An exothermic reaction


An exothermic reaction $X \rightarrow Y$ has an activation energy $30 \mathrm{~kJ} \mathrm{~mol}^{-1}$. If energy change $\Delta \mathrm{E}$ during the reaction is $-20 \mathrm{~kJ}$, then the activation energy for the reverse reaction in $\mathbf{k J}$ is



$\Delta \mathrm{H}=\mathrm{E}_{\mathrm{a}, \mathrm{f}}-\mathrm{E}_{\mathrm{a}, \mathrm{b}}$

$-20=30-\mathrm{E}_{\mathrm{a}, \mathrm{b}}$

$\mathrm{E}_{\mathrm{a}, \mathrm{b}}=50 \mathrm{~kJ} / \mathrm{mole}$

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