brit., 450,519 (July 20, 1936)
RECOVERING WEAK GASEOUS ACIDS.
1. G. Farbenindustrie A. -G.
CA 31, 223
Brit., 457,343 (Nov. 23, 1936)
REMOVING WEAK GASEOUS ACIDS FROM GASES.
1. G. Farbenindustrie A. -G.
CA 31, 3245
Brit., 437, 579 (June 17, 1937)
RECOVERING WEAK GASEOUS ACIDS FROM GASES.
1. G. Farbenindustrie A. -G.
CA 31, 8894
Brit., 468,972 (July 16, 1937)
RECOVERING ACIDIC GASES FROM GAS MIXTURES.
Robinson Brothers Ltd. (Deric W. Parkes and Richard B.
CA 32, 755
Brit., 470,440 (Aug. 16, 1937)
RECOVERING WEAK GASEOUS ACIDS FROM GASES.
1. G. Farbenindustrie A. -G.
CA 32, 1078
Evans)
Brit., 484,714 (May 10, 1938)
RECOVERING SULFUR DIOXIDE.
Board of Trustees of the University of illinois
CA 32, 8087
Brit., 506,002 (May 19, 1939)
RECOVERING SULFUR DIOXIDE.
Imperial Chemical Industries Ltd.
CA 33, 9561
Brit., 523,845 (July 24, 1940)
SULFUR DIOXIDE RECOVERY.
Murray Guggenheim, (Solomon R.
and Medley G. B. Whelpley)
CA 35, 6400
Guggenheim, Elias A. C. Smith,
Brit., 534,935 (March 24, 1941)
MORPHOLINE COMPOUNDS.
Harris-Seybold-Potter Co.
CA 36, 1334
BATTELLE-NORTHWEST
-------
293.
294.
295.
296.
297.
298.
299.
300.
B-37
Brit., 564,734 (Oct. 11, 1944)
RECOVERING SULFUR DIOXIDE FROM A GAS MIXTURE.
American Smelting & Refining Co.
CA 40, 3577
Brit., 675,831 (July 16, 1952)
SOL UTIONS OF SULFUR DIOXIDE.
Societe Anon. Des Manufactures Des Glaces Et Produits
Chimiques De Saint-Gobain, Chauny Et Cirev.
CA 46, 11608
Brit., 692,804 (June 1953)
PURIFICATION OF SYNTHESIS AND FUEL GASES.
Gesellschaft Fur Linde's Eismaschinen A. G. and Lurgi
Gesellschaft Fur Warmetechnik M. B. H.
CA 48, 1657
Brit., 734,577 (Aug. 3, 1955)
PURIFICATION OF SYNTHESIS AND FUEL GASES.
Gesellschaft Fur Linde's Eismaschinen A. G. and Lurgi
Gesellschaft Fur Warmetechnik M. B. H.
CA 50, 1292
Brit., 901,272 (July 18, 1962)
PURIFICATION OF FUEL GASES.
Metallgesellschaft A-G.
CA 57, 12808
Brit., 983, 391 (Feb. 17, 1965/ Appl. May 27, 19(0)
REMOVAL OF VOLATILE SULFUR COMPOUNDS FROM FUEL
GAS.
Coal Industry (Patents) Ltd. (Walter T. Summers)
CA 62, 10258
Brit., 1,030,541 (May 35, 1966/ Appl. Jan. 2, 1964)
MEASUREMENT OF GAS CONCENTRATION IN GAS MIXTURES.
Central Electricity Generating Board (Peter J. Jackson and
James W. Laxton)
CA 65, 3006
Can., 317,948 (Dec. 15, 1931)
SEPARATION OF SULFUR DIOXIDE FROM GASEOUS
MIXTURES.
(Maitland C. Boswell)
CA 26, 1728
BATTELLE-NORTHWEST
-------
301.
302.
303.
304.
305.
306.
307.
308.
309.
310.
B-38
Can., 335,155 (Aug. 29, 1933)
SEPARATION OF SULFUR DIOXIDE FROM GAS MIXTURES.
