SEPA
EPA/600/R-09/037 | April 2009 | vwwv.epa.gov/athens
United States
Environmental Protection
Agency
Composition and Behavior of
Fuel Ethanol
Ecosystems Research Division, Athens, GA 30605
National Exposure Research Laboratory
Office of Research and Development
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EPA/600/R-09/037
April 2009
Composition and Behavior of Fuel Ethanol
by
James W. Weaver(a)
Sheldon A. Skaggs(b)
David L.Spidle(a)
Guthrie C. Stone(c)
(a) Ecosystems Research Division, National Exposure Research Laboratory, Office of Research and
Development, United States Environmental Protection Agency, Athens, Georgia
(b) Sheldon Skaggs, Inc, Athens, Georgia
(c) The University of Georgia, Athens Georgia
Ecosystems Research Division
National Exposure Research Laboratory
Office of Research and Development
United States Environmental Protection Agency
Athens, Georgia 30605
U.S. Environmental Protection Agency
Office of Research and Development
Washington, DC 20460
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Notice
The U.S. Environmental Protection Agency through its Office of Research and
Development funded and managed the research described here. It has been subjected to
the Agency's peer and administrative review and has been approved for publication as an
EPA document. Mention of trade names or commercial products does not constitute
endorsement or recommendation for use.
The information provided in this paper is not intended for determining compliance with
state or federal regulations for air quality, gasoline composition or other similar purposes.
For these purposes, information should be obtained from the appropriate local, state and
federal regulatory agencies, the Clean Air Act, the United States Code, the Code of
Federal Regulations, the Federal Register and other sources.
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Abstract
Ethanol usage in the United States has increased due in part to the elimination of
methyl tert-butyl ether from the fuel supply and to the mandates of Congress. Two
samples, one each from a wet mill and a dry mill ethanol plant, were obtained before
denaturing. Each of these samples contained mostly ethanol, but also low concentrations
of water, methanol, and higher molecular weight alcohols (up to five carbons). The wet
mill sample also contained ethyl acetate and an ether, 1,1-diethoxyethane. The allowable
denaturants for fuel ethanol are similar to gasoline. Since the denaturants are immiscible
with water, the ability of the denatured fuel ethanol to absorb water is limited.
Experiments with E95 and E85 showed that these both began to phase separate when
about 15% water was added to the E95 or E85. The gasoline was released gradually as
water was added to the fuel. For E95, there is a smaller amount of gasoline in the fuel
(2% to 5%) so less gasoline can be released. The changes in volume when water and
ethanol or water and E85 are mixed displayed a deficit of 3% at maximum. The
byproducts of fuel ethanol production are less soluble, sorb more, diffuse less readily,
and are less volatile than ethanol. It's likely, however, that the increased ethanol
concentration in water will increase the solubility of the byproducts, as it does the
petroleum hydrocarbons The production byproducts compose less than 1% of the mass of
the fuel. Releases of fuel ethanol will be dominated by the ethanol.
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Foreword
The National Exposure Research Laboratory's Ecosystems Research Division (ERD) in
Athens, Georgia, conducts research on organic and inorganic chemicals, greenhouse gas
biogeochemical cycles, and land use perturbations that create direct and indirect,
chemical and non-chemical stresses, exposures, and potential risks to humans and
ecosystems. ERD develops, tests, applies and provides technical support for exposure
and ecosystem response models used for assessing and managing risks to humans and
ecosystems, within a watershed / regional context.
The Regulatory Support Branch (RSB) conducts problem-driven and applied research,
develops technology tools, and provides technical support to customer Program and
Regional Offices, States, Municipalities, and Tribes. Models are distributed and
supported via the EPA Center for Exposure Assessment Modeling (CEAM) and through
access to Internet tools (www.epa.gov/athens/onsite).
Fuel composition provides the starting point for evaluation of releases to the
environment. For ethanol gasolines, the composition of the fuel differs from typical
gasoline by the addition of large amounts of ethanol and the presence of fermentation
byproducts. Physically, the fuel can be subject to phase separation upon contact with
water. This report provides basic information on usage of ethanol in U.S. gasoline, fuel
ethanol production methods, analytical methods for fuel and water samples, fuel ethanol
composition and properties, and phase behavior. This information forms the starting
point for evaluation of potential environmental impacts and ecosystem and human
exposures.
Eric J. Weber, Ph.D.
Acting Director
Ecosystems Research Division
Athens, Georgia
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Oil Spill Report Series
A series of research reports is planned to present data and models for oil spill planning
and response. To date, these include:
1. Oil Composition
James W. Weaver, Sheldon A. Skaggs, David C. Spidle, Guthrie Stone, 2009,
Composition of Fuel Ethanol, United States Environmental Protection
Agency, Washington, D.C., EPA/600/R-09/037.
Zhendi Wang, B.P. Hollebone, M. Fingas, B. Fieldhouse, L. Sigouin, M. Landriault, P.
Smith, J. Noonan, and G. Thouin, 2003, Characteristics of Spilled Oils, Fuels, and
Petroleum Products: 1. Composition and Properties of Selected Oils, United
States Environmental Protection Agency, National Exposure Research
Laboratory, EPA/600/R-03/072.
2. Dispersants
George Serial, Subhashini Chandrasekar, James W. Weaver, 2004, Characteristics of
Spilled Oils, Fuels, and Petroleum Products: 2a. Dispersant Effectiveness Data
for a Suite of Environmental Conditions - The Effects of Temperature,
Volatilization, and Energy, United States Environmental Protection Agency,
National Exposure Research Laboratory, EPA/600/R-04/119.
3. Simulation Models
James W. Weaver, 2004, Characteristics of Spilled Oils, Fuels, and Petroleum Products:
3a. Simulation of Oil Spills and Dispersants Under Conditions of Uncertainty,
United States Environmental Protection Agency, National Exposure Research
Laboratory, EPA/600/R-04/120.
As more reports are added to the series, they may be found on EPA's web site at:
http://www.epa.gov/athens/publications.
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Leaking Underground Storage Tank Assessment Report
Series
A series of research reports is planned to present data and models for leaking
underground storage tank risk assessments. To date these include:
1. Gasoline Composition
James W. Weaver, Sheldon A. Skaggs, David C. Spidle, Guthrie Stone, 2009,
Composition of Fuel Ethanol, United States Environmental Protection
Agency, Washington, D.C., EPA/600/R-09/037.
James W. Weaver, Linda R. Exum, Lourdes M. Prieto, 2008, Gasoline Composition
Regulations Affecting LUST Sites, United States Environmental Protection
Agency, Washington, D.C., EPA/600/R-08/xxx.
Weaver, James W., Lewis Jordan and Daniel B. Hall, 2005, Predicted Ground Water, Soil
and Soil Gas Impacts from US Gasolines, 2004: First Analysis of the Autumnal
Data, United States Environmental Protection Agency, Washington, D.C.,
EPA/600/R-05/032.
2. Simulation Models
Gorokhovski, Vikenti M. and James W. Weaver, 2007, A Catalog of Ground Water Flow
Solutions for Plume Diving Calculations, United States Environmental Protection
Agency, Washington, D.C.
Weaver, James W., 2004, On-line Tools for Assessing Petroleum Releases, United States
Environmental Protection Agency, Washington, D.C., EPA 600/R-04/101.
3. Model Background and Evaluation
Weaver, James W. and C. S. Sosik, 2007, Assessment of Modeling Reports for Petroleum
Release and Brownfields Sites, United States Environmental Protection Agency,
Washington, D.C., EPA 600/R-07/101.
As more reports are added to the series, they may be found on EPA's web site at:
http://www.epa.gov/athens/publications.
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Contents
Notice 2
Abstract 3
Foreword 4
Oil Spill Report Series 5
Leaking Underground Storage Tank Assessment Report Series 6
Contents 7
Figures 8
Tables 10
Terminology 11
Introduction 12
Background and Literature Review 14
Regulatory History of Gasoline 14
Ethanol Use in Gasoline 14
Gasoline Production in the United States 16
Fuel Ethanol 21
Byproducts inFuel Ethanol 22
Analytical Methods 24
Phase Separation and Co-solvency 24
Fuel Ethanol Analyses 29
Phase Separation 35
Fuel Ethanol Component Properties 39
Solubility 39
Octanol-Water Partition Coefficient 41
Water and Air Phase Diffusion Coefficients 41
Vapor Pressure 41
Henry's Constant 42
Property Variation with Temperature 42
Discussion and Conclusions 46
References 48
Appendix A Analytical Methods 52
Fuel Ethanol Analysis 52
Phase Separation 53
Appendix B Detected and tentatively identified chemicals from an ethanol plant in
Minnesota [10] 55
Appendix C Ethanol and Water Mixtures 57
Appendix D Comparison of results from the EPI Suite calculator and SPARC for Kow
for 5 °C and 25 °C 59
Appendix E SPARC Property Results for 5 °C to 45 °C 61
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Figures
Figure 1 Renewable and biofuel mandates from the Energy Policy Act (EPAct) of 2005
and the Energy Independence and Security Act (EISA) of 2007 15
Figure 2 DOE gasoline production and importation data. Prior to the Clean Air Act
Amendments, there was no distinction between conventional and reformulated gasoline.
