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(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and compl

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$B$ and $C$ Only

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(C) The Arrhenius equation is $k = A e^{-E_a/RT}$.Statement $A$ is incorrect because the Arrhenius equation is applicable to both elementary and complex reactions.Statement $B$ is correct because $A$ (the frequency factor) has the same units as the rate constant $k$.Statement $C$ is correct because a lower activation energy $(E_a)$ results in a larger value of $e^{-E_a/RT}$,leading to a faster reaction rate.Statement $D$ is incorrect because $A$ and $E_a$ are generally considered temperature-independent constants for a given reaction.Statement $E$ is incorrect as $A$ and $E_a$ are independent parameters.Therefore,only statements $B$ and $C$ are correct.

Similar Questions

The activation energy of a reaction at a given temperature is found to be $2.303 \ RT \ J \ mol^{-1}$. The ratio of rate constant to the Arrhenius factor is

From the given data for the reaction $H_2 + I_2 \rightarrow 2HI$,calculate the activation energy $(E_a)$:
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