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Technology Administration

National Institute of Standards and Technology

NIST Technical Note 14 12

Thermochemical and Chemical Kinetic Data

for Fluorinated /Hydrocarbons

D. R. F. Burgess, Jr., M. R. Zacharlah, W. Tsang, and R R. Westmoreland

CH3F CH2F2 CHF3

CH2F

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/

\ =?\ / CHF / \ CF2

CF3 ^^ /I

CH3O \ // CH A-^-CF V \ I CF3O

' ^ \ / ^, I / / A I / /

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J

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At Boulder, CO 80303. 'Some elemenis at Boulder, CO 80303.
NIST Technical Note 1412

Thermochemical and Chemical Kinetic Data

for Fluorinated Hydrocarbons

D. R. F. Burgess, Jr., M. R. Zachariah, W. Tsang

Chemical Science and Technology Laboratory

National Institute of Standards and Technology

Gaithersburg, MD 20899-0001

and

R R. Westmoreland

Department of Chemical Engineering

University of Massachusetts

Amherst, MA 01003-3110

July 1995

*'-4TES o«

U.S. Department of Commerce

Ronald H. Brown, Secretary

Technology Administration

Mary L. Good, Under Secretary for Technology

National Institute of Standards and Technology

Arati Prabhakar, Director
National Institute of Standards U.S. Government Printing Office For sale by the Superintendent of and Technology Washington: 1995 Documents

Technical Note 1412 U.S. Government Printing Office

Natl. Inst. Stand. Technol. Washington, DC 20402

Tech. Note 1412

163 pages (July 1995)

CODEN: NTNOEF
EXECUTIVE SUMMARY

A comprehensive, detailed chemical kinetic mechanism was developed and is presented

for Ci and C2 fluorinated hydrocarbon destruction and flame suppression. Existing fluorinated

hydrocarbon thermochemistry and kinetics were compiled from the literature and evaluated. For

species where no or incomplete thermochemistry was available, these data were calculated

through application of ab initio molecular orbital theory. Group additivity values were

determined consistent with experimental and ab initio data. For reactions where no or limited

kinetics was available, these data were estimated by analogy to hydrocarbon reactions, by using

empirical relationships from other fluorinated hydrocarbon reactions, by ab initio transition state

calculations, and by application of RRKM and QRRK methods. The chemistry was modeled

considering different transport conditions (plug flow, premixed flame, opposed flow diffusion

flame) and using different fuels (methane, ethylene), equivalence ratios, agents (fluoromethanes,

fluoroethanes) and agent concentrations. This report provides a compilation and analysis of the

thermochemical and chemical kinetic data used in this work.

Ill

Table of Contents

1. Introduction 1 1.1. Overview 1 1.2. Background 3

1.3. Mechanism Development 5

1.4. Acknowledgments 5

2. Thermochemistry 7

2.1. Overview 7

2.2. H/O/F and Hydrocarbon Species 11

2.3. Ci Fluorinated Hydrocarbons 13

2.3.1. Fluoromethanes 13

2.3.2. Fluoromethyl Radicals 14

2.3.3. Fluoromethylenes and Fluoromethylidyne Radical 16

2.3.4. Carbonyl Fluorides and Fluoromethoxy Radicals 17

2.4. C2 Fluorinated Hydrocarbons 19

2.4.1. Fluoroethanes 19

2.4.2. Fluoroethyl Radicals 21

2.4.3. Fluoroethylenes and Fluorovinyl Radicals 22

2.4.4. Fluoroacetylenes, Fluoroketenes, and Fluoroketyl Radical 24

2.5. BAC-MP4 Ab Initio Predictions 25

2.6. Thermochemical Tables 29

2.6.1. Table 1: AHf°, S°, Cp°(T) - H/0 Species, Hydrocarbons 29

2.6.2. Table 2: AHf^ S^ Cp°(T) - H/F/0 Species, Ci Fluorocarbons 30

2.6.3. Table 3: AUf, S°, Cp°(T) - C2 Fluorocarbons 31

2.6.4. Table 4: AR° - Calculated, Literature Values, Uncertainties 32

3. Reaction Kinetics 35

3.1. Overview 35

3.1.1. Figure 1. Fluorinated Hydrocarbon Reaction Pathways 37

3.2. Hydrocarbon and H/O/F Chemistry 39

3.3. Cj Fluorinated Hydrocarbon Chemistry 41

3.3.1. Overview 41

3.3.2. Fluoromethanes: Decompositions 42

3.3.3. Fluoromethanes: H Abstractions by H Atoms 44

3.3.4. Fluoromethanes: H Abstractions by O Atoms and OH Radicals 46

3.3.5. Fluoromethanes: H Abstractions by F and F Abstractions by H 48

3.3.6. Fluoromethanes: Metathetical Reactions 50

3.3.7. Fluoromethyl Radical Destruction 51

3.3.8. Fluoromethylene Destruction 54

3.3.9. Fluoromethylidyne Destruction 56

3.3.10. Carbonyl Fluoride Chemistry 57
3.4. C2 Fluorinated Hydrocarbon Chemistry 59

3.4.1. Overview 59

3.4.2. Fluoroethanes: Thermally and Chemically Activated Decompositions .... 60

3.4.3. Fluoroethanes: Fluoromethyl/methylene Disproportionations/Insertions ... 62

3.4.4. Fluoroethanes: Abstractions 63

3.4.5. Fluoroethyl Radical Destruction 65

3.4.6. Fluoroethylene Chemistry 66

3.4.7. Fluorovinyl Radical Destruction 69

3.4.8. Fluoroethyne, Fluoroketene, and Fluoroketyl Radical Chemistry 70

3.5. BAC-MP4 Ab Initio Predictions 71

4. Future Mechanism Refinement 75

4.1. Overview 75

4.2. Thermochemistry 79

4.3. Kinetics 83

5. Reaction Set (Table 5) 85

5.1. Description of Listing 85

5.2. H/0 Reactions 89

5.3. Hydrocarbon Reactions 90

5.4. NIST HFC Mechanism 95

5.4.1. H/F/0 Species 95

5.4.2. Fluoromethanes 96

5.4.3. Fluoromethyl Radicals 98

5.4.4. Fluoromethylenes 99

5.4.5. Fluoromethylidyne Radical, Fluoromethoxy Radical 100

5.4.6. Carbonyl Fluorides 101

5.4.7. Fluoroethanes: Decompositions 102

5.4.8. Fluoroethanes: Abstractions 106

5.4.9. Fluoroethyl Radicals 110

5.4.10. Fluoroethylenes 112

5.4.11. Fluorovinyl Radicals 115

5.4.12. Fluoroethynes, Fluoroketenes 116

5.4.13. F Atom Reactions 117

5.5. Reference Reactions 118

5.6. Notation 122

5.7. Citation Index 123

VI
6. Bibliography 127

6.1. Overview 127

6.2. General Thermochemistry and Kinetics 129

6.3. Hydrocarbon Chemistry 133

6.4. Fluorine Chemistry 135

6.5. Fluorocarbon Thermochemistry 137

6.6. Oxidized Fluorocarbon Thermochemistry 145

6.7. Fluorocarbon Kinetics (Decompositions) 147

6.8. Fluorocarbon Kinetics (Abstractions) 151

6.9. Fluorocarbon Kinetics (Oxidations) 155

6.10. Oxidized Fluorocarbon Kinetics 159

6.11. Fluorocarbon Kinetics (Other) 163

6.12. Flame Inhibition (Halogens) 169

6.13. Flame Inhibition (non-Halogens) 173

Vll

1. Introduction

1.1. Overview

The thermochemical and chemical kinetic data presented here were compiled as a part

of flame-inhibition modeling that was part of a large, short-term, intensive effort at NIST that

evaluated (for the U.S. Air Force, Navy, Army and Federal Aviation Administration) potential

fluorinated hydrocarbons and other agents as replacements for Halon 1301 (CFjBr). The

modeling effort complemented the many experimental measurements in the overall NIST program, which characterized the effectiveness of various potential replacements. Our work

focused on agent chemistry. This report is to provide documentation of the thermochemical and

chemical kinetic data used in the modeling work. Further details of the evaluation of the

thermochemical and chemical kinetic data and the ab initio calculations will be provided

elsewhere, as will the results of the simulations of flame inhibition.

Halon 1301 is very effective as a chemical extinguisher. However, it is also extremely

effective for depleting stratospheric ozone. Consequently, its production and use are restricted.

The major objective of the modeling part of the overall work was to provide a chemical basis

for rationalizing the relative degree of effectiveness of each candidate agent. A fundamental

understanding of the chemistry of these agents in hydrocarbon flames should facilitate

identification of desired characteristics of effective agents. That is, utilization of simple

chemical concepts should enable screening and selection of potential agents with minimal time

and human resources.

In order to accomplish this goal, it was necessary to develop a chemical mechanism based on elementary reaction steps for their destruction, their participation in and influence on

hydrocarbon flame chemistry, as well as for prediction of potential by-products of incomplete

combustion. However, neither a comprehensive mechanism nor a general review of the relevant

the relevant chemistry existed prior to this study. Consequently, a significant effort was

required in order simply to construct such a comprehensive mechanism prior to its use in any

simulations. Further refinement of the mechanism requires experimental validation by flame

measurements.
The focus of the mechanism development work was restricted to the chemistry involving

only fluoromethanes and fluoroethanes. This includes both four of the candidate agents

specifically being considered as replacements (i.e., CH2F2, CF3-CH2F, CF3-CHF2, CF3-CF3),

as well as all of the other possible fluoromethanes and fluoroethanes. Larger fluorinated

hydrocarbon agents (e.g., C3F8) and chlorine-substituted agents (e.g., CHFjCl) were not

explicitly considered in our study, because these additions significantly increase the complexity

of the chemistry that must be considered. However, the effectiveness of each can be estimated

to some degree by analogy to the other agents that were studied. This can be done by using the

qualitative trends observed and the fundamental understanding of the chemistry developed by this

and future work.

The complete set of fluoromethanes and fluoroethanes were studied for two basic reasons. These are discussed below.

First, when the four specific candidate agents being considered decompose in the flame,

they generate a pool of fluorinated hydrocarbon stable species and radicals, which results in the

formation of many of the other fluoromethanes and fluoroethanes. Consequently, in order to

describe the decomposition of the four specific agents (and resultant chemistry) adequately, it

is necessary to describe the chemistry of all of the many intermediates and products that are

created, including most of the other fluoromethanes and fluoroethanes. For example, the lowest

energy and primary decomposition pathway for one of the candidate agents, CF3-CF3, involves

dissociation of the C-C bond to form (two) "CFj radicals. These -CFj radicals will then react

with methyl radicals, •CH3, which are present in significant concentrations in hydrocarbon

flames. This radical-radical combination reaction has two decomposition channels whose relative

importance is dependent upon temperature and pressure. One channel results in the formation

of a fluoroethylene, CH2=CF2 (and HF by-product). The other channel results in the formation

of another fluoroethane, CH3-CF3. It is important that the mechanism adequately predicts the

combustion products, the magnitude and rate of heat release in the flame, and ultimately the

effectiveness of the added agent. Consequently, this requires that the mechanism also be able

to describe correctly the decomposition of these two additional stable fluorinated hydrocarbon

species (CH3-CF3, CH2=CF2). When one considers all decomposition channels for both the
candidate agents and their decomposition products, one essentially must include all chemistry

describing almost all of the fluoromethanes and fluoroethanes.

Second, given that there are to date few experimental data with which to make

comparisons, it is imperative to provide a level of self-consistency to this purely modeling work

by considering a range of modeling parameters, including different reactor/flame geometries,

different fuels, different (potential) agents, and many other conditions. In doing so, it allowed

us to develop confidence in the validity of the qualitative trends that we observed. Quantitative

prediction of the absolute or even relative effectiveness of the specific agents will require

successful comparison of the simulations with experimental measurements.

1.2. Background

There has been a significant amount of work over many years that has investigated the

effectiveness of halogenated fire suppressants, as well as other types of fire suppressants (see

Bibliography section). We will not review this body of work, but refer the reader to these and

other relevant sources. A large part of our work is based on the pioneering work in this area by Biordi and coworkers (e.g., Biordi et al, 1973), Dixon-Lewis {e.g., Dixon-Lewis, 1977),

Fristrom {e.g. , Fristrom and Van Tiggelen, 1979) and Westbrook (1983). In earlier experiments on a range of candidates, CFsBr was identified as being very effective for extinguishing flames.

However, the mechanism for inhibition by CFjBr was not understood. Biordi and coworkers

measured both stable and radical species in methane flames doped with CFjBr using a flamesampling molecular beam mass spectrometer. Many of the relevant elementary reactions that

describe the decomposition of CFjBr, its chemistry, and its influence on hydrocarbon flames

were determined in this work. Westbrook developed the first comprehensive chemical

mechanism to describe in detail the chemistry of CFjBr and modeled inhibition in hydrocarbon

flames. As a result of this work, it is generally agreed that flame suppression by brominecontaining compounds is a result of catalytic destruction of H atom species by Br atoms. The

ability of bromine to recycle in the chemical system in the flame is directly related to the weak

molecular bonds formed by bromine. Thus, bromine when complexed in molecules such as

CFjBr, CHjBr, HBr, and Brj, can through a number of reactions regenerate Br atoms. It was
also determined in these studies that -CFj, formed by decomposition of CFjBr, also removes H

atoms by competition with radicals important to combustion {e.g., H, O, OH, HO2).

There are a variety of ways in which fire suppressants act in inhibiting hydrocarbon

flames. Most of these effects are intimately related. For example, a heat loss means a

temperature decrease, which causes the chemistry to slow, which means fewer radicals leading

to product formation, which means less heat generated, which results in a further temperature

decrease and so on. One can separate suppression effects into two general categories: physical

and chemical (although there is overlap). Chemical effects are directly related to the

characteristics of the specific molecule (e.g., H, F, or CI substitution), while physical effects,

in general, are not. For example, the heat capacity of a molecule is a physical effect, since to

a first approximation it is largely a function of the number of atoms in the molecule and their

connectivity but not the identity of the molecule (i.e., its chemical composition).

There are a number of physical effects that relate to fluid mechanics, mass transport, and

heat transport processes that were not specifically studied as a part of this modeling work.

Physical effects that should be taken into account are, for example, PVT properties (pressurevolume-temperature), discharge dynamics, dispersion mechanics, as well as more complex flow

reactor geometries than could be considered in this work. We will not discuss these physical

effects in any detail here. However, it is necessary to understand the impact of these effects as

they relate to our results in order to provide a framework for transfer of the results of our

simulations to more realistic conditions. Some of the fluid mechanics and mass transport effects

include dilution, turbulent mixing, diffusive mixing, thermal diffusion, and buoyancy. Heat

related effects, which cannot directly be addressed in the simulations, include the latent heat of

vaporization and non-adiabatic effects, such as radiative cooling or heat losses for flames

attached to a cold surface.

There are a number of different types of chemical effects. Most of these involve

different competing factors. First, all of the fluorinated hydrocarbons will eventually decompose

and then bum (forming CO2, H2O, and HF). This liberates heat and increases flame

temperatures (this speeds flame chemistry). On the other hand, the agents considered as

replacements are large molecules with many atoms. Consequently, their high heat capacities

may result in a decrease in flame temperature prior to complete combustion (this slows flame
chemistry). The competition between these two factors is strongly dependent upon conditions;

most important of which is the mechanics of mixing of the fuel and the oxidizer. Another set

of competing effects involves fluorinated radicals produced by agent decomposition. These

radicals are slower to bum than their pure hydrocarbon analogues, because the C-F bond is significantiy stronger than the C-H bond. Consequentiy, reactions involving these radicals may

effectively compete with analogous pure hydrocarbon chemistry by creating less "flammable"

intermediates, thereby inhibiting combustion of the hydrocarbon fuel. For example, since the

agents are added to the air stream, their immediate decomposition products (radicals) are formed

in oxygen-rich, relatively cold regions of the flame. Consequentiy, these radicals may be

involved in termination steps, such as •CF^ + H02* -* CHF3 4- O2, slowing radical chain

reactions and inhibiting the flame. These radicals also compete with hydrocarbon radicals for

important H, O, and OH radicals. On the other hand, these radicals also react with stable

molecules in the colder air stream {e.g., O2), generating more radicals, such as O atoms, and

thereby initiating chemistry or promoting combustion of the fuel.

1.3. Mechanism Development

We constructed a large comprehensive reaction set or "mechanism" for fluorinated

hydrocarbon chemistry involving Cj and C2 stable and radical hydrocarbon species, including

partially oxidized fluorinated hydrocarbons. The mechanism should be considered only a framework for future model development, rather than a finished product. Future refinements

will require experimental validation by high-temperature flow reactor, premixed flame, and

diffusion flame measurements, as well as measurements of important, yet currentiy uncertain rate

constants.

1.4. Acknowledgments

The authors wish to acknowledge support of the project "Agent Screening for Halon 1301

Aviation Replacement" by the U.S. Naval Air Systems Command, the U.S. Army Aviation and

Troop Command, the Federal Aviation Administration Technical Center, and the U.S. Air

Force. This program at NIST was under the direction of Mr. Michael Bennett at the Wright
Patterson AFB Flight Dynamics Laboratory, Vehicle Subsystems Division, Survivability

Enhancement Branch. The authors also wish to express their gratitude to Dr. Carl F. Melius

of Sandia National Laboratories for use of the BAG (Bond Additivity Corrections) code.
2. Thermochemistry

2.1. Overview

Existing thermochemical data were compiled and evaluated. Where few or no data

existed for potential species of interest (most of the radicals), we estimated that thermochemistry

using both empirical methods, such as group additivity (Benson, 1976), and also through

application of ab initio molecular orbital calculations (Melius, 1990; Curtiss et al. , 1991; Frisch

et al, 1992). In all cases (experimental, empirical, and ab initio), significant effort was made

to utilize thermochemical data for each species that was consistent with data for all other species.

There are a number of general sources of relevant compiled and evaluated thermochemical data. These include The Chemical Thermodynamics of Organic Compounds (Stull et

al, 1969), JANAF Thermochemical Tables (Stull and Prophet, 1971; Chase et al, 1985),

Thermochemical Data ofOrganic Compounds (Pedley et al , 1986), TRC Thermodynamic Tables

(Rodgers, 1989), Physical and Thermodynamic Properties of Pure Chemicals (Daubert and

Danner, 1985), and NIST Structures and Properties Database and Estimation Program (Stein

et al , 1991). There are two compilations/evaluations of fluorinated hydrocarbons in the Journal

of Physical and Chemical Reference Data: "Ideal Gas Thermodynamic Properties of Six

Fluoroethanes" (Chen et al , 1975) and "Ideal Gas Thermodynamic Properties of Halomethanes"

(Kudchadker and Kudchadker, 1978). There are two compilations/evaluations of fluorinated

hydrocarbons in the Russian Chemical Reviews: "Thermochemistry of Halogenomethanes"

(Kolesov, 1978) and "Thermochemistry of Haloethanes" (Kolesov and Papina, 1983). There are

a few individual sources of more recent data for thermochemistry that are relevant. These include "Thermochemistry of Fluorocarbon Radicals" (Rodgers, 1978), "Hydrocarbon Bond

Dissociation Energies" (McMillen and Golden, 1982), "A Kinetic Study of the Reactions of OH

Radicals with Fluoroethanes. Estimates of C-H Bond Strengths in Fluoroalkanes" (Martin and

Paraskevopoulos, 1983), and "Halomethylenes: Effects of Halogen Substitution on Absolute

Heats of Formation" (Lias et al, 1985). There are numerous other references with

thermodynamic data for fluorinated hydrocarbons that we have compiled as part of this work.

