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

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$\Delta H < \Delta U$

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(D) The relationship between enthalpy change and internal energy change is given by the equation: $\Delta H = \Delta U + \Delta n_g RT$. For the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$,the change in the number of moles of gaseous species is calculated as: $\Delta n_g = \sum n_p - \sum n_r = 2 - (1 + 3) = 2 - 4 = -2$. Substituting $\Delta n_g = -2$ into the equation,we get: $\Delta H = \Delta U - 2RT$. Since $2RT$ is a positive value,it follows that $\Delta H < \Delta U$.

For the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$ at constant temperature and pressure,if $\Delta H$ and $\Delta U$ are the enthalpy and internal energy changes for the reaction,which of the following equations is correct?

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