Chemistry

Problem

A reaction occurs in three rate determining steps having rate constants

K_1, K_2

and

K_3

respectively and Arrhenius factor

A_1, A_2, A_3

respectively. The overall rate constant

K = \frac{K_1 K_2}{K_3}

. If energy of activations for each step is

E_{a_1}, E_{a_2}

and

E_{a_3}

respectively, then overall energy of activation is : a.

E_{a_1} + E_{a_2} + E_{a_3}

\frac{E_{a_1} \times E_{a_2}}{E_{a_3}}

E_{a_1} + E_{a_2} - E_{a_3}

K_3 \left[ \frac{E_{a_1}}{K_2} + \frac{E_{a_2}}{K_1} + \frac{K_3 E_{a_3}}{K_1 K_2} \right]