O. Dobis et Sw. Benson, TEMPERATURE COEFFICIENTS OF RATES OF ETHYL RADICAL REACTIONS WITH HBRAND BR IN THE 228-368 K TEMPERATURE-RANGE AT MILLITORR PRESSURES, The journal of physical chemistry. A, Molecules, spectroscopy, kinetics, environment, & general theory, 101(34), 1997, pp. 6030-6042
The rates of the reactions of ethyl radicals with HBr (k(7)) and with
Br atoms (k(8)) have been measured in the temperature range 228-368 K
at millitorr pressures using the very low pressure reactor (VLPR) tech
nique. The Arrhenius function for the H atom abstraction reaction is f
ound to be k(7)=(1.43+/-0.06) x 10(-12) exp-[-(444 +/- 26)/RT] cm(3)/(
molecule s), while the ethyl radical disproportionation with Br atom s
hows no temperature dependence. Its average value over the entire temp
erature range is k(8)=(1.18+/-0.05) x 10(-11) cm(3)/(molecule s). Reac
tion 7 is significantly slower than has been reported in the only othe
r two direct measurements, both finding a negative activation energy f
or k(7) of from -1.0 to -1.1 kcal/mol. The small positive activation e
nergy found in this work for k(7) fits standard models for H atom meta
thesis. Combination with all known kinetic information for ethane brom
ination gives an average reaction enthalpy of Delta H-7(0)=13.0+/-0.2
kcal/mol using both the second-and third-law thermochemical calculatio
ns. It sets the heat of ethyl radical formation to Delta(f)H(0)(C2H5)=
28.40+/-0.25 kcal/mol and the bond dissociation enthalpy, DH0-(C2H5-H)
=100.5+/-0.3 kcal/mol.