Consider A k_ 1 ~B and C k_ 2 D are two reactions. If the rate...

Consider $\mathrm{A} \xrightarrow{\mathrm{k}_{1}} \mathrm{~B}$ and $\mathrm{C} \xrightarrow{\mathrm{k}_{2}} \mathrm{D}$ are two reactions. If the rate constant \left(\mathrm{k}_{1}\right)$of the$\mathrm{A} \longrightarrow \mathrm{B}$reaction can be expressed by the following equation$\log _{10} \mathrm{k}=14.34-\frac{1.5 \times 10^{4}}{\mathrm{~T} / \mathrm{K}}$and activation energy of$C \longrightarrow D$reaction \left(E a_{2}\right)$ is $\frac{1}{5}$ th of the $A \longrightarrow B$ reaction \left(E a_{1}\right)$, then the value of \left(E a_{2}\right)$ is $\_\_\_\_ \mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest Integer)