Chemistry Question from JEE Main 2026 · 22 January, Shift 2

Consider $A \xrightarrow{k_1} B$ and $C \xrightarrow{k_2} D$ are two reactions. If the rate constant ($k_1$) of the $A \rightarrow B$ reaction can be expressed by the following equation

$$\log_{10} k = 14.34 - \frac{1.5 \times 10^{4}}{T/K}$$

and activation energy of $C \rightarrow D$ reaction ($E_{a2}$) is $\dfrac{1}{5}$th of the $A \rightarrow B$ reaction ($E_{a1}$), then the value of ($E_{a2}$) is _____ $\text{kJ mol}^{-1}$ (Nearest Integer).