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(D) According to the Arrhenius equation,$k = A e^{-E_a / RT}$.For two reactions with the same pre-exponential factor $A$,the ratio of rate constants i

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$2.16 	imes 10^4$

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(D) According to the Arrhenius equation,$k = A e^{-E_a / RT}$.For two reactions with the same pre-exponential factor $A$,the ratio of rate constants is $\frac{k_1}{k_2} = \frac{A e^{-E_{a1} / RT}}{A e^{-E_{a2} / RT}} = e^{(E_{a2} - E_{a1}) / RT}$.Given $\Delta E_a = E_{a2} - E_{a1} = 24.9 \, kJ \, mol^{-1} = 24900 \, J \, mol^{-1}$.$T = 300 \, K$ and $R = 8.314 \, J \, K^{-1} \, mol^{-1}$.$\frac{k_1}{k_2} = e^{24900 / (8.314 	imes 300)} = e^{24900 / 2494.2} \approx e^{9.983} \approx 21655 \approx 2.16 	imes 10^4$.

For two reactions,the values of the pre-exponential factor are the same. However,the difference between their activation energy values is $24.9 \, kJ \, mol^{-1}$. The ratio of their rate constants at $300 \, K$ is ....

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