The proportion of conventional gasoline (2/3) has remained roughly constant over the
period 1995 to 2007 17
Figure 3 Production of reformulated gasoline with ether and alcohol, conventional
gasoline with alcohol and total gasoline production on a weekly basis 18
Figure 4 Benzene and ethanol content in conventional gasoline collected by Northop
Grumman in 2007 20
Figure 5 Benzene and ethanol content in reformulated gasoline collected by Northop
Grumman in 2007 20
Figure 6 Methanol-Water-Hydrocarbon phase diagram 25
Figure 7 Estimated benzene solubility using the co-solvency relationship developed by
Heerman and Powers [19]. The hypothetical mixtures consisted of blendstock containing
1 vol % benzene mixed with ethanol containing 2% of a denaturant that itself contained
1% benzene. Curves are plotted for the average parameters from Heerman and Powers
[19] and their extreme parameter sets giving the lowest and highest peak benzene
concentrations 28
Figure 8 Wet mill sample chromatogram. Retention times are shown in Error! Reference
source not found 30
Figure 9 Dry mill sample chromatogram. Retention times are shown in Table 1 31
Figure 10 QA blank showing internal standard (1, 3-Dibromo-2-propanol with
retention time of 17.089 minutes) and alcohol matrix (retention time of 2.192 and 2.326
minutes) 31
Figure 11 Unbranched alcohols: Methanol CFLiO (top) and Ethanol C2HeO (center) and
1-Propanol C3H8O (bottom) molecules 32
Figure 12 Branched chain alcohols: Isobutyl alcohol C4HioO (top), 2-methyl 1-butanol
C5Hi2O (center) and 3-methyl 1-butanol C5Hi2O (bottom) molecules 33
Figure 13 Ethyl acetate C4HgO2 molecule 34
Figure 14 Ethers: The di-ether 1,1-diethoxyethane CeHi/tC^ (top) and MTBE CeH^O
(bottom) molecules 34
Figure 15 Release of gasoline from E95 (top) and E85 (bottom) at varying amounts of
water added. The gasoline is normalized to the nominal amount of gasoline in the E95
(5% of 7 ml) or E85 (15% of 20 ml). The water is normalized to the volume of E95 (7
ml) or E85 (20 mL) 37
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Figure 16 Volume changes as water is added to a sample of E85. All the volumes are
normalized to the volume of E85 (20 ml) 38
Figure 17 Total volume reduction during addition of water to ethanol 38
Figure 18 Benzene CeHemolecule 40
Figure 19 Estimates from the EPA EPI Suite calculator, SPARC at 5 °C and 25 °C
plotted against experimental results reported with EPI Suite results 59
Figure 20 Example of variation in SPARC results given an assumed variability (error) of
one-half log unit. The left hand graph shows results on a log-log scale. The right hand
graph shows the same variation on a linear scale 60
Figure 21 Solubility of the alcohols found in the wet and dry mill samples. Ethanol and
methanol do not appear because their solubility is infinite 61
Figure 22 Solubility of ethyl acetate and 1,1-diethoxy ethane, compounds found in the
wet mill sample. Solubilities of bezene and MTBE are plotted for comparison 61
Figure 23 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for methanol and ethanol estimated by the
SPARC calculator 62
Figure 24 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for 1-propanol and isobutyl alcohol
estimated by the SPARC calculator 63
Figure 25 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for 2-methyl 1-butane and 3-methyl 1-
butane estimated by the SPARC calculator 64
Figure 26 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for ethyl acetate estimated by the SPARC
calculator 65
Figure 27 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for 1,1-diethoxy ethane estimated by the
SPARC calculator 66
Figure 28 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion
coefficient, octanol/water partition coefficient) for benzene and methyl tert-buty\ ether
(MTBE) estimated by the SPARC calculator 67
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Tables
Table 1 Compounds identified by GC-MS in two samples of fuel ethanol.
Concentrations were determined by retention time analysis using GC-FID 30
Table 2 Solubility, Henry's Constant, Vapor Pressure, Air Phase Diffusion Coefficient
and Octanol-Water Partition Coefficient estimated by the SPARC calculator for fuel
ethanol components, benzene andMTBE at 15 C 43
Table 3 SPARC estimated properties at 15 °C ranked from lowest to highest 44
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Terminology
Following ASTM D 4806 - 08a Standard Specification for Denatured Feul Ethanol for
Blending with Gasolines for Use as Automotive Spark-Ignition Engine Fuel.
Denaturant a material added to fuel ethanol to make it unsuitable for beverage
use, but not for unsuitable for automotive use.
Fuel Ethanol ethanol with impurities common to its production including
water but not denaturants.
Denatured Fuel Ethanol - fuel ethanol made unfit for beverage use by the
addition of denaturants.
Higher Molecular Weight Alcohols - aliphatic alcohols of general formula
CnH2n+iOH with n from 3 to 8.
Following the Code of Federal Regulations (40 CFR) Part 80 - Regulation of Fuels and
Fuel Additives:
Reformulated Gasoline (RFG) is any gasoline whose formulation has been
certifited under 40 CFR § 80.40 and which meets each of the standards and
requirements prescribed under 40 CFR § 80.41.
From 1995 until 2006, RFG was required to contain 2 % by weight oxygen-
containing compounds ("oxygenates")
Conventional Gasoline (CG) is any gasoline which has not been certified under
40 CFR § 80.40.
Oxygenated Gasoline (OG) is any gasoline which contains a measurable amount
of oxygenate.
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Introduction
Gasoline composition has changed because of engine requirements, clean-air and
energy-policy legislation, and EPA rule-making. Although ethanol has been in use in
motor gasolines for many years, its usage began to increase after 2000 due to concerns
over methyl tert-buty\ ether (MTBE) pollution of ground waters and the resulting state
bans of MTBE. Later Congress passed legislation that both removed the oxygenate
requirement for reformulated gasoline and required increased use of renewable fuels.
Thus since 2006 there has been a large increase in the use of ethanol in the U.S.
The object of this report is the composition and behavior of fuel ethanol,
denatured fuel ethanol, and consumer blends (particularly the 15% gasoline-containing
E85). Because of Bureau of Alcohol and Tobacco regulations, producers of fuel ethanol
generally do not distribute their product in a non-denatured form. Further, analysis of
denatured fuel ethanol is complicated by the addition of the numerous constituents of the
typical denaturant, namely gasoline. An objective of this research was to obtain samples
of non-denatured fuel ethanol. One sample each of the two main production methods -
wet milling and dry milling was obtained for analysis. The quantity of these samples
was limited so analyses were performed on slightly less limited quantities of denatured
fuel ethanol (E95) and the easily obtained consumer product E85.
These samples were used to investigate composition of fuel ethanol. Literature
on alcohol production for fuel and beverages was used as a guide for the possible
constituents of these products. Gas chromatography (GC) coupled with mass
spectroscopy (MS) was used for unambiguous identification of the constituents.
Subsequent analyses using GC with a flame ionization detector (FID) and Karl Fischer
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titration was used to quantify the concentrations of the constituents. Properties of the
identified components of fuel ethanol were then estimated using the SPARC chemical
property estimator. SPARC was used so that temperature dependence of properties could
be explored.
Phase separation of E95 and E85 was studied because when spilled or released to
the environment, in most cases these fuels will encounter either surface water in the form
of flowing streams, creeks, or rivers; ponds, lakes or estuaries; or soil moisture and
ground water. Response to incidents may vary if the fuel forms a separate phase or mixes
with water. Since the fuels have a certain water tolerance, phase separation may depend
on the composition of the fuel and the nature of the release to water. Ethanol and water
are known not to mix in direct proportion to their volumes. This effect might change the
behavior of the fuel/water system during releases. Simple experiments were devised to
determine the volume changes in various ethanol/gasoline blends.
The report is intended to provide a brief overview of the composition and
properties of ethanol fuels and contains the following sections describing four topics:
composition, chemical properties, phase separation and volume changes.
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Background and Literature Review
The background and literature review is divided into seven sections, each of which
bears on the objectives of the report. The topics are
Regulatory History of Gasoline,
Ethanol Use in Gasoline,
Gasoline Production in the United States,
Fuel Ethanol,
Byproducts in Fuel Ethanol,
Analytical Methods, and
Phase Separation and Co-solvency.
Regulatory History of Gasoline
The Clean Air Act Amendments of 1990 introduced a number of different
requirements that had a major impact on gasoline composition throughout the entire
United States from their implementation in 1992 and 1995 until the present. See Weaver
et al. [1] for more detail. The most important factors for understanding the current usage
of ethanol were the total ban on lead in gasoline, requirements for conventional gasoline
(CG), reformulated gasoline (RFG), and oxygenated gasoline (OG). Both RFG and OG
programs required usage of oxygenated gasoline additives, and for the first years of the
programs, the most commonly used oxygenate was MTBE.
Ethanol Use in Gasoline
Because of subsurface water quality concerns from releases of fuels containing
MTBE, states began in 2000 to ban MTBE and, in some cases, other ethers and alcohols
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as fuel additives. Since they were actions taken by state legislatures, they did not affect
federal requirements for oxygenate usage. The bans had the effect of causing ethanol
usage as a fuel oxygenate to increase in the U.S. The oxygen mandate for reformulated
gasoline was removed by the Energy Policy Act of 2005. The act also required usage of
renewable fuels, causing another increase in ethanol usage. The Energy Independence
and Security Act (EISA) of 2007 increased the mandated amounts of biofuels for 2008
through 2012 and extended the period of required use of biofuels to 2022. The EISA also
required targeted amounts of advanced and cellulosic biofuels for the periods 2009 to
2022 and 2010 to 2022, respectively (Figure 1).
40 i
CD
Renewable Fuel Mandates
EISA 2007 Renewable Fuel
EISA 2007 Conventional Biofuel
EISA 2007 Conventional and Cellulosic Biofuel
EPAct 2005 Renewable Fuel
Other
Advanced
Cellulosic
0
Conventional (starch based)
w
2006 2008 2010 2012 2014 2016 2018 2020 2022
Year
Figure 1 Renewable and biofuel mandates from the Energy Policy Act (EPAct) of 2005 and the
Energy Independence and Security Act (EISA) of 2007.
