The bond dissociation energy of the C-H bond in ethanol. A kinetic study of the reaction i2 + ethanol

Ze'ev B. Alfassi; David M. Golden

doi:10.1021/j100667a003

The bond dissociation energy of the C-H bond in ethanol. A kinetic study of the reaction i₂ + ethanol

Ze'ev B. Alfassi, David M. Golden

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Abstract

The reaction of iodine with ethyl alcohol has been studied in a static system in the temperature range 203-252° and in the pressure range 30-750 Torr. The rate-determining step of this reaction has been found to be I + CH₃CH₂OH →¹ CH₃ĊHOH + HI and k₁ is given by the equation log (k₁/M^-1 sec^-1) = (11.5 ± 0.3) - (22.7 ± 0.6)/θ, θ = 2.303RT kcal mol^-1. From the activation energy and the assumption E_-1 = 1 ± 1 kcal mol^-1, it has been calculated that D[CH₃CH(OH)-H] = 93.0 ± 1.0 and ΔH_f°(CH₃ĊHOH,g) = -15.2 ± 1.0 kcal mol^-1. The data of the reaction I₂ + CH₃OH are reinterpreted, increasing log A by 0.3.

Original language	English
Pages (from-to)	3314-3319
Number of pages	6
Journal	Journal of Physical Chemistry
Volume	76
Issue number	23
DOIs	https://doi.org/10.1021/j100667a003
State	Published - 1 Jan 1972
Externally published	Yes

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Engineering (all)
Physical and Theoretical Chemistry

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@article{7704784bfcd34b54ab656ecab45d1890,

title = "The bond dissociation energy of the C-H bond in ethanol. A kinetic study of the reaction i2 + ethanol",

abstract = "The reaction of iodine with ethyl alcohol has been studied in a static system in the temperature range 203-252° and in the pressure range 30-750 Torr. The rate-determining step of this reaction has been found to be I + CH3CH2OH →1 CH3ĊHOH + HI and k1 is given by the equation log (k1/M-1 sec-1) = (11.5 ± 0.3) - (22.7 ± 0.6)/θ, θ = 2.303RT kcal mol-1. From the activation energy and the assumption E-1 = 1 ± 1 kcal mol-1, it has been calculated that D[CH3CH(OH)-H] = 93.0 ± 1.0 and ΔHf°(CH3ĊHOH,g) = -15.2 ± 1.0 kcal mol-1. The data of the reaction I2 + CH3OH are reinterpreted, increasing log A by 0.3.",

author = "Alfassi, {Ze'ev B.} and Golden, {David M.}",

year = "1972",

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doi = "10.1021/j100667a003",

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volume = "76",

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journal = "Journal of Physical Chemistry",

issn = "0022-3654",

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T1 - The bond dissociation energy of the C-H bond in ethanol. A kinetic study of the reaction i2 + ethanol

AU - Alfassi, Ze'ev B.

AU - Golden, David M.

PY - 1972/1/1

Y1 - 1972/1/1

N2 - The reaction of iodine with ethyl alcohol has been studied in a static system in the temperature range 203-252° and in the pressure range 30-750 Torr. The rate-determining step of this reaction has been found to be I + CH3CH2OH →1 CH3ĊHOH + HI and k1 is given by the equation log (k1/M-1 sec-1) = (11.5 ± 0.3) - (22.7 ± 0.6)/θ, θ = 2.303RT kcal mol-1. From the activation energy and the assumption E-1 = 1 ± 1 kcal mol-1, it has been calculated that D[CH3CH(OH)-H] = 93.0 ± 1.0 and ΔHf°(CH3ĊHOH,g) = -15.2 ± 1.0 kcal mol-1. The data of the reaction I2 + CH3OH are reinterpreted, increasing log A by 0.3.

AB - The reaction of iodine with ethyl alcohol has been studied in a static system in the temperature range 203-252° and in the pressure range 30-750 Torr. The rate-determining step of this reaction has been found to be I + CH3CH2OH →1 CH3ĊHOH + HI and k1 is given by the equation log (k1/M-1 sec-1) = (11.5 ± 0.3) - (22.7 ± 0.6)/θ, θ = 2.303RT kcal mol-1. From the activation energy and the assumption E-1 = 1 ± 1 kcal mol-1, it has been calculated that D[CH3CH(OH)-H] = 93.0 ± 1.0 and ΔHf°(CH3ĊHOH,g) = -15.2 ± 1.0 kcal mol-1. The data of the reaction I2 + CH3OH are reinterpreted, increasing log A by 0.3.

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VL - 76

SP - 3314

EP - 3319

JO - Journal of Physical Chemistry

JF - Journal of Physical Chemistry

SN - 0022-3654

IS - 23

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The bond dissociation energy of the C-H bond in ethanol. A kinetic study of the reaction i₂ + ethanol

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