These are included in the Bibliography section and some of them will be cited and, possibly, be

discussed in more detail in the relevant sections.
It should be noted that for some of the stable species and for many of the radicals, we

have relied upon recent ab initio calculations of thermochemical data. This includes both ab

initio calculations done as part of work and those done previously by other workers.

Tschuikow-Roux and coworkers have calculated thermochemistry for the fluoroethyl radicals

(Chen et al, 1990a, 1990b; Chen et al, 1991a, 1991b). Nyden (1993) has used ab initio

calculations to obtain thermochemical data for a number of the fluoroethanes and fluoroethyl

radicals. Details of our ab initio calculations can be found elsewhere (Burgess et al , 1994;

Zachariah et al., 1995).

The thermochemical data that was used is given Tables 1-3 for hydrogen/oxygen and

hydrocarbon species (Table 1), H/F species and Cj fluorinated hydrocarbons (Table 2), and C2

fluorinated hydrocarbons (Table 3). These tables include enthalpies of formation, entropies (at

standard state), and temperature-dependent heat capacities. Comparisons between our calculated

values (Zachariah et al., 1995) and different literature values (experimental and estimated) for

heats of formation are given in Table 4. Reported uncertainties in the literature values are also

given in Table 4.

A discussion of the uncertainties in the thermochemical data is given in the text with each

class of species. The literature values include those which have been calculated using ab initio

methods. A critical evaluation of the ab initio values in comparison with experimentally derived

values will be given in a future publication. In each case where the uncertainty in the data from

the literature was not assigned, we have provided a value based on our limited evaluation of the

data and typical uncertainties for that type of data.

The literature values for heats of formation consist of a number of different types of data.

Many are good quality, experimentally derived values based on heat of combustion or heat of

reaction data, where the other reactants and products have well-established heats of formation.

The uncertainty in these data are typically less than 4 kJ/mol. Some of the data, although

experimentally derived, have somewhat higher uncertainties due to side reactions or where the

other reactants and products have somewhat uncertain heats of formation. Typically, these

values have heats of formation with uncertainties of about 4-8 kJ/mol.
In some cases, the literature values are based, in whole or in part, on bond additivity,

group additivity, or other trends in heats of formation of related species. Typically, these values

have heats of formation with uncertainties of about 8-12 kJ/mol. Many of the radicals have

literature values for their heats of formation that were determined using the heats of formation

of the parent species and bond dissociation energies that were either indirectly measured or were

reasonable estimates based on trends in other molecules. For example, Martin and

Paraskevopoulos (1983) have estimated C-H bond strengths in fluoromethanes and fluoroethanes

(and, consequently, heats of formations for the fluoromethyl and fluoroethyl radicals) through

correlations between the rates of H atom abstraction by OH radicals, C-H vibrational

frequencies, and known C-H bond strengths. We have supplemented these data with our own

estimates in order to provide heats of formation for the other fluoroethyl radicals in the absence

of other literature values.

2.2. H/O/F and Hydrocarbon Species

We used standard hydrogen/oxygen cind hydrocarbon thermochemistry, most of which

can be found in the JANAF tables (Stull and Prophet, 1971; Chase et al. , 1985) or in a Sandia

compilation (Kee et al., 1987), as can data for F and HP, There is a more recent value for

the heat of formation of HP (Johnson et al. , 1973). However, we used the JANAP value for

consistency, because many thermochemical and rate data for fluorinated species are based on the

JANAF recommendation. More recent data on thermochemistry for C2H3 and HCO have been

utilized. Future mechanism refinements should include re-adjustment of any other

thermochemistry (or rate constants) that are based upon older values for the heat of formation

of these species.

Other simple species (e.g. , P2, PO», HOP, FOP, FOO», HOOP) were initially considered

in the mechanism but were later excluded because they did not contribute to the overall

chemistry.

11

2.3. Ci Fluorinated Hydrocarbons

2.3.1. Fluoromethanes

We have chosen to employ heats of formation for the fluoromethanes recommended by

Kolesov (1978) with the entropy and heat capacity data found in a review article (Rodgers et ah ,

1974) in the Journal of Physical and Chemical Reference Data (JPCRD). We note that heats of

formation for the fluoromethanes from our ab initio calculations (Zachariah et al. , 1995) using

the BAC-MP4 method (Melius, 1990) are within about 2 kJ/mol of these recommended values.

There are a number of sources of compiled or evaluated thermochemical data for the

fluoromethanes (CH3F, CHjFj, CHF3, and CF4). Thermochemical data for the fluoromethanes

has been reviewed by Lacher and Skinner (1968), by Stull et al. (1969), and by Cox and Pilcher

(1970). Thermochemical data can also be found in the JANAF tables (Stull and Prophet, 1971),

has been re-examined subsequently in JPCRD (Rodgers et al, 1974), by Pedley et al. (1986),

and mostly recently, by Gurvich, Veyts, and Alcock (1991). The most recent edition of the

JANAF tables (Chase et al, 1985) did not re-examine thermochemical data for the

fluoromethanes. Recommendations for the heats of formation of the fluoromethanes have been

also been made by Kolesov (1968). Gelles and Pitzer (1953) have tabulated entropy at standard

state and heat capacity as a function of temperature for the fluoromethanes (and other

halogenated methanes).

Heats of formation for CHjFj and CF4 are the best known, with uncertainties of less than

1.5 kJ/mol, and are derived from their heats of combustion. The JPCRD recommended value

for the heat of formation of CH2F2 is based on a measurement by Neugebauer and Margrave

(1958) of the heat of combustion of CH2F2. The heat of formation of CF4 is based on

measurements of a number of different heats of reactions involving CF4 by Scott et al. (1955),

Good et al. (1956), Neugebauer and Margrave (1956), Cox et al. (1965), Wood et al. (1967),

Domalski and Armstrong (1967), and Greenberg and Hubbard (1968).

The heat of formation of CHF3 has a slightly higher uncertainty (than for CH2F2 and CF4)

of about 4 kJ/mol due to side reactions (producing CF4) in its combustion. The JPCRD

recommended value for the heat of formation of CHF3 is based on a heat of combustion

measurement by Neugebauer and Margrave (1958). The heat of formation of CHF3 has also

13
been calculated using equilibrium data with CFjBr and CF3I as measured by Corbett et al.

(1963), Goy et al (1967), Coomber and Whittle (1967). The heat of formation of CHF3 can

also be calculated assuming a heat of formation for -CFj and kinetic data (forward and reverse

reactions) involving HCl, HBr, and HI as measured by Coomber and Whittle (1966), Amphlett

and Whittle (1968), and Goy et al. (1967), respectively.

The heat of formation of CH3F has been estimated (with an uncertainty of about 10

kJ/mol) employing empirical trends in heats of formation of the other fluoromethanes, since

there are no experimentally derived values (other than from appearance potential measurements).

Although CH3F is unlikely to be a key species in fluorinated hydrocarbon-inhibited hydrocarbon

flames, as the simplest fluorinated hydrocarbon, its heat of formation is significant for

benchmarking heats of formation of other fluorinated hydrocarbons. Empirical estimates for the

heat of formation of CH3F have also been made by Zahn (1934), Allen (1959), Bernstein (1965),

Rodgers (1967), and Lacher and Skinner (1968). The recommended value in the JANAF tables

(Stull and Prophet, 1971) is based on appearance potentials for CH3'^ from CH3F measured by

Lossing et al. (1954). Dibeler and Reese (1955) and Tsuda et al. (1964) have also measured

roughly the same appearance potential,

2.3.2. Fluoromethyl Radicals

We have chosen to employ the heats of formation recommended by McMillen and Golden

(1982). For entropies at standard state and heat capacity data, we used values for •CF3 from

the JANAF tables. Since (to our knowledge) no experimentally derived entropy and heat

capacity data exist for •CH2F and 'CHFj, we used that derived from our BAC-MP4 ab initio

calculations. We note that the calculated heats of formation for the fluoromethyl radicals are

within about 4 kJ/mol of the recommended experimental values.

There are a few sources of compiled or evaluated thermochemical data for the

fluoromethyl radicals. Thermochemical data for the perfluoromethyl radical (•CF3) can be found

in the JANAF tables (Stull and Prophet, 1971) and have been re-examined subsequently by

Rodgers (1978). The heat of formation of •C¥^ has an uncertainty of about 5 kJ/mol.

Experimentally derived heats of formation (from bond dissociation energies and heat of reac14
tions) for all of the fluoromethyl radicals (•CRJF, 'CHFj, •CF3) can be found in evaluations by

McMillen and Golden (1982) and Pickard and Rodgers (1983) with uncertainties of less than 10

kJ/mol.

The evaluated thermochemical data for •CH2F and •CHF2 are based on a number of

different experimental measurements. Okafo and Whittle (1974) have used heat of reaction data

to determine the bond dissociation energy for CHFj-Br, from which the heat of formation of

•CHF2 can be calculated, Martin and Paraskevopoulos (1983) have measured the rates of

reaction of OH with some fluoromethanes and fluoroethanes and developed correlation between

C-H bond dissociation energies, C-H stretching frequencies, and rates of abstraction of H atoms

by OH radicals from fluoroalkanes. From heats of formation of the parent fluoromethanes and

estimated C-H bond dissociation energies, one can determine values for the heats of formation

of 'CHjF, •CHF2, and -CFj. Whittle and coworkers have used heat of reaction data to

determine the bond dissociation energies of CHF2-H and CHF2-Br (Okafo and Whittle, 1974),

from which the heat of formation of •CHF2 can be calculated. Using kinetic data, bond

dissociation energies for CHjF-H have obtained by Pritchard and Perona (1969) and for CHF2-H

by Kerr and Timlin (1971), from which one can calculate the heats of formation of the

corresponding radicals.

The evaluated thermochemical data for •CF^ are based on a number of different

experimental measurements. The heat of formation of ^CF^ has been calculated assuming a heat

of formation for CHF3 and kinetic data (forward and reverse reactions) involving HCl, HBr, and

HI, as measured by Coomber and Whittle (1966), Amphlett and Whittle (1968), and Goy et al.

(196 7), respectively. It can also be calculated assuming a heat of formation of CF3I and kinetic

data for its reaction with I2, as determined by Coomber and Whittle (1966). Pritchard and

Thommarson (1964) used kinetic data from competing reactions to determine the CF3-H bond

dissociation energy and, consequently, the heat of formation of -CFj can be calculated assuming

a heat of formation for CHF3. Whittle and coworkers have used heat of reaction data to

determine the bond dissociation energies for CF3-CF3 (Coomber and Whittle, 1967), CF3-Br

(Ferguson and Whittle, 1972), and CF3-I (Okafo and Whittle, 1975), from which the heat of

formation of •CF3 can be calculated. Tsang (1986) has determined a value for the heat of

15
formation of 'CFj based on the bond dissociation energy of CF3-Br from shock tube

decomposition studies.

2.3.3. Fluoromethylenes and Fluoromethylidyne Radical

We used heats of formation for tCFj as adopted by Rodgers (1978) and for :CHF as

provided by Pritchard et al. (1984). For entropies at standard state and heat capacity data of

both species, we used values from the JANAF tables. We note that heats of formation for both

species from our BAC-MP4 ab initio calculations (Zachariah et al. , 1995) are within about 15

kJ/mol of the recommended experimental values.

There are a few sources of thermochemical data for the closed-shell fluoromethylenes

(:CHF and tCFj). Thermochemical data for these species can be found in the JANAF tables

(Stull and Prophet, 1971). More recently, Rodgers (1978) has recommended a value for the heat

of formation of tCFj based largely upon kinetic data. Hsu et al. (1978) and Pritchard et al.

(1984) have independently made a recommendation for the heat of formation of :CHF based

upon heat of reaction and kinetic data. Lias et al. (1985) have provided values for the heat of

formation of both :CHF and iCFj based upon appearance and ionization potentials.

Unfortunately (since :CHF and tCFj are important species), there are significant uncertainties

in their heats of formation. The values for rCFj are the best (± 10 kJ/mol) and are derived from

a number of different types of measurements. The uncertainty in the heat of formation for :CHF

is even greater (±30 kJ/mol) due to the lack of direct, reliable data.

The experimental data for the heat of formation of iCFj comes from a number of

different measurements. The heat of formation of rCFj has been calculated from heat of reaction

or kinetic data from the decomposition of C^^ by Modica and LaGraff (1965, 1966), by Zmbov

et al. (1968), by Schug and Wagner (1968), and by Carlson (1971). Using equilibrium data in

experiments by Farber et al. (1969), one can also determine a value. The heat of formation of

rCFj has also been calculated from the decomposition of various halomethanes: from the

decomposition of CHF3 by Schug and Wagner (1978), from the decomposition of CHFjBr by

Okafo and Whittle (1974), and from the decomposition of CHFjCl by Dalby (1964), Gozzo and

Patrick (1964), Edwards and Small (1965), and Schug and Wagner (1968). The ionization

16
potential of rCFj has been used to estimate its heat of formation by Fisher et al. (1965), Pottie

(1965), and Zmbov et al. (1968). Various appearance potential measurements by Walter et al.

(1969), Herman et al. (1981), and Paulino and Squires (1991) have also been used to estimate

a value for the heat of formation of :CF2. The ionization and appearance potential measurements

have been reviewed in detail by Lias et al. (1985) and Paulino and Squires (1991).

Thermochemical data for fluoromethylidyne (-CF) can be found in the JANAF tables

(StuU and Prophet, 1971). More recently, Gurvich et al. (1991) have also provided

thermochemical data for -CF. In the latter review, more recent measurements by Hildenbrand

(1975) were also considered, in addition to earlier measurements by Modica (1966) and Farber

et al. (1969). We used the more recent value from Gurvich et al. (1991) for the heat of

formation with the entropy and heat capacity data provided in the JANAF tables. The reported

uncertainties in the heat of formation are about 10 kJ/mol. We note that our BAC-MP4 ab initio

heat of formation for -CF is within about 10-20 kJ/mol of the recommended values.

2.3.4. Carbonyl Fluorides and Fluoromethoxy Radicals

Thermochemical data for the carbonyl fluorides (CHF=0, CF2=0, •CF=0) can be

found in the JANAF table. We have employed these data. The uncertainty in the heat of

formation of CF2=0 is reported to be about 2 kJ/mol. For the other two carbonyl fluorides,

where there is little or no experimental data, the estimated uncertainty in their heats of formation

are probably at least 15 kJ/mol.

Gurvich et al. (1991) have recommended a value for the heat of formation of •CF=0

that is similar to the JANAF recommendation (about 8 kJ/mol higher). This recommendation

is based upon appearance potential measurements of McNeil and Thynee (1969) and heat of

reaction measurements by Heras et al. (1962).

We note that heats of formation for these species from our BAC-MP4 ab initio

calculations (Zachariah et al, 1995) are within about 20 kJ/mol of the recommended

experimental values, except for CF2=0, where the ab initio value is about 40 kJ/mol higher.

Other ab initio calculations (Montgomery et al, 1994; Schnieder and Wallington, 1994) using

different approaches also predict a heat of formation for CF2=0 that is higher (by about 30

17
kJ/mol) than the experimental value. Because of this significant difference, both uncertainties

in the experimental measurements and ab initio calculations warrant further examination.

The biggest uncertainties here are for CHF=0 (±20 kJ/mol) and •CF=0 (±10 kJ/mol),

where there are little or no direct experimental data available and, consequently, their heats of

formation were estimated (Stull and Prophet, 1971) using average bond dissociation energies

from other related compounds. Given that reliable experimental data exists for the unimolecular

decomposition of CHF=0 (Saito et al, 1985), uncertainty in its heat of formation may be

unimportant. However, under some conditions the bimolecular reaction •CF=0 + HjO -» CHF=0 + OH (roughly 80 kJ/mol endothermic) may contribute. Consequently, uncertainty

in the heat of formation of CHF=0 may play some role. In contrast, the heat of formation of

•CF = is very important, since there are not experimental data for its unimolecular

decomposition, which is a primary decomposition pathway (competing with H atom combination

followed by HF elimination).

We used an experimentally derived value for the heat of formation of the

perfluoromethoxy radical CFjO* (Batt and Walsh, 1982) with a reported estimated uncertainty

of about 6 kJ/mol. For entropy at standard state and heat capacity data, we used that derived

from our BAC-MP4 ab initio calculations (Zachariah et ah, 1995). The heat of formation of

CFjO* from the ab initio calculations is within about 30 kJ/mol of the experimentally derived

value.

A number of other species, such as the other fluoromethoxy radicals (CHjFO*, CHFjO*),

fluoromethanols {e.g., CF3OH), or fluoromethylperoxy radicals {e.g., CFjOO*), were initially

considered in the mechanism (using ab initio thermochemical data). These species were later

excluded, because they did not contribute to the overall chemistry. In many cases, these species were present in steady state concentrations and, consequently, the creation and destruction

reactions could be combined into a single overall reaction. Although these species may be

important in atmospheric chemistry, they are present in extremely low concentrations at high

temperatures in hydrocarbon/air flames.

18
2.4. C2 Fluorinated Hydrocarbons

2.4.1. Fluoroethanes

We chose to use thermochemical data from a Journal of Physical and Reference Data

(JPCRD) review (Chen et al., 1975) for the six simple fluoroethanes (CH3-CH2F, CH3-CHF2,

CH3-CF3, CH2F-CF3, CHF2-CF3, CF3-CF3). For CH2F-CH2F, we used a heat of formation

calculated using the C-C bond dissociation energy as determined by Kerr and Timlin (1971) and

the heat of formation for •CH2F as recommended by McMillen and Golden (1982). We used

the heat of formation of CH2F-CHF2 as recommended by Lacher and Skinner (1968). For

CHF2-CHF2, we used a heat of formation calculated using the C-C bond dissociation energy as

determined by Millward et al. (1971) and the heat of formation for •CEF2 as recommended by

McMillen and Golden (1982). Standard state entropy and heat capacities for these other 3

fluoroethanes were computed based on vibrational frequencies and moments of inertia from our

ab initio calculations. We note that heats of formation for all of the fluoroethanes from our BAC-MP4 ab initio calculations are within about 10-20 kJ/mol of the recommended experimental

or empirical values.

