For the gas phase reaction A_{2(g)} + B_{2(g) | vedclass

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(B) $1$. For an ideal gas reaction, the relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equa

Vedclass · Accepted Answer

$\Delta H = \Delta U$

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(B) $1$. For an ideal gas reaction, the relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U + \Delta n_g RT$.$2$. In the given reaction $A_{2(g)} + B_{2(g)} ightarrow 2AB_{(g)}$, the change in the number of moles of gaseous species $(\Delta n_g)$ is calculated as: $\Delta n_g = n_{	ext{products}} - n_{	ext{reactants}} = 2 - (1 + 1) = 0$.$3$. Substituting $\Delta n_g = 0$ into the equation, we get: $\Delta H = \Delta U + (0)RT = \Delta U$.$4$. Therefore, $\Delta H = \Delta U$ must be correct for this reaction.

For the gas phase reaction $A_{2(g)} + B_{2(g)} \rightarrow 2AB_{(g)}$ taking place at constant pressure and temperature where all gases behave ideally, which of the following must be correct?

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