The rate of a reaction doubles, when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be R=8.314JK−1mol−1and log 2=0.301)

From Arrhenius equation, log k2k1=−Ea2.303R1T2−1T1Given, k2k1=2,T2=310 K and T1=300 KOn putting values,           ⇒ log 2=−Ea2.303×8.3141310−1300          ⇒ Ea=53598.6J/mol≈53.6kJ/mol