Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane

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Standard

Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane. / Nelson, Linda; Shanahan, Imelda; Sidebottom, Howard W.; Treacy, Jack; Nielsen, Ole J.

I: International Journal of Chemical Kinetics, Bind 22, Nr. 6, 01.01.1990, s. 577-590.

Publikation: Bidrag til tidsskrift › Tidsskriftartikel › Forskning › fagfællebedømt

Harvard

Nelson, L, Shanahan, I, Sidebottom, HW, Treacy, J & Nielsen, OJ 1990, 'Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane', International Journal of Chemical Kinetics, bind 22, nr. 6, s. 577-590. https://doi.org/10.1002/kin.550220603

APA

Nelson, L., Shanahan, I., Sidebottom, H. W., Treacy, J., & Nielsen, O. J. (1990). Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane. International Journal of Chemical Kinetics, 22(6), 577-590. https://doi.org/10.1002/kin.550220603

Vancouver

Nelson L, Shanahan I, Sidebottom HW, Treacy J, Nielsen OJ. Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane. International Journal of Chemical Kinetics. 1990 jan. 1;22(6):577-590. https://doi.org/10.1002/kin.550220603

Author

Nelson, Linda ; Shanahan, Imelda ; Sidebottom, Howard W. ; Treacy, Jack ; Nielsen, Ole J. / Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane. I: International Journal of Chemical Kinetics. 1990 ; Bind 22, Nr. 6. s. 577-590.

Bibtex

@article{de374b405b474f04829387084d9b2324,
title = "Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane",
abstract = "The reaction mechanisms for oxidation of CH3CCl2 and CCl3CH2 radicals, formed in the atmospheric degradation of CH3CCl3 have been elucidated. The primary oxidation products from these radicals are CH3CClO and CCl3CHO, respectively. Absolute rate constants for the reaction of hydroxyl radicals with CH3CCl3 have been measured in 1 atm of Argon at 359, 376, and 402 K using pulse radiolysis combined with UV kinetic spectroscopy giving 퓀(OH + CH3CCl3) = (5.4 ± 3) 10−12 exp(−3570 ± 890/RT) cm3 molecule−1 s−1. A value of this rate constant of 1.3 × 10−14 cm3 molecule−1 s−1 at 298 K was calculated using this Arrhenius expression. A relative rate technique was utilized to provide rate data for the OH + CH3 CCl3 reaction as well as the reaction of OH with the primary oxidation products. Values of the relative rate constants at 298 K are: 퓀(OH + CH3CCl3) = (1.09 ± 0.35) × 10−14, 퓀(OH + CH3CClO) = (0.91 ± 0.32) × 10−14, 퓀(OH + CCl3CHO) = (178 ± 31) × 10−14, 퓀(OH + CCl2O) < 0.1 × 10−14; all in units of cm3 molecule−1 s−1. The effect of chlorine substitution on the reactivity of organic compounds towards OH radicals is discussed.",
author = "Linda Nelson and Imelda Shanahan and Sidebottom, {Howard W.} and Jack Treacy and Nielsen, {Ole J.}",
year = "1990",
month = jan,
day = "1",
doi = "10.1002/kin.550220603",
language = "English",
volume = "22",
pages = "577--590",
journal = "International Journal of Chemical Kinetics",
issn = "0538-8066",
publisher = "JohnWiley & Sons, Inc.",
number = "6",

}

RIS

TY - JOUR

T1 - Kinetics and mechanism for the oxidation of 1,1,1‐trichloroethane

AU - Nelson, Linda

AU - Shanahan, Imelda

AU - Sidebottom, Howard W.

AU - Treacy, Jack

AU - Nielsen, Ole J.

PY - 1990/1/1

Y1 - 1990/1/1

N2 - The reaction mechanisms for oxidation of CH3CCl2 and CCl3CH2 radicals, formed in the atmospheric degradation of CH3CCl3 have been elucidated. The primary oxidation products from these radicals are CH3CClO and CCl3CHO, respectively. Absolute rate constants for the reaction of hydroxyl radicals with CH3CCl3 have been measured in 1 atm of Argon at 359, 376, and 402 K using pulse radiolysis combined with UV kinetic spectroscopy giving 퓀(OH + CH3CCl3) = (5.4 ± 3) 10−12 exp(−3570 ± 890/RT) cm3 molecule−1 s−1. A value of this rate constant of 1.3 × 10−14 cm3 molecule−1 s−1 at 298 K was calculated using this Arrhenius expression. A relative rate technique was utilized to provide rate data for the OH + CH3 CCl3 reaction as well as the reaction of OH with the primary oxidation products. Values of the relative rate constants at 298 K are: 퓀(OH + CH3CCl3) = (1.09 ± 0.35) × 10−14, 퓀(OH + CH3CClO) = (0.91 ± 0.32) × 10−14, 퓀(OH + CCl3CHO) = (178 ± 31) × 10−14, 퓀(OH + CCl2O) < 0.1 × 10−14; all in units of cm3 molecule−1 s−1. The effect of chlorine substitution on the reactivity of organic compounds towards OH radicals is discussed.

AB - The reaction mechanisms for oxidation of CH3CCl2 and CCl3CH2 radicals, formed in the atmospheric degradation of CH3CCl3 have been elucidated. The primary oxidation products from these radicals are CH3CClO and CCl3CHO, respectively. Absolute rate constants for the reaction of hydroxyl radicals with CH3CCl3 have been measured in 1 atm of Argon at 359, 376, and 402 K using pulse radiolysis combined with UV kinetic spectroscopy giving 퓀(OH + CH3CCl3) = (5.4 ± 3) 10−12 exp(−3570 ± 890/RT) cm3 molecule−1 s−1. A value of this rate constant of 1.3 × 10−14 cm3 molecule−1 s−1 at 298 K was calculated using this Arrhenius expression. A relative rate technique was utilized to provide rate data for the OH + CH3 CCl3 reaction as well as the reaction of OH with the primary oxidation products. Values of the relative rate constants at 298 K are: 퓀(OH + CH3CCl3) = (1.09 ± 0.35) × 10−14, 퓀(OH + CH3CClO) = (0.91 ± 0.32) × 10−14, 퓀(OH + CCl3CHO) = (178 ± 31) × 10−14, 퓀(OH + CCl2O) < 0.1 × 10−14; all in units of cm3 molecule−1 s−1. The effect of chlorine substitution on the reactivity of organic compounds towards OH radicals is discussed.

UR - http://www.scopus.com/inward/record.url?scp=0025446476&partnerID=8YFLogxK

U2 - 10.1002/kin.550220603

DO - 10.1002/kin.550220603

M3 - Journal article

AN - SCOPUS:0025446476

VL - 22

SP - 577

EP - 590

JO - International Journal of Chemical Kinetics

JF - International Journal of Chemical Kinetics

SN - 0538-8066

IS - 6

ER -

ID: 214272993