We believe some re-examination of all of the heat of formation data is warranted. For

example, the heat of formation of CH3-CF3 recommended in the JPCRD review is based on old

values for •CH3 and •CF3. In addition, employing a group additivity scheme with an ionic

correction should yield better values for both CHjF-CHjF and CHF2-CHF2.

There are a number of sources of compiled or evaluated data for the fluoroethanes.

Thermochemical data for some of the fluoroethanes can be found in JPCRD (Chen et al. , 1975)

and the DIPPR compilation (Daubert and Danner, 1985). Recommendations for the heats of

formation of some of the fluoroethanes have been made by Kolesov and Papina (1983) and by

Pedley et al. (1986). There are no experimentally derived heats of formation for two of the

fluoroethanes (CH3-CH2F, CH2F-CF3). These have been estimated using bond additivity, group

additivity, or other trends in heats of formation. However, there are significant uncertainties

in using these procedures, because of non-covalent or ionic contributions to the stability of these

species due to the high electronegativity of fluorine. For example, CH3-CF3 is about 33 kJ/mol

more stable than predicted using heats of formation of CH3-CH3 and CF3-CF3. All three of these

19
species have heats of formation that were derived from good quality experimental measurements.

The additional stabilization can be rationalized as an ionic contribution to the C-C bond strength

because of large differences in net charges on the carbon atoms of the -CH3 and -CF3 groups due

to the high electronegativity of the F atoms.

There are a number of different sources of experimental data for the heats of formation

of the fluoroethanes. These various sources are described in the paragraphs below.

The heat of formation of ethyl fluoride (CH3-CH2F) has been estimated (Chen et al. ,

1975) using group additivity and heat of reaction data for propyl fluoride (Lacher et al. , 1956).

A recommendation for the heat of formation of ethyl fluoride (CH3-CH2F) has recently been

given by Luo and Benson (1988) based on electronegativity correlations of heats of formation

of substituted alkanes and is significantly lower (15 kJ/mol) than other recommendations. The

reasons for this significant difference warrant further examination. CH3-CH2F is unlikely to be

important as a species in the fluorocarbon-inhibited hydrocarbon flames. However, as a simple,

single-substituted fluorinated hydrocarbon (like CH3F), its heat of formation is important as a

reference point for the heats of formation of other species. For example, another -CHjF

substituted fluoroethane, CH2F-CF3, has no experimentally derived heats of formation. Any

uncertainties in the heats of formation and, consequently, stability of the fluoroethanes will

influence product channels for fluoromethyl combinations {e.g. , •CH3 -\- •CF3 -» CH3-CF3 versus •CH3 + •CV^ -* CH2=CF2 + HF).

Kolesov et al. (1968) have measured the heat of combustion of CH3-CHF2, from which

one can calculate its heat of formation. The heat of formation of CH3-CHF2 could be

determined from the enthalpy of hydrogenation of CF2=CCl2 as measured by Lacher et al.

(1956) given a reliable value for the heat of formation of CF2=CCl2 could be obtained.

We calculated a heat of formation for CH2F-CH2F based on the C-C bond dissociation

energy (368.6 kJ/mol) as determined by Kerr and Timlin (1971) and the heat of formation for

•CH2F (-32.6 kJ/mol) as recommended by McMillen and Golden (1982). The bond dissociation

energy was determined from the critical energy (E^,) calculated using RRKM analysis of

experimental kinetic data for thermal (Chang and Setser, 1969) and chemically activated

decomposition of CH2F-CH2F.

20
Kolesov et al. (1965) have determined a heat of formation for CH3-CF3 by measuring its

heat of combustion. Kinetic data for the forward and reverse reactions for •CH3 + CF3 <—

»

CH3-CF3 can be used to obtain a heat of formation for 1,1,1-trifluoroethane. Kinetic data for

this reaction have been obtained by Giles and Whittle (1965), Pritchard and Perona (1970), and

Chang et al. (1972). These data have been reviewed by Rodgers and Ford (1973).

The heat of formation of CHjF-CHFj has been determined (Kolesov and Papina, 1983)

from the enthalpy of hydrogenation of CF2=CFC1 as measured by Lacher et al. (1956).

We have calculated a heat of formation for CHF2-CHF2 based on the C-C bond

dissociation energy (382.4 kJ/mol) as determined by Millward et al. (1971) and the heat of

formation for •CHF2 (-247.7 kJ/mol) as recommended by McMillen and Golden (1982). The

bond dissociation energy was set equal to the activation energy for thermal decomposition of

CHF2-CHF2, which was determined from analysis of experimental kinetic data.

The heat of formation of CHF2-CF3 can be obtained from equilibrium data with CF3-

CFzBr (and group additivity) as measured by Whittle and coworkers (Coomber and Whittle,

1967; Ferguson and Whittle, 1972) and from heat of reaction data for the bromination of

CF2=CF2 (and group additivity) as measured by Lacher et al. (1956). In addition, one can

calculated a value for the heat of formation for CHF2-CF3 from the heat of formation of the

perfluoroethyl radical (CF3-CF2*) and the CF3CF2-H bond dissociation energy. Wu and Rodgers

(1976) determined the heat of formation of the perfluoroethyl radical by measuring the enthalpy

of its reaction with I2. Values for the bond dissociation energy of CF3CF2-H have been

determined by Bassett and Whittle (1972) and Martin and Paraskevopoulos (1983).

The heat of formation of CF3-CF3 has been determined from equilibrium data with CFjBr

as measured by Coomber and Whittle (1967), with CF3-CN as measured by Walker et al.

(1970), and with CF4 (and NF3 as the oxidizer) as measured by Sinke (1966).

2.4.2. Fluoroethyl Radicals

In the absence of reliable experimental data, we used the calculated thermochemical data

for the fluoroethyl radicals as provided by Tschuikow-Roux and coworkers (Chen et al. , 1990a,

1990b; Chen et al., 1991a, 1991b) for consistency. However, we believe some re-examination

21
of all of the heat of formation data (both experimental and ab initio) is warranted. For the

radical CHj-CHF*, we used the average of the heats of formation reported by Martin and

Paraskevopoulos (1983) and Tschuikow-Roux and Salomon (1987). For the three fluoroethyl

radicals, CHjF-CHF*, CHFj-CFj*, and CFj-CHF*, we calculated heats of formation based on C-H bond dissociation energies determined by Martin and Paraskevopoulos (1983). We note

that heats of formations for the fluoroethyl radicals from our BAC-MP4 ab initio calculations

(Zachariah et ah , 1995) are within about 10-20 kJ/mol of the recommended literature values.

There are a number of sources of heats of formation for the fluoroethyl radicals. There

are experimentally derived thermochemical data (Rodgers, 1978) for a few of the fluoroethyl

radicals (CHj-CFj*, CFj-CHj*, CFj-CFj*). Heats of formation for the others have been

estimated using heats of formation for the fluoroethanes and C-H or C-F bond dissociation

energies for CHj-CHF* and CFj-CHF* by Martin and Paraskevopoulos (1983), for CHj-CHF*

by Tschuikow-Roux and Salomon (1987), and for all of the other fluoroethyl radicals by Burgess

and Zachariah (this work). Thermochemistry for all of the fluoroethyl radicals have been

calculated using ab initio molecular orbital theory by Tschuikow-Roux and coworkers (cited

above). They used the experimentally derived heats of formation of the 3 fluoroethyl radicals

recommended by Rodgers (1978). For the others, they used their calculated energies in

conjunction with isodesmic-homodesmic reactions (with known experimental reaction enthalpies)

to provide values that approach the "true" heats of formation.

2.4.3. Fluoroethylenes and Fluorovinyl Radicals

We used the heat of formation of CH2=CHF as recommended by Gurvich et al. (1991).

Entropy at standard state and heat capacity data were taken from the DIPPR compilation

(Daubert and Banner (1985). These data can also be found in the TRC Thermodynamic Tables

(1990). The heat of formation data are based on measurements by Kolesov and Papina (1970)

of the heat of combustion of vinyl fluoride. Pedley et al. (1986) have also made a recommendation based on this experimental data. A heat of formation was also determined by

Williamson et al. (1976) based on appearance potential measurements.

22
We have chosen to use heats of formation for CHF=CHF(E) and CHF=CHF(Z) based

on appearance ionization potential measurements by Stadelman and Vogt (1980) and entropies

at standard state and heat capacities based on geometries and vibrational frequencies from our BAC-MP4 ab initio calculations (Zachariah et ah, 1995). Gurvich et al. (1991) have also

estimated heats of formation for these species using a bond additivity method. For CH2=CF2,

we used the heat of formation recommended by Gurvich et al. (1991) with entropy at standard

state and heat capacity data taken from Stull et al. (1969). Recommendations for the heat of

formation for 1,1-difluoroethylene have also been made by Lacher and Skinner (1968), Stull et

al. (1969), Cox and Pilcher (1970), and Pedley et al. (1970). All of these recommendations are

based on heat of combustion measurements by Neugebauer and Margrave (1956) and Kolesov

et al. (1962).

We used thermochemical data for CHF=CF2 as recommended by Gurvich et al. (1991).

The heat of formation data is based on an experimental measurement by Kolesov et al. (1962)

of the heat of combustion of trifluoroethylene. Recommended values (also based on these

experiments) can be found in the evaluations of Stull et al. (1969), Cox and Pilcher (1970), and

Pedley et al. (1986).

We used thermochemical data for CF2=CF2 from the JANAF tables (Stull and Prophet,

1971). The recommended heat of formation is based the heat of reaction data for conversion

to amorphous carbon by Neugebauer and Margrave (1956) and Kolesov et al. (1962). Lacher

and Skinner (1968), Stull et al. (1969), Cox and Pilcher (1970), Kolesov and Papina (1983),

Pedley et al. (1986), and Gurvich et al. (1991) have all reviewed the existing experimental data

and made recommendations. These evaluations were made based upon a number of different

sources of experimental heat of reaction data for perfluoroethylene, including the data of Lacher

et al. (1949), Lacher et al. (1950), Kirkbride and Davidson (1954), von Wartenberg and

Schiefer (1955), Duus (1955), Neugebauer and Margrave (1956), Lacher et al (1956), Scott et

al. (1956), Kolesov et al. (1962), and Edwards and Small (1964).

We note that the heats of formation for the fluoroethylenes that we have calculated using

the BAC-MP4 ab initio method are within about 10 kJ/mol of the recommended experimental

values.

23
There are not any experimentally derived thermochemical data (to our knowledge) for

the fluorovinyl radicals, other than the heat of formation for CF2=CF«. The heat of formation

of the perfluorovinyl radical has been estimated by Bryant (1962) based on trends in C-F bond

dissociation energies for perfluorocarbons. Gurvich et al. (1991) recommended a value based on a review of appearance potential measurements by Thynee and MacNeil (1970), Lifshitz and

Crajower (1972), and Bibby and Caster (1966). Because of the lack of experimental data for

most of the fluorovinyl radicals, we chose to use thermochemical data from our BAC-MP4 ab

initio calculations (Zachariah et al. , 1995) in order to provide a consistent set. We note that our

calculated value is within about 10 kJ/mol of the experimentally derived value that was

recommended by Gurvich et al. (1991).

lAA, Fluoroacetylenes, Fluoroketenes, and Fluoroketyl Radical

Data on the thermochemistry of the fluoroacetylenes (CjHF, C2F2) can be found in the

JANAF tables (Stull and Prophet, 1971), however, with relatively large uncertainties: ±60

kJ/mol and ±20 kJ/mol in the heats of formation, respectively. Fluoroketenes (CHF=C=0 and

CF2=C=0) and the fluoroketyl radical (•CF=C=0) can be formed through a number of

channels. These channels are analogous to those considered in pure hydrocarbon chemistry for

ketene (CH2 = C=0). To assess the importance of the fluoroketene species and relevant

reactions, we included these species in the mechanism. There are not any experimentally

derived data for these species. Consequently, we used data from our BAC-MP4 ab initio

calculations (Zachariah et al, 1995).

A number of other partially oxidized species, such as CH3-CFO, were excluded from the

mechanism based on the assumption that they would be only present in steady state

concentrations at flame temperatures. For lower temperatures, these species may become

important and, consequently, our assumption should be re-examined. It is possible that

perfluoro-oxidized species, such as CF3-CFO, may be present at flame temperatures. For

example, since both •CV^ and "CFO are present in significant concentrations, the combination

of these species (and stabilization) may be a source of CF3-CFO. This should be examined in

future refinements of this mechanism.

24
2.5. BAC-MP4 Ab Initio Predictions

For a number of species considered in the reaction set, especially the radicals, there are

little or no thermochemical data. Consequently, we have estimated that data using BAC-MP4

ab initio calculations (see description below). In order to quantify the uncertainties in the

calculated data, we have also performed calculations on many related species where there is good quality experimental data.

Structures, energies, and thermochemical data for a large number of Cj and Cj

hydrocarbons, oxidized hydrocarbons, hydrofluorocarbons, and oxidized hydrofluorocarbons,

including radical species, were calculated using the BAC-MP4 procedure as outlined by Melius

(1986). This procedure involves ab initio molecular orbital calculations using the Gaussian

series of programs (Frish et al., 1990), followed by application of a bond additivity correction

(BAC) procedure to the ab initio calculated energies. The BAG procedure enables energies to

be calculated at accuracies that are necessary for chemical applications, without the need to

resort to large basis sets or configuration interaction terms. This is a particularly important issue

when the goal is the generation of a sufficiently complete data set necessary for development of

a detailed chemical mechanism.

Equilibrium geometries, vibrational frequencies, and zero point energies were calculated

at the Hartree-Fock level using a 6-31G(d) basis set (HF/6-31G*). Using these geometries,

single point energies were calculated with 4th order Moller-Plesset theory using a 6-31G(d,p)

basis set (MP4/6-31G**), to which the BAG procedure was applied. In the BAG method, errors

in the electronic energy of a molecule are bond-wise additive and depend on bonding partner,

distance, and next-nearest neighbors. The energy per bond is corrected by calibration at a given

level of theory against molecules of known energy.

Table 4 lists calculated heats of formation for most of the species in the reaction set, as

well as literature values (where available). We note that we have calculated thermochemical data

for a number of related species that are not included in the reaction set. These data are also

included in Table 4 for purposes of comparison. Of the approximately 110 species, where we

have calculated heats of formation, about 70 species have literature values. We note that the

25
literature values consist of a number of different types of data, including estimated and

calculated values, in addition to those that are derived from experimental measurements.

The average difference between the BAC-MP4 and the literature values is about 9.5

kJ/mol, while the standard deviation is about 7.5 kJ/mol. From these data, we conclude that

for the fluorinated hydrocarbon system, that heats of formation calculated using the BAC-MP4

method provide values that are accurate to less than 10 kJ/mol or comparable to the majority of

the experimentally derived values. We believe that the precision of the ab initio values for any

homologous series to be significantly better than that which is typically obtainable from

experimental measurements. This becomes evident when calculated bond dissociation energies

are compared to those derived from experimental measurements. A more detailed discussion

and comparison can be found elsewhere (Zachariah et al., 1995).

Of all the species, CF2=0 has the largest difference between calculated and experimental

values. Although the quoted uncertainty for this molecule is small, there is reason to believe

that the experimental data may have had side reactions complicating its determination. In

addition, other recent calculations (Schnieder and Wallington, 1994; Montgomery et ah, 1994)

using other ab initio methods predict a heat of formation for CF2=0 that is consistent with our BAC-MP4 calculated value. There are a number of other oxyfluoro-species that have significant

differences between calculated and literature values. However, the heats of formation of these

species were derived based on heats of reactions involving CF2=0. Consequently, if the true

value for CF2=0 was closer to the calculated value, then the experimentally derived values for

these other species would also be closer to their respective calculated values.

There are a number of other species with significant differences between calculated and

literature values. The uncertainties in many of these literature values are high because they are

only indirectly tied to experimental measurements. For example, the heat of formation of the

HCOO* radical is an estimate based on group additivity. The heats of formation of two

fluoroethyl radicals (CFj-CHF* and CH2F-CF2*) were determined from estimated from C-H bond

dissociation energies based on correlations between rates of H atom abstractions, C-H bond

frequencies, and known C-H bond strengths.

To reiterate, from analysis of the data presented in Table 4, we can conclude that for the

fluorinated hydrocarbon system, that heats of formation calculated using the BAC-MP4 method

26
provide values that are accurate to less than 10 kJ/mol or comparable in accuracy to the majority

of the experimentally derived values. Furthermore, from trends in bond dissociation energies,

we believe that the precision of the ab initio values for any homologous series to be significantly

better than that which is typically obtainable from experimental measurements.

