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  • 1
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 16 (1984), S. 423-443 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Methods are described for including the participation of bound electronically excited states in calculations on radical recombination reactions. These methods are illustrated by applying them to the reactions \documentclass{article}\pagestyle{empty}\begin{document}$$ \begin{array}{*{20}c} {{\rm O}\left( {^{\rm 3} P} \right)\,\, + \,{\rm O}\left( {^{\rm 3} P} \right)\,\, + \,\,{\rm M} \to {\rm O}_{{\rm 2}\,} \,\, + \,\,{\rm M}\,} \\ {{\rm O}\left( {^{\rm 3} P} \right)\,\,\, + \,\,{\rm NO}\left( {{\rm X}^{\rm 2} {\rm II}} \right)\, + \,\,{\rm M} \to {\rm NO}_{{\rm 2}\,} \,\, + \,\,{\rm M}} \\ {{\rm OH}\left( {{\rm X}^{\rm 2} {\rm II}} \right)\,\, + \,\,{\rm NO}_{\rm 2} \left( {\tilde X^2 A_1 } \right)\, + \,\,{\rm M} \to {\rm HNO}_{3\,} \,\, + \,\,{\rm M}\,\,\,} \\ \end{array} $$\end{document} For O2, accurate ab initio potentials are used in calculations which show that the electronic degeneracy and long-range part of the potential are likely to be crucial in determining the contribution of a given electronic state to the overall reaction, as long as the state is not so weakly bound that it dissociates thermally before being electronically quenched. Weak collision effects are allowed for using a Monte Carlo technique and an assumed exponential form for the distribution of energies transferred in collisions with a third body. For larger systems it is evident that the role of bound excited states in the low-pressure regime falls rapidly as the size of the system increases. As the high-pressure limit is approached, however, the contribution of excited states is likely to come close to that expected simply on the basis of electronic degeneracy.
    Additional Material: 3 Ill.
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  • 2
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 12 (1980), S. 729-739 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Pulsed laser photolysis of O3 in a large excess of N2 has been used to generate O(3P) atoms in the presence of OCS. By observing chemiluminescence from the small fraction of electronically excited SO2 formed in the reaction of SO with O3, rate constants of (1.7 ± 0.2) × 10-14 and (8.7 ± 1.6) × 10-14 cm3/molecule sec have been determined at 296 ± 4 K for the reactions and In addition, it has been shown that any reaction between SO and OCS has a rate constant 10-14 cm3/molecule sec.
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  • 3
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 15 (1983), S. 63-73 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: It is shown that, by deliberate activation of the reaction vessel, heterogeneous reaction at the wall can be made to dominate chain termination in a complex gas-phase reaction. For a homogeneous process, characterized, as is often the case, by multiple terminations, this has the effect of simplifying the mechanism and allowing explicit solution of the relevant steady-state equations so that the rate constants of some individual steps can be evaluated without assumption as to the values of those of others.The pyrolysis of propane, in the vicinity of 500°C, has been used as an example of this approach. Enhancement of the wall activity leads to the reaction providing, almost exclusively, chain termination. As a result, rate constants for the initiation step can be directly determined. The results of this study provide the Arrhenius equation \documentclass{article}\pagestyle{empty}\begin{document}$$ \log k_1 (s^{ - 1}) = 16.71 \pm 0.54 - 83400 \pm 1950{\rm cal}/{\rm mol}/2.303RT $$\end{document} In combination with current thermochemical values this result gives k-1 = 1013.40 cm3/mol·s which, in turn, implies, via the geometric mean rule, kEt-Et = 1012.9 cm3/mol·s for ethyl-ethyl recombination, in good accord with the most recent determinations and compatible with the newly proposed value of the enthalpy of formation of ethyl.The first-order wall constant k8 has been evaluated as k8〈104.2 s-1. This appears to be the first occasion on which a wall constant has been evaluated from data for a high-temperature complex gas reaction.
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  • 4
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 15 (1983), S. 167-185 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The bond dissociation energies of tetramethyl germane, triethyl stibine, tetraethyl lead, and triethylphosphine were determined using the technique of very-low-pressure pyrolysis. Arguments are presented for log A ≥ 17.0. The respective dissociation energies ΔH298 are 83, 57, 54, and 68 (±2) kcal/mol. A consistent set of methyl bond energies to main group metals is determined from these and previous results, and is examined for trends. Bond energies for various radicals to tin are also derived.