(Maitland C. Boswell and George P. BeaU
CA 27, 5491
Can., 362,537 (Dec. 15, 1935)
SULFUR DIOXIDE
American Lurgi Corp. (Conway van Girsewald, Hans Weidman,
and Gerhard Roesner)
CA 31, 15632
Can., 375,230 (July 19, 1938)
RECOVERY OF SULFUR DIOXIDE.
(Rocco Fanelli, cO-inventor)
CA 32, 7226
Can., 375,231 (July 19, 1938)
RECOVERY OF SULFUR DIOXIDE.
(Rocco Fanelli, co- inventor)
CA 32, 7226
Can., 375,232 (July 19, 1938)
RECOVERY OF SULFUR DIOXIDE.
(Rocco Fanelli, co-inventor)
CA 32~ 7226
Can., 385, 341 (Nov. 28, 1939)
RECOVERY OF SULFUR DIOXIDE FROM GASES.
Guggenheim Bros. (George H. Gleason and Alfred C.
CA 34, 1447
Loonam)
Czech. , 107,940 (July 15, 1963)
REMOVING SULFUR DIOXIDE FROM INDUSTRIAL
EXHALATIONS.
(Emil Krejcar)
CA 60, 6525
Dan., 52,359 (Nov. 30,
COLLOIDAL SULFUR.
(Torben E. Neesby)
CA 31, 2761
1936)
Fr., 685,992 (Dec. 3,
SEPARATING GASES.
The Girdler Corp.
CA 24, 5898
1929)
Fr. 725,253 (Oct. 19,
SULFUR DIOXIDE.
Edeleanu-Ges. m. b. H.
CA 26, 4921
1931)
BATTELLE-NORTHWEST
-------
311.
312.
313.
314.
315.
316.
317.
318.
319.
320.
321.
B-39
Fr., 738,747 (June 17, 1932)
PURIFYING GASES.
1. G. Farbenind. A. -G.
CA 27, 1952
Fr., 755,255 (Nov. 22, 1933)
SULFUR DIOXIDE.
Imperial Chemical Industries Ltd.
CA 28, 1482
Fr., 771,452 (Oct. 9, 1934)
RECOVERY OF SULFUR DIOXIDE.
Metallgesellschaft A. -G.
CA 29, 895
Fr., 46,137 (Mar 5, 1936)
SULFUR DIOXIDE RECOVERY.
Metallgesellschaft A. -G.
CA 30, 6146
Fr., 816,024 (July 28, 1937)
SYNTHETIC RESINS.
E. 1. du Pont de Nemours & Co.
CA 32, 1356
Fr., 817,819 (Sept. 11, 1937)
SULFUR DIOXIDE.
Imperial Chemical Industries Ltd.
CA 32, 2301
Fr., 849,036 (Nov. 13, 1939)
See Brit., 523,845
Fr., 1,224,892 (June 28, 1960)
EXTRACTION OF SULFUR DIOXIDE FROM GASES.
Nobel- Bozel (Henri Georges Luois Marcheguet, Louis Gaudon)
CA 55, 20357
Fr., 1,353,646 (Feb. 28, 1964)
SULFUR DIOXIDE SEPARATION.
Nobel- Bozel (Henri G. L. Marcheguet and Louis Gaudon)
CA 31, 336 .
Fr., 1,356,116 (March 20, 1964, Span. Appl. May 3, 1962)
RECOVERY OF SULFUR DIOXIDE FROM INDUSTRIAL GASES.
Empresa Auxiliar de la Industria S. A.
CA 62, 2525
Fr., 1,463,790 (Dec. 30, 1966)
REMOVAL OF SULFUR COMPOUNDS AND CARBON DIOXIDE
FROM FUEL GAS.
Institut Francais du Petrole, des Carburants et Lubrifiants
(Phillippe Renault)
CA 67, 55941
BATTELLE-NORTHWEST
-------
322.
323.
324.
325.
326.
327.
328.
329.
330.
B-40
Fr., 1,435,314 (Jan. 6, 1957/Fin. Appl. Jan. 25, 1955)
MANUFACTURE OF SULFUR FROM GAS CONTAINING SULFUR
DIOXIDE.
Outokumpu Oy
CA 87, 66107
Ger. (East) 54,451 (March 5, 1967/Appl. Dec. 20, 1965)
REMOVAL OF SULFUR -CONTAINING ORGANIC COMPOUNDS
FROM COKE OVEN GAS.