27

TABLE 1. Enthalpy of Formation, Entropy, Heat Capacities for H/O, Hydrocarbons

SPECIES AirK298)

kJ/mol

S''(298) J/mol/K

CpCT) J/mol/K Ref

300 500 800 1000 - 1200 1500 2000 3000

Nj 0.0 191.5 29.07 29.63 31.39 32.76 33.70 34.80 35.98 37.02 a Hi 0.0 130.6 28.87 29.27 29.58 30.16 31.07 32.35 34.23 37.11 a o. 0.0 205.0 29.33 31.11 33.75 34.93 35.59 36.49 37.78 39.84 a H2O -241.8 188.7 33.46 35.33 38.58 41.31 43.87 47.10 51.14 55.77 a H2O2 -136.1 232.9 43.57 51.65 59.80 63.64 66.75 70.50 74.80 78.91 a H 218.0 114.6 20.78 20.78 20.78 20.78 20.78 20.78 20.78 20.78 a 249.2 160.9 21.89 21.25 20.98 20.91 20.88 20.84 20.82 20.94 a OH 39.0 183.6 29.93 29.57 29.84 30.68 31.66 32.94 34.63 36.76 a HO2 10.5 229.0 34.87 39.69 45.10 47.64 49.59 52.10 55.33 59.10 a CH4 -74.9 186.0 35.26 46.60 62.75 72.15 78.71 86.32 94.49 101.36 a •CHj 145.7 194.0 38.62 45.33 53.85 59.07 63.19 68.06 73.45 78.30 a ':CH2 387.0 195.5 34.50 37.15 41.57 44.21 46.36 49.11 52.45 55.33 a ^CH2 424.7 188.7 33.79 36.00 41.20 44.38 46.63 49.48 52.88 55.58 a •CH 594.1 182.9 29.09 29.49 30.82 32.56 34.38 36.61 39.18 41.44 a CJtU -83.9 229.0 52.61 77.89 108.05 122.59 132.68 144.83 158.64 171.05 a C2HS. 117.2 251.6 47.37 66.73 94.48 106.71 114.07 123.66 135.76 146.83 a C2H4 52.5 219.2 42.82 62.52 83.90 94.17 101.38 109.70 118.54 125.81 a C2H3. 294.5 227.9 45.77 57.82 71.91 78.77 83.27 89.21 96.90 104.31 a C2H2 226.7 200.9 44.44 54.73 63.90 68.23 71.97 76.46 81.65 87.09 a CH3OH -201.1 239.6 43.98 59.64 79.80 89.53 96.40 104.66 114.00 121.99 a CH3O. 16.3 228.5 37.99 52.02 69.58 77.81 83.38 90.00 97.32 103.23 a •CH2OH -17.2 246.3 47.38 60.16 73.37 78.62 82.59 87.65 93.73 98.76 a CH2O -115.9 218.6 35.15 43.94 55.90 62.27 66.34 70.99 75.80 79.54 a •CHO 43.5 224.5 34.49 38.81 44.93 48.20 50.22 52.53 54.96 57.04 a CO -110.5 197.5 29.08 29.85 31.86 33.25 34.15 35.17 36.27 37,21 a CO2 -393.5 213.7 37.28 44.56 51.54 54.36 56.20 58.29 60.43 62.19 a CH2CO -51.9 241.8 52.01 65.54 78.63 84.70 88.88 93.89 99.49 104.15 a •CHCO 177.6 254.1 52.93 59.53 67.25 70.43 72.56 75.24 78.39 80.77 a HCCOH 85.5 245.6 55.30 67.62 80.10 84.94 88.59 93.24 98.81 103.38 a

29
TABLE 2. Enthalpy of Formation, Entropy, Heat Capacities for H/F/O, Ci Fluorocarbons

SPECIES AirK298)

kJ/mol

S''(298) J/mol/K

C%(T) J/mol/K Ref

300 500 800 1000 1200 1500 2000 3000

F: 0.0 202.7 31.37 34.34 36.46 37.19 37.66 38.20 38.87 39.87 a HF -272.5 173.7 29.12 29.20 29.55 30.14 30.98 32.25 34.01 36.21 a F 78.9 158.7 22.77 22.10 21.46 21.25 21.14 21.03 20.93 20.84 a CHjF -232.6 222.8 37.50 51.26 68.90 77.30 83.34 90.21 96.81 102.59 b

CHiFi ^52.2 246.6 42.96 58.91 76.33 83.55 88.84 94.35 99.47 103.97 b

CHFj -697.6 259.6 51.15 69.26 85.10 91.01 94.89 98.83 102.42 105.39 b

CF4 -933.0 261.3 61.30 80.67 94.49 98.73 101.41 103.67 105.52 106.90 b

.CH2F -32.6 234.4 38.71 48.67 59.29 64.20 67.92 72.02 76.06 79.71 c,d

• CHF2 -247.7 256.0 42.21 54.10 65.33 69.66 72.60 75.69 78.47 80.92 c,e

• CFj ^67.4 265.0 49.94 63.30 73.24 76.37 78.27 79.92 81.29 82.30 c,e :CHF 163.2 223.2 34.63 39.25 45.21 47.93 50.05 52.43 55.43 61.04 f,e :CF2 -186.6 240.7 39.01 46.45 52.35 54.18 55.28 56.31 57.14 58.37 g.e

• CF 242.1 212.9 30.05 32.24 34.79 35.77 36.32 36.96 37.53 38.20 P CHF=0 -376.6 246.7 40.50 51.65 63.12 67.92 71.20 74.70 77.94 80.67 d

CF2=0 -638.9 258.8 47.41 60.49 70.82 74.39 76.71 78.78 80.58 81.96 d

• CF=0 -171.5 248.4 38.99 45.06 50.63 52.76 54.14 55.44 56.57 57.45 d

CFjO. -655.6 275.2 56.44 73.91 86.83 90.89 93.40 95.56 97.32 98.66 h,e

References for Tables 1-3 |

a Keeetal. (1987) i Chen etal. (1975)

b Kolesov(1978) J this work, see text

c McMillen and Golden (1982) k Lacher and Skinner ( 1 968)

d Stall and Prophet (1971) 1 Chenetal. (1990, 1991)

e Zachariah et al. (1995) m Daubert and Danner (1985)

f Pritchardetal. (1984) n Stadelman and Vogt (1980) g Rodgers(1978) StuU etal. (1969) h Batt and Walsh (1982) P Gurvich etal. (1991)

30
TABLE 3. Enthalpy of Formation, Entropy, Heat Capacities for Cj Fluorocarbons

SPECIES AHV298)

kJ/mol

S*(298)

J/moI/K

C*p(T) J/mol/K Ref

300 500 800 1000 1200 ISOO 2000 3000

CH3-CH2F -263.2 265.0 59.83 87.22 116.47 129.62 139.71 150.28 159.35 164.18 i CH2F-CH2F -433.9 288.2 67.88 95.13 124.30 136.74 145.96 155.31 162.30 163.96 j.e CHi-CHFi -500.8 282.5 68.72 97.11 124.65 136.47 145.39 154.49 161.85 165.39 i CH2F-CHF2 -664.8 311.7 75.31 107.53 133.47 143.93 151.98 159.92 169.26 177.71 k.e CH3-CF3 -745.6 287.4 78.81 108.32 133.82 144.08 151.47 158.99 165.10 167.67 i CHF2-CHF2 -877.8 314.8 85.23 115.25 141.25 150.60 156.64 163.29 169.67 173.93 j.e CH2F-CF3 -895.8 316.2 86.58 118.04 143.15 152.09 158.17 164.43 169.66 171.50 i CHF2-CF3 -1104.6 333.8 96.09 127.53 151.13 158.85 164.06 168.60 170.64 169.74 i CF3-CF3 -1342.6 332.1 106.79 139.13 160.34 166.68 169.89 172.97 175.77 177.09 i CH2F-CH2. -44.6 279.8 58.13 80.27 103.74 114.31 122.42 130.91 138.24 142.37 1 CH3-CHF. -76.3 274.0 58.79 79.75 103.33 114.06 122.34 130.91 138.07 141.89 j,l CHjF-CHF. -238.5 293.4 69.59 91.24 111.69 119.75 125.52 131.33 136.07 139.86 j.l CHF2-CH2« -277.2 297.8 67.06 90.20 111.94 121.10 128.00 135.04 140.63 142.60 1 CH3-CF2* -302.5 290.4 67.34 89.22 111.30 120.80 127.83 135.52 142.85 147.42 g,l CH2F-CF2* -446.0 311.1 74.07 97.38 118.86 127.24 133.22 139.11 143.42 144.90 1 CHFz-CHF. -451.9 310.7 76.14 99.54 119.95 127.91 133.70 139.35 143.30 143.80 1 CF3-CH2* -517.1 302.6 77.37 101.75 121.27 128.88 134.26 139.75 145.42 149.64 g.l CHF2-CF2. -664.8 328.4 84.32 107.31 127.04 134.10 138.83 143.26 145.92 145.88 j.l CF,-CHF. -680.7 326.3 85.84 109.68 128.34 135.01 139.45 143.76 147.55 149.47 j.l CF3-CF2» -891.2 340.5 92.84 118.29 136.19 141.80 145.18 148.11 150.50 151.09 g,l CH2=CHF -140.1 262.3 50.61 71.66 91.80 100.57 107.42 114.10 118.92 121.04 p,m

CHF=CHF [Z] -297.1 268.6 58.06 79.62 99.16 107.13 112.47 118.31 124.29 128.86 n,e CHF=CHF [E] -292.9 267.8 59.82 80.44 99.61 107.53 112.83 118.70 124.91 129.77 n,e CH2=CF2 -336.4 265.2 59.33 81.55 100.20 107.74 113.14 118.70 123.44 125.80 P.o CHF=CF2 -491.0 292.7 69.45 90.32 107.48 113.93 118.67 124.16 130.07 134.34 p.o CF2=CF2 -658.5 299.9 80.70 100.40 115.53 120.89 123.89 126.87 129.64 131.27 d CHF=CH. [E] 124.3 258.0 50.61 67.10 81.56 87.66 92.21 97.15 101.75 104.49 e CHF=CH. [Z] 123.0 257.0 50.74 67.33 81.76 87.92 92.44 97.29 101.69 104.19 e CH2=CF. 109.2 256.8 50.22 66.10 80.71 86.89 91.30 96.37 101.64 105.58 e CHF=CF« [E] -41.0 279.3 59.30 74.51 87.79 92.80 96.05 99.66 103.21 105.68 e CHF=CF« [Z] -42.7 279.3 59.30 74.51 87.79 92.80 96.05 99.66 103.21 105.68 e CF2=CH. -67.8 277.0 59.20 76.36 89.73 94.73 97.78 100.81 103.08 103.88 e CF2=CF« -216.3 300.5 68.26 83.42 95.36 99.41 101.77 104.39 106.90 108.21 e CiHF 125.5 231.5 52.48 62.17 69.69 73.22 75.83 78.82 81.96 84.57 d

C2F2 20.9 244.0 57.07 67.96 76.67 79.74 81.54 83.46 85.20 86.16 d CHF=C=0 -147.2 270.5 56.75 71.49 84.93 90.34 94.31 98.24 101.99 102.12 e CF2=C=0 -290.4 288.8 68.30 81.79 92.56 96.66 99.61 102.48 104.72 106.77 e .CF=C=0 69.0 276.2 56.80 65.85 73.77 76.59 94.38 98.22 101.97 103.19 e

31
Table 4. Ci and C2 Fluorinated Hydrocarbon Heats of Formation:

Calculated Values (BAC-MP4), Literature Values, and Uncertainties

SPECIES BAC Lit 1Uncert Ref Lit Ref SPECIES BAC Lit Uncert Ref Lit Ref

CH4 -74.8 -74.9 0.4 a C2H5. 120.6 118.5 a CHjF -233.8 -232.6 8.4 b -247.3 y CH2F-CH2* -56.2 -47.7 1.9 m ^14.6 z CH2F2 ^51.1 -452.2 1.8 b -460.7 y CH3-CHF. -75.6 -76.3 5.9 m -72.4 z CHF3 -699.5 -697.6 4.2 b -697.9 y CHzF-CHF. -247.3 -238.5 12.5 m -235.5 z CF4 -934.1 -933.0 0.4 b -934.3 y CHFj-CHj.

CHj-CFj*

-280.9

-300.2

-285.8

-302.5

15.0

8.4 m -277.2 z .CH3 146.0 145.7 1.3 a •CHjF -31.4 -32.6 8.4 c -32,0 aa CH2F-CF2. -460.1 -449.8 15.0 m -446.0 z .CHF2 -247.3 -247.7 8.4 c -252.0 aa CHF2-CHF. ^59.8 ^56.1 15.0 m ^51.9 z •CF3 ^71.9 ^67.4 8.4 c -472.0 aa CF3-CH2*

CHF2-CF2.

CF3-CHF.

-526.6

-671.1 -703.0

-517.1 -660.7

-680.7

4.2 18.7

9.6 m

P

-660.2 z :CH2 429.8 424.7 4.2 d -688.3 z :CHF

:CF2

131.7

-203.3

163.2 -186.612.6

6.3

e

f

105.0 -180.0aaaa

CF3-CF2. -907.6 -891.2 4.2 -896.0 aa

1 •CH 613.7 594.1 0.4 g C2H4 51.5 52.4 0.8 a •CF 236.3 242.1 10.0 aa 255.2 g CH2=CHF

CHF=CHF[Z]

CHF=CHF[£]

-139.2

-301.3

-302.2

-140.1

-297.1 -292.9

2.5 10.0

10.0

aa

r

r

-138.9

-306.5 aa CH2=0 -108.5 -108.6 6.3 h -303.6 aa CHF=0 -382.3 -376.6 15.0 g CH2=CF2 -340.1 -336.4 4.0 aa -345.2 s CF2=0 -598.4 -638.9 1.7 g

-640.0 aa CHF=CF2

CF2=CF2

^85.6

-653.7 ^91.0-658.5

9.0 2.9

aa

g

^95.8 s .CH=0 -659.5 aa .CF=0

38.9 -182.937.2 -175.78.4 15.0ag -179.0 aa 1 C2H3.

CHF=CH. [Z]

297.1

123.1

286.2 4.2 a CH3OH -204.8 -201.2 0.4 a CF3OH -919.4 -893.3 12.6 i CHF=CH«[E]

CH2=CF.

124.1 CH3OF -92.0 -72.4 12.6 i 109.1 CF3OF -750.1 -764.8 12.6 a CFIF^CF. [Z] ^1.1

CH3O. 27.6 16.7 2.9 J CHF=CF. [E] -42.5 CF3O. -628.3 -655.6 6.3 i CF2=CH.

CF2=CF.

-67.7 -216.4 -227.0 20.0 aa -192.1 t CH3OOH

CF3OOH

-124.6

-807.5

-131.0

-803.3

8.4 15.0hm

1 C2H2 226.8 226.7 0.8 a CH3OO. 25.3 28.0 12.6 a C2HF 117.8 125.5 22.0 g CF3OO. -627.5 -602.5 12.6 1 C2F2 .C2H

31.8 550.5

20.9 564.821.0

4.2 g IIC(0)OH -387.3 -378.6 0.4 h c FC(0PH

HC(Op.

FC(Op.

-614.9

-124.9

-336.9

-150.6 8.4 k

•C2F 453.9 460.2 22.0 m

1 CH2=C=0

CHF=C=0

CF2=C-0

-40.6 -147.2

-290.4

^7.7 2.5 u

C2H6 -86.9 -84.1 0.4 a CH3-CH2F -272.4 -263.2 1.6 1 .CH=C=0 187.3 177.4 8.4 V CH2F-CH2F

CH3-CHF2

CH2F-CHF2

^46.0

-505.3

-671.5

-433.9

-500.8

-664.8

11.8

6.3 4.2

m

1n

-497.0 -691.0 qq

•CF=C=0 69.0

1 CH3-CHO -161.1 -166.2 0.4 h CH3-CF3

CHF2-CFIF2

-755.4

-883.3

-745.6

-877.8

1.6 17.61 m

-747.3 q CF3-CHO -774.3 CH3-C0* -7.5 -10.2 1.7 a CH2F-CF3

CHF2-CF3

-913.3 -1124.1-895.8 -1104.6

4.2 4.61

1

CF3-CO. -609.9

CF3-CF3 -1357.0 -1342.7 6.3 1 -1344.0 q

32
Table 4. Ci and C2 Fluorinated Hydrocarbon Heats of Formation:

Calculated Values (BAC-MP4), Literature Values, and Uncertainties

a Tsang and Hampson (1986) q Kolesov and Papina ( 1 970)

bKolesov(1978) r Stadelmann and Vogt (1980)

c McMillen and Golden (1982) s Stull etal. (1969) d Keeetal(1987) t Bryant (1962)

e Pritchardetal(1984) uNuttall etal. (1971)

f Rodgers(1978) V Lias etal. (1988) g Stull and Prophet (1971) w Kerr and Timlin (1971)

h Baulchetal(1984) X Tschuikow-Roux and Salomon (1987)

i Batt and Walsh (1982) y Rodgers et al. (1974)

j Batt etal (1974) zChenetal. (1990, 1991)

k Benson (1976) aaGurvich etal (1991)

1 Chen etal. (1975)

m this work, see text H((298) Calculated Heat of Formation at 298 K

n Lacher and Skinnner ( 1 968) Lit Literature Value for H,<298)

oRodgers(1978) Uncert Reported Uncertainty in Literature Value

p Martin and Paraskevopoulos (1983) Ref Literature Reference

33

3. Reaction Kinetics

3.1. Overview

The reaction set or "mechanism" is too large to be described in detail here and,

consequently, only an overview of important classes of reactions will be presented. Utilizing

the species identified as potentially important, a grid of possible reactions was constructed.

Existing chemical rate data involving these fluorinated species was then compiled and evaluated.

Where rate data were available, but only over limited temperature ranges or at different

pressures (for unimolecular or chemically activated steps), RRKM (Robinson and Holbrook,

1972) and QRRK (Dean and Westmoreland, 1987) methods were used to estimate the

temperature dependencies (at 1 atmosphere) of the rates and to predict relative rates where

multiple product channels were possible. Where no rate data were available for potential

reactions, the rate constants were estimated by analogy to other hydrocarbon or substituted

hydrocarbon reactions. The prefactors were adjusted for reaction path degeneracy and the

activation energies were adjusted empirically based on relative heats of reaction or relative bond

energies {i.e., Evans-Polanyi relationships).

Initially, upper limits were used for estimated rate constants. If as a result of simulations

under a variety of conditions (using different agents, flame geometries, etc.), it was observed

that a specific reaction with an upper limit rate constant did not significantly contribute to the

destruction or creation of any of the species in the "mechanism," then that estimate was

continued to be used. However, if a specific reaction contributed to the chemistry and its rate

constant was an upper-limit estimate, then its value was re-examined and possibly refined. For

important contributing reactions where no good analogy was available, where significant

uncertainty existed in the barrier (generally reactions with tight transition states and modest-tolarge barriers), or where multiple, energetically similar product channels were possible, we

calculated the geometries and energies of the transition states (Zachariah et al. , 1995) using the

BAC-MP4 ab initio method. RRKM methods were then applied to obtain the temperature (and

pressure) dependence of the rate constant.

35
A listing of the rate constants in the reaction set or mechanism used in the simulations

is given below in Table 5. In addition, other reactions were also considered but were observed

not to contribute under the conditions tested. Many of the relevant rate constants can be found

in the "NIST Chemical Kinetics Database" (Mallard et al, 1993).

A qualitative discussion of the uncertainties in the rate expressions is provided with each

class of reaction. For rate expressions traceable to experimental measurements, quantitative

evaluation of the uncertainties can be found in the original sources. A schematic of the possible reaction pathways for the fluorinated hydrocarbon mechanism

is given in Figure 1 . This schematic provides no indication of the relative contributions of each

of the possible reaction pathways since this is highly dependent upon conditions. Rather, this

schematic gives an indication of the connectivity between all of the species and how the different

types of reaction {e.g., thermal decompositions, chemically activated decompositions,

abstractions, etc.) provide this connectivity between different types of species. For example,

the linkages between each fluoromethane and the corresponding fluoromethylene is due to

thermal decomposition and are indicated with bold solid arrows. Other thermal decompositions

involving HF elimination {e.g., fluoroethanes - fluoroethylenes, CHF=0 -* CO) are also

represented by bold solid arrows. Thermal decompositions involving H and F atom elimination

are represented by plain dotted arrows. H atom addition/elimination reactions are represented

by reversible plain dotted arrows {e.g., CHj-CHF* **• CH2=CHF + H). Similarly, chemically

activated decompositions, such as fluoromethyls -* ["hot" fluoromethanes] -* fluoromethylenes,

<u"e represented by bold dashed arrows (for reactions involving H atoms) and plain dashed

arrows (for reactions involving O atoms and OH radicals). Abstraction type reactions {e.g.,

fluoromethanes -^ fluoromethyls) are represented by plain solid arrows. A few of the potential

reaction pathways are not shown in Figure 1 for purposes of maintaing clarity in the schematic

representation.

