Chemistry Question from JEE Main 2023 · 31 January, Shift 1

$\textbf{A} \rightarrow \textbf{B}$

The rate constants of the above reaction at $200 \, \text{K}$ and $300 \, \text{K}$ are $0.03 \, \text{min}^{-1}$ and $0.05 \, \text{min}^{-1}$ respectively.

The activation energy for the reaction is _____ $\text{J}$ (Nearest integer)

Given: $\ln 10 = 2.3$, $R = 8.3 \, \text{J K}^{-1} \text{mol}^{-1}$, $\log 5 = 0.70$, $\log 3 = 0.48$, $\log 2 = 0.30$