The activation energy for a reaction at the t | vedclass

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(A) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Here,$k$ is the rate constant,$A$ is the Arrhenius factor (frequency factor),$E_a$ is the

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$10^{-1}$

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(A) The Arrhenius equation is given by $k = A e^{-E_a / RT}$.Here,$k$ is the rate constant,$A$ is the Arrhenius factor (frequency factor),$E_a$ is the activation energy,$R$ is the gas constant,and $T$ is the temperature.We are given $E_a = 2.303 \ RT \ J \ mol^{-1}$.Substituting the value of $E_a$ into the Arrhenius equation:$k = A e^{-(2.303 \ RT) / RT}$$k = A e^{-2.303}$Since $e^{-2.303} = 10^{-1}$ (because $\ln(10) = 2.303$,so $e^{2.303} = 10$,which implies $e^{-2.303} = 1/10 = 10^{-1}$),$k = A 	imes 10^{-1}$.Therefore,the ratio of the rate constant to the Arrhenius factor is $k/A = 10^{-1}$.

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

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