For any given condition {e.g., temperature, concentration) and any given fluorocarbon,

only a subset of the reactions pathways will be relevant. For each reaction pathway that is

possible, each will have a different relative importance. A discussion of each of the different

reaction types for each species type can be found in the following sections.

36
Figure 1. Fluorinated Hydrocarbon Reaction Pathways

( CH0-i-CH3~~

) (cH0*CH2f) (cFO+CHar)

V V V

rCPO+CHP2j ( CHO+CHF2) (^CF2-*-CF20^

CH2-CH2-

CH3-CH2 \ /

CHF=CHF ^L CH2F-CHF2

i CH2P-CF2 I CHF2-CHF/

\ 1 v^

CH2-CHF:-^ " CH2-CF2'^ CHF=CP2 CF2»CP2 /''""-.>••" /^-xjV--

CH3-CHF / //CH2F-CHP\ CH3-CF2 CF3-CH2 I . , vncif v\t \l \/ X

,-'•"

CHF2-CF2 CF3-CF2

CH3-CH3 ''^>^CH3-CH2F '^^CH2F-CH2F \ CH3-CHF2 CH3-CF3 /'' /CHF2-CHF2 CF3-CF3 CHF2-CF3 ^ ^^ ^ ^ Z^

CH4

+CH3 +CH3 +CH2F +CH3 +CHF2 +CH3 +CF3

\

I. ! 1 J 1 7—

\ CH3F ^ / CH2F2 I / CHF3 ] / CF4

CH3 I ^CH2F CHF2 CF3-^

I \ ^^ / '

/ \ ' / -H02

\ TM2 / /CHF / \ ^F2

/ W \ T ^^ ^^ Mf I M^ I ^ I V

,/ V > / ^ \/ ' / *

/y CH—+HF A*-CF V y"/ CF3O

/ \\ +H2O /+H2O / \ I / -F

CH2O \ |\ CHFO +O2 / CF2O

L£S£III2

-^- abstraction by H,0,OH

bimolecular reaction

with specie B

unimoleculeu: decomposition

with F atom elimination

"^- unimolecular decomposition

with H atom elimination

_^^. unimolecular decomposition

with BF elimination

chemically-activated

decomposition, reaction with H atom

-~^. chemically-activated

decomposition, reaction with 0,0H

i-B —^- chemically-activated

decomposition, reaction with specie B

bimolecular reaction

F displacement by H

37

3.2. Hydrocarbon and H/O/F Chemistry

The C/H/O subset is derived from the Miller-Bowman mechanism (Miller and Bowman,

1989) and consists of about 30 species and 140 reactions (see reactions HO-xx, HC-xx in Table

5). Any other hydrocarbon mechanism could be used instead. For example, the GRIMECH set (Bowman et al. , 1995) is a new hydrocarbon mechanism that accurately reproduces flame speeds

for methane mixtures.

The H/O/F subset consists of 3 species (F, HF) and 8 reactions (reactions HF-xx in Table

5) that are relatively well known. This is the chemistry of fluorine atoms with hydrogen- and

oxygen-containing species, such as Hj, OH, and H2O. There are three reactions of this type that were determined to participate in the chemistry under a variety of conditions. These reactions

are the combination of H and F to form HF (and the reverse decomposition) and the hydrogen

atom transfer reactions by F atoms from H2 and HjO.

The HF decomposition reaction has been measured only at temperatures above about 4000

K (Jacobs et al, 1965; Blauer, 1968, Blauer et ah, 1971). Although this reaction in the

decomposition direction is unimportant at typical flame temperatures, the reverse H -I- F = HF

combination must be considered. Extrapolating the recommended value (Baulch et al, 1981)

for decomposition to 1000 K may result in an uncertainty of as much as a factor of ten,

especially when considering non-simple Arrhenius dependence to the rate and different thirdbody efficiencies. However, since many other reactions (F + H2, HjO, RH) contribute to F

atom destruction, the uncertainty in the absolute rate of the forward or reverse reaction is most

likely unimportant.

The hydrogen abstraction reactions of F atoms with Hj and HjO have been measured only

near room temperature (Wurzberg and Houston, 1980; Stevens et al, 1989; Walther and

Wagner, 1983). These values were extended to higher temperatures by fitting the rep>orted

values to extended Arrhenius expressions. For the Hj reaction, an expression with T°^

dependence was chosen consistent with the value recommended by Cohen and Westberg (1983).

For the HjO reaction, an expression with T'^ dependence was chosen by analogy to other

reactions.

39
There are a number of other reactions which were included in the mechanism, but were

never observed to contribute significantly to the chemistry. These reactions include the

combination of F atoms to form Fj and the hydrogen abstractions by F atoms from OH, HO2,

and H2O2. The oxy-fluoro-species F0», HOF, F00», and F2O were also initially considered

in the mechanism. However, given the very low concentration of F atoms at high temperatures

in the hydrocarbon/air flame, these species are present in extremely low concentrations and do

not contribute to the overall chemistry. The rate constants used for reactions involving these

species will be detailed later in another publication.

40
3.3. Ci Fluorinated Hydrocarbon Chemistry

3.3.1. Overview

The Ci subset of the reaction set (approximately 150 reactions) consists of chemistry of

14 species containing one carbon (and hydrogen/fluorine/oxygen) with H, O, OH, HjO, and

other flame species (see reactions MD-xx, MA-xx, NN-xx, PP-xx, CF-xx in Table 5). The

C,/H/F/0 species used in this reaction set are the fluoromethanes (CHjF, CHjFj, CHF3, CF4),

the fluoromethyl radicals (-CHjF, •CHFj, "CFj), the fluoromethylenes (:CHF, rCFj), and the

fluoromethylidyne radical ('CF). The oxidized Cj fluorocarbon species contained in this reaction

set are the perfluoromethoxy radical (CFjO*) and the carbonyl fluorides (CHF=0, CF2=0,

•CF=0). Other oxidized C, fluorocarbon species were initially considered in the development

of the mechanism, but later were excluded, as were the other fluoromethoxy radicals (CHjFO*,

CHFjO*), the fluorohydroxymethyl radicals ('CHFOH, •CF2OH), the perfluoromethylperoxy

radical (CFjOO*), and perfluoromethanol (CF3OH). Although these species (and others) may

be important in atmospheric chemistry, our initial simulations suggest that they are present in

extremely low concentrations at high temperatures in hydrocarbon/air flames and do not

contribute to the overall chemistry.

Both thermally and chemically activated decompositions are considered (e.g., CH2F2 -» :CHF + HF and •CHF2 + H ^ :CHF + HF). Fluoromethane decompositions via abstraction

of H atoms by H, O, and OH radicals are important pathways. Fluoromethane metathesis

reactions with methyl, ethyl, vinyl, and fluoromethyl radicals are also considered. The reaction

set also includes reactions of fluoromethyls with 02,0, and OH to form carbonyl fluorides

{e.g., CF2=0) and other products, and reactions of the fluoromethylenes (e.g., :CF2) with H

to form •CF and O2, O, or OH to form carbonyl fluorides. The carbonyl fluorides (i.e.,

CHF=0, CF2=0, and •CF=0) can be destroyed via unimolecular decomposition, by reactions

with H atoms (both abstractions and addition/eliminations), and through reactions with OH

radicals (abstractions). Destruction of CF2 = through complex formation with HjO and

subsequent decompositions are also considered.

41
3.3.2. Fluoromethanes: Decompositions

The fluoromethanes are primarily destroyed in hydrocarbon flames by H atom abstraction

by H and OH and through unimolecular decomposition. Destruction by H atom abstraction by

O atoms is a minor channel. The biggest uncertainties for the destruction of the fluoromethanes

are the unimolecular decompositions. Although there are good quality experimental data for

these reactions, their strong temperature and pressure dependence results in a level of uncertainty

to these reactions at flame temperatures. Further mechanism refinements should provide better

rate expressions for these reactions.

Both thermally and chemically activated decompositions of the fluoromethanes were

considered {e.g., CHF3 -* rCFj + HF and -CHFj + H -* tCFj + HF). There have been a number of measurements of the unimolecular decomposition of fluoromethanes (with HF

elimination). We employed rate expressions for HF elimination from CH3F and CHF3 that are

fits using an extended Arrhenius form to the experimental data of Schug and Wagner (1973) and

Hidaka et al. (1991), respectively. These experimental data were obtained at different

temperatures and pressures than are relevant to atmospheric flames. The experimental data were

interpolated or extrapolated and fit using temperature dependencies (T**) that were consistent with

the experimental data and our RRKM calculations. For HF elimination from CH2F2, we

employed a rate expression from our BAC-MP4/RRKM calculations, although there is

reasonable experimental data by Politanskii and Shevchuk (1968). For H2 elimination (minor

channel) from CH3F and CHjFj, we used rate expressions from our RRKM calculations using

our BAC-MP4 ab initio barriers (Zachariah et al, 1995). F atom eliminations from the

fluoromethanes are negligible decomposition channels, except for CF4, where it is the only

possible pathway. For this reaction, we used a rate expression from our RRKM calculations

that is based on the room-temperature measurement of the reverse reaction (•CF3 + F) by Plumb

and Ryan (1986).

There have been no measurements (to our knowledge) for reactions involving chemically

activated or "hot" fluoromethanes other than room temperature measurements of the rate

constant for CF3 + H ^ Products {e.g., Ryan and Plumb, 1984; Tsai and McFadden, 1989).

In order to estimate values for these various reactions, as well as for the stabilized fluoromethane

42
channels, we used RRKM methods with experimental (where they existed) or our BAC-MP4 ab

initio barriers (Zachariah et al. , 1995) for insertion of :CHF and iCFj into HF and H2 and the

energetics of the reaction pathways. Although there are no experimental rate measurements at

flame temperatures for chemically activated fluoromethane decompositions and these are primary

pathways for destruction of fluoromethyl radicals, the corresponding uncertainties in the rates

are small, since these are barrierless combinations.

There have been a number of measurements of the unimolecular decomposition of fluoromethanes (with HF elimination): at least two for CH3F (Politanskii and Shevchuk, 1967; Schug

and Wagner, 1973), at least one for CHjFj (Politanskii and Shevchuk, 1968), and several for

CHF3 (Tschuikow-Roux, 1965; Tschuikow-Roux and Marte, 1965; Modica and LaGraff, 1966;

Politanskii and Shevchuk, 1968; Biordi et al, 1978; Schug et al, 1979; Hidaka et al, 1991).

In addition, there have been quite a few measurements of the unimolecular decomposition of

other halomethanes (eliminating HF, HCl, or HBr) such as CHFjCl (Norton, 1957; Edwards and

Small, 1964; Gozzo and Patrick, 1964; Edwards and Small, 1965; Gozzo and Patrick, 1966;

Barnes et al, 1971; Kushina et al, 1972; Schug et al, 1979; Zhitnev et al, 1990; Zhitnev et

al, 1991), CHFjBr (Cox and Simmons, 1971) , CHFCI2 (Kushina et al, 1972), and CHCI3

(Shilov and Sabirova, 1960; Schug et al, 1979). All of these halomethane decomposition

reactions have a small-to-moderate barrier in the reverse direction {i.e., carbene insertion into

HF, HCl, or HBr) of 10-40 kJ/mol. Consequently, all of the halomethane measurements are

important from the point of evaluating the fluoromethane values (both experimental and

calculated) for consistency. Furthermore, the barriers-to-insertion for :CHF and :CF2 in these

reactions can be used as reference reactions for reactions of :CHF and rCFj with many other

important molecules where there is no or little information available {i.e. , the reactions of :CHF

and :CF2 with H2, H2O, CH4, C2H6, fluoromethanes, fluoromethyls, etc.).

43
3.3.3. Fluoromethanes: H Abstractions by H Atoms

In this work, we have used our fits to extended Arrhenius form to the experimental data

of Westenberg and deHaas (1975), Ridley et al. (1972), and Arthur and Bell (1978) for H atom

abstraction from CH3F, CH2F2, and CHF3, respectively. A temperature dependence of T^'' was

used in analogy to the recommended value (Tsang and Hampson, 1986) for H atom abstraction

from methane (CH4). The experimental data were all obtained at modest temperatures (600 K9(X) K) and, consequently, the uncertainties in extrapolation of these data to flame decomposition

temperatures are most likely acceptable. We note that based on our limited evaluation (Burgess

et al, 1994), the trends in the rate expressions for this homologous series appear to be

consistent with the number of H atoms in the molecules and the C-H bond strengths (or heats

of reaction).

There have been a quite a number of measurements for H atom abstractions from

fluoromethanes by H radicals, but only a few for H atom abstraction by O or OH radicals. For

H atom abstraction by H radicals, there have been at least four measurements for CH3F

(Parsamyan et al. , 1967; Hart et al. , 1974; Westenberg and deHaas, 1975; Aders et al. , 1975),

at least two measurements for CH2F2 (Parsamyan and Nalbanddyan, 1968; Ridley et al., 1972),

and quite a few for CHF3 (Ayscough and Polanyi, 1956; Pritchard et al., 1956; Skinner and

Ringrose, 1965; Amphlett and Whittle, 1967; Arthur and Bell, 1968; Fagarash and Moin, 1968,

Kibby and Weston, 1968; Berces et al., 1972; Kondratiev, 1972; Arthur et al., 1975; Arthur

and Bell, 1978; Richter et al., 1994). We should note that many of the measurements for the

CHF3 reactions are actually measurements of the reverse rate or •CF3 + H2 -* CHF3 + H. Two

of the citations (Kondratiev, 1972; Arthur and Bell, 1978) are evaluations of the experimental

data. We have also calculated (Zachariah et al., 1995) the structure and energy of each

transition state for these H atom abstraction reactions from the fluoromethanes using the BACMP4 ab initio method. The calculated energy barriers compare well with the experimental

values.

For the CH3F + H reaction, all of the workers cited above incorrectly identified the

reaction as abstraction of F atoms rather than H atoms. These workers only measured the

disappearance of the reactants and simply assigned the product channel by analogy to the CH3Br

44
+ H reaction, where it is known that the halogen atom (Br) is abstracted. However, the C-F

bond is much stronger than the C-Br bond or even the C-H bond. Consequently, in CH3F, the

H atom, rather than the F atom, is abstracted. Our ab initio calculations (Zachariah et al.

,

1995) also support this argument, where H atom abstractions from the fluoromethanes by H

atoms were calculated to have energy barriers of 49.4, 40.6, 53.6 kJ/mol for the CH3F, CHjFj,

CHF3 series, respectively. These same calculations yield barriers-to-abstraction of F atoms of

131.4, 142.7, 168.6, 171.1 kJ/mol for the CH3F, CH2F2, CHF3, CF4 series, respectively. This

is a significant difference and clearly supports assignment of H atom abstraction as the dominant

channel.

Richter et al. (1994) have recently measured the rate of H atom abstraction from CHF3

by H in H2/O2 premixed flames and report an activation energy of about 73 kJ/mol. This barrier

would appear to be inconsistent with and significantly higher than typical values of 40-50 kJ/mol

for H atom abstraction by H from hydrocarbons {e.g. , CH4, C2H6) and other fluoromethanes (see

references above).

45
3.3.4. Fluoromethanes: H Abstractions by O Atoms and OH Radicals

In this work, for H atom abstraction by O atoms, we fit experimental data for CH3F

(Parsamyan et ai, 1967), CHjFj (Parsamyan and Nalbandyan, 1968), and CHF3 (Jourdain et

ah, 1978) using an extended Arrhenius expression with a temperature dependence (T*-^) by

analogy to methane (Tsang and Hampson, 1986). For H atom abstraction by OH radicals, we

used rate expressions recommended by Cohen and Benson (1987a, 1987b) that have temperature

dependencies based on transition state theory. These recommendations are based on

experimental measurements at relatively low temperatures (about 300 K-500 K). Since these

reactions are primary decomposition pathways for the fluoromethanes, it would be valuable to

have experimental measurements of these rates at higher temperatures (closer to flame

conditions). We note that based on our limited evaluation, the trends in the rate expressions for

these homologous series (both O and OH) appear to be consistent with changes in the number

of H atoms and the C-H bond strengths or heats of reaction.

There have been a quite a number of measurements for H atom abstractions from

fluoromethanes by H radicals, but only a few for H atom abstraction by O or OH radicals.

Parsamyan and coworkers have measured the rate of reaction for CH3F + O (Parsamyan et al. ,

1967) and for CHjFj + O (Parsamyan and Nalbandyan, 1968). Jourdain et al. (1978) and

Miyoshi et al. (1993) have measured the rate of reaction for CHF3 + O. We have not used the

more recent value by Miyoshi et al. (1993), because it appears that these data may be

complicated by the CHF3 -> rCFj + HF decomposition reaction at the highest temperatures.

This should be examined in more detail, since our conclusion was based on a limited evaluation

of the data. Richter et al. (1994) have recently measured the rate of H atom abstraction from

CHF3 by O in H2/O2 premixed flames and report an activation energy of about 13 kJ/mol. This

barrier would appear to be inconsistent with and significantly lower than typical values of 35-40

kJ/mol for H atom abstraction by O from hydrocarbons (e.g., CH4, CjH^) and other

fluoromethanes (see references above).

As indicated above, Cohen and Benson (1987a, 1987b) used transition-state theory

calculations to analyze and predict rate coefficients for reaction of OH radicals in a series of

halogen-substituted methanes and ethanes. Much of their analysis is based on the experimental

46
data of Jeong and Kaufman (1982), but it is also consistent with other measurements for

fluoromethanes (Howard and Evenson, 1976; Clyne and Holt, 1979; Nip et ah, 1979; Talukdar

etal, 1991).

47
3.3.5. Fluoromethanes: H Abstractions by F and F Abstractions by H

There have been a number of measurements of H atom abstraction from methane (CH,)

by F atoms near room temperature (Wagner et al. , 1971; Pollock and Jones, 1973; Williams and

Rowland, 1973; Manning et al, 1975; Smith et al, 1977; Clyneand Hodgson, 1983; Pagsberg

et al, 1988). In our work, we used a fit to extended Arrhenius form to the rate constant of

recommended by Atkinson et al. (1992) using a reasonable temperature dependence (T^-^) in

order to extend the rate expression to flame temperatures. Although there is some uncertainty

here in extrapolating the rate constant to flame temperatures, it is most likely unimportant. This

is because this reaction occurs on almost every collision (that is, the rate cannot change by

much). Furthermore, there are many other reactions {e.g., F + Hj, F + H2O, and F + other

hydrocarbons) that contribute to F atom destruction.

