Which of the following statements is correct | vedclass

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(D) The activation energy $(E_a)$ is the minimum energy required for a chemical reaction to occur. According to the Arrhenius equation,$k = A e^{-E_a

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It is nearly independent of temperature,over a wide range of temperature.

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(D) The activation energy $(E_a)$ is the minimum energy required for a chemical reaction to occur. According to the Arrhenius equation,$k = A e^{-E_a / RT}$,where $k$ is the rate constant,$A$ is the frequency factor,$R$ is the gas constant,and $T$ is the temperature. For most reactions,the activation energy $(E_a)$ is considered to be a characteristic property of the reaction path and is nearly independent of temperature over a wide range of temperatures. Therefore,option $D$ is the correct statement.

Which of the following statements is correct for the activation energy of a reaction?

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