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.

Question

Deon

Physics

28 November, 05:58

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.

+1

Answers (1)

Know the Answer?

Saige Waller · 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