Arrhenius studied the effect of temperature on the rate of a reaction and postulated that rate constant varies with temperture exponentially as `K=A.e^(-Ea//RT)`. This method is generally used for finding the activation energy of reaction . Keeping temperature constant , effect of catalyst on activation energy has also been studied.
If on addition of catalyst to a reaction at 300 K, rate of reaction increase by `e^(20)` , then difference of activation energy in a absence in absence of catalyst and in presence of catalyst is –
A. 15 kcal/mole
B. 18 kcal/mole
C. 12 kcal/mole
D. 24 kcal/ mole
If on addition of catalyst to a reaction at 300 K, rate of reaction increase by `e^(20)` , then difference of activation energy in a absence in absence of catalyst and in presence of catalyst is –
A. 15 kcal/mole
B. 18 kcal/mole
C. 12 kcal/mole
D. 24 kcal/ mole
Correct Answer – C