JEE Main 2026 — 22 January, Evening Shift — Question 66

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 $\left(k_{1}\right)$ of the $A \rightarrow B$ 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 $\mathrm{C} \rightarrow \mathrm{D}$ reaction $\left(\mathrm{Ea}_{2}\right)$ is $\frac{1}{5}$ th of the $\mathrm{A} \rightarrow \mathrm{B}$ reaction $\left(\mathrm{Ea}_{1}\right)$, then the value of $\left(\mathrm{Ea}_{2}\right)$ is $\_\_\_\_$ $\mathrm{kJ} \mathrm{mol}^{-1}$. (Nearest Integer)