A mixture of 2 mol of CO_{(g)} and 1 mol of | vedclass

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(C) The balanced chemical equation for the combustion of carbon monoxide is: $CO_{(g)} