1983
DOI: 10.1139/v83-155
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A kinetic study of the reactions of OH radicals with fluoroethanes. Estimates of C—H bond strengths in fluoroalkanes

Abstract: PARASKEVOPOULOS. Can. J. Chem. 61, 861 (1983). A kinetic study of the reactions of OH radicals with a series of fluoroethanes in the gas phase is prcsented. OH radicals were generated by flash photolysis of H 2 0 vapor in the vacuum uv (A > 165 nm) and were monitored in absorption by timc-rcsolved attenuation of resonance radiation at 308.15 nm [OH(A'C' + X'n)]. The following absolute rate constants (in units of 10%m3 mol-' s-I at the 95% confidence limit) were determined at 298 K: kcli2rcli,r = 67.7 + 7.2, kC… Show more

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Cited by 43 publications
(23 citation statements)
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“…In addition, the error bars do not overlap. However, the source of the discrepancy can be easily identified, it is the auxiliary heat of formation data of CF 3 –CH 2 F. The currently accepted value, –906.2 ± 3.2 kJ/mol, differs by −10.4 kJ/mol from that used in ref . After recalculating Δ f H 298 ° (CF 3 –CHF) with this auxiliary value one can arrive at −691.1 ± 5.3 kJ/mol which agrees well with our result.…”
Section: Resultssupporting
confidence: 88%
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“…In addition, the error bars do not overlap. However, the source of the discrepancy can be easily identified, it is the auxiliary heat of formation data of CF 3 –CH 2 F. The currently accepted value, –906.2 ± 3.2 kJ/mol, differs by −10.4 kJ/mol from that used in ref . After recalculating Δ f H 298 ° (CF 3 –CHF) with this auxiliary value one can arrive at −691.1 ± 5.3 kJ/mol which agrees well with our result.…”
Section: Resultssupporting
confidence: 88%
“…CH 3 −CHF. In 1983 Martin and Paraskevopoulos investigated the kinetics of reactions that took place between OH radicals and fluoroethanes, 48 and for Δ f H 298 °(CH 3 −CHF) − 78.2 ± 6.7 kJ/mol was derived. Four years later Tschuikow and Salomon 49 studied the photobromation of C 2 H 5 Cl, and analyzing the kinetics and thermochemical data of related compounds they got a somewhat higher value, −74.1 ± 4.6 kJ/ mol, for Δ f H 298 °(CH 3 −CHF).…”
Section: ■ Results and Discussionmentioning
confidence: 99%
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“…However, the reaction enthalpy for reaction R1 can be estimated from the enthalpies of formation for reactants and products: ∆H f°( OH • ) ) 9.4, 9 ∆H f°( H 2 O) ) -57.8, 9 ∆H f°( CH 3 CH 2 F) ) -62.9, 10 and ∆H f°( CH 3 CHF • ) ) -18.7 ( 1.6 kcal mol -1 . 11 ∆H f°( CH 3 CHF • ) is calculated from ∆H f°( CH 3 CH 2 F) ) -62.9, 10 ∆H f°( H • ) ) 52.1, 12 and the bond dissociation energy D e (CH 3 CHF-H) ) 96.3 kcal mol -1 , which is estimated 11 from an empirical correlation between the rate constants of alkane and haloalkane reactions with OH radical and their C-H bond dissociation energies. The estimated reaction enthalpy (-23.0 kcal mol -1 ) for reaction R1 is in a fair agreement with the calculated value at the G2 level of theory.…”
Section: A Optimized Structures and Vibration Frequenciesmentioning
confidence: 99%
“…No comprehensive unified treatment of all the three reactions was made and comparisons with the experiments were selective. [20][21][22][23][24] On the other hand, the detailed kinetics of HFCs in combustion environments, by contrast, has not been subject to extensive experimental investigation due to lack of proper measurement methods for flame inhibition chemistry. [25][26][27][28] At present, the synchrotron radiation-molecular beam mass spectrometry (SR-MBMS) techniques have been successfully used in studying hydrocarbon combustion and proven to be befitting and powerful tools in flame chemistry.…”
Section: Introductionmentioning
confidence: 99%