For completeness in the reaction set (although it is unlikely that they will contribute), we

have also included H atom abstractions from the fluoromethanes by F atoms. There have been

a number of measurements for these reactions near room temperature for CH3F (Pollock and

Jones, 1973; Smith et al, 1977; Manocha et al, 1983), for CHjFj (Pollock and Jones, 1973;

Smith et al , 1977; Manocha et al , 1983, Clyne and Hodgson, 1985; Nielsen et al , 1992), and

for CHF3 (Pollock and Jones, 1973; Goldberg and Schneider, 1976; Smith et al, 1977; Clyne

and Hodgson, 1983; Maricq and Szente, 1992). For these reactions, rate expressions were used

where the rate constant prefactor relative to that recommended by Atkinson et al , 1992) for CH4

4- F was adjusted to account for reaction path degeneracy (i.e. , fewer number of H atoms) and

the activation energy was adjusted such that the rate was consistent with the measurements at room temperature. Use of extended Arrhenius form in these cases is not justified, because of

the lack of temperature-dependent experimental measurements.

For F atom abstractions from CH3F, CHjFj, and CHF3 by H radicals, we employed rate

expressions derived from our BAC-MP4 ab initio calculations (Zachariah et al, 1995). The F

atom abstraction pathways are negligible channels and these reactions were included simply for

completeness in development of this reaction set. However, for reaction of H atoms with CF4,

the only possible pathway is F atom abstraction. For this reaction, we have used the

experimentally derived rate expression of Kochubei and Moin (1969, 1971). This reaction is

48
very important pathway for CF4 destruction, competing with the only other possible channel

unimolecular decomposition of CF4 to 'CFj and F.

49
3.3.6. Fluoromethanes: Metathetical Reactions

There have been quite a few measurements of metathetical reactions of

methyl/fluoromethyl radicals with methane/fluoromethanes. These will not be reviewed here.

In our work, we used the recommendations of Kerr and Parsonage (1976), which are consistent

with the majority of the experimental data and empirical relationships for the barriers-toreactions (activation energies). The values recommended by Kerr and Parsonage are largely

based on the pioneering work in this area by Pritchard and coworkers (e.g., Pritchard et ah,

1965), Whittle and coworkers {e.g. , Chamberlain and Whittle, 1972), and Arthur and coworkers

{e.g., Arthur and Bell, 1978). We note that based on our limited evaluation, the trends in the

preexponentials and activation energies in the rate expressions for this homologous series appear

to be consistent with changes in the number of H atoms and the C-H bond strengths or heats of

reaction, respectively.

Although there have been no experimental measurements of metathetical reactions of

vinyl radicals (C2H3) with the fluoromethanes, one can estimate their rates by analogy to the

methyl radical (CH3) reactions. We used rate expressions for these reactions, where the

activation energy was reduced by 10%. This amount determined using the roughly 6 kj/mol

decrease in the heat of reaction and an empirical relationship we determined for a series of

abstraction reactions (Burgess et al., 1994).

Given the abundance of H and OH radicals in hydrocarbon flames and the somewhat

higher barrier for H atom abstraction by methyl/fluoromethyl and vinyl radicals, these are

secondary reaction pathways. However, under pyrolytic conditions they may contribute

(especially the C2H3 reactions which have the lowest barriers) and, consequently, for

completeness should be retained in the reaction set. The experimental measurements for H atom

abstractions by the methyl/fluoromethyl radicals were all made at relatively low temperatures

(about 300 K-600 K). Extrapolation of these measurements to flame decomposition temperatures

may introduce significant uncertainty in the rates, especially since these reactions should have

considerable non-simple Arrhenius temperature dependencies. In further refinement of this

mechanism, these data should be critically evaluated. Experimental measurements at

significantly higher temperatures would also be extremely valuable.

50
3.3.7. Fluoromethyl Radical Destruction

Fluoromethyl radicals are destroyed by three general pathways whose relative importances

are sensitive to conditions. 1) They can combine with H atoms forming chemically activated

fluoromethanes that eliminate HF (creating methylene/fluoromethylenes). 2) They can react with

oxygen-containing species (i.e., Oj, O, OH), resulting in the formation of fluoromethoxy

radicals and carbonyl fluoride species. 3) They can combine with methyl or fluoromethyl

radicals, forming chemically activated fluoroethanes that may be either stabilized or eliminate

HF (creating ethylene/fluoroethylenes). This latter class of reactions is included with the

fluoroethane (C2) chemistry.

The fluoromethyl radicals are primarily formed by H atom abstractions from the fluoromethanes. However, there are several other channels that can contribute to their formation and

are classified as Cj chemistry. For example, the reactions CH2=CHF -I- O ^ 'CHjF -I- HCO

and CHFj-CFj* + H -> ^CHFj + -CHFj contribute to the formation of fluoromethyl radicals.

Similarly, there are a number of other decomposition channels that can be classified as Q or C3

chemistry, such as -CHjF -h C2H4 -* •CH2-CH2-CH2F.

There are four potential reaction product channels following association of fluoromethyl

radicals (e.g., -CHFj) with O2 (by analogy to hydrocarbon and chlorinated hydrocarbon

chemistry). 1) Stabilization of the fluoromethylperoxy radicals (e.g., CHF200* product).

2) Internal abstraction of a hydrogen atom followed by 0-0 bond breakage (e.g. , CF2=0 -I- OH

products). 3) Internal abstraction of a fluorine atom followed by 0-0 bond breakage (e.g.,

CHF=0 -I- OF products). 4) Direct dissociation of the 0-0 bond (e.g., CHF20* + O

products). The first channel (stabilization) should be negligible at flame temperatures, but may

need to be considered at lower temperatures and for ignition delays. The second channel (H

abstraction) should be a secondary pathway at flame temperatures, but clearly should be re- examined at lower temperatures. The third channel (F abstraction) can clearly be disregarded,

because of the strong C-F bond. This contrasts to the analogous reactions that are assumed to

occur in chlorinated hydrocarbon chemistry (e.g., Ho et al., 1992). Consequently, eliminating

the first three potential pathways, we must only explicitly consider the fourth channel (direct O51
O bond dissociation) to form fluoromethoxy radicals and oxygen atoms (e.g., CHF20* + O

products).

There have been a number of rate measurements for the reaction of •CF3 with O2 near room temperature (Vedeneev et ah, 1978; Ryan and Plumb, 1982; Caralp et ah, 1986; Cooper

et al, 1988; Orlando and Smith, 1988), but none (to our knowledge) for reaction of the other

fluoromethyl radicals with Oj. At low temperatures the only possible product pathway is

formation of the fluoromethylperoxy radical. These types of radical species are known to play

a role in atmospheric chemistry. At high temperatures in a flame, these species will be present

in significantly smaller concentrations and there are other possible product pathways for the

fluoromethyl + O2 reactions. For 'CFj + 02^ CFjO* + O, we estimated a rate expression

from our RRKM calculations using the reasonable assumption that there is no barrier in the

reverse direction. For the other two fluoromethyl reactions, we assumed the fluoromethoxy

radical would be present in steady state concentrations and that they would rapidly eliminating

HF after being formed. Based on these assumptions then, we simply used the "CFj rate

expression after adjusting for reaction enthalpies. For lower temperature conditions (than

flames), these assumptions and the relevant reaction pathways and rate expressions should be

re-examined.

For reaction of the perfluoromethyl radical (-CFj) with O atoms (eliminating F), we used

a rate constant corresponding to the room temperature value measured by McFadden and

coworkers (Tsai et ah, 1989). For reaction of the other fluoromethyl radicals with O atoms

(eliminating H), we used rate constants scaled between that for -CHj and •CF^. For reaction

of the fluoromethyl radicals with OH radicals, we used rate constants identical to that for 'CHj.

Fluoromethyl radicals are primarily destroyed in hydrocarbon flames through reactions

with H, OH, and •CRj, radicals. Reactions with O atoms are minor channels. The biggest

uncertainty here is likely the reactions with -CHj radicals (HF elimination versus stabilization),

which are very temperature and pressure dependent. Further refinements of this mechanism

should provide better rate expressions for these reactions, benchmarking them to experimental

data that exists (see brief discussion in Fluoroethane Chemistry section).

Reaction of fluoromethyl radicals with HO2 may be important for correctly describing

ignition delays. There are two possible product channels: 'CHFj + HO2 -* CH2F2 + O2

52
(disproportionation and chain termination) versus 'CHFj + HO2 -*• CHF20* + OH (combination/elimination and chain propagation). We estimated rate expression by analogy to the

corresponding reaction. We assumed the fluoromethoxy radicals immediately eliminate an H

atom, since the C-H bond strengths are only 25-30 kJ/mol. This eliminates the need for

explicitly including these species in the mechanism. For the CFjO* product, a fast subsequent

F atom elimination step (which is explicitly included in the reaction mechanism) does not happen

immediately, since the C-F bond dissociation energy is about 1 10 kj/mol. If these reactions (for

CHjFO* and CHF20«) are shown to be important for ignition delays, then the rates and

branching ratios should be re-examined.

53
3.3.8. Fluoromethylene Destruction

Estimates for the rates of reactions of the fluoromethylenes (:CHF and :C¥^ with many

species are somewhat uncertain, because reactions involving these species are significantly

slower than the analogous reactions for singlet methylene ('tCHj). There also appear to be

conflicting experimental data on their reactivities. This will not be discussed here. The

fluoromethylenes can be destroyed in a number of different ways.

1) They can be destroyed by reaction with H atoms, where we used rate expressions

consistent with the room temperature values measured by McFadden and coworkers (Tsai and

McFadden, 1989; Tsai and McFadden, 1990). For :CF2 + H (which was slightly slower), this

necessitates a small barrier (5 kJ/mol) to be used.

2) They can be destroyed by reaction with O atoms, where we used rate expressions

consistent with the room temperature values measured by McFadden and coworkers (Tsai and

McFadden, 1990). A small barrier (4 kJ/mol) for the tCFj reaction was used.

3) They can be destroyed by reaction with OH radicals, where we used rate expressions

consistent with the value for CFj: determined by Biordi et al. (1978) in their flame measurements. Again a small barrier (14 kJ/mol) was used for iCFj and no barrier for :CHF.

4) They can be destroyed by reaction with O2, where we used the rate expression for

rCFj measured by Keating and Matula (1977). For :CHF, we used an equivalent rate expression

(after adjusting for reaction enthalpy) with a significantly reduced, but still modest (24 kJ/mol)

barrier. Since the :CHF reaction barrier has no experimental basis, if it is identified as a

reaction that significantly contributes to the destruction of :CHF, then this reaction should be

re-examined. An ab initio transition state calculation would be extremely useful in resolving this

uncertainty.

5) They can be destroyed via insertion into H2O (a major flame species). We estimated

barriers to reaction of 25 and 100 kJ/mol for :CHF and rCFj, respectively, from our BAC-MP4

ab initio calculations.

6) The fluoromethylenes can also be destroyed via reaction with hydrocarbons (see brief

discussion in Fluoroethane Chemistry section).

54
The fluoromethylenes (:CHF and rCFj) are largely destroyed in hydrocarbon flames via

reaction with H atoms. Reactions with O and OH radicals are minor channels. There are good

quality experimental data for all of the reactions, which proceed with small barriers. An open

question here is the probable addition of the fluoromethylenes to ethylene. This class of

reactions has been ignored in this mechanism in order to minimize the number of species in the

reaction set, because these reactions would lead to the formation of C3 fluorinated hydrocarbons.

55
3.3.9. Fluoromethylidyne Destruction

The rates of reactions of fluoromethylidyne ('CF) with many species are somewhat

uncertain given they are significantly slower than the analogous reactions for methylidyne (•CH).

There also appear to be conflicting experimental data on its reactivity. This will not be

discussed here. For the reactions of -CF with O2, H, and O, we used rate expressions with

reasonable prefactors and barriers that are consistent with the room temperature rate measurements of McFadden and coworkers (Tsai et al, 1989; Tsai and McFadden, 1990) and

Peeters et al. (1992). We note that to date we have (mis)assigned the products of the reaction

•CF + H ^ C + HF (about 25 kJ/mol exothermic) as CH + F (about 20 kJ/mol endothermic).

This was done to eliminate C, QH, C4H2, and other fuel rich species in order to minimize the

number of species in the reaction set. If a hydrocarbon sub-mechanism is used that includes

these species, the correct product channel should be used. For ^CF + OH -^ CO + HF, we

assumed that there was no barrier to reaction. For "CF + HjO -* Products, we estimated an

activation energy of 70 kJ/mol by analogy to other Radical + HjO reactions. -CF can also be

formed via CH + HF -^ "CF + H2 (roughly 70 kJ/mol exothermic). For reaction of •CF with

other molecules, we assumed upper limits that should be re-examined if those reactions are

observed to contribute to -CF destruction.

In the reaction set, fluoromethylidyne (-CF) is largely destroyed via reaction with O2 and

OH. Reaction with H atoms and H2O are minor channels. Given that there is no experimental

measurements for reaction of 'CF with HjO, limited (and inconsistent) data for reaction with O2,

and both of these reactions are likely to have modest barriers, these reactions provide a

significant uncertainty to this reaction set. Further refinements of this mechanism should address

these issues for :CHF, iCFj, and -CF.

56
3.3.10. Carbonyl Fluoride Chemistry

An important set of species to fluorocarbon species are the carbonyl fluorides (CHF=0,

CF2O, •CF=0). CHF=0 can be destroyed via unimolecular decomposition and H atom

abstraction by H, O, and OH radicals. For the unimolecular decomposition (eliminating HF),

we have fit the experimental data of Saito et al. (1985) using an extended Arrhenius expression

(using the value for Eo (threshold energy) that they recommend based on their analysis). For

the abstractions, we have substituted accepted rate expressions for the analogous CH2=0

reactions. However, there is some significant uncertainty for abstraction by H atoms. The C-H

bond dissociation energy in CHF=0 is about 45-50 kJ/mol stronger than in CH2=0.

Consequently, as an abstraction the barrier should be somewhat higher. On the other hand, H

atom addition followed by H2 elimination could be more facile than the pure abstraction.

CF2=0 can be destroyed via unimolecular decomposition (F atom elimination), by

reactions with H atoms, through reactions with OH radicals, and through reactions, potentially,

with H2O. The unimolecular decomposition is likely a minor channel due to the strong C-F

bond. There are a number of possible reactions with H atoms: 1) direct abstraction of a F atom

abstraction; 2) addition to the oxygen followed by 1,2 elimination of HF; and 3) addition to the

carbon followed by 1,1 elimination of HF. Biordi et al. (1974) have estimated a rate constant

for the net reaction of H with CF2=0 at 1800 K based on their molecular beam sampling measurements in low pressure flames. More recently, Richter et al. (1994) have estimated a rate

expression based upon measurements at several different temperatures. We have also BAC-MP4

ab initio transition state calculations (Zachariah et al. , 1995) followed by RRKM analysis to

provide rate expressions for each of the possible channels. Our calculations are in excellent

agreement with the experimental values and indicate that the addition/ 1,2 elimination channel

dominates (92 kJ/mol barrier), the addition/ 1,1 elimination channel is about a factor of ten

slower (101 kJ/mol barrier), and the direct abstraction channel is negligible (188 kJ/mol barrier).

CF2=0 may also be destroyed via addition of OH to the carbon atom followed by 1,2-

elimination of HF. However, this is likely a minor channel for destruction, since from our BAC-MP4 ab initio transition state calculations (Zachariah et al., 1995), we estimate a barrier

of about 105 kJ/mol. Because of the low reactivity of CF2=0 and the large amounts of HjO

57
in hydrocarbon flames, CFjO + HjO reactions must be considered. We have calculated

(Zachariah et ah , 1995) rate expressions for CF2=0 + HjO complex formation followed by HF

elimination. Modeling results suggest that it is a secondary destruction pathway to the H atom

addition/ 1,2 elimination pathway, but, nevertheless, still needs to be considered.

•CF=0 can be destroyed via unimolecular decomposition and reactions with H, O, OH,

and 'CHj radicals. Modeling results suggest that the unimolecular decomposition and the

reaction with H atoms are the primary decomposition pathways. For reaction with H atoms, we

used a rate constant identical to that for the analogous HCO reaction. For the unimolecular

decomposition, we determined a rate expression based on the reasonable assumption that

combination reaction (reverse direction) is barrierless. There is significant uncertainty in the

heat of formation of •CF=0 and, consequently, there is significant uncertainty in this rate.

Future refinements of this mechanism should address this issue.

58
3.4. Cj Fluorinated Hydrocarbon Chemistry

3.4.1. Overview

The C2 subset of the reaction set (approximately 370 reactions) consists of chemistry of

34 species containing two carbons (and hydrogen/fluorine/oxygen) with H, O, OH, H2O, and

other flame species (see reactions ED-xx, EC-xx, EA-xx, ER-xx, GG-xx, JD-xx, JA-xx, JO-xx,

KK-xx, CF-xx in Table 5). The Cj/H/F/O species used in this reaction set are the 9

fluoroethanes (e.g., CH2F-CF3), the 11 fluoroethyl radicals (e.g., CHjF-CFz*), the 6

fluoroethylenes (e.g., CHF=CF2), the 7 fluorovinyl radicals (e.g., CF2=CH«), the

fluoroacetylenes (C2HF, C2F2), and the fluoroketenes and fluoroketyl radical (CHF=CO,

CF2=C0, •CF=CO). This reaction set will not be described here in detail. Briefly, the

fluoroethane destruction pathways (like fluoromethanes) consist of thermally and chemically

activated decompositions and H atom abstraction reactions. Fluoroethyl radicals can react with

H atoms creating fluoroethylenes via chemically activated fluoroethanes and HF elimination.

Fluoroethyl radicals can also react with oxygen-containing species (O2, O, OH), resulting in the

formation of oxidized fragments (e.g., CF3-CF2* + O - 'CFj + CF2=0). Fluoroethylenes

(produced from thermally and chemically activated fluoroethane decompositions) are predominantly destroyed via reaction with O radicals, resulting in the formation of oxidized fragments

(e.g., CH2=CF2 + O -* •CH=0 + -CHFj). Fluoroethylenes are also destroyed to a lesser

degree through H atom abstraction by radicals such as OH, resulting in formation of fluorovinyl

radicals (e.g., CH2=CF2 + OH ^ CF2=CH» -I- H2O). Fluorovinyl radicals Gike fluoromethyl

and fluoroethyl radicals) are destroyed via reactions with H radicals, as well as with oxygencontaining species.

