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 :

Options

A. 1.2 kcal/mole
B. 1.4 kcal / mole
C. 1.8 kcal / mole
D. 2.4 kcal/ mole

Answer

B