Reactions A and B are both elementary bimolecular gas-phase reactions carried out at…
CHEMISTRY · Multi-part · CBSE · Chemistry · Chemical Kinetics · Chemical Kinetics
Problem
Reactions A and B are both elementary bimolecular gas-phase reactions carried out at 298 K in separate vessels of equal volume. Reaction A has an activation energy of 65 kJ·mol⁻¹, whereas reaction B has an activation energy of 150 kJ·mol⁻¹. In both reactions the orientation factor (the fraction of collisions with the proper geometry) is identical.
(a) Identify which reaction is expected to have the larger rate constant at 298 K.
(b) Describe, in terms of the molecular energy distribution and collision theory, why the difference in activation energy leads to the difference in rate you stated in part (a). Your explanation should specifically reference the fraction of collisions possessing sufficient energy to react.