59
3.4.2. Fluoroethanes: Thermally and Chemically Activated Decompositions

Both thermally and chemically activated decompositions of the fluoroethanes were

considered, as well as stabilization of hot fluoroethanes (e.g., CH3-CF3 -* CH2=CF2 + HF,

•CH3 + 'CFj -* CH2=CF2 + HF, and •CH3 + -CFs -* CH3-CF3). There have been quite a few measurements (mainly in shock tubes) of the unimolecular decomposition of the

fluoroethanes. The kinetics of decomposition of most of the fluoroethanes (HF elimination) has

been measured in a comprehensive series of work by Tschuikow-Roux and coworkers

(Tschuikow-Roux et al., 1970; Tschuikow-Roux and Quiring, 1971; Tschuikow-Roux et ah,

1971; Millward et al, 1971; Millward and Tschuikow-Roux, 1972; Sekhar and TschuikowRoux, 1974). Data for HF elimination from the other fluoroethanes have been obtained by Kerr

and Timlin (1971) and Trotman-Dickenson and coworkers (Day and Trotman-Dickenson, 1969;

Cadman et al. 1970). Fluoroethane decomposition kinetics have also been measured by a few

other workers (Kochubei et al, 1980; Mitin et al, 1988). We selected experimental values

from these and other sources and used them without modification. The validity of employing

these high pressure limit values should be re-examined for those fluoroethanes which have only

a few fluorine substitutions, especially when using the reaction set at low pressures (and high

temperatures).

There have been a number of measurements for reactions of a few of the chemically

activated or "hot" fluoroethanes produced by combination of fluoromethyl radicals by Kim et

al (1973), by Trotman-Dickenson and coworkers (Kirk et al, 1968; Phillips and TrotmanDickenson, 1968; Cadman et al , 1976), and by Pritchard and coworkers (Pritchard et al , 1964;

Bryant and Pritchard, 1967; Bryant et al, 1967; Pritchard and Thommarson, 1967; Perona et

al, 1968; Pritchard and Bryant, 1968; Pritchard and Perona, 1970; Follmer and Pritchard,

1974). Some of this work includes measurements of branching ratios between product channels

(i.e. , HF elimination versus stabilization). There are no measurements (to our knowledge) for

decomposition of hot fluoroethanes following combination of fluoroethyl radicals and H atoms.

We used rate expressions for all of the hot fluoroethanes for the various product channels based

on our RRKM calculations in order to provide a consistent set. Further refinements of this

60
mechanism should include using the existing experimental data as reference values for the

RRKM calculations.

61
3.4.3. Fluoroethanes: Fluoromethyl Disproportionations, Fluoromethylene Insertions

There has been a number of measurements of disproportionations between methyl and

fluoromethyl radicals (Pritchard and Follmer, 1973; Nilsson and Pritchard, 1982; Pritchard et

ai, 1984, 1985, 1987, 1990, 1991, 1992). These studies suggest a branching ratio for

disproportionation versus combination (HF elimination or stabilization) of about 10-20% at 350-

500 K. We employed these data in combination with estimated barriers from our BAC-MP4 ab

initio calculations and determined rate expressions consistent with the available experimental

data. The activation energies or barriers-to-disproportionation are about 3-9 kJ/mol for reactions

involving •CHFj (/.e. ,:CF2 product) and 14-19 kJ/mol for reactions involving 'CHjF (i.e. , :CHF

product). :CHF and iCFj may also insert into C-H bonds in methane and fluoromethanes. We

used rate expressions based on estimated barriers from our BAC-MP4 ab initio calculations of

63 and 130 kJ/mol for insertions of :CHF and iCFj, respectively. These are rather significant

when compared to rCHj, which inserts into C-H bonds with little barrier. Our BAC-MP4 ab

initio calculations suggest these barriers result from ionic repulsion between the electropositive

H atom on the (fluoro) methane and the highly electropositive carbon atom on the

fluoromethylene. For example, the H atom on CH, has a Mulliken charge of -1-0. 17 and the C

atom on rCFj has a Mulliken charge of +0.54. However, there is some experimental evidence

to suggest that the barriers are significantly smaller (DiFelice and Ritter, 1994). This apparent

conflict for these important species should be addressed in future mechanism refinements.

62
3.4.4. Fluoroethanes: Abstractions

There have been quite a few measurements of H atom abstractions from fluoroethanes

by OH radicals. Cohen and coworkers (Cohen and Benson, 1980; Cohen and Westberg, 1987)

have used transition-state theory calculations to analyze and predict rate coefficients for a series

of halogen-substituted methanes and ethanes. Much of their analysis is based on the

experimental data of Clyne and Holt (1979) and Jeong et al. (1984). Other experimental data

included in their analysis was from the measurements by Howard and Evenson (1976),

Handwerk and Zellner (1978), Nip et al. (1979), and Martin and Paraskevopoulos (1983). In

our work to date, we have used values recommended by Cohen and Benson (1987). For the

three asymmetric fluoroethanes (CH3-CH2F, CH3-CHF2, CHjF-CHFj), where there are different

functional H substitutions, we have estimated the branching ratios (based on relative bond

strengths). Recently, there have been a number of precise measurements for these abstraction

reactions for a number of the fluoroethanes by Huie and coworkers (Liu et al. , 1990; Zhang et

al., 1992), by Ravishankara and coworkers (Talukdar et al, 1991; Gierczak et al., 1991), and

by Nielsen (1991). Based on some of the more recent measurements there are newer

recommendations by Cohen and Westberg (1991) for some of these reactions. The biggest

changes are for reactions involving CH3-CHF2 and CHF2-CF3. However, the changes in the rate

expressions are only significant at temperatures well below flame temperatures (because of T''

dependence). These recommendations are based on experimental measurements at relatively low

temperatures (about 300 K-500 K) and these reactions are primary decomposition pathways for

the fluoroethanes at significantly higher temperatures. Consequently, it would be valuable to

have experimental measurements of these rates at near flame temperatures. We note that based

on our limited evaluation, the trends in the rate expressions for this homologous series appear

to be consistent with changes in the number of H atoms and the C-H bond strengths or heats of

reaction.

Although there have been a number of measurements of H atom abstractions by OH

radicals from many of the fluoroethanes, there have been no measurements (to our knowledge)

for H atom abstractions by H and O atoms from any of the fluoroethanes. Consequently, we

utilized an empirical correlation that we determined for other H abstraction reactions (Burgess

63
et al. , 1994). For abstraction by H atoms, we used activation energies that were a factor of 2.5

times that for the analogous abstraction by OH radicals. For abstraction by O atoms, a factor

of 2.7 was employed.

The fluoroethanes are largely destroyed via unimolecular decomposition and abstraction

by OH radicals. Good quality experimental data are available. Future refinements of this

mechanism need only to re-evaluate this work.

64
3.4.5. Fluoroethyl Radical Destruction

Fluoroethyl radicals can be destroyed via reaction with the flame species O2, H, O, OH,

and •CH3. For reaction with O2, O, and OH, we used the accepted rate expressions for the

analogous ethyl radical reactions. Reactions of fluoroethyl radicals with H atoms form hot

fluoroethanes and we used rate expressions from our RRKM calculations as mentioned

previously. Fluoroethyl radicals may combine with •CH3 to form hot fluoropropanes (which

most likely will be stabilized except at the highest temperature). Fluoroethyl radicals may also

disproportionate with -CHj to form CH4 and fluoroethylenes. The first channel (combination)

was simply ignored in order to exclude C3 fluorinated species from the reaction set. The rate

constants for the second channel (disproportionation) were set identical to that accepted for the

reaction 'CjHs + •CH^ -» C2H4 + CH4.

65
3.4.6. Fluoroethylene Chemistry

There are experimental measurements (Simmie and Tschuikow-Roux, 1970; Simmie et

al. , 1970) for the rate of pyrolysis of at least two of the fluoroethylenes (eliminating HF). For

the other fluoroethylenes, we used these rate expressions as reference points and adjusted the

activation energy based on the reaction enthalpy. For thermal decomposition or pyrolysis of

perfluoroethylene (CF2=CF2 -* tCFj + tCFj), we used rate expressions from our RRKM fits

to the experimental data of Schug and Wagner (1978). These data are also consistent with

experimental rate expression of Modica and LaGraff (1966). For the other thermally and

chemically activated fluoroethylene decompositions (e.g., :CHF + :CHF -^ CHF=CHF or CjHF + HF), we used rate expressions from our RRKM calculations (based on the reverse

reaction or combination). Fluoroethylenes are primarily destroyed via reaction with O atoms

(e.g., CH2 = CF2 + O -* •CHF2 + HCO). For these reactions, we used the recommendations

of Cvetanovic (1987). There is some evidence (Gilbert et al. , 1976) to suggest that the assumed

methyl+formyl products (e.g., •CHF2 + HCO) may not be the only product channel (e.g.,

CHF = CHF + O ^ CHF=C = + HF or CHF = CHF + O -* CHF=0 + :CHF). Future

refinements of this mechanism should resolve this issue.

Fluoroethylenes can also be destroyed via reaction with H atoms. This includes H atom

addition followed by stabilization of the fluoroethyl radical produced (e.g., CH2=CF2 + H -»

CHj-CFj* or CHF2-CH2*), as well as H atom addition followed by F atom elimination (e.g.,

CH2=CF2 + H -^ CH2 = CHF + F). There are some experimental data for these reactions,

however, there appears to be some conflict between them. Consequently, in this mechanism,

we simply employed an accepted rate expression for the H atom addition/stabilization for the

analogous ethylene reaction. That is, we used rate expressions for the reactions of

fluoroethylenes with H atoms by analogy to the recommendations of Tsang and Hampson (1986)

for the two pathways C2H4 + H ^ C2H5 and C2H4 + H -* C2H3 + Hj.

For the F atom eliminations, we assumed barrierless addition in the reverse direction.

However, there are some significant uncertainties here. First, it is likely the barrier to addition

will be influenced by the degree of fluorine substitution on the alpha carbon. Secondly, the

efficiency of stabilization of the chemically activated or "hot" fluoroethyl radical will be strongly

66
influenced by the degree of fluorine substitution. Fluoroethylenes may also be destroyed by OH

addition/elimination reactions. This would result in the formation of (fluoro)vinoxy radicals

{e.g., CHO-CHF*). However, in order to minimize the number of species in the reaction set, we have not considered these reactions. Future refinements of this mechanism should investigate

whether or not these types of reactions significantly contribute to the chemistry.

Fluoroethylenes may also be destroyed via reaction with OH radicals. We have only

considered H atom abstraction (and not addition/elimination). For abstraction of H atoms from

the fluoroethylenes by OH radicals, we have used our fit (with an estimated T^ ° dependence)

to the values recommended by Baulch et al. (1992) for C2H4 + OH -» C2H3 + HjO, which is

based on a measurement by Tully (1988). Clearly the C-H bond strength will be significantly

influenced by fluorine substitution. This issue should be addressed in future refinements of this

mechanisms.

We have not considered another possible reaction pathway with OH; that is, OH addition

followed by HF elimination {e.g., CF2=CF2 + OH -* [•CF2-CF2-OH] -* •CF2-CF=0). There

are a number of uncertainties here and, consequently, this reaction pathway was simply not

pursued (because of potential complexities). First, this pathway results in the production of a number of new species in the reaction set (fluorovinoxy radicals, e.g., •CF2-CF = 0), whose

thermochemistry is unknown. Second, the effect of fluorine substitution on the barrier to OH

addition is not known (but probably could be estimated reasonably well). Third, the relative

rates for three competing reactions must be known; that is, 1) stabilization of the

fluorohydroxyethyl radicals {e.g., •CF2-CF2-OH), 2) reversion to reactants, and 3) HF

elimination. Furthermore, if the fluorohydroxyethyl radicals are sufficiently stabilized, then they

are a new set of species that must be considered. Fourth, there are a number of reactions which

must be considered for the fiuorovinoxy radicals. Future refinements of this mechanism should

investigate the potential importance of the OH addition/HF elimination reactions for the

fluoroethylenes. Most likely, only the perfluorocompounds may need to be considered (by

analogy to the sole importance of the perfluoromethoxy radical).

There have been quite a few measurements of the reactions of O atoms with

fluoroethylenes. These will not be reviewed here. In our work, we have used our fits to

67
extended Arrhenius form to the recommendations of Cvetanovic (1987) in order to extrapolate

the low temperature values (300-500 K) to flame temperatures. A temperature dependence of

T* ° was used in analogy to other reactions. The recommended values by Cvetanovic are largely

based on work in this area by Herron and Huie (1973), Jones and Moss (1974), Atkinson and

Pitts (1977), and Gutman and coworkers (Park et al, 1984).

For this class of reactions, it is generally understood that the dominant pathway is where

the products are the fluoromethyl and (fluoro)formyl radical {e.g. CH2=CHF + O -» HCO +

•CHjF) following dissociation of the chemically activated fluoroethylene oxide formed by O

atom attack on the double bond. That is, the O atom first "adds" to the carbon with the least

number of electronegative substituents (in this case F). An H atom on this carbon, then

"migrates" to the other carbon. The numerous other possible channels are generally considered

to be minor pathways: fluorine-substitute analogs of 1) stabilized ethylene oxide, 2) stabilized

acetaldehyde, 3) formaldehyde -f- methylene, 4) acetyl radical 4- H, 5) ketene -h Hj, and 6)

vinyl radical + OH. The latter, abstraction of H atom, is a separate reaction from the first four

(addition/elimination). For completeness in the reaction set, we have included the latter

abstraction reaction and used rate expressions based on analogy to the value estimated by Fontijn

and coworkers (Mahmud et al. , 1987) for the unsubstituted ethylene reaction. It should be noted

that for perfluoroethylene, the only possible channel is CF2=CF2 + O -* CF2=0 -I- rCFj {i.e., no H migration possible). It should also be noted that for CH2=CHF there are two possible

channels ("addition" of the O atom to one side or the other). We have used an estimated

additional 4 kJ/mol for "addition" of the O atom to the fluorinated carbon. This is consistent

with an upper limit measurement at room temperature for this reaction by Gutman and

coworkers (Slagle et al, 1974). Given that this is a primary decomposition pathway for the

fluoroethylenes and that the rate expression that we have chosen to use is based on experimental

measurements at low temperatures (300 K-500 K), it would be very valuable to have

measurements of these reactions and product channels at near flame temperatures.

68
3.4.7. Fluorovinyl Radical Destruction

Westmoreland (1992) has calculated the temperature (and pressure) dependencies of the

rate for the chemically activated reaction C2H3 + 03-^ CH2O + HCO. We have used these

values for the analogous fluorovinyl radical reactions. In our work, we have used the values

recommended by Wamatz (1984) and Tsang and Hampson (1986) for the C2H3 + O -* Products

and C2H3 + OH -* Products reactions, respectively, for the analogous fluorovinyl radical

reactions. The values recommended by Wamatz for the first reaction is based on measurements

by Heinemann et al. (1988).

69
3.4.8. Fluoroethyne, Fluoroketene, and Fluoroketyl Radical Chemistry

For reactions involving the fluoroethynes (C2HF, C2F2), the fluoroketenes (CHF=C=0,

CF2=C=0), and the fluoroketyl radical (•CF=C=0), we have used rate expressions by

analogy to the corresponding hydrocarbons (C2H2, CH2CO, •HCCO). For reaction of H atoms

with the two fluoroacetylenes (C2HF, C2F2), we have used rate expressions derived from the

recommendation of Warnatz (1984) for C2H2 + H -* C2H3, which is based on measurements by

Payne and Stief (1976). For these H atom addition reactions, we employed third-body

stabilization efficiencies and low pressure limits identical to that for acetylene. Future

refinements of this mechanism should provide better estimates for these reactions.

70
3.5. BAC-MP4 Ab Initio Predictions

For a number of reactions considered in the mechanism, there are no or little

experimental rate data. Consequently, we have estimated that data using BAC-MP4 ab initio

calculations of the transition state geometries and energies and RRKM/master equation analysis.

A short description of the BAC-MP4 ab initio calculations is given in the section titled

Thermochemistry: BAC-MP4 Ab Initio Predictions. The transition state for a reaction was

obtained by searching for a geometry with one negative eigenvalue. This corresponds to a

saddle point on the potential energy surface. This is then followed by a steepest-descent reaction

path analysis to ensure that the calculated transition state corresponds to the appropriate reactants

and products. BAC corrections are then assigned in the same manner as with the equilibrium

structures. In order to quantify the uncertainties in the calculated data, we have also performed

calculations on a number of related reactions where there is good quality experimental data.

We have calculated transition states for a number of sets of reactions, including the

following:

1. HF elimination from the fluoromethanes (e.g., CH3F -* :CH2 + HF);

2. Hj elimination from the fluoromethanes (e.g., CH3F -* :CHF -I- H2);

3. H atom abstraction by H from the fluoromethanes (e.g., CH3F + H -» -CHaF + Hj);

4. F atom abstraction by H from the fluoromethanes (e.g., CH3F + H -» •CH3 + HF);

5. reactions of HjO with the fluoromethylenes (e.g. , :CHF + H2O ^ CH2FOH ^ CHjO + HF);

6. reactions of H2O with carbonyl difluoride (e.g., CF2=0 + H2O ^ FCOjH + HF);

7. F atom abstraction by H from carbonyl difluoride (i.e., CF2=0 + H -^ •CF=0 4- HF);

8. H atom addition to carbonyl difluoride (e.g., CF2=0 + H - •CF2OH ^ •CF=0 -I- HF);

9. OH addition to carbonyl difluoride (i.e., CF2=0 + OH ^ -OCFsCOH) -* FC(0)0» -I- HF).

The ab initio geometries and energies of the transition states were then used as inputs to RRKM/master equation analysis in order to calculate rate expressions. The calculated rate

expressions agree well with those derived from experimental measurements (where they exist).

Further discussion of the ab initio transition state calculations can be found elsewhere (Zachariah

etaL, 1995).

71
There is one reaction that is very important to the chemistry of fluorinated hydrocarbon

destruction and where the calculated rate expression can be compared with good quality

experimental measurements. The rate of reaction of H atoms with CF2=0 has been estimated

based on measurements in flames of the rate of disappearance of carbonyl difluoride. Biordi et

al. (1974) estimated a rate constant at 1800 K for this reaction in CFjBr inhibited

methane/oxygen/argon premixed flames. More recently, Richter et al. (1994) have determined

rate coefficients at 1175-1490 K for this reaction in CF3H inhibited hydrogen/oxygen/argon

premixed flames.

The reaction of H atoms with CF2=0 has three distinct pathways, one is a direct

abstraction and the other two are addition/elimination reactions.

First, H atoms can abstract fluorine {i.e., CF2 = + H -» •CF=0 + HF). Our BACMP4 transition state calculations suggest a barrier of about 150 kJ/mol for this reaction and

barriers of about 130-170 kJ/mol for F atom abstraction from the fluoromethanes. These

barriers are consistent with that measured by Kochubei and Moin (1971) for F atom abstraction

by H from CF4. They reported an activation energy of about 190 kJ/mol at 1200 K-1600 K.

