Question

The activation energy for a reaction is 122137.5 J/ mol. If the rate constant at 330K is 0.5 min^-1, then the value of rate constant (in min^-1) at 360K by Arrhenius law is ____

(a) 20.42

(b) 18.65

(c) 30.12

(d) 12.32

I have been asked this question during an online interview.

My question is based upon Kinetics of Homogeneous Reactions topic in chapter Kinetics of Homogeneous Reactions of Chemical Reaction Engineering

Answer 1

Correct answer is (a) 20.42

For explanation I would say: ln(\(\frac{k_2}{k_1}) = -\frac{E}{R} (\frac{1}{T_2} – \frac{1}{T_1}) \)

ln(\(\frac{k_2}{0.5}) = -\frac{E}{8.314} (\frac{1}{360}- \frac{1}{330}) \)

k2 = 20.42 min^-1.