It has been found that for a chemical reaction with rise in temperature by 9K the rate constant gets doubled. Assuming a reaction to be occurring at 300 K, the value of activation energy is found to be________ kJ mol^-1. (in nearest integer)

(Given: In 10 = 2.3, R = 8.3 JK-1 mol^-1, log2 = 0.30)

Kindly go through the solution 

$K=A.e^{-Ea/RT}=\left(6.5\times 10^2\right)e^{-26000K/T}$

$\frac{Ea}{8.314}=26000$

Ea = 216.164kJ/mol $\cong$ $$ 216

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