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Gasoline Production in the United States
Gasoline production data compiled by the Department of Energy's Energy
Information Agency (EIA) documents the production and importation of conventional
and reformulated gasoline [2]. These data show that production of RFG began in
September 1994 shortly before the implementation of the RFG program (Figure 2). RFG
replaced part of the total production of gasoline in the U.S. The remainder became
conventional gasoline simply by definition (see 40 CFR §80.2). Production of both types
of gasoline tended to increase, although RFG production increased faster than
conventional gasoline production. Even so, conventional gasoline accounts for roughly
two thirds of U.S. gasoline, a proportion that has been consistent since the beginning of
the RFG/CG designation. EIA began differentiating RFG containing ether, alcohol or no
oxygenate in 2004 (Figure 3). By this time most of the MTBE bans were in place so
alcohol use in RFG was highest. The use of MTBE was slowly declining until the
oxygenate mandate was removed by the Energy Policy Act of 2005 (EPAct 2005). In
mid 2006 MTBE was abruptly removed from the fuel supply (Figure 3) and the amount
of RFG made with ether decreased to a negligible amount, while the amount of RFG
made with alcohol abruptly increased. The EPAct 2005 legislation also required
increased use of biofuels. Conventional gasoline showed increasing amounts of alcohol,
especially after mid 2007. In 2007 the Energy Independence and Security Act mandated
increased levels of biofuel usage through 2022. As of March, 2009, EIA data show that
75% of the total gasoline produced in the U.S. contained alcohol.1
1 For the week ending March 6, 2009, there were 8539 thousand barrels produced per day of finished
motor gasoline. Of this there were 2896 thousand barrels produced per day of reformulated gasoline
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8000
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Figure 2 DOE gasoline production and importation data. Prior to the Clean Air Act Amendments,
there was no distinction between conventional and reformulated gasoline. The proportion of
conventional gasoline (2/3) has remained roughly constant over the period 1995 to 2007.
containing alcohol and 3549 thousand barrels produced per day of conventional gasoline containing
alcohol.
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Figure 3 Production of reformulated gasoline with ether and alcohol, conventional gasoline with
alcohol and total gasoline production on a weekly basis.
Petroleum product surveys are conducted annually by Northrop Grumman [3].
Samples are collected from service stations and analyzed for selected compositional and
physical properties. The benzene and ethanol data presented below were determined by
ASTM methods [3]. These data show the variability of ethanol content within the
conventional and reformulated classes from cities representing the continental United
States. The benzene data were included because it is an important gasoline component
and is subject to specific regulation by the Clean Air Act.
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For the summer sampling of 2007, conventional gasoline (Figure 4) contained
varying amounts of ethanol with two dominant levels: about 10% and, with fewer
samples, none. The samples with about 10% ethanol represent E10 and illustrate the
observed variability for summer 2007. Outliers contained as much as 14.4% ethanol.
Both premium (defined here as octane numbers (ON) greater than 90) and regular had
ethanol contents throughout the range from 0 to 11%. Benzene levels ranged to 3.6%
which is due to the benzene levels in conventional gasoline being set from 1990
producer/importer baselines [1] The summer 2007 reformulated gasoline (Figure 5)
showed also showed two dominant ethanol levels: around 10% and just under 6%..
Regular and premium gasoline showed no discernable patterns, but were represented
throughout the data range. Compared to conventional gasoline, benzene levels were
lower in reformulated gasoline due to clean air act requirements. Most samples showed
benzene levels below 1% by volume.
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Conventional Gasoline
3.5
3 -
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N
C
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CO
2.5
1.5
0.5
A
A
6 8 10
Ethanol (vol %)
12
14
16
Figure 4 Benzene and ethanol content in conventional gasoline collected by Northop Grumman in
2007.
Reformulated Gasoline
3.5 -
3 -
2 -
O
I
C 1.5
0.5 -
6 8 10
Ethanol (vol %)
12
14
16
Figure 5 Benzene and ethanol content in reformulated gasoline collected by Northop Grumman in
2007.
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Fuel Ethan ol
Fuel ethanol is produced by several methods. The most common is the dry mill
process that accounts for 75% of current production. Dry mill plants typically produce
ethanol as the primary product with animal feed (called Dried Distiller's Grains with
Solubles, DDGS) and carbon dioxide as co-products. In dry milling the entire corn
kernel is ground and used as the feed stock for ethanol production [4, 5]. In wet milling,
the corn is first separated into its components: starch, fiber, gluten and germ [4]. These
plants produce ethanol as one of several food industry products including corn oil, corn
syrup, and corn sugar. After fermentation the alcohol is distilled to 190 proof to reduce
the water content. Afterward, molecular sieve technology is used to remove the
remaining water.
For use as a fuel, ethanol is made unfit for drinking by addition of a denaturant.
ASTM [6] gives requirements for fuel ethanol and acceptable denaturants for use in
automobile engines. Fuel ethanol is permitted by ASTM to contain 1.76% to 5.0%
denaturant. Beginning on January 1, 2009, the 2008 Food, Conservation, and Energy
Act allows a full ethanol production credit only so long as the denaturant content is no
more than 2% [7]. Because of measurement difficulties, the Internal Revenue Service is
temporarily allowing credits as long as the denaturant(s) do not exceed 2.5% of the
volume of the fuel ethanol [8]. The allowable denaturants are:
natural gasoline,
gasoline components, or
unleaded gasoline.
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The ethanol content, after denaturing, is to be a minimum of 92.1% at the time of
blending with gasoline and the water content of the fuel ethanol is to be less than 1%.
ASTM also specifies prohibited denaturants:
hydrocarbons with an end boiling point above 225 °C,
methanol not meeting ASTM D1152,
pyrroles,
turpentine,
ketones, and
tars.
These substances are said to have potentially extreme adverse effects on fuel stability,
automotive engines, and fuel systems. Since the typical boiling range of gasoline is 90
°C to 200 °C [9], the first prohibited denaturant listed above indicates that denaturants for
fuel ethanol are intended to be very much like gasoline.
Byproducts in Fuel Ethanol
Fermentation of corn starch produces ethanol and other compounds. Although
ethanol is the dominant alcohol produced, a variety of others have been documented
[10]. Air emissions from a beer brewer/dry-mill ethanol plant were monitored and a
number of hydrocarbons were identified. Classes of compounds included tearing agents
(lacrimators), respiratory irritants and odorants. Specific examples included
formaldehyde, acetaldehyde, furfural, 2-Furancarboxaldeyde, acrolein, benzene,
methanol, ethanol, glycerol, styrene, lactic acid and acetic acid [11]. The complete list
of compounds is given in Appendix B, although most of these have not been reported as
constituents of fuel ethanol itself. The main byproducts of ethanol production are
isopropyl and isobutyl alcohols, but also include methyl, amyl, iso-amyl, n-propyl,
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glycerol (1,2,3-propanetriol), higher alcohols, ethers, acetic aldehyde and acids. The
presence of pentoses leads to production of furfural (furan-2-carbaldehyde), which
degrades rubber or elastomeric seals2. Production of the byproducts can reduce ethanol
production by 10%. Because of competition among microorganisms, the longer that
fermentation continues, the more equilibrium shifts toward the higher alcohols,
aldehydes, acids or methane [11].
For comparison purposes, the following literature on beverage alcohol production
was reviewed as a related production activity might show insight into issues of fuel
ethanol. In production of beverages [13] found acetals (i.e., 1-1 diethoxyethane)
occurring in small quantities. The occurrence of acetals began to be significant after 4
hours of fermentation and is related to higher acidity related to infections of acid-forming
bacteria. Esters are formed from organic acids and predominantly ethanol. In the first
hours of fermentation ethyl and methyl esters of acetic acid were produced. In later
stages of fermentation esters of higher alcohols appeared (isoamyl acetate, isobytyl
acetate, and ethyl hexanate). Other compounds produced include 2-propanol, acroleine
(in the form of acroleine diethylacetal), acetic aldehyde [13] .
Production of fermentation byproducts is important to beverage producers or
consumers because volatile esters impart flavors [13, 14], contaminants can be present in
illegally produced alcohol [15], and reduction in some byproducts is needed for food-
grade alcohol [16]. Fan and Qian found a large number of flavor imparting compounds
in increased concentration in five-year old Chinese Liquor which was aged in a clay
vessel [14]. In a study of contaminants of illegally-produced drinking alcohol, analysis
2 Corrosion of steel is attributed to the formation of ethanol/water molecular structures as well as the
amount of water itself [12].
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was performed for the ethanol, isopropanol, acetone, methanol, ethylene glycol and lead
contents [15]. A later summary of studies indicated analysis for ethanol, methanol, 1-
propanol, iso-butanol and isoamyl alcohol were commonly analyzed in evaluation of
these liquors [17].
Analytical Methods
There are common aspects of analytical methods for alcohol analyses. ASTM
specifies a long nonspecific narrow-bore capillary column and direct injection to a gas
chromatograph (GC) with a flame ionization detector (FID) [18]. Others have used
direct injection to a CG-FID [19] using a wax column [13] or non-polar fused silica
column [20]. Trace level analyses of ethanol, MTBE and other alcohols and ethers have
been conducted with solid phase micro extraction (SPME) using a DVB/Carbozen/PDMS
fiber, a GC equipped with a fused silica column and mass selective detector [14, 21].
Solid phase extraction was used to concentrate impurities in Brazilian ethanol prior to
GC-MS identification [22].
Phase Separation and Co-solvency
Although water and gasoline are mutually immiscible, a small amount of each is
soluble in the other. Typical water contents of non-ethanol gasolines are on the order of
0.01%. As the ethanol content increases, the amount of water that can be accommodated
in the fuel increases. There is a limit, however, to this tolerance beyond which the fuel
separates into a predominantly water phase and a predominantly gasoline phase. Phase
24
-------
partitioning data that represent this phenomena are commonly represented on tri-linear
phase diagrams, where a boundary separates the single- from the two-phase regions. An
example phase diagram is shown in Figure 6. The solid curve on the diagram represents
the boundary between a one-phase region and a two-phase region. At any point on the
diagram, the amount of water, ethanol and hydrocarbon can be read from the three axes.