Gerhard Dalluege .
CA 57, 56023
Ger., 202,349 (Mar. 7, 1907)
IN THE PRODUCTION OF SULPHUR BY THE REACTION.
Walther Feld, Zehlendorf
CA 3, 477
Ger... 212,902 (Jan. 9, 1907)
PROCESS OF MFG. COMPOUNDS OF ORGANIC SALTS
WITH SULPHUR DIOXIDE, DEPENDENT UPON THE ACTION
OF S02.
Farbwerke Vorm. Meister Lucius & Bruning, Hochst aiM
CA 4, 251
Ger., 454,010 (July 26, 1928)
DOUBLE COMPOUNDS OF SULFUR DIOXIDE WITH ALDEHYDES
OR KETONES.
. Rudolf Bayer Chemische Fabrik
CA 22, 4131
Ger., 484,836 (April 18, 1926)
AROMATIC p-DIAMINES.
1. G. Farbenind. A. -G.
CA 24, 1120
Ger., 508, 839 (July 13, 1929)
PRODUCTS OF HYDROCARBONS AND SULFUR DIOXIDE.
Hermann Staudinger
CA27,522
Ger., 570,027 (Dec. 10, 1929)
RECOVERING SULFUR DIOXIDE FROM GAS MIXTURES BY
WASHING WITH TETRAHYDRONAPHTHALENE.
F. Raschig G. m. b. H. Chem. Fab.
CA 27, 2539
Ger., 606,447 (Dec. 3, 1934)
SUL FU R DIOXIDE.
Metallges. A. -G. (Conway Freiherr von Girsewald and
Hans Weidmann, and Gerhard Roesner, inventors)
CA 29, 1594
BATTELLE-NORTHWEST
-------
------------
,
331.
332.
333.
334.
335.
336.
337.
338.
339.
B-41
Ger., 621,760 (Nov. 13, 1935)
SULFUR DIOXIDE.
Metallgesellschaft A. -G. (Conway Freiherr
Hans Weidmann, inventors)
CA 30, 2334
Ger., 623,018 (Dec. 11, 1935). Addn. to 606,447
SULFUR DIOXIDE.
Metallges. A. -G. (Conway Freiherr von Girsewald,
Hans Weidmann and Gerhard Roesner, inventors)
CA 30, 2334
von Girsewald and
Ger., 645,879 (June 4, 1937). Addn. to 606,447
SULFUR DIOXIDE.
Metallges. A. -G. (Conway Freiherr von Girsewald,
Hans Weidmann and Gerhard Roesner, inventors)
CA 31, 6425
Ger., 648,448 (Aug. 2, 1937}.
SULFURIC ESTERS.
Chemische Fabrik R. Baumheier A. -G.
(Rudolf Kern, inventor)
CA 31, 8545
Ger., 660,286 (May 23, 1938)
SULFUR DIOXIDE.
Metallges. A. -G. (Conway v. Girsewald and Gerhard Roesner,
inventors)
CA 32, 6408
Ger., 703,676 (Feb. 13, 1941)
RECOVERY OF ORGANIC BASES USED AS GAS-WASHING
SOL UTIONS.
Metallgesellschaft Akt. -Ges. (Conway Freiherr von Girsewald,
Gerhard Roesner and Max Wohlwill, inventors)
CA 36, 2534
Ger., 705,024 (March 13, 1941)
RECOVERY OF SULFUR DIOXIDE.
Edeleanu -Gesellschaft m. b. H. (Alfred Hoppe,
CA 36, 2095
inventor)
Ger., 706,833 (May 8, 1941)
REMOVING SULFUR DIOXIDE FROM GASES.
Rocco Fanelli and Raymond F. Bacon (to Raymond F.
CA 37, 2547
Ger., 707,132 (May 15, 1941)
RECLAIMING SULFUR FROM GASES.
Metallgesellschaft Akt. -Ges. (Max Wohlwill,
CA 36, 2099
Bacon)
inventor}
BATTELLE-NORTHWEST
-------
340.
341.
342.
343.
344.
345.
346.
