Question

The activation energy of a reaction is 155326 J/ mol. The rate constant of the reaction at and 300K as a function of rate constant at 400K, obtained by the Collision theory is ____

(a) k1 = 1.5 × 10^-7k2

(b) k1 = 1.2 × 10^-6 k2

(c) k1 = 1.5 × 10^-6 k2

(d) k1 = 1.2 × 10^-7 k2

This question was addressed to me at a job interview.

I need to ask this question from Kinetics of Homogeneous Reactions in section Kinetics of Homogeneous Reactions of Chemical Reaction Engineering

Answer 1

Right choice is (a) k1 = 1.5 × 10^-7k2

The explanation: By collision theory, ln(\(\frac{k_2}{k_1}) = -\frac{E}{R} (\frac{1}{T_2} – \frac{1}{T_1}) + 0.5ln(\frac{T_2}{T_1}) \)

ln(\(\frac{k_2}{k_1}) = -\frac{155326}{8.314}(\frac{1}{400} – \frac{1}{300}) + 0.5ln(\frac{400}{300}) \)

Hence, k1 = 1.5 × 10^-7k2.