Question

If the activation energy for a given compound is found to be 42.0 kJ/mol, with a frequency factor of 8.0 × 1010 s-1, what is the rate constant for this reaction at 298 K? A) 2.9 × 10-4 s-1. B) 7.4 × 10-4 s-1. C) 1.4 × 109 s-1. D) 4.6 × 10 5 s-1. E) 3.5 × 103 s-1.

Answer 1

The problem is related to Arrhenius' equation that correlates rate constant and temperature using activation energy and frequency factor as constants.
k = ko e ^ -E/RT where E is the activation energy and ko as frequency factor. substituting,
k = 8.10x10^10 e ^ -42.0 x 10^3 J/mol-/8.314 *298 K
k = 3474.52 s-1