The rate of a reaction double when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R=8.314 JK−1 mol−1 and log2 = 0.301)

From Arrhenius equation, log⁡k2k1=−Ea2.303R(1T2−1T1)Given, k2k1=2; T2=310 KT1=300 KOn putting values, ⇒log⁡2=−Ea2.303×8.314(1310−1300)⇒ Ea=53603.93 J/mol = 53.6 kJ/mol