This would suggest a barrier of about 160 kJ/mol assuming a T^ dependence to the rate. The second pathway consists of H atom addition to the carbon atom on the carbonyl

difluoride followed by 1,1 elimination of HF from the chemically activated fluoromethoxy

intermediate {i.e. , CF2 = + H -» [CHF20*]' -* •CF=0 -I- HF). The third pathway is also an

addition/elimination reaction, but consists of H atom addition in this case to the oxygen atom

on the carbonyl difluoride followed by 1,2 elimination of HF from the "hot"

hydroxyfluoromethyl intermediate (CF2=0 -I- H ^ [•CF20H]' -* •CF=0 -I- HF).

Our ab initio transition state calculations suggest barriers of about 50 kJ/mol and 65

kJ/mol for addition to the carbon and oxygen sides of the carbonyl difluoride, respectively. It

is slightly more energetically favorable for the H atom to add to the carbon side. However, the

subsequent 1,1 HF elimination step in this case in order to form the •CF=0 product involves

a transition state that is an additional 80 kJ/mol higher (a total of 130 kJ/mol). The overall

energetics of this pathway is significantly less favorable than the 1,2 HF elimination step that

follows H atom addition to the oxygen side. This involves a transition state that is only

72
additional 15 kJ/mol higher (a total of 80 kJ/mol). We have derived rate expressions based on RRKM/master equation calculations using the geometries and energies of the ab initio transition

states. These calculated rate expressions (Zachariah et al. , 1995) agree extremely well with the

experimental rate constants reported by Biordi et al. (1974) and Richter et al. (1994).

Further discussion of the ab initio transition state calculations can be found elsewhere

(Zachariah et al., 1995).

73
I
4. Future Mechanism Refinement

4.1. Overview

The purpose of this section is to highlight uncertainties in the reaction set that may impact

its ability to predict adequately the chemistry of fluorinated hydrocarbon destruction and the

behavior of fluorinated hydrocarbon-inhibited hydrocarbon flames. We will mention known

significant uncertainties, both those that may influence and those that are unlikely to influence

the overall chemistry. For example, the heats of formation of many of the species must be

estimated using empirical methods, such as group additivity. However, much of the chemistry

of the destruction of fluorinated hydrocarbon species in hydrocarbon flames is irreversible. That

is, it is the rates of mainly highly exothermic steps that are important and not thermodynamic

considerations (free energies) or endothermic steps. For example, although there is significant

uncertainty in the heat of formation of :CHF, this should have little impact on the chemistry in

hydrocarbon flames, since :CHF is overwhelmingly destroyed through reactions with radicals

such as H and OH, and not through unimolecular decompositions. In general, the uncertainties

in the reaction set will only be highlighted here.

The reaction set presented here should be considered a framework for development of

a model that accurately describes the decomposition of fluorinated hydrocarbons and their impact on hydrocarbon flame inhibition chemistry. It should not be considered a finished product, since

to date there has been very little comparison of its predictions with experimental measurements.

Future refinement and validation of the mechanism will require input from measurements of

flame speed, flame temperature, concentration profiles, and temperature profiles in fluorinated

hydrocarbon-inhibited flames.

In the reaction set or mechanism presented here, there are a number of species with

uncertain thermochemistry and a number of reactions with uncertain rate expressions. These can

be divided (arbitrarily) into several classes. 1) In most cases, the uncertainties are derived from

the lack of direct or even indirect experimental data for these species and reactions. 2) In some

cases, certain classes of species and reactions were not included in the reaction set, because of

lack of experimental data and uncertainty in the chemistry. 3) In the other cases, experimental

75
data exist, but because of the magnitude of the reaction set, we have not yet verified that the rate

expressions employed in the reaction set are fully consistent with the available experimental data.

For example, the JANAF recommended heat of formation for CHF=0 is simply the

average of the heats of formation of the analogous CH2=0 and CF2=0. Consequently, there

is significant uncertainty introduced from this procedure (bond dissociation energies are strongly

dependent upon alpha- substitution), irrespective of the uncertainties in the heats of formation of

the reference compounds. For example, using the heats of formation of CH4 (-75 kJ/mol) and

CH2F2 (-453 kJ/mol), one would estimate using this procedure a heat of formation for CH3F of

-264 kJ/mol that is 26 kJ/mol lower than the accepted value (-238 kJ/mol).

An analogous example for estimated rate constants is for the hydrogen abstraction

CHF=0 -I- H ^ •CF = -I- H2. In this case, we have simply used an accepted rate expression

for the analogous reaction CH2=0 -I- H -* HCO -I- H2. Given that the C-H bond dissociation

energy in CHF=0 is about 45-55 kJ/mol stronger than in CH2 = 0, it is likely that the barrier

to abstraction for the CHF=0 reaction is somewhat higher than the barrier for the CH2=0

reaction. Although we have estimated that the barrier is about 10 kJ/mol higher (based upon

trends in other halogen-substituted hydrocarbons), we have not (to date) employed this estimate

because of some uncertainties. For example, it is likely that this reaction is not an abstraction,

but rather an addition to the oxygen (e.g., CH2=0 -H H -» 'CHjOH) followed by a 1,2-

elimination of H2, because H atom abstractions by H should have a barrier closer to 40 kJ/mol

(like CH4 -I- H -* •CH3 + H2). Consequently, the effective "barrier" may not be significantly

influenced by the C-H bond strength.

Another important example of uncertainties in rate constants can found for H atom

addition/stabilization to the fluoroethylenes (e.g. , CH2=CF2 + H -* CH3-CF2* and CHF2-CH2*).

We have simply employed an accepted rate expression for the H atom addition/stabilization for

the analogous C2H4 -f H -* •C2H5 reaction. However, there are some significant uncertainties

here. First, it is likely the barrier to addition will be influenced by the degree of fluorine

substitution on the alpha carbon. For example, the barrier to addition for the above reaction

involving CH2=CF2 may be on the order of 8 kJ/mol versus 30 kJ/mol for addition to the

unsubstituted versus substituted carbon, respectively. Secondly, the efficiency with which the

"hot" fluoroethyl radical is stabilized will be strongly influenced by the degree of fluorine

76
substitution (e.g. , CHF2-CF2* versus CHj-CHF*). The relative barriers to addition and relative

stabilization efficiencies could be calculated satisfactorily using ab initio and RRKM methods,

respectively. However, to date we have not done these calculations.

77

4.2. Thermochemistry

There are a number of other species in this reaction set that have significant uncertainties

in their heats of formation, because of lack of direct experimental data.

The heat of formation of CH3F has been estimated based on trends in the heats of

formation of the other fluoromethanes. Although CH3F is unlikely to be a key species in

fluorinated hydrocarbon-inhibited hydrocarbon flames, as the simplest fluorinated hydrocarbon,

its heat of formation is significant as a reference point for heats of formation of other fluorinated

hydrocarbons. An experimentally derived heat of formation for CH3F would be very valuable.

The value recommended in the JANAF tables for the heat of formation of :CHF is based

on the average of the heats of formation of iCHj and rCFj. Other values are based on estimates

of bond dissociation energies or the absence of :CHF as a product in certain reactions

(Staemmler, 1974; Hsu et al. , 1978; Pritchard et al. , 1984). Consequently, there are significant

uncertainties introduced from these procedures (i.e., bond dissociation energies are strongly

dependent upon alpha-substitution). Most reactions that create or destroy :CHF are highly

irreversible reactions (e.g., :CHF -f- H -» CH -I- HF) and, consequently, are unaffected by the

energetics of the reactions. However, disproportionation reactions involving :CHF may proceed

with small barriers and have modest heats of reaction (e.g., •CUj + "CHjF - CH4 -I- :CHF).

For these reactions, the uncertainty in the heat of formation of :CHF may be important.

The literature value for the heat of formation of CF2=0 is reported with a relatively low

uncertainty. However, our BAC-MP4 ab initio calculations predict a value that is about 40

kJ/mol higher than the experimental number. Other ab initio calculations (Montgomery et al.

,

1994; Schnieder and Wallington, 1994) using different approaches also predict a heat of

formation for CF2=0 that is higher (by about 30 kJ/mol) than the experimental value. There

is reason to believe that there may have been side or wall reactions that complicated the

measurement. Furthermore, the heats of formation of all the other oxygenated C, fluorocarbons

(e.g., CFjO*, •CF = 0, etc.) are referenced to CF2=0. Because of these issues, both

uncertainties in the experimental measurements and ab initio calculations warrant further

examination. A new, reliable experimental measurement would be ideal.

79
The JANAF recommended heat of formation for CHF=0 is based on the average of the

heats of formation of the analogous CH2=0 and CF2=0. Although this procedure introduces

significant uncertainty, it may not be important, since there are relatively good experimentally

derived rate expressions for thermal decomposition of formyl fluoride (CHF=0 -* CO + HF).

The literature value for the heat of formation of CF2=0 is reported with a relatively low

uncertainty. However, our BAC-MP4 ab initio calculations predict a value that is about 40

U/mol higher than the experimental number. Other ab initio calculations (Montgomery et al.

,

1994; Schnieder and Wallington, 1994) using different approaches also predict a heat of

formation for CF2=0 that is higher (by about 30 kJ/mol) than the experimental value. There

is reason to believe that there may have been side or wall reactions that complicated the

measurement. Furthermore, the heats of formation of all the other oxygenated Cj fluorocarbons

{e.g., CFjO*, •CF=0, etc.) are referenced to CF2=0. Because of these issues, both

uncertainties in the experimental measurements and ab initio calculations warrant further

examination. A new, reliable experimental measurement would be ideal.

The value recommended in the JANAF tables for the heat of formation of •CF=0 is

based on estimates of the C-F bond dissociation energy in CF2 = 0, In contrast to that for

CHF=0, the heat of formation of •CF=0 is important, since there are no experimental data

for the unimolecular decomposition •CF = -^ CO + F, which is a primary destruction pathway

for •CF=0 (competing with H atom combination followed by HF elimination). Therefore, it would be very useful to obtain a better value (smaller uncertainty) for the heat of formation of

•CF=0 that is based on some type of experimental measurement.

There are no experimentally derived heats of formation for many of the fluoroethanes

(CH3-CH2F, CHF2-CHF2, CH2F-CF3). These have been estimated using bond additivity, group

additivity, or other empirical trends in heats of formation. However, there are significant

uncertainties in using these procedures, because of non-covalent or ionic contributions to the

stability of these species due the high electronegativity of fluorine. Furthermore, the stability

of the fluoroethanes will influence product channels for fluoromethyl combination reactions

(e.g., -CHj + ^CFj -* CH3-CF3 versus •CH3 + •CF3 -» CH2=CF2 + HF).

80
There are experimentally derived heats of formation (i.e. , heat of reaction data) for only

three of the fluoroethyl radicals (CHj-CFz*, CFj-CHj*, CFa-CFj*)- Values for the eight other

fluoroethyl radicals have been estimated using heats of formation of the parent fluoroethanes

(which is some cases are also estimates) and C-H and C-F bond dissociation energies (largely

estimates). The stability of the fluoroethyl radicals can be of importance for destruction of

fluoroethylenes {e.g., CH2=CF2 + H -^^ CHj-CFa* and CHj-CFj* + H -* CH2=CHF + HF).

There are no experimentally derived heats of formation for the fluorovinyl radicals and

these values cannot be estimated empirically. Consequently, in this reaction set we have

employed values that we have calculated using ab initio methods. However, the uncertainties

in these values may not be significant, since these species are largely formed via H atom

abstraction (by OH) and consumed via combination with flame radicals such as H atoms. One

possible uncertainty here is the effect of reaction energy on product channels for combination

of H atoms (e.g. CF2=CH» + H ^ CH2=CF2 [stabilized] versus C2HF + HF [elimination]).

There are no experimentally derived heats of formation for the fluoroketenes

(CHF=C=0, CF2=C=0) and the fluoroketyl radical (•CF=C = 0). In order to include these

potential important species in the mechanism, it was necessary to use thermochemical data from

our ab initio calculations. There are a number of reversible reactions involving these species

that are important under stoichiometric to fuel rich conditions. Consequently, the uncertainties

in the heats of formation of these species may contribute to uncertainties in flame speeds, flame

temperatures, and flame products. These uncertainties should be better quantified in future

mechanism refinements.

81

4.3. Kinetics

A brief discussion of the major uncertainties in the rate expressions used in this

mechanism can be found in each individual section.

83

5. Reaction Set

5.1. Description of Listing

The reaction set listing (Table 5) is divided into sets of similar reaction types (e.g.,

Fluoromethanes: thermally and chemically activated decompositions, Fluoromethanes: atom

abstraction and metathesis, Fluoromethyls: oxidation, etc.). For each reaction, the reaction

number and reaction are given and followed by the Arrhenius parameters. The listing is

essentially a CHEMKIN II reaction input file (Kee et al, 1989).

The reactions are numbered according to the following scheme.

HO-xx Hydrogen/Oxygen Chemistry

HC-xx Hydrocarbon Chemistry

HF-xx Hydrogen/Oxygen/Fluorine Chemistry

MD-xx Fluoromethanes: Thermal and Activated Decompositions

MA-xx Fluoromethanes: Abstractions

NN-xx Fluoromethyl, Fluoromethylene, Fluoromethylidne Chemistry

PP-xx Carbonyl Fluorides and Fluoromethoxy Chemistry

ED-xx Fluoroethanes: Thermal and Activated Decompositions

EC-xx Hot Fluoroethanes & Fluoroethyls: Fluoromethylene Reactions

EA-xx Fluoroethanes: Abstractions by X (H, O, OH)

ER-xx Fluoroethanes: Abstractions by R (CxHy)

GG-xx Fluoroethyl Chemistry

JD-xx Fluoroethylenes: Thermal and Activated Decompositions

JA-xx Fluoroethylenes: Additions and Abstractions

JO-xx Fluoroethylenes & Fluorovinyls: Oxidations

KK-xx Fluoroethynes & Fluoroketenes Chemistry

CF-xx H Atom Abstractions by F

The symbol " = " in the reaction indicates a reversible reaction and the symbol " = >

indicates an irreversible reaction. For reference purposes, the heat of reaction is also given for

a number of the reactions (but not all). In addition, a notation and references are given to

provide traceability on each rate expression. A detailed legend for the notation given for each

reaction is at the end of Table 5. For example in the listing, CH3F + H = CHjF + Hj

(reaction MA-13) has Arrhenius parameters A=2.70E03, b=3.00, E/R=2667., where the rate

expression is k = A*T''*exp(-E/RT). The units are Ai = mol/s, A2=mol/cmVs, A3 = mol/cmVs

(for first, second, and third order reactions, respectively), T=K, E=kJ/mol, and R = 8.314

J/mol/K or 1.987 cal/mol/K). Please note 1 cal = 4.184 J (for conversion from SI units). For

this reaction example, the notation and references "xf", "75WES/DEH", and "nist" indicate that

the rate expression is our fit to the experimental data of Westenberg and deHaas (1975).

85
A number of the unimolecular reactions have rate expressions with third-body efficiencies

and/or low pressure fall-off parameters. For example, H + O2 -* HO2 + M (reaction HO-13)

has explicit third-body efficiencies for M = H2O, CO2, H2, CO, and N2. An example, of a rate

expression with low pressure fall-off parameters is the reaction CH3 + CH3 -» C2H5 -I- M

(reaction HC-16), where "LOW" and "TROE" are low pressure and Troe fall-off parameters.

The reader is referred to Kee et al. (1989) for more details on third-body efficiencies and fall-off

parameters.

For reference purposes at the end of Table 5, the experimental rate expression

(A = 1.80E13, b=0.00, E/R=4803.) and the temperature range (T=600-900K) from this work

(75WES/DEH) are also given. In some cases, where rate expressions were estimated relative

to a reference reaction, the A-factor or activation energy were adjusted. For example in the

listing, the reaction CH3F + C2H3 = CHjF -f- C2H4 (reaction MA-20) has the notations "r CH3"

and "E*0.9". These indicate that an activation energy was used that was 90% of the activation

energy for the analogous abstraction by CH3, a reaction that is slightly more exothermic.

In order to reduce (slightly) the number of species in the reaction set, the isomers

CHF = CHF(E), CHF = CH(£), and CHF=CF(£) were excluded (retaining the Z isomers). The

differences in energies and chemistries are sufficiently small that this is justified. We note that

a number of the fluoroethanes and fluoroethyl radicals have both trans and gauche forms. In

this work, we used thermochemistry for the most stable or trans isomers.

The hydrogen/oxygen and hydrocarbon reaction subsets of the mechanism are derived

from the Miller-Bowman mechanism (Miller and Bowman, 1989) and consists of about 30

species and 140 reactions. Any other hydrocarbon mechanism could be used instead. For

example, the GRIMECH set (Bowman et al, 1995) is a recent hydrocarbon mechanism that

accurately reproduces flame speeds for methane mixtures.

In this work, some modifications to the Miller-Bowman mechanism were made. All

nitrogen-containing species and reactions were removed. A number of the rich species {e.g.,

CjH, C4H2) were eliminated from the mechanism in order to keep the number of species in the

mechanism to a manageable level. A number of species {e.g., CH3OH) were also added to the

mechanism. In addition to these addition and deletions, a number of rate constants for a number

86
of reactions (e.g. , CH3+OH) were adjusted to provide correct falloff and product-channel ratios.

In this section of the reaction set, the notation for the reference is slightly different. For

example, for CH4 + H = CH3 + Hj (reaction HC-1), the notation "73CLA/DOV MBA004"

means that this rate expression was determined by Clark and Dove (1973) and was reaction #4

in table A of the Miller-Bowman mechanism (Miller and Bowman, 1989). Where only the

Miller-Bowman reference is given, either the expression is directly attributable to that work or

the origins/traceability of the expression is not clear.

87

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6. Bibliography

6.1. Overview

A list of references is given below that was compiled and reviewed as part of this work.

The list of references is divided into a number of different sections:

(6.2) General Thermochemistry and Kinetics,

(6.3) Hydrocarbon Chemistry,

(6.4) Fluorine Chemistry,

(6.5) Fluorocarbon Thermochemistry,

(6.6) Oxidized Fluorocarbon Thermochemistry,

(6.7) Fluorocarbon Kinetics (Decompositions),

(6.8) Fluorocarbon Kinetics (Abstractions),

(6.9) Fluorocarbon Kinetics (Oxidations),

(6.10) Oxidized Fluorocarbon Kinetics,

(6.11) Fluorocarbon Kinetics (Other),

(6.12) Flame Inhibition (Halogens), and

(6.13) Flame Inhibition (non-Halogens).

The references for "Hydrocarbon Kinetics" are not meant to be comprehensive, but rather

documentation of those rate constants used in this work. The references for "Flame Inhibition"

are also not meant to be comprehensive, but rather representative of flame inhibition chemistry

as related to this work. In the other reference sections, all relevant references are included, both

those references for which thermochemical or kinetic data were utilized in the reaction set, as

well as other related sources of relevant data.

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NISTTechnical Publications

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