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  • 5
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 16 (1984), S. 41-55 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The absolute rate constants for the reactions of OH + HO2NO2 (1) and OH + HNO3 (2) have been measured with the technique of flash photolysis resonance fluorescence over the temperature ranges of 240-330 K at 760 torr He for reaction (1) and of 240-370 K at 50 and 760 torr He for reaction (2). Reactant concentrations were monitored continuously by ultraviolet and infrared spectrophotometry. The data can be fitted to the following Arrhenius expressions: \documentclass{article}\pagestyle{empty}\begin{document}$$ k_1 = \left( {5.9 \pm 0.4} \right) \times 10^{ - 13} \exp \left[ {{{\left( {650 \pm 30} \right)} \mathord{\left/ {\vphantom {{\left( {650 \pm 30} \right)} T}} \right. \kern-\nulldelimiterspace} T}} \right]{{{\rm cm}^{\rm 3} } \mathord{\left/ {\vphantom {{{\rm cm}^{\rm 3} } {{\rm molecule} \cdot {\rm s}}}} \right. \kern-\nulldelimiterspace} {{\rm molecule} \cdot {\rm s}}} $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ {\rm CH}_{\rm 3} {\rm SiD}_{\rm 3} \mathop {\longrightarrow} \limits^3 {\rm CH}_{\rm 2} \raise1pt\hbox{=\kern-3.45 pt=} {\rm SiD}_{\rm 2} \left( {0.14} \right) $$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$ k_2 = \left( {8.3 \pm 0.9} \right) \times 10^{ - 15} \exp \left[ {{{\left( {850 \pm 40} \right)} \mathord{\left/ {\vphantom {{\left( {850 \pm 40} \right)} T}} \right. \kern-\nulldelimiterspace} T}} \right]{{{\rm cm}^{\rm 3} } \mathord{\left/ {\vphantom {{{\rm cm}^{\rm 3} } {{\rm molecule} \cdot {\rm s}}}} \right. \kern-\nulldelimiterspace} {{\rm molecule} \cdot {\rm s}}} $$\end{document} These results are in very good agreement with recent studies of reaction (2), and also of reaction (1) at 295 K.
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  • 6
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 16 (1984), S. 213-220 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: Energetic H atoms produced by photolysis of gaseous HI react with CD3Br by D abstraction (1) and Br abstraction (2) and possibly also by the substitution reactions (4) and (5). Yields of HD and CD3H have been determined for several defined initial translational energies of H*. The phenomenological threshold energy of reaction (1) is 53 ± 5 kJ/mol. Over the range of initial energies of 76-109 kJ mol the integral probability of reaction (1) increases substantially, but the sum of the integral probabilities of reactions (2) and (5) shows little change. The ratio of the sum of the integral yields of reactions (2) and (5) to the integral yield of reaction (1), when normalized to equal numbers of Br and D atoms, is 69 ± 33 at an initial energy of 76 kJ/mol and 31 ± 6 at 109 kJ/mol.
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  • 7
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 14 (1982), S. 679-697 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: A nozzle-beam-skimmer sampling system is used to measure species concentration profiles for a lean one-dimensional premixed CO—O2—Ar flame, into which small amounts of sulfur dioxide are introduced. The net formation rate for sulfur trioxide is obtained from the flux fraction profile for this species. The kinetic scheme is then utilized, along with the measured temperature profiles, to evaluate the rate coefficients k1 and k2 over the temperature range of 1435-1850 K. The most satisfactory agreement between the measured net formation rate for SO3 and that calculated on the basis of reactions (1) and (2) is obtained with the rate coefficients \documentclass{article}\pagestyle{empty}\begin{document}$$k_1 = 4.4 \times 10^{14} \exp [3163/T]{\rm cm}^{\rm 6} {\rm /mol}^{\rm 2} \cdot {\rm s}$$\end{document} \documentclass{article}\pagestyle{empty}\begin{document}$$k_2 = 1.32 \times 10^{12} \exp [- 3070/T]{\rm cm}^{\rm 3} {\rm /mol} \cdot {\rm s}$$\end{document} Reactions (1) and (2) are found to be nearly balanced in a substantial region of the flame. Here the data are more sensitive to the difference in activation energies, as opposed to a particular value for either. Implications of this observation on the uncertainty of the deduced temperature dependence for each reaction are discussed, as are some of the procedures used in the data analysis.
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  • 8
    Electronic Resource
    Electronic Resource
    New York, NY : Wiley-Blackwell
    International Journal of Chemical Kinetics 16 (1984), S. 1151-1160 
    ISSN: 0538-8066
    Keywords: Chemistry ; Physical Chemistry
    Source: Wiley InterScience Backfile Collection 1832-2000
    Topics: Chemistry and Pharmacology
    Notes: The absolute rate constant for the OH + HCl reaction has been measured from 240 to 295 K utilizing the techniques of laser/flash photolysis-resonance fluorescence. The HCl concentrations were monitored continuously by ultraviloet and infrared spectrophotometry. The results can be fit to the following Arrhenius expression: \documentclass{article}\pagestyle{empty}\begin{document}$$k_1 = (4.6{\rm } \pm {\rm }0.3){\rm } \times {\rm }10^{ - 12} \exp [- (500{\rm } \pm {\rm }60)/T{\rm cm}^3 /{\rm molecule} \cdot {\rm s}$$\end{document} The rate constant values obtained in this study are 20-30% larger than those recommended previously for modeling of stratospheric chemistry.
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