For which of the following reactions is Delta | vedclass

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(C) 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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$H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$

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(C) 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 $\Delta H = \Delta U$ to hold true,the term $\Delta n_g$ must be equal to $0$.$\Delta n_g$ is defined as the difference between the number of moles of gaseous products and gaseous reactants.For the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$:$\Delta n_g = (2) - (1 + 1) = 0$.Therefore,for this reaction,$\Delta H = \Delta U$.

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

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