The energies of activation for forward and re | vedclass

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(D) The enthalpy change of a reaction $(\Delta H_R)$ is defined as the difference between the activation energy of the forward reaction $(E_f)$ and th

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$-20$

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(D) The enthalpy change of a reaction $(\Delta H_R)$ is defined as the difference between the activation energy of the forward reaction $(E_f)$ and the activation energy of the reverse reaction $(E_b)$: $\Delta H_R = E_f - E_b$.
Given $E_f = 180 \ kJ \ mol^{-1}$ and $E_b = 200 \ kJ \ mol^{-1}$,$\Delta H_R = 180 - 200 = -20 \ kJ \ mol^{-1}$.
$A$ catalyst lowers the activation energy of both forward and reverse reactions by the same amount,but it does not change the enthalpy of the reaction $(\Delta H_R)$.
Therefore,the enthalpy change remains $-20 \ kJ \ mol^{-1}$.

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