347.
348.
B-42
Ger., 711,821 (Sept. 11, 1941)
ORGANIC SULFUR COMPOUNDS.
1. G. Farbenind. A. -G. (Friedrich Asinger,
CA 37, 4405
inventor)
Ger., 715,846 (Dec. 4,1941)
ORGANIC SULFUR COMPOUNDS.
1. G. Farbenind. A. -G. (Paul Herold, Karl Smeykal,
Friedrich Asinger and Horst Dietrich Frhr. von der Horst,
inventors) .
CA 38, 2050
Ger., 719,059 (March 5, 1942)
ORGANIC COMPOUNDS CONTAINING SULFUR.
1. G. Farbenindustrie A. -G.
(Horst-Dietrich Freiherr v. der Horst, inventors)
CA37,1722
Ger., 721,892 (May 14, 1942)
ORGANIC SULFUR COMPOUNDS.
1. G. Farbenind. A. -G.
(K. Smeykal and R. Kuhn, inventors)
CA 37, 541 7
Gf'r., 725,800 (Aug. 13, 1942)
ORGANIC S COMPOUNDS.
1. G. Farbenind. A. -G. (Friedrich Asinger,
CA 37, 5984
inventor)
Ger., 728,223 (Oct 22,1942). Addn. to Ger., 715,846
ORGANIC SULFUR COMPOUNDS.
1. G. Farbenind. A. -G.
(Karl Smeykal, Horst Dietrich Frhr. von der Horst and
Georg Peinze, inventors)
CA 37, 5984
Ger., 737,031 (May 27,
GAS WASHING.
Heinrich Koppers G. m.
CA 38, 3803
Ger., 742,741 (October 21, 1943)
ORGANIC SULFUR COMPOUNDS.
1. G. Farbenind. A. -G.
(Walter Reppe, August Spaeth, and Hans Krzikalla, inventors)
CA 40, 1169
1943)
b. H. (Alfred Karl, inventor)
Ger., 950, 9 51 (Oct. 18, 1956)
GAS PURIFICATION
Karl Fehr
CA 53, 12641
BATTELLE-NORTHWEST
-------
349.
350.
351.
352.
353.
354.
355.
356.
357.
B-43
Ger., 952,892 (Nov. 22, 1958)
ABSORPTION OF SULFUR DIOXIDE FROM GASES.
Metallgesellschaft Akt. -Ges.
(Wilhelm Thumm, Ernst Wegener, Gerhard Roener,
and Josef Harwasser, inventors)
CA 53, 4705
Ger., 1,025,400 (Mar. 6, 1958)
RECOVERY OF SULFUR DIOXIDE FROM GAS MIXTURES.
Metallgesellschaft Akt. -Ges.
(Wilhelm Thumm, inventor)
CA 54, 13611
Ger., 1,098,922 (Feb. 9, 1961)
SULFUR DIOXIDE MAKE-UP FOR SULFITE PULP.
Metallgesellschaft Akt. -Ges. (Wilhelm Thumon, inventor)
CA 55, 26443
Ger., 1,118,168 (Nov. 30, 1961 Span. Appl. April 12, 1958)
RECOVERY OF PURE SULFUR FROM SULFUR DIOXIDE-
CONTAINING GASES.
Instituto Nacional de Industria (Angel Vian Orturo, inventor)
CA 56, 11232
Ger., 1,166,751 (April 2, 1964)
REMOVAL OF HYDROGEN SULFIDE AND SULFUR DIOXIDE
FROM EXHAUST GASES.
Aktiengesellschaft fuer Chemische Industrie
(Manfred Mueller, inventor)
CA 61, 1534
Ger., 1, 222, 048 (Aug. 4, 1966, Appl. Dec. 8, 1964)
SULFONES AND POLYSULFONES BY REACTION OF S02
AND ACRYLIC COMPOUNDS.
Farbenfabriken Bayer A. -G. (Kuno Wagner, inventor)
CA 65, 13545
Hung., 126,899 (May 15, 1941)
SEPARATION OF SULFUR DIOXIDE FROM GAS MIXTURES.
Jeno Pap.