If a mixture contained 85% ethanol, 15% hydrocarbon and no water, its location on the
diagram is the beginning point of the dashed arrow. The mixture would exist as a single
phase. By increasing the water content, the mixture moves in the direction of the arrow.
Once the phase boundary is reached, then the mixture breaks into two phases: a
predominantly aqueous/alcohol phase and an predominantly oil phase. Note, however,
each of the three components is present to some degree in the two phases.
o 1
0.2
1 ' T
0.4 0.6
% Hydrocarbon
r
0.8
Figure 6 Methanol-Water-Hydrocarbon phase diagram.
For gasoline fuels, the tri-linear diagram has some conceptual utility, but there are
many more than three species present. Regardless, the approach allows for a visual
25
-------
representation of the various combinations of water, ethanol, and "gasoline" that co-exist
in solution in either a single or dual phase. Letcher et al. [23] measured phase separation
in gasoline-water-alcohol systems and found somewhat suppressed phase separation at
higher temperatures. Phase separation was also suppressed in the order: methanol, 1-
butanol, ethanol and 1-propanol. K. Y. Lee [24] compared published phase equilibrium
data against predicted phase boundaries in three phase water/solvent and BTEX systems
and also in systems with a mixed solvent. These showed reasonable agreement for
ethanol and methanol as solvents. Nakayama [25] described phase separation in
methanol-gasolines as potentially including three layers: water, emulsified water-
gasoline and gasoline. Higher molecular weight alcohols were shown by H. K. Lee and
coworkers [26] to have suppressed phase separation at low temperatures in methanol-
surrogate gasoline blends. French and Mai one [27] presented an extensive review of the
effects of ethanol on gasoline, including increased vapor pressure at certain ethanol
concentrations, materials compatibility and the influence of temperature on phase
separation. More detail on potential impacts from subsurface releases from ethanol fuels
can be found in Rixey and co-workers [28].
In multicomponent systems, ethanol has the ability to increase the apparent
solubility of a partly miscible compound. For the case of the ethanol gasoline, there
might be sufficient ethanol present to increase the concentration of gasoline components
in water. Heermann and Powers [19] determined the equilibrium phase concentrations of
benzene, toluene, ethylbenzene and xylenes (BTEX) for various amounts of ethanol in
solution. Their purpose was to determine the degree of co-solvency caused by the
alcohol and to identify modeling approaches for predicting equilibrium concentrations.
26
-------
They concluded that the best fit consisted of a piecewise model that had a linear
relationship for low ethanol contents (approximately 25% or less) and a log-linear
relationship for higher ethanol contents. Data were fit to a surrogate gasoline consisting
of eight compounds and then used to predict BTEX concentrations for commercial
gasolines.
Estimated aqueous concentrations of benzene calculated from the method
developed by Heerman and Powers are shown in Figure 7. The aqueous concentration of
benzene from a gasoline mixture depends on the amount of benzene present in the fuel
and the co-solvency due to the presence of ethanol in water3. As the amount of ethanol
increases, so does the co-solvency, but this effect is balanced by the decline in benzene-
containing blendstock used in formulating higher ethanol content fuels. A hypothetical
mixture of blendstock containing 1% benzene and denatured fuel ethanol is plotted in
Figure 7. The fuel ethanol was assumed to be denatured with 2% gasoline which itself
contained 1% benzene. At ethanol contents below about 25 volume %, there is no
increase in benzene solubility for this mixture. The aqueous benzene concentration peaks
at about 85% ethanol. Higher ethanol content causes a decline in the benzene
concentration due to the reduction in benzene content of the fuel. The plot shows the
estimated concentration for the average parameter set and the extreme values of the fitted
parameters that give the lowest and highest peak concentration. The latter are included
because Heerman and Powers gave 95% confidence limits on their fitted parameters. The
estimate of benzene concentration from these considerations is 645 +/- 85 mg/L at a
3 When phase separation of an ethanol blend gasoline occurs the bulk of the ethanol partitions to the water
phase [23]. thus, assuming that most of the alcohol initially present in the gasoline phase moves to the
water phase is reasonable. This behavior differs from mixtures where 1-propanol or 1-butanol serve as the
alcohol phase. For these the bulk of the alcohol stays with the gasoline phase.
27
-------
volume fraction of 87.5% denatured alcohol. This value is about 20 times the aqueous
phase concentration of benzene when no ethanol is present (i.e., 33.7 mg/L).
Estimated Benzene Concentration
800
C
o
'^
re
4-i
C
0)
o
C
o
o _
Q) J
C O) 400
a E
C -
30°
700 -
600 -
500 -
200 -
(A
LLI
100 -
0.1 0.2 0.3 0.4 0.5 0.6 0.7
Ethanol Volume Fraction
0.8
0.9
Figure 7 Estimated benzene solubility using the co-solvency relationship developed by Heerman and
Powers [19]. The hypothetical mixtures consisted of blendstock containing 1 vol % benzene mixed
with ethanol containing 2% of a denaturant that itself contained 1% benzene. Curves are plotted for
the average parameters from Heerman and Powers [19] and their extreme parameter sets giving the
lowest and highest peak benzene concentrations.
28
-------
Fuel Ethanol Analyses
Two samples of corn-based, fuel ethanol (non-denatured) were obtained from
their manufacturers and analyzed according to the following procedure. There was one
sample each from a wet mill and dry mill process. First, gas chromatography/mass
spectroscopy (GC/MS) was used to identify the unknown constituents of the samples,
followed by quantitation of the concentration using GC/FID, and Karl Fischer titration of
the samples for their water content. The details of the analytical methods used in this
study are presented in Appendix A.
Analysis of the wet and dry mill samples showed that the fuel ethanol samples
included one-, two- and three-carbon unbranched alcohols: methanol, ethanol and
propanol (Table 1 and Figure 11); four- and five-carbon branched alcohols: isobutyl
alcohol and the two isomers of pentanol (also known as amyl alcohol, see Figure 12): 2-
methyl 1-butanol (active amyl alcohol) and 3-methyl, 1-butanol (isoamyl alcohol). The
wet mill sample contained two additional compounds both known byproducts of
fermentation: ethyl acetate (Figure 13) and, the di-ether, 1,1-diethoxyethane (Figure 14).
Although higher molecular weight alcohols were found in each sample, the bulk
of the samples, 97.30% of the wet mill and 96.60% of the dry mill sample were
composed of ethanol. The three to five carbon alcohols composed 0.26% and 0.19% of
the samples, respectively. Subtracting the total weight percents of the quantitated
compounds and water from 1.00, gives the amount of unidentified material as 1.28% and
3.00% respectively.
29
-------
Table 1 Compounds identified by GC-MS in two samples of fuel ethanol. Concentrations were
determined by retention time analysis using GC-FID.
Name
Formula
CAS. Number
Retention
Time
(min)
Water0 >
Methanol
Ethanol(2)
1-Propanol
Isobutyl Alcohol
2-Methyl 1-
Butanol
3 -Methyl 1-
Butanol
Ethyl Acetate
1,1-
Diethoxyethane
H2O
CH4O
C2H60
C3H80
C4H100
C5H12O
C5H12O
C4H802
C6H14O2
7732-18-15
67-55-1
64-17-5
71-23-8
78-83-1
137-32-6
123-51-3
141-78-6
105-57-7
n.a.
2.191
2.324
2.673
3.186
5.147
5.033
3.077
4.958
Concentration (wt. %)
Wet Mill Dry Mill
Sample Sample
0.65
0.07
97.3
0.03
0.10
0.06
0.21
0.02
0.28
(1) Determined by Karl Fischer titration
(2)Determined by remainder of other compounds
0.08
0.06
96.60
0.08
0.08
0.01
0.02
FI02 B. {071608\002B0201TJj~
450 -
400-
3SO H
1
1
300 J
250 j
i
i
200 |
i
150^
100-
50
0 -
0
10
15
Figure 8 Wet mill sample chromatogram. Retention times are shown in Error! Reference source not
found..
30
-------
F1D2B, (071608\003BQ301.D)
pA ,
450-
400
350-
300-
250-
200-
150
100-
50-
ft ..
ff}
CO
o
10
15
Figure 10 QA blank showing internal standard (1,3-Dibromo-2-propanol with retention time of
17.089 minutes) and alcohol matrix (retention time of 2.192 and 2.326 minutes).
31
-------
Figure 11 Unbranched alcohols: Methanol CH4O (top) and Ethanol C2H6O (center) and 1-Propanol
C3H8O (bottom) molecules.
32
-------
Figure 12 Branched chain alcohols: Isobutyl alcohol C4H10O (top), 2-methyl 1-butanol CSH12O
(center) and 3-methyl 1-butanol CSH12O (bottom) molecules.
33
-------
Figure 13 Ethyl acetate C4H8O2 molecule.
Figure 14 Ethers: The di-ether 1,1-diethoxyethane C6H14O2 (top) and MTBE C6H12O (bottom)
molecules.
34
-------
Phase Separation
Phase separation results for an E95 and an E85 sample are shown in Figure 15. A
limited amount of E95 was available for testing so a simplified procedure was used (See
Appendix A). The results show that phase separation occurs with addition of water to
each of these fuels. Each fuel accommodated a certain amount of water. In both cases
this was approximately 15% to 20% of the fuel volume. When the water added to the
fuel increased beyond this level, gasoline was released from the fuel. The release of
gasoline, however, occurred over an interval of water additions that continued until
approximately 45% of the E95 volume and 50% of the E85 volume. At higher amounts
of water added, the maximum amount of gasoline was released. Since the amount of
gasoline in the E95 and E85 was unknown the released volumes might not have reached
the presumed total (i.e, the normalized gasoline levels are below 1.0). Particularly for the
E95, the volume of gasoline was very small (0.21 mL or less), so that the measurement
accuracy is fairly low.
