Relative rate constants of the gas-phase decomposition reactions of thes-butoxy radical

1985 ◽  
Vol 17 (2) ◽  
pp. 167-176 ◽  
Author(s):  
Roger M. Drew ◽  
J. Alistair Kerr ◽  
Jonathan Olive
Keyword(s):  
Gas Phase ◽  
Rate Constants ◽  
Relative Rate ◽  
Phase Decomposition ◽  
Decomposition Reactions ◽  
Relative Rate Constants ◽  
Butoxy Radical

Secondary deuterium kinetic isotope effects on the thermolysis of 1-pyrazolines

1968 ◽  
Vol 46 (21) ◽  
pp. 3301-3304 ◽  
Author(s):  
Basil H. Al-Sader ◽  
Robert J. Crawford
Keyword(s):  
Gas Phase ◽  
Rate Constants ◽  
Relative Rate ◽  
Isotope Effects ◽  
Kinetic Isotope Effects ◽  
Kinetic Isotope ◽  
Relative Rate Constants

Secondary kinetic isotope effects on four deuterated 1-pyrazolines support the formation of a trimethylene intermediate during gas phase thermolysis. Calculation of cyclization relative rate constants for the trimethylene intermediates reveals that substitution of hydrogen by deuterium has no effect when the terminal methylenes are substituted, but the rate constants are decreased when the central methylene's hydrogens are substituted. Explanations are advanced for all of the observed effects.

Absolute and relative rate constants for the gas-phase reaction of OH radicals with CH3NO2, CD3NO2 and CH3CH2CH3 at 295 K and 1 ATM

1988 ◽  
Vol 146 (3-4) ◽  
pp. 197-203 ◽  
Author(s):  
Ole J. Nielsen ◽  
Howard W. Sidebottom ◽  
Denis J. O'Farrell ◽  
Michael Donlon ◽  
Jack Treacy
Keyword(s):  
Gas Phase ◽  
Rate Constants ◽  
Relative Rate ◽  
Oh Radicals ◽  
Phase Reaction ◽  
Gas Phase Reaction ◽  
Relative Rate Constants

Gas-phase reactions of Cl atoms with hydrochloroethers: relative rate constants and their correlation with substituents' electronegativities

2008 ◽  
Vol 21 (5) ◽  
pp. 393-396 ◽  
Author(s):  
Pablo R. Dalmasso ◽  
Raúl A. Taccone ◽  
Jorge D. Nieto ◽  
Pablo M. Cometto ◽  
Silvia I. Lane
Keyword(s):  
Gas Phase ◽  
Rate Constants ◽  
Relative Rate ◽  
Gas Phase Reactions ◽  
Relative Rate Constants ◽  
Cl Atoms

Kinetics of the successive chlorination of 1,2-dichloroethane in the liquid phase

1969 ◽  
Vol 22 (6) ◽  
pp. 1177 ◽  
Author(s):  
DS Caines ◽  
RB Paton ◽  
DA Williams ◽  
PR Wilkinson
Keyword(s):  
Liquid Phase ◽  
Rate Constants ◽  
Relative Rate ◽  
Stirred Tank ◽  
Continuous Stirred Tank Reactor ◽  
Alternative Pathways ◽  
Tank Reactor ◽  
Relative Rate Constants ◽  
Continuous Stirred Tank ◽  
Kinetics Of

Liquid 1,2-dichloroethane has been chlorinated by dissolved chlorine to a succession of chloroethanes up to the ultimate hexachloroethane. The results of both batch and continuous stirred tank reactor systems have been analysed by computer techniques to give a set of relative rate constants from which one can predict the product composition for a given chlorine uptake, the aim in this work being to optimize the production of tetrachloroethanes. An unusual feature of the kinetics is that 1,1,1,2- and 1,1,2,2-tetrachloroethanes provide alternative pathways between 1,1,2-trichloroethane and pentachloroethane.

RECOMBINATION OF OPPOSITELY CHARGED AQUEOUS CLUSTER IONS USING ELECTROSTATICALLY MERGED ION BEAMS

1996 ◽  
Vol 03 (01) ◽  
pp. 655-660 ◽  
Author(s):  
B. PLASTRIDGE ◽  
K.A. COWEN ◽  
D.A. WOOD ◽  
M.H. COHEN ◽  
J.V. COE
Keyword(s):  
Rate Constants ◽  
Cluster Size ◽  
Collision Energy ◽  
Relative Rate ◽  
Center Of Mass ◽  
Cluster Ions ◽  
Charged Cluster ◽  
Relative Rate Constants ◽  
Oppositely Charged ◽  
Electrostatic Quadrupole

A new method for studying cluster-cluster interactions is introduced which involves merging mass-selected beams of oppositely charged cluster ions with an electrostatic quadrupole deflector. Recombination is monitored by measuring the rate of fast neutral production. Relative rate constants have been measured for the reaction of H 3O+( H 2 O )n+ OH −( H 2 O )m as a function of cluster size (m=n=0–3), which display a pronounced enhancement with clustering. Relative rate constants have also been measured as a function of center-of-mass collision energy for a heavily clustered reaction (n=3, m=3) and a lightly clustered reaction (n=1, m=0) revealing that clustering produces a dramatic change in the reaction mechanism.

Sign in / Sign up

Export Citation Format

Share Document