CA 35. 7665
Japan, 172,814 (May 31, 1946)
RECOVERING OF SULFUR DIOXIDE
Furukawa Kogyo K. K. (Tamaki Nakazono,
CA 43, 7201
Neth. Appl, 6, 506,804 (Nov. 29. 1966, Appl. May 28,
TRIMETHYLAMINE-SULFUR TRIOXIDE COMPLEX.
Baldwin -Montrose Chemical Co.
CA 67, 85456
inventor)
1965)
BATTELLE-NORTHWEST
-------
358.
359.
360.
361.
362.
363.
364.
365.
366.
B-44
Neth. Appl., 6,613,112 (March 20, 1967), Fr. Appl. Sept. 18,
1965
WASHING OF SULFUR-CONTAINING GASES.
Institut Francais du Petrole, des Carburants et Lubrifiants
CA 67, 75127
Span., 261,844, Appl. Oct. 20, 1960
RECUPERA TION OF SULFUR DIOXIDE FROM INDUSTRIAL
GASES OF ANY CONCENTRATION.
Empresa Auxiliar de la Industria, S. A. (Angel Vian Ortune,
inventor)
CA 56, 11232
Swed. 124, 600 (April 12, 1949)
SEPARATING GASES IN MIXTURES.
A. R. Persson, J. O. Naucler
CA 43, 8758
Swed., 126, 527 (Oct. 25, 1949)
CONCENTRATING GASES CONTAINING SULFUR DIOXIDE.
Aktiebolaget Kaukas Fabrik (V. H. Somer, T. E. Brehmer,
inventors)
CA 44, 3684 and 3712
U. S., 927,342 (July 6)
RECOVER Y OF SULPHUR FROM GAS.
Walther Feld, Zeklendorf, and Anton Jahl,
CA 3, 2354
U. S., 1, 260, 49 2 (M ar . 26)
RECOVERING SULFUR DIOXIDE FROM FURNACE GASES.
U. Wedge and F. A. Eustis
CA 12, 1499
Honninger, A. R.
U. S. 1,315,189 (Sept. 2)
RECOVERING SULFUR DIOXIDE FROM COMBUSTION GASES.
H. K. Moore and G. A. Richter
CA 13, 2747
U. S. 1,398,791 (Nov. 29)
ABSORPTION OF SULFUR DIOXIDE.
P. Pascal
CA16,800
U. S. 1. 726.252 (Au!!. 27)
COMPLEX COMPOUNDS OF AROMATIC p-DIAMINES WITH
SULFUR DIOXIDE. .
1. G. Farbenind. A. -G. (Richard Wolffenstein, inventor)
CA 23, 4949
BATTELLE-NORTHWEST
-------
367.
368.
369.
370.
371.
372.
373.
374.
B-45
U. S., 1,834,016 (Dec. 1)
SEPARATING ACIDIC GASES.
The Girdler Co. (Robert R. Bottoms,
CA 26, 1046
U. S., 1, 910, 341 (May 23)
SEP ARA TING SULFUR DIOXIDE FROM LIQUID
HYDROCARBONS.
Edeleanu G. m. b. H. (Paul Jodeck, 111Ventor)
CA 27, 4069
inventor)
U. S., 1,946,489 (Feb. 13)
RECOVERY OF GASES SUCH AS SULFUR DIOXIDE FROM
DILUTE MIXTURES SUCH AS SMELTER GASES.
Fredrik W. de Jahn (to Jacob D. Jenssen)
CA 28, 2433
U. S., 1,951,992 (March 20)
SEPARATING ACID GASES FROM GASEOUS MIXTURES.
Carbide & Carbon Chemicals Corp. (Granville A. Perkins,
inventor)
CA 28, 3564
u. S., 1,954,959 (April 17)
FREEING HYDROCARBON OILS FROM SULFUR DIOXIDE.
Standard Oil Development Co.
(Reginald K. Stratf ord and William P. Doohan, inventor)
CA 28, 3887
U. S., 1,972,074 (Sept. 4)
SEPARATING SULFUR DIOXIDE FROM GASEOUS MIXTURES.
Maitland C. Boswell
CA 28, 6536
U. S., 2, 082, 006 (June 1)
REMOVING AND RECOVERING SULFUR DIOXIDE FROM
WASTE GASES.