For higher levels of water added to E85, the gasoline volume was reduced from
its maximum. This might have occurred because of the small volumes of gasoline
released, the presence of an emulsified layer, and volume changes when E85 and water
are combined. When ethanol is added to gasoline, the volume of the mixture is slightly
greater than the sum of the volumes. When water is added to ethanol the volume of the
mixture is less than the sum of the volumes. This phenomena occurs because some of the
polar ethanol molecules are accommodated within the structure that forms from the polar
water molecules [29]. The volume reduction for alcohol-water mixtures is on the order
35
-------
of 5%. (See Appendix C for a discussion of the physical chemistry of these ethanol-
water volume effects.)
Figure 16 shows the volume changes observed when water was added to E85.
Here the average values from the four experiments plotted in Figure 15 were used to
determine the average volume of the aqueous phase (solid line), the average volume of
the gasoline phase and the total volume (dot-dash line). These are compared against the
total volume added during the experiments (upper dashed line). The figure shows that
the total volume resulting from the addition of water to E85 is less than the sum of the
water and E85 combined (upper dashed line). The deficit of volume was about 3% for
these experiments. Figure 17 shows experimental and theoretical results for the volume
of mixtures of water and ethanol. The theoretical calculation was made from the theory
presented in Appendix C and the data published by Pecar and Dolecek [30]. The
maximum reduction found in both the experiment and theoretical calculation of about
3.5% roughly corresponds to the reduction in volume observed for mixtures of E85 and
water (Figure 16).
36
-------
(/) 1 1
CO
0
s. °s-
0
C nfi
O
CO
O 0.4
0
.N 0.2
CO
E
O °
T
1
I E85 and E95
f
f
f
f
i1
r'
r i ' i ' i i i
0
CO
_0
0
0.4 0.8 1.2 1.6
Normalized Water Addition
~Zi 0.8
0
.E 0.6
(0
O
D
0
N
"(0
E
E85 and E95
E85-1
E85-2
E85-3
E85-4
0.4
0.2
r
1.6
T ' i ' r
0 0.4 0.8 1.2
Normalized Water Addition
Figure 15 Release of gasoline from E95 (top) and E85 (bottom) at varying amounts of water added.
The gasoline is normalized to the nominal amount of gasoline in the E95 (5% of 7 ml) or E85 (15% of
20 ml). The water is normalized to the volume of E95 (7 ml) or E85 (20 mL).
37
-------
2.8
N
"ro
E
2
1.6
1.2
0.8
Volume Effects
Cumulative Volume Added
^~ ^~ Average Aqueous and Fuel Phases
Average Aqueous Phase
0 0.4 0.8 1.2 1.6 2
Normalized Water Added
Figure 16 Volume changes as water is added to a sample of E85. All the volumes are normalized to
the volume of E85 (20 ml).
3
0)
a:
-------
Fuel Ethanol Component Properties
The properties of the chemicals found in the fuel ethanol samples were estimated
using the SPARC calculator [31] that is available for use via the Internet.4 These
estimates were used, because all parameters were not found in the literature for all
chemicals and, more importantly, measured values are not available for all temperatures
of interest (5 °C to 45 °C). For comparison purposes, properties of benzene and methyl
tert-buty\ ether (MTBE) were also estimated from SPARC. Appendix D contains a
comparison of SPARC-generated and EPI Suite-generated properties, along with an
estimate of error in SPARC properties.
Table 2 shows the results for 15 °C from SPARC for solubility, Henry's constant,
vapor pressure, the air phase diffusion coefficient, the water phase diffusion coefficient,
and the octanol-water partition coefficient. The compounds are ordered first by number
of oxygen atoms (one or two) and then by number of carbon atoms. Table 3 shows the
same 15 °C results ordered by parameter value.
Solubility
Solubility can be viewed as a direct measurement of hydrophobicity or the
tendency of water to exclude a substance from solution. The solubility is the maximum
concentration which an aqueous solution will tolerate before the onset of phase separation
[32]. Ethanol and methanol are infinitely soluble in water. Any amount of ethanol or
methanol can be dissolved in water without forming a separate phase. All of the other
4 http://ibmlc2.chem.uga.edu/sparc/
39
-------
compounds found in the samples have finite solubility. Alcohols, though, have a greater
affinity for water than either benzene, MTBE or the 1,1-diethoxyethane. Benzene is non-
polar (observe the symmetric structure with no oxygen in Figure 18) so it's solubility is
the lowest of this group. Figure 21 and Figure 22 show the variation in solubility from 5
°C to 45 °C.
The actual water phase concentrations resulting from partitioning of these
compounds or other constituents of gasoline are significantly lower than these
solubilities. In effect the concentration obtained from a mixture depends on the solubility
of a component and the amount present in the mixture [33]. Consequently the solubilities
presented in Table 2, Table 3, Figure 21 and Figure 22 are much greater than the
concentrations that would be observed in water contacted with gasoline.
Figure 18 Benzene C6H6 molecule.
40
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Octanol-Water Partition Coefficient
The octanol-water partition coefficient, KOW; is a measure of the tendency for a
chemical to preferentially partition from water to organic matter [34]. This coefficient is
generally inversely related to solubility and provides information similar to the
compound's solubilityalbeit in an inverse sense. The most soluble compounds have
the least degree of partitioning to octanol. The SPARC results show almost a direct
reversal from solubility. In the environment the octanol-water partition coefficient
corresponds to the tendency to partition to soil organic matter or animal tissues.
Water and Air Phase Diffusion Coefficients
The diffusion coefficients for water and air are measures of the ability of the
molecule to diffuse through intermolecular collisions [34]. Generally, the air phase
diffusion coefficients are roughly four orders of magnitude higher than the water phase
diffusion coefficients. Obviously, diffusion through air occurs much more readily that
diffusion in water (similarly diffusion coefficients in solids are again much lower than
those for water). Generally smaller molecules diffuse more readily than larger molecules
and this trend is evident in the SPARC results for both water and air.
Vapor Pressure
Vapor pressure is a measure of the maximum possible concentration of a
compound in the gas phase at a given temperature. This quantity represents equilibrium
partitioning of an organic chemical between the gaseous phase and compound itself
41
-------
(liquid or solid). It provides information on the attractive forces among the compound's
molecules in the condensed phase [35]. Table 3 shows that at 15 °C the vapor pressures
of the alcohols were inversely related to their molecular weight. Therefore methanol had
the highest vapor pressure and 3-methyl 1-butanol the lowest.
Henry's Constant
The Henry's Constant measures equilibrium partitioning between air and water.
Table 3 shows that for the alcohols the Henry's Constants increase with increasing
molecular weight. The ordering is generally inverse to that for the solubility, as the
higher the water solubility the less tendency to partition to the air.
Property Variation with Temperature
The SPARC calculator provides prediction of temperature-dependence of all its
estimated property values. The variation over the range of 5 °C to 45 °C of the properties
discussed here are presented in Appendix E.
42
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Table 2 Solubility, Henry's Constant, Vapor Pressure, Air Phase Diffusion Coefficient and Octanol-Water Partition Coefficient estimated by the
SPARC calculator for fuel ethanol components, benzene and MTBE at 15 C.
Name
Methanol
Ethanol
1-Propanol
Isobutyl Alcohol
2-Methyl 1-Butanol
3-Methyl 1-Butanol
Benzene
MTBE
Ethyl Acetate
1,1-Diethoxy ethane
Formula
SPARC(1) estimated properties at 15 C
CH4O
C2H60
C3H80
C^ioO
C5H12O
C5H12O
CcHc
CgHnO
C4H802
C6H1402
Solubility
(mg/L)
Infinite
Infinite
2.2 x 105
9.3 x 104
2.8 x 104
1.9 xlO4
1.0 xlO3
1.8x10*
4.3 x 104
2.1 xlO4
Henry's
Constant
(atm
m3/mol)
3.4 x ID'6
5.4 x 10 6
7.3 x lO'6
9.0 x lO'6
l.lxlO'5
1.2X10'5
7.0 x Iff3
1.2 x Iff3
1.5 x 10"4
1.8 xlO"4
Vapor
Pressure
(torr)
77
46
15
7
3
2
69
190
54
24
Air Diffusion
Coefficient
(cm2/s)
0.150
0.110
0.094
0.081
0.072
0.071
0.085
0.074
0.080
0.062
Water
Diffusion
Coefficient
(cm2/s)
1.3 x 1Q-5
1.0 x 10 5
8.7 x 10'6
7.7 x 10'6
7.0 x 10'6
6.9 x 10'6
8.7 x Iff6
6.5 x Iff6
7.4 x 10"6
5.8 x 10"6
Octanol-Water
Partition
Coefficient
(dimensionless)
0.24
0.74
3.31
8.51
23.40
33.11
147.91
34.67
7.08
34.67
(1) SPARC estimates were generated from May 2008 release w4.2.1405-s4.2.1408, http://ibmlc2.chem.uga.edu/sparc/ on 8/30/2008 and 8/31/2008
43
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Table 3 SPARC estimated properties at 15 °C ranked from lowest to highest.
