Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as `k=Ae^(E_(a)//RT)` . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied.
If the rate of reaction doubles for `10^(@)C` rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately:
a) 40 Kcal `mol^(-1)`
b) 12 Kcal `mol^(-1)`
c) 60 Kcal `mol^(-1)`
d) 70 Kcal `mol^(-1)`

Options

A. 40 Kcal `mol^(-1)`
B. 12 Kcal `mol^(-1)`
C. 60 Kcal `mol^(-1)`
D. 70 Kcal `mol^(-1)`

Answer

B