Assertion : For a reaction 2NH_{3(g)} to N_{2 | 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 + \Del

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If the Assertion is correct but Reason is incorrect.

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(C) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta E)$ is given by the equation $\Delta H = \Delta E + \Delta n_g RT$.For the reaction $2NH_{3(g)} 	o N_{2(g)} + 3H_{2(g)}$,the change in the number of gaseous moles is $\Delta n_g = (1 + 3) - 2 = +2$.Since $\Delta n_g$ is positive,$\Delta H = \Delta E + 2RT$,which implies $\Delta H > \Delta E$. Thus,the Assertion is correct.However,the Reason states that enthalpy change is always greater than internal energy change,which is false because if $\Delta n_g$ is negative (e.g.,$N_{2(g)} + 3H_{2(g)} 	o 2NH_{3(g)}$),then $\Delta H < \Delta E$.

Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$
Reason : Enthalpy change is always greater than internal energy change.

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Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$ Reason : Enthalpy change is always greater than internal energy change.