Solubility Octanol-Water Partition Water Diffusion Coefficient
Coefficient
g/L (dimensionless) cm2/s
name value name value name value
Benzene
MTBE
l.OxlO3 Methanol
0.24 1,1-Diethoxy ethane 5.8x10"'
l.SxlO3
Ethanol
0.74
MTBE
3-methyl 1-butanol 1.9xl04 1-Propanol 3.31 3-methyl 1-butanol
1,1-Diethoxy ethane 2.1 x 104 Ethyl Acetate 7.08 2-methyl 1-butanol
2-methyl 1-butanol 2.8 x 104 Isobutyl Alcohol 8.51 Ethyl acetate
Ethyl acetate 4.3 x 104 2-Methyl 1-Butanol 23.40 Isobutyl alcohol
Isobutyl alcohol 9.3 x 104 3-Methyl 1-Butanol 33.11 Benzene
1-Propanol 2.2 x 105 1,1-Diethoxy ethane 34.67 1-Propanol
Ethanol
Methanol
Infinite
infinite
MTBE
Benzene
34.67
147.91
Ethanol
Methanol
6.5x10-*
6.9 x 10'6
7.0 x 10"6
7.4 x 10"6
7.7 x 10'6
8.7x Iff6
8.7 x 10"6
1.0x Iff5
1.3 x 10'5
44
-------
Table 3 (continued) SPARC estimated properties at 15 °C ranked from lowest to highest.
Henry's Constant
atm m3/mol
name
Methanol
Ethanol
value
Vapor Pressure
torr
Name value
3.4 x 1(T 3-Methyl 1-Butanol
Air Diffusion Coefficient
cm2/s
Name value
1,1-Diethoxy ethane 0.062
5.4x Iff6 2-Methyl 1-Butanol 3 3-Methyl 1-Butanol 0.071
1-Propanol 7.3 x 10"6 Isobutyl Alcohol
Isobutyl Alcohol 9.0 x 10"6 1-Propanol
2-methyl 1-Butanol 1.1 x 10"5 1,1-Diethoxyethane
3-methyl 1-Butanol 1.2 xlO"5 Ethanol
Ethyl Acetate 1.5 x 10"4 Ethyl Acetate
1,1-Diethoxyethane l.SxlO"4 Benzene
MTBE
Benzene
1.2x10"
7.0 x Iff"
Methanol
MTBE
7 2-Methyl 1-Butanol 0.072
15
24
54
69
77
190
MTBE
Benzene
1-Propanol
Ethanol
Methanol
0.074
Ethyl Acetate 0.080
46 Isobutyl Alcohol 0.081
0.085
0.094
0.110
0.150
45
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Discussion and Conclusions
Ethanol usage in the United States has increased due in part to the elimination of
methyl tert-butyl ether from the fuel supply and to the mandates of Congress. Required
amounts of ethanol in fuel with increase the total through the year 2022. Current data
show that 75% of U.S. produced gasoline contains ethanol. For the year 2007, the
amounts in conventional gasoline ranged from none to 10.5%, with outliers at higher
concentration. Premium gasoline showed two maximums one near 6% and the other at
about 10%. Two samples of non-denatured fuel grade ethanol, one each from a wet mill
and a dry mill ethanol plant, were obtained before denaturing. Each of these samples
contained mostly ethanol, but also low concentrations of water, methanol, and higher
molecular weight alcohols (up to five carbons). The wet mill sample also contained ethyl
acetate and an ether, 1,1-diethoxyethane. These two compounds might have been
present due to the difference in production method, as wet milling is intended to produce
a wide range of products from the components of corn.
The allowable denaturants for fuel ethanol are similar to gasoline. Unleaded
gasoline, gasoline range hydrocarbons, natural gasoline or condensate can be used for this
purpose. Since pure ethanol, the primary constituent of fuel ethanol is miscible in water,
a large amount of water can be accommodated in fuel ethanol. Since the denaturants are
immiscible with water, the ability of the denatured fuel ethanol to absorb water is limited.
Experiments with E95 and E85 showed that these both began to phase separate when
about 15% water was added to the E95 or E85. The gasoline was released gradually as
water was added to the fuel. Because about 50% water was needed for complete phase
46
-------
separation of the E95 and E85, phase separation effects in flowing water can be
estimated: If the flow in the receiving water body is 50% or greater than the release rate
of the E95 or E85 phase separation is a likelihood. In these cases an "oil" slick composed
of gasoline should be expected. For E95, there is a smaller amount of gasoline in the fuel
(2% to 5%) and the slick would be less massive than for the same spill of E85. The
changes in volume when water and ethanol or water and E85 are mixed displayed a
deficit of 3% at maximum. For example, a fuel spill that caused a release to a creek
would increase the flow volume by its volume less 3%. This phenomena for is unlikely
to be environmentally significant.
The byproducts of fuel ethanol production are less soluble, sorb more, diffuse
less readily, and are less volatile than ethanol. It's likely, however, that the increased
ethanol concentration in water will increase the solubility of the byproducts, as it does the
petroleum hydrocarbons. The byproducts compose less than 1% of the mass of the fuel
so releases of fuel ethanol will be dominated by the ethanol. Increased solubility of
petroleum hydrocarbons is possible when the ethanol fraction is greater than about 20%.
The solubility of benzene could increase by a factor of 20 due to the presence of the
ethanol.
47
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chromatography - olfactometry dilution analysis of young and aged Chinese
"Yanghe Daqu" liquors. Journal of Agricultural and Food Chemistry, 2005. 53: p.
7931-7938.
15. Holstege, C., J. Ferguson, C. Wolf, A. Baer, and A. Poklis, Analysis of moonshine
for contaminants. Journal of Toxicology - Clinical Toxicology, 2004. 42(5): p.
597-601.
16. van Leeuwen, H., R. Wood, and J. Koziel, Method and system for purifying
ethanol, Patent 20070284310 2007: United States.
48
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17. Lachenmeier, D. W., Rapid quality control of spirit drinks and beer using
multivariate data analysis of Fourier transform infrared spectra. Food Chemistry,
2007. 101(2): p. 825-832.
18. ASTM International, Standard Test Method for Determination ofEthanol Content
of Denatured Fuel Ethanol by Gas Chromatography D5501-04. 2004, ASTM
International: West Conshohocken, PA.
19. Heermann, S.E. and S.E. Powers, Mo deling the partitioning of B TEX in water-
reformulated gasoline systems containing ethanol. Journal of Contaminant
Hydrology, 1998. 34: p. 315 - 341.
20. Rahman, M.A., M. Asadullah, M.S. Rahman, M.N. Nabi, and M.A.K. Azad,
Extraction of gasohol grade ethanol from aqueous solution using gasoline as
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287-298.
21. Cassada, D.A., Y. Zhang, D.D. Snow, and R.F. Spalding, Trace analysis of
ethanol, MTBE, and related oxygenate compounds in water using solid-phase
microextraction and gas chromatograhpy/mass spectrometry. Analytical
Chemistry, 2000. 72: p. 4654 - 4658.
22. Vilar, R., R. da Silva, P. Schossler, R. Veses, C. Piatnicki, D. Samios, and E.
Caramao, Preliminary characterization of anhydrous ethanol used in Brazil as
automotive fuel. Journal of Chromatography A, 2003. 985: p. 367-373.
23. Letcher, T.M., S.W. Hey ward, andB. Shuttleworth, Ternary phase diagrams for
gasoline-water-alcohol mixtures. Fuel, 1986. 65: p. 891 - 894.
24. Lee, K.Y., Phase partitioning modeling of ethanol, isopropanol, andmethanol
with BTEXcompounds in water. Environmental Pollution, 2008. 154: p. 320 -
329.
25. Nakayama, M., Water tolerability ofmethanol-gasoline blends (phase separation
and SI engine performances). SAE Technical Paper Series. 852200: p. 185 - 191.
26. Lee, H.K., D.O. Shah, and N.D. Brinkman, Enhancing low-temperature phase
stability of a 50/50 methanol/hydrocarbon blend. SAE Technical Paper Series,
1988. 881680: p. 1 -8.
27. French, R. and P. Malone, Phase equilibria of ethanol fuel blends. Fluid Phase
Equilibria, 2005. 228-229: p. 27 - 40.
28. Rixey, W.G., X.H. He, and B.P. Stafford, The Impact of Gasohol and Fuel-Grade
Ethanol on BTXand Other Hydrocarbons in Ground Water: Effect on
Concentrations Near a Source, API Soil and Groundwater Technical Task Force
No. 23. 2005, American Petroleum Institute: Washington, DC.
29. Pinho, S.P. and E.A. Macedo, Experimental measurement and of modeling KBr
solubility in water, methanol, ethanol, and its binary mixed solvents at different
temperatures. Journal of Chemcial Thermodymanics, 2002. 34: p. 337 - 360.
30. Pecar, D. and V. Dolecek, Volumetric properties ofethanol-water mixtures under
high temperature and pressures. Fluid Phase Equilibria, 2005. 230: p. 36 - 44.
31. Karickhoff, S.W., V.K. McDaniel, C. Melton, A.N. Vellino, D.E. Nute, and L.A.
Camera, Predicting chemical reactivity by computer. Environmental Toxicology
and Chemistry, 1991. 10: p. 1405-1416.
49
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32. Mackay, D., Solubility in Water., in Handbook of Property Estimation Methods for
Chemicals, Environmental and Health Sciences, R.S. Boethling and D. Mackay,
Editors. 2000, Lewis Pulishers: Boca Raton, p. 125-139.
33. Cline, P.V., JJ. Delfmo, and P.S.C. Rao, Partitioning of aromatic constituents
into water from gasoline and other complex solvent mixtures. Environmental
Science and Technology, 1991. 25: p. 914-920.
34. Gustafson, J.B., J.G. Tell, and D. Orem, Selection of Representative TPH
Fractions Base on Fate and Transport Considerations. Total Petroleum
Hydrocarbon Criteria Working Group Series. Vol. 3. 1997, Amherst,
Massachusetts: Amherst Scientific Publishers. 102.
