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 $\Delta E$ is given by the equation: $\Delta H = \Delta E + \Delta

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$2NO_{(g)} \longrightarrow N_{2(g)} + O_{2(g)}$

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(D) 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 $\Delta H$ to be approximately equal to $\Delta E$,the term $\Delta n_g$ must be equal to $0$. $\Delta n_g$ is the difference between the number of moles of gaseous products and gaseous reactants. For option $D$: $2NO_{(g)} \longrightarrow N_{2(g)} + O_{2(g)}$,$\Delta n_g = (1 + 1) - 2 = 0$. Since $\Delta n_g = 0$,$\Delta H = \Delta E$.

For which of the following reactions is $\Delta H$ approximately equal to $\Delta E$?

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