ISSN:
0538-8066
Keywords:
Chemistry
;
Physical Chemistry
Source:
Wiley InterScience Backfile Collection 1832-2000
Topics:
Chemistry and Pharmacology
Notes:
The pyrolysis kinetics of several ethyl esters with polar substituents at the acyl carbon have been studied in the temperature range of 319.8-400.0°C and pressure range of 50.5-178.0 torr. These eliminations are homogeneous, unimolecular, and follow a first-order rate law. The rate coefficients are given by the Arrhenius equations: for ethyl glycolate, log k1 (s-1) = (12.75 ± 0.30) - (201.4 ± 3.8) kJ/mol/2.303RT; for ethyl cyanoacetate, log k1 (s-1) = (12.19 ± 0.18) - (191.8 ± 2.1) kJ/mol/2.303RT; for ethyl dichloroacetate, log k1 (s-1) = (12.62 ± 0.36) - (193.9 ± 4.3) kJ/mol/2.303RT; for ethyl trichloroacetate, log k1 (s-1) = (12.27 ± 0.09) - (185.1 ± 1.0) kJ/mol/2.303RT. The results of the present work together with those reported recently in the literature give an approximate linear correlation when plotting log k/k0 vs. σ* values (ρ* = 0.315 ± 0.004, r = 0.976, and intercept = 0.032 ± 0.006 at 400°C). This linear relationship indicates that the polar substituents affect the rate of elimination by electronic factors. The greater the electronegative nature of the polar substituent, the faster is the pyrolysis rate. The alkyl substituents yield, within experimental error, similar values in rates which makes difficult an adequate assessment of their real influence.
Additional Material:
1 Ill.
Type of Medium:
Electronic Resource
URL:
http://dx.doi.org/10.1002/kin.550161009
