Question

If the rate constant of a reaction at 275K is 1 min^-1 and the rate constant at 300K is 2 min^-1, what is the activation energy (in J/ mol) as obtained by Arrhenius law?

(a) 24655

(b) 19019.14

(c) 366543.2

(d) 18989.32

The question was asked during an online interview.

Query is from Kinetics of Homogeneous Reactions topic in chapter Kinetics of Homogeneous Reactions of Chemical Reaction Engineering

Answer 1

The correct answer is (b) 19019.14

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

ln(2) = –\(\frac{E}{8.314} (\frac{1}{360}- \frac{1}{275}) \)  

E = 19019.14 J/ mol.