For a reaction $A+B ightleftharpoons 2 C+D, \quad$ if the activation energy of the forward and backward…

For a reaction $A+B ightleftharpoons 2 C+D, \quad$ if the activation energy of the forward and backward reactions are $25 \mathrm{~kJ}$ $\mathrm{mol}^{-1}$ and $35 \mathrm{~kJ} \mathrm{~mol}^{-1}$ respectively. The enthalpy change of the reaction is
  1. $10 \mathrm{~kJ} \mathrm{~mol}^{-1}$
  2. $-10 \mathrm{~kJ} \mathrm{~mol}^{-1}$
  3. $60 \mathrm{~kJ} \mathrm{~mol}^{-1}$
  4. $-60 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Solution

$\Delta H=E_{\mathrm{a}(\mathrm{f})}-E_{\mathrm{a}(\mathrm{b})}=(25-35) \mathrm{kJ} \mathrm{mol}^{-1}=-10 \mathrm{~kJ} \mathrm{~mol}^{-1}$

Asked in: JEE-TOPICTESTS-CHEMISTRY

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