At constant T and P,which one of the followin | vedclass

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

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$\Delta H < \Delta E$

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(C) 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 the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} 	o CO_{2(g)}$,the change in the number of moles of gaseous species is calculated as: $\Delta n_g = n_{p(g)} - n_{r(g)} = 1 - (1 + 0.5) = 1 - 1.5 = -0.5$. Since $\Delta n_g = -0.5$ (which is negative),the term $\Delta n_g RT$ is negative. Therefore,$\Delta H = \Delta E - 0.5 RT$,which implies that $\Delta H < \Delta E$.

At constant $T$ and $P$,which one of the following statements is correct for the reaction,$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$?

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