AIIMS 2019 Chemistry Arrhenius Equation MCQ Question

The calculation of the rate constant $k$ using the Arrhenius equation demonstrates that the exponential factor $e^{-E_a/RT}$ significantly influences the value of $k$. In this case, substituting the activation energy $E_a = 54.7 \times 10^3 \, \text{J/mol}$ and the temperature $T = 800 \, \text{K}$ into the equation yields a rate constant of approximately $10.7 \times 10^6 \, \text{s}^{-1}$, confirming option B as correct. Other options are not relevant since they do not provide valid answers or calculations related to the Arrhenius equation. Understanding this relationship helps clarify how temperature and activation energy affect reaction rates in chemical kinetics.