35. Schwarzenbach, R.P., P.M. Gschwend, and D.M. Imboden, Environmental
Organic Chemistry. Second ed. 2003, Hoboken, New Jersey: Wiley-Interscience.
36. Harris, D.C., Quantitative Chemical Analysis. 5th ed. 1999, New York: W. H.
Freeman and Company.
37. Silbey, R.J. and R.A. Alberty, Physical Chemistry. 2000, New York, New York:
John Wiley & Sons. 959.
50
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Acknowledgments
The authors appreciate the assistance of Mark Toso, Andrew Sedeky, and Tom Higgins
of the Minnesota Pollution Control Agency; Ileana Rhodes of Shell Global Solutions;
Stephen Duirk, Said Hilal and Susan Richardson of the U.S. EPA, Office of Research and
Development in Athens, Georgia. The authors also appreciate the comments from
reviewers representing academia, industry and government.
51
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Appendix A Analytical Methods
Fuel Ethanol Analysis
The undenatured fuel ethanol samples were directly injected into an Agilent 6890
GC with a 5973 MSD. The 2.0 uL injected sample was split in the injector at a 200:1
ratio with the injector temperature at 250°C. Separation of the compounds was achieved
with a 30m Restek Rtx-200 MS column with an ID of 250 um, film thickness of 0.5 um,
and a flow rate of 0.7 mL / minute. Initial oven temperature was 40°C for 4 minutes,
followed by a 1°C / minute temperature ramp to 50°C. A final temperature ramp of 30°C
/ minute to 250°C was used to elute late boilers and clean the column. Once reaching
250°C, there was a final hold time of 5.33 minutes. Total run time was 26 minutes. The
transfer line to the MSD was kept at 280°C, the MS source at 230°C, and the MS
quadrupole at 150°C for the entire analysis. The sample was ionized as it entered the
MSD by electron impact. The MSD was turned on after a 1 minute solvent delay, and
scanned from 15 to 550 M/Z.
Subsequently, chemical standards were obtained and three calibration curves were
developed for an Agilent 6890 gas chromatograph with a flame ionization detector (GC-
FID). For all the compounds except ethanol 1.0 uL was injected and the split ratio and
temperature programs were the same. Ethanol analysis was achieved by first diluting the
sample in acetone to 0.5% of the starting concentration and only splitting the sample
50:1. Compound separation was achieved with a 30m J&W HP-5 column with an ID of
320 um, film thickness of 0.25 um, and flow of 0.5 mL per minute. Calibration curve
points were 2.0%, 1.0%, 0.5%, 0.2%, 0.1%, and 0.05% by volume of each suspected
52
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compound. Linear correlation lines were compared to area counts from the fuel samples
to determine the percentages of compounds in the samples. Because of overlapping
retention times, 3-Methyl 1-Butanol and ethanol were calibrated separately from the rest
of the compounds. An internal standard of 0.1% by volume of 1, 3-Dibromo-2-propanol
was spiked into every sample.
The Karl Fischer (KF) coulometric method was used to determine the water
content in the ethanol samples [36]. Samples were analyzed using a Brinkman Metrohm
Titrino 831 KF Coulometer with Coulomat AG reagent. This system detects trace
amounts of water by titrating the sample to a bipotentiometric end point and is selective
to water. One to three milliliters of sample was weighed to the nearest 0.0001 g. The
sample was then injected into the titration vessel, and the sample weight was entered into
the titrator software. The sample was automatically titrated by the instrument and the
water content calculated by the software which was displayed to the nearest 0.01%.
Water content values were manually recorded into a laboratory notebook.
Phase Separation
Separation experiments were conducted by adding various amounts of deionized
water to a fixed amount of E-85 fuel at ambient temperature. E-85: water ratios included
5:0.5, 5: 0.625, 5:0.75, 5:0.875, 5:1, 5:1.5, 5:2, 5:2.5, 5:3, 5:3.5, 5:4, 5:4.5, 1:1, 1:1.25,
1:1.5, 1:1.75, and 1:2. First, 20 ml of E-85 was transferred by class "A" volumetric
pipette into a separately funnel that was appropriately sized for the total volume
expected. Amounts of deionized water were then added to the E-85 to the desired ratio
by class "A" volumetric pipette. The separately flask was then gently shaken and vented
53
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three times before allowing the mixture to remain undisturbed for five minutes in order to
allow separation to occur. After five minutes the aqueous (bottom) phase was slowly and
carefully drained into an appropriately sized graduated cylinder. The remaining oil (top)
phase was then slowly and carefully drained into an appropriately sized graduated
cylinder. The volume of the liquid in each cylinder was then recorded for each phase.
A screening method was developed for rapid assessment of phase separation
potential, that was particularly useful since the available volume of sample was limited.
Measured portions of three commercial ethanol/gasoline mixed samples (E10, E85, and
E95) were placed in a 10 ml graduated cylinder. A burette was used to deliver 0.1 ml of
deionized water at set increments. Sample mixing was obtained by a continual stirring of
a magnetic stir bar at the base of the graduated cylinder. Emulsions were allowed to stir
for five minutes before any readings were taken. The affects of the addition of the water
(emulsion and/or the presence of two phase behavior) was noted after each addition. The
volume of the bottom phase (assumed to be ethanol/water) was read from the markings
on the graduated cylinder. Shrinkage of the total volume was also noted by reading the
total volume of the solution in the graduated cylinder compared to the initial
ethanol/gasoline volume plus the added water volume. Synthetic samples of
approximately E25 and E35 were created by adding 1 ml and 2 ml of 100% Ethanol to 5
ml of El 0. These were tested in the same manner as the E10.
54
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Appendix B Detected and tentatively identified
chemicals from an ethanol plant in Minnesota [10].
Chemical
Detected
Methanol
Ethanol
Toluene
Ethylbenzene
Acetone
Formaldehyde
Acetaldehyde
Acrolein
Benzene
Styrene
Lactic Acid
Acetic Acid
Furfuraldehyde
Chemical Tentatively
Identified
Chemical Tentatively
Identified
Plant Location: DDGS Dryer Stack
1,3-butadiene
1,3-butadiene, 2-methyl-
1,3-pentadiene
1-2-propadiene
1-4-pentadiene
1-decene
1-dodecene
1-heptene
1-hexene
1 -methy-2-cyclopropene
1-nonene
1-octene
1-undecene
2-butanone
2-butenal
2-furancarboxaldehyde
2-heptenal
2-m ethyl-1 -pentene
2-methyl-2-propenal
2-methyl-butanal
2-methyl-furan
2-methypropenal
2-pentyl-furan
2-propen-l-ol
2-propenal
3-methyl-butanal
6-heptenoic acid
acetaldehyde
benzaldehyde
ethanol
furan
hexanal
Nitro-methane
nonanal
propene
55
-------
Chemical Detected Chemical Tentatively Identified
Plant Location: Distillation Dryer Stack
Methanol 1 butanol 3-methyl
Ethanol 1 butanol 3-methyl, aceta
Carbonyl Sulfide 1-butanol, 3methyl- (S)
Formaldehyde 1-butanol, 3methyl- aceta
Acetaldehyde butane
MEK/Butyraldehydes butane, 2, 2-dimethyl
m,p-Tolualdehyde butane, 2, 3-dimethyl
butane, 2-methyl
cyclopentane, methyl-
ethanol
ethyl acetate
heptane
hexane
hexane 2-methyl
hexane, 3-methyl
pentane
pentane, 2 methyl
2-methyl-1 -pentene
2-methyl-2-propenal
Chemical Detected Chemical Tentatively Identified
Plant Location: Fermetation Scrubber
Methanol 1 butanol 3-methyl
Ethanol 1 butanol 2-methyl
Carbonyl Sulfide 1 butanol 2-methyl (s)
Formaldehyde 1-butanol, 3methyl- aceta
Acetaldehyde 1,3-pentadiene
Hydrogen Sulfide 1-propanol
Dimethyl Sulfide 1-propanol, 2-methyl
acetaldehyde
dimethyl sulfide
ethanol
ethyl acetate
formic acid
pentane
propanoic acid
56
-------
Appendix C Ethanol and Water Mixtures
When water and ethanol form a mixture, a unique volumetric effect occurs: the
resulting volume is less than the sum of the individual water and ethanol volumes. This
phenomenon of contracting volume is a result of interstitial packing and molecular
interaction (hydrogen bonding) between water and ethanol molecules in solution.
Because the volume of the solution depends on its composition, it is convenient to
discuss volumetric effects of ethanol -water mixtures in terms of partial molar volume.
The partial molar volume, Vj, is defined as follows:
The equation above can be stated by saying that Vj is the change in total volume per mole
of "i" added, when some amount of "i" is added to the mixture at constant temperature,
pressure and amount of other substances [37]. Using partial molar volumes, the total
volume of a solution can be given by the following equation:
VT = (dV/dni)Tjpjnj * ni + (3V/dn2)T,p,nj * n2 + + (dV/dnN)T^nj * nN
The total volume of the solution can be discovered by determining the partial
molar volumes of ethanol and water, as well as the mass fractions of the mixture. Partial
molar volumes of water and ethanol can be found using the equation below [30].
= (u + oow(dV/dooe)T3p3nj .) Me & Fw = (u
In this equation, u refers to the specific volume of the solution, co represents the mass
fraction, M is indicative of molecular weight, and the subscripts "e" and "w" refer to
57
-------
water and ethanol, respectively. The densities of 54 different water-ethanol mixtures are
given by Pecar and Dolecek along with their respective mole fractions of ethanol. The
mass fraction of ethanol and its corresponding specific volume are calculated using the
data provided for these different mixtures. Specific volumes are plotted against the mass
fraction of ethanol and the best fit curve is applied to the data-plot by the third degree
polynomial. Then, the derivative of this polynomial is deduced, and the partial molar
volume can be determined. The total volume of solution can then be predicted using the
following equation:
VT = (dV/dne)Tjpjnj * ne + (dV/dnw)Tjpjnj * n2
By assuming that 1 mole of solution is present, ne & nw can be set equal to the mole
fractions of ethanol and water, respectively.
