For which of the following reactions is Delta | vedclass

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

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

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(D) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + \Delta n_g RT$. For $\Delta H 
eq \Delta U$,the condition $\Delta n_g 
eq 0$ must be satisfied,where $\Delta n_g$ is the change in the number of moles of gaseous products and reactants. $(A)$ $\Delta n_g = 2 - (1 + 1) = 0$. $(B)$ $\Delta n_g = 0$ (as all reactants and products are in aqueous or liquid state). $(C)$ $\Delta n_g = 1 - 1 = 0$. $(D)$ $\Delta n_g = 2 - (1 + 3) = -2$. Since $\Delta n_g 
eq 0$ only in option $(D)$,the correct answer is $(D)$.

For which of the following reactions is $\Delta H \neq \Delta U$?

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