Consider A → k_1 B and C → k_2 D are two reactions. If the rate constant ( k_1) of the A → B reaction can be expressed by the following equation…

Consider $\displaystyle \mathrm{A} \xrightarrow{\mathrm{k}_1} \mathrm{~B}$ and $\displaystyle \mathrm{C} \xrightarrow{\mathrm{k}_2} \mathrm{D}$ are two reactions. If the rate constant $\displaystyle \left(\mathrm{k}_1\right)$ of the A $\displaystyle \longrightarrow B$ reaction can be expressed by the following equation $\displaystyle \log _{10} \mathrm{k}=14.34-\frac{1.5 \times 10^4}{\mathrm{~T} / \mathrm{K}}$ and activation energy of C ⟶ D reaction $\displaystyle \left(\mathrm{Ea}_2\right)$ is $\displaystyle \frac{1}{5}$ th of the A ⟶ B reaction $\displaystyle \left(\mathrm{Ea}_1\right)$, then the value of $\displaystyle \left(\mathrm{Ea}_2\right)$ is $\displaystyle \_\_\_\_$ $\displaystyle \mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest Integer)