For which one of the following reactions,Delt | vedclass

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(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \De

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$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$

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(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation: $\Delta H = \Delta E + \Delta n_g RT$,where $\Delta n_g$ is the change in the number of moles of gaseous species.$\Delta H$ is not equal to $\Delta E$ when $\Delta n_g 
eq 0$.For option $A$: $\Delta n_g = 2 - (1 + 1) = 0$.For option $B$: $\Delta n_g = 1 - 1 = 0$.For option $C$: $\Delta n_g = 2 - (1 + 3) = -2 
eq 0$.For option $D$: $\Delta n_g = 0$ (as there are no gaseous species).Therefore,for the reaction in option $C$,$\Delta H 
eq \Delta E$.

For which one of the following reactions,$\Delta H$ is not equal to $\Delta E$?

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