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(C) The rate of a chemical reaction is inversely related to the activation energy $(E_a)$ of the reaction.According to the Arrhenius equation,$k = Ae^

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The activation energy for $2NO + O_2 \rightarrow 2NO_2$ is lower than that for $2CO + O_2 \rightarrow 2CO_2$.

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(C) The rate of a chemical reaction is inversely related to the activation energy $(E_a)$ of the reaction.According to the Arrhenius equation,$k = Ae^{-E_a/RT}$,a lower activation energy leads to a higher rate constant $(k)$ and thus a faster reaction rate.The reaction $2NO + O_2 \rightarrow 2NO_2$ has a significantly lower activation energy compared to the reaction $2CO + O_2 \rightarrow 2CO_2$ at room temperature.Therefore,the reaction between $NO$ and $O_2$ is fast,while the reaction between $CO$ and $O_2$ is slow.

At room temperature,the reaction between $NO$ and $O_2$ to form $NO_2$ is fast,whereas the reaction between $CO$ and $O_2$ is slow because:

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