Board of Trustees of the Univ. of Ill.
(Henry F. Johnstone, inventor)
CA 31, 51 39
U. S., 2,106,435 (Jan. 25)
REMOVING ACIDIC GASES FROM GASEOUS MIXTURES SUCH
AS AIR OR HYDROGEN.
Robinson Bros. Ltd.
(Deric W. Parkes and Richard B. Evans, inveYltors)
CA 32, 2719
BATTELLE-NORTHWEST
-------
375.
376.
377.
378.
379.
380.
381.
382.
383.
B-46
U. S., 2,112,986 (Apr. 5)
RESINOUS REACTION PRODUCTS.
Phillips Petroleum Co. (Frederick E.
inventors)
CA 32, 3858
U. S., 2, 128, 027 (Aug. 23)
RECOVERY OF SULFUR DIOXIDE FROM GAS MIXTURES.
Imperial Chemical Industries Ltd. (Arthur M. Clark, inventor)
CA 32, 8087
Frey and Robert D. Snow,
U. S., 2,134,481 (Oct. 25)
RECOVERING SULFUR DIOXIDE FROM WASTE GASES SUCH
AS BOILER AND FURNACE GASES.
Commonwealth Edison Co. (Henry F. Johnstone, inventor)
CA33,1110
U. S., 2,139,375 (Dec. 6)
REMOVAL OF S02 FROM GASES SUCH AS NITROGEN.
Shell Development Co.
(Russell W. Millar and Herbert P. A. Groll, inventor)
CA 33, 2293
u. S., 2, 142, 987 (J an. 1 0)
SULFUR DIOXIDE RECOVERY FROM GASES SUCH AS THOSE
FROM ORE ROASTING.
Raymond F. Bacon and Rocco Fanelli (to Raymond F. Bacon)
CA 33, 3082
U. S.. 2, 174, 111 (Sept. 26)
TREATING BENZENE WITH CHLORINE AND SULFUR DIOXIDE,
AND SIMILAR REACTIONS.
Cortes F. Reed (50% to Charles L. Horn)
CA 34, 4535
U. S., 2, 18 5, 311 (Jan. 2)
RECOVERY OF SOLVENTS SUCH AS SULFUR DIOXIDE AND
BENZENE USED FOR TREATING LUBRICATING OILS.
Union Oil Co. of Calif.
(Edward G. Ragatz and Donald E. McFaddin, inventors)
CA 34, 3074
U. S., 2, 186,453 (Jan. 9)
SULFUR DIOXIDE RECOVERY FROM GASES.
Guggenheim Bros. (Ceo. H. Glea,30n and Alfred C.
inventors)
CA 34, 3455
Loonam,
U. S., 2, 192,461 (Mar. 5)
SULFUR DIOXIDE RECOVERY FROM GASES SUCH AS
RESIDUAL ROASTING-FURNACE GASES.
American Lurgi Corp. (Con-.vay Baron von Girsewald,
Gerhard .Roesner a.'.1d Max Wohlwill, inventors)
CA 34, 4529
e P. T TEL L E - NOR T H \'1/ EST
-------
384.
385.
386.
387.
388.
389.
390.
B-47
U. S., 2, 228, 598 (J an. 14)
PURIFICATION OF HYDROCARBON-SiJLFUR DIOXIDE-
CHLORINE REACTION PRODUCTS.
(Arthur L. Fox, Clyde O. Henke and Cortes F. Reed, inventors)
E. 1. du Pont de Nemours & Co. (Fox ~~'ld I-Ienke)
Charles L. Horn (Reed one-sixth)
CA 35, 3011
U. S., 2, 270,490 (Jan. 20)
MORPHOLINE COMPOUNDS.
Harris -Seybold - Potter Co. (Wm.
CA 36, 3298
H. Wood, inventor)
U. S., 2, 295, 587 (Sept. 15)
RECOVERY OF SULFUR DIOXIDE FROM GAS MIXTURES
S1JCH AS SMELTER SMOKE.
American Smelting and Refining Co.
