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 + \De

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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 $\Delta n_g = 2$ (which is positive),$\Delta H = \Delta E + 2RT$,implying $\Delta H > \Delta E$. Thus,the Assertion is correct.The Reason states that enthalpy change is always greater than internal energy change,which is false because if $\Delta n_g$ is negative or zero,$\Delta H$ can be less than or equal to $\Delta E$.

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.