Using the equations above and data provided by Pecar & Dolecek it can be shown
that approximately one mole of ethanol and a relatively small amount of water has a total
volume nearly equal to the molar volume of ethanol. However, when significant amounts
of both water and ethanol are present in a mixture, the total volume is less than the
individual volumes of ethanol and water standing alone. A table illustrating these
volumetric effects is provided with a maximum contraction of-3.4% occurring at an
ethanol mole fraction of 0.2745.
58
-------
Appendix D Comparison of results from the EPI Suite
calculator and SPARC for Kowfor 5 °C and 25 °C.
Figure 19 shows a comparison of log Kow results from SPARC at 5 °C and 15 °C,
EPI-Suite, and experimental data reported by EPI-Suite. Generally good agreement
was seen among these sources. The SPARC results show more variation with temperature
at higher Kows than for the low values. Figure 20 shows assumed variability of one-half
log unit in SPARC Kow results on both log-log and linear scales. Note that as the value of
Kow increases so does the variability on the linear scale.
3 i
2
D)
O
ID 1 ~~
"ro
E
"w
LU
0
Comparison
O EPI Suite
n SPARC 5 C
A SPARC 25 C
D
O
D
D
-10123
EPI Suite Reported Experimental Log Kow
Figure 19 Estimates from the EPA EPI Suite calculator, SPARC at 5 °C and 25 °C plotted against
experimental results reported with EPI Suite results.
59
-------
c
O)
(D
CO
T3
CD
O)
*
v/>
*
-202
Log Median Value
Vai ration
- Median
Median - 1/4 log unit
Median + 1/4 log unit
2000 -
1600
1200
800
400
/
200 400 600 800
Median Value
1000
Figure 20 Example of variation in SPARC results given an assumed variability (error) of one-half
log unit. The left hand graph shows results on a log-log scale. The right hand graph shows the same
variation on a linear scale.
60
-------
Appendix E SPARC Property Results for 5 °C to 45 °C
IP
!5
-5 100000
w
1-Propanol
10 20 30 40
Temperature (C)
Figure 21 Solubility of the alcohols found in the wet and dry mill samples. Ethanol and methanol do
not appear because their solubility is infinite.
Ethyl Acetate
20 30
Temperature (C)
Figure 22 Solubility of ethyl acetate and 1,1-diethoxy ethane, compounds found in the wet mill
sample. Solubilities of bezene and MTBE are plotted for comparison.
61
-------
.g 5E-005
*§ *o 4E-005
o E
O ^ 3E-005
5 E
ro | 2E-005
w ^ 1E-005
c o
CD U
5E-005 i
4E-005
3E-005
2E-005
^,^^ 1E-005
^^^^^^^ ~
I ' I ' I ' I ' I 0
l_ll ICll I\JI
^/
^^^^
^^^^^
ii i i i i i i ii
X 0 10 20 30 40 50 0 10 20 30 40 50
1000 -a
CD E
5 100 -i
W ^-. =
CD b =
CL ° 10 -=
,_ t E
O
Q. 1 -=
CC =
> =
n -i
U. I
1000 -g
^^^^ =
100 -i
^^^^^^ zz
Z
10 -g
1 ^
=
z
n 1
I i I i I i I i I U.I
~~
^^^^^^^^^
^^^^
I | I | I | I | I |
0 10 20 30 40 50 0 10 20 30 40 50
1 °-2 n
-------
.g 5E-005
*§ IT 4E-005
o E
O ^ 3E-005
5 E
ro E 2E-005
w CTS, 1E-005
c n
CD U
-i-rropanoi 5E.005
4E-005
y 3E-005
^S 2E-005
fttlltl^^ 1E-005
' I ' I ' I ' I ' I 0
isoouiyi Aiconoi
J
J
^p
^s
^^^
I I I I I I I I I I
1 0 10 20 30 40 50 0 10 20 30 40 50
1000 -|
5 100 -i
w ,. =
CD fc =
o: o 10 -g
S. 1
cc
> =
n 1
U. I
1000 -g
^, 100 -i
^^^^^^^^^^
^^^^^^^^^
^^^ 10 -|
-I _I
=
n 1
| i | i | i | i | U. I
^^^^0
^^^^^^^^^
^^^^
I I I I I I I I
0 10 20 30 40 50 0 10 20 30 40 50
£ 0-2 i
CD
CD *~>
_2 ° ^2 0.12
D_ ^*^ J~
.!_ C J3, 0.08
< S§ 0.04
fc
n
U
0.2 ,
0.16
_ 0.12
^
^ 0.08
0.04
n
| i | i | i | i | U
^^^^^^^^^^^
"
I I I I I I I I
0 10 20 30 40 50 0 10 20 30 40 50
c 3E-005 |
CD
CD 'O
t/> i^
^ CD ^ 2E-005
ro .1 ~^ 1E-005
it
r^ 0
3E-005 |
2E-005
^^^^^ 1E-005
-
, , , , , , , , , 1 r\
LJ u ' I ' I ' I ' I ' I U
0 10 20 30 40 50 C
c 15 |
i_ CD
0) '0
rot
> CD 10
> o
oO
^ c _
JS o 5
o ±i
0 t
ro
CL 0
15 |
10
5 _
^^^^^^^^_^^_
^^^^^^^^^^m _
I ' I ' I ' I ' 0
^^^^
} 10 20 30 40 50
^^
^^^.^
^*"" >-.
I i I i I i I i
0 10 20 30 40 50
Temperature (C)
0 10 20 30 40 50
Temperature (C)
Figure 24 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion coefficient,
octanol/water partition coefficient) for 1-propanol and isobutyl alcohol estimated by the SPARC
calculator.
63
-------
.g 5E-005
t ^
0 o
o E
O ^ 3E-005
4E-005
ro
w
CO
0
o
a.
5
o
w "0
ro o
2E-005
1E-005
1000
100
10
1
0.1
0.2
0.16
0.12
± g O, 0.08
^ 0.04
t
Q 0
c
0
0 'O
81
o
t
b
3E-005
2E-005
- 1E-005
0
c 50
>- .9i
i8 30
oO
§§ 20
Si 10
2 0
1-Butanol 3-Methyl 1-Butanol
5E-005 -
4E-005
3E-005
2E-005
1E-005
0
0 10 20 30 40 50
0 10 20 30 40 50
0 10 20 30 40 50
0 10 20 30 40 50
1000
100
10
1
0.1
0.2
0.16
0.12
0.08
0.04
0
3E-005
2E-005
1E-005
0
50
40
30
20
10
0
0 10 20 30 40 50
Temperature (C)
0 10 20 30 40 50
0 10 20 30 40 50
0 10 20 30 40 50
0 10 20 30 40 50
0 10 20 30 40 50
Temperature (C)
Figure 25 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion coefficient,
octanol/water partition coefficient) for 2-methyl 1-butane and 3-methyl 1-butane estimated by the
SPARC calculator.
64
-------
0.001
0.0008
CD
'o
>t ^
CD °
o E
O co~ 0.0006
ro 0.0004
y> "ro 0.0002
CD
I
Ethyl
CD
CO
CD 1?
O
Q.
cc
0 10 20 30 40 50
1000 -g
100 -=
0.'
°-2
«o| 0.12
- g I 0-08
w
i
b
CD
CD 'O
CD
0.04
0
3E-005
2E-005
1E-005
Q
,_
-------
.5j 0.002
£ 0s 0.0016
o E
Oc^- 0.0012
ro _ 0.0008
w 15 0.0004
1,1-Diethoxyethane
CD
Q. 1 -=
cc
> =
n 1
U. I | i | i | i | i |
0 10 20 30 40 50
E 0-16
w CD -^
CD _
> o 6
oO
c c 4
co o
ni 2
0 ro
n n
0 10 20 30 40 50
Temperature (C)
Figure 27 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion coefficient,
octanol/water partition coefficient) for 1,1-diethoxyethane estimated by the SPARC calculator.
66
-------
MTBE
5 °-01 ~n
1 0s 0.008
o E
O ^ 0.006
5 E
cc _ 0.004
w ^ o.002
c o
CD U
i 1^1 i^_wi iw
0.01 ,
^^ 0 008 _I
^^^^^^^^^^^^
0.006
0.004
0.002
~
' I ' I ' I ' I ' I 0
\v\ 1 I/ l__
^
_^^^
^^^^^^
II 1 1 1 1 1 1 II
X 0 10 20 30 40 50 0 10 20 30 40 50
1000 -g
w 100 -i
w ^-. =
CD t =
(to 10 -=
I =
Q_ 1 -=
CD E
n -i
U. 1
1000 -g
^******~~ 100 -I
z
10 -g
1 _I
=
n 1
| i | i | i | i | U. I
_
1 1 1 1 1 1 1 1 1 1
0 10 20 30 40 50 0 10 20 30 40 50
1 °'2 "I
(DIE °'16
W CD
> O
o O 100
TO §
"G £ 50
O t
TO
0. 0
200 |
V
150
100
_
50
' I I I I I 0
^^
^^^^^^^^^^^^^^^
1 1 1 1 1 1 1 1 1 1
0 10 20 30 40 50
Temperature (C)
0 10 20 30 40 50
Temperature (C)
Figure 28 Properties (Henry's Law coefficient, vapor pressure, air phase diffusion coefficient,
octanol/water partition coefficient) for benzene and methyl tert-butyl ether (MTBE) estimated by the
SPARC calculator.
67
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