(Edward P. Fleming and T. Cleon Fitt.. inventors)
CA37,1234
U. S., 2,301,779 (Nov. 10)
SEPARATE RECOVERY OF HYDROGEN CHLORIDE AND
SULFUR DIOXIDE FROM GAS MIXTURES SUCH AS THOSE
FROM HYDROCARBON-OIL TREATMENT.
Alien Property Custodian (Paul Herold and Georg Mar.kus,
inventors)
. CA 37, 2145
U. S., 2, 368, 545 (Jan. 30, 19.15)
RECOVERY OF SULFUR DIOXIDE FROM MIXTURES WITH
OTHER GASES OR WITH LOW-BOILING HYDROCARBONS.
The Dow Chemical Co.
(George W. Hooker, Lewis R. Dra:
-------
391.
392.
393.
394.
395.
396.
397.
398.
B-48
U. S., 2, 370, 020 (Feb. 20, 1945)
SEPARATION OF SULFUR DIOXIDE FROM GASES.
Union Oil Co. of California (Thomas F. Doumani, inve:1tor)
CA 39, 5072
U. S., 2,381,257 (Aug. 7, 1945)
ADDITION COMPOUND OF SULFUR DIOXIDE WI TH ANOTHER
INSECTICIDE AND METHOD OF DISPENSING AN INSECTICIDE.
Frank L. Campbell and W. Conard Fernelius
CA 40, 1 63 .
U. S., 2, 384, 376 (Sept. 4, 1945)
RECOVERY OF SULFUR DIOXIDE AND DIOLEFINS FROM
SULFONES.
Dow Chemical Co. (Geo. M. Hebbard, inventor)
CA 40, 344
U. S., 2,33.1,378 {Sept. 4,1945)
SEPARATION OF SULFUR DIOXIDE AND LOW-BOILING
HYDROCARBONS.
Dow Chemi.cal Co.
(George W. Hooker a~d Franc A. Landee, inventors)
CA 40, 718
0. S., 2,385,704 (Sept. 25, 1945)
RECOVERING SULFUR DIOXIDE.
The Dow Chemica: Co.
(George W. Hooker, Stephen C. Stowe,
inventors)
CA 40, 185
U. S., 2,395,050 (Feb. 19, 1946)
SEPARATION OF 1, 3-BUTADIENE FROM MIXTURES BY USING
SULFUR DIOXIDE.
Dow Chemical. Co. (George W. Hooker, Lewis R. Drake, and
Stephen C. Stowe, inventors)
CA 40, 3124
and Lewis R. Drake,
U. S., 2,395,278 (Feb. 19, 19,~6)
TREATMENT OF ABIETYL COMPOUNDS WITH SULFUR
DIOXIDE.
Ridbo Laboratories, Inc, (Nicholas L. Kalman, inventor)
CA 40, 3137
U. S., 2,399,013 (Apr. 23,1945)
SULFUR DIOXIDE RECOVERY.
American Smelting a~d Refining Co.
(Edward P. Fleming and T. Cleon Fitt,
CA 40, 7538
inventors)
BP- T TEL L E - NOR T H \"v' EST
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--
I
399.
400.
.101.
402.
403.
404.
405.
406.
I -
407.
B-49
U. S., 2,40:'3,319 {July 2, 1946)
HYDROGEN SULFIDE REMOVAL FROM GASES.
Standard Oil Development Co. (Milton Williams, in'Jen-~or)
CA40, 5549
U. S., 2,40'1,854 (July 30, 19(16)
REGENERA TION OF ABSORBENT.
Phillips Petroleum Co.
(John W. Latchuffi, Jr., and James S.
CA 40, 6230 -
Connars, inven:ors)
U. S., 2,539,871 (Jan. 30, 1951)
SOL UTIONS OF GASES.
Aktieboiaget Centrallaboratorium (T.
CA 45, 4497
H. Smedslund, inventor)
U. S., 2,676,872 (Apr. 27, 1954)
GLYCOL SULFITE IN HANDLING OF SULFUR DIOXIDE.
Societe Ano~. des Manufactures des Glaces et Produits
ChimiQues de Saint -Gobain, Chauny & Circy
(Marcel. J. Viard, inventor)
CA 48, 11018
U. S., 3, 023, 0:38 (Feb. 27, 1962)
SULFUR.
Uni.versal Oil Products Co.
(Peter Urban, and Lester G. Massey, in'rentors)
CA 56, 1 379 6
U. S., 3,18.3,145 (May 11, 1965)
ODOR CONTROL AND HEAT RECOVERY IN WOOD PULPING.
Theron T. Collins, Jr.
CA 64, 6892
U. S., 3,226,430 (Cl. 260-50.l)(Dec. 23, 1965, Appl.
Feb. 26, 1962 and April 7, 1964)
CYCLOHEXYLAMINE CYCLOHEXYLSULFAMATE.
Abbatt Laboratories (Madhukar ~. Mhatre, inve!ltor)
CA 64, 8054
1962)
U. S., 3,287,389 (Nov. 22, 1966, Appl. Sept. 14,
COMPLEXES OF S03 WITH NITRILES.
Monsanto Co. (George L. Broussalian, inventor)
CA 67, 37459
U. S., 3,346,505 (Oct. 10, 1967, Appl. March 15, 19133)
SULFONA TION OF ORGANIC COMPOUNDS.
Colgate-Palmolive Co.
(John M. Blakeway and Philip Marshall, inventors)
CA 63, 77976
BP.TTELLE-NORTHWEST
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B-50
408.
U. S., 3,350,470 (Oct. 31, 1967, Appl. Dec. 1, 1961)
LIQUID-LIQUID EXTRACTION PROCESS.
Union Oil Co. of California (Art C. McKinnis, inventor)
CA 68,51847
409. U. S., 3, 363, 939 (Jan. 16, 1968, Appl. Nov. 4, 1965)
REMOVAL OF SULFUR-CONTAINING GASES FROM GASEOUS
MIXTURES.
Shell Oil Co.
(Carl H. Deal, Jr., a':1d Michael N. Papadopoulos, inventors)
CA 68, 61410
410. Brit. 708,095 (April 28, 1954)
REMOVAL OF SULFUR OXIDES FROM FLUE GASES AND THEIR
CONVERSION TO AMMONIUM SULFATE.
Walter G. Lowenstein-Lorn (to Standard Oil Development Co.).
CA 48: 11 033a (1954)
411. Brit. 744,465 (Feb. 8, 1956)
WASHING AND COOLING OF GASES CONTAINING SULFUR DIOXIDE.
Chemiebau Dr. A. Zieren G. m. b. H.
CA 50: 13411 (1956)
412. Can. 410,409 (Feb. 2, 1943)
RECOVERY OF SULFUR DIOXIDE FROM DIGESTER GASES.
Horace A. DuBois (to Paper Patents Co. ).
CA 37: 21831 (L)
413. Ger. 679, 709 (Aug. 12, 1939)(Cl. 12e. 5).
ELECTROFILTER FOR PURIFYING GASES.
1. G. Farbenind. A. -G.
CA 33: 91606 (L)
414. U. S. 2, 137, 311 (Nov. 22)
SULFUR DIOXIDE RECOVERY FROM SULFITE LIQUORS.
Karl L. Springer (to Standard Oil Development Co. ).
CA 33: 18921 (L)
415. U. S. 2, 173,877 (Sept. 26)
SULFUR DIOXIDE RECOVERY FROM GAS MIXTURES, SUCH
AS THOSE FROM ORE ROASTING.
Arthur M. Clark, William E. Batten and Charles F. R. Harrison
(to Imperial Chemical Industries Ltd. ).
CA 34: 5948 (L)
416. U. S. 2,180,495 (Nov. 21) .
RECOVERY OF SULFUR DIOXIDE FROM GASES.
Raymond F. Bacon
CA 34: 1826t
BATTELLE-NORTH Vii EST
. .
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"
B-51
417. U. S. 2, 676, 090 (April 20, 1954)
RECOVERY OF SULFUR DIOXIDE FROM WASTE GASES.
Henry F. Johnstone (to Texas Gulf Sulphur Co. ).
CA48: 1l018b(1954)
418. U. S. 2, 718, 453 (Sept. 20, 1955)
DESULFURIZATION OF FLUE GASES.
John W. Beckman.
CA 50: 1292c (1956)
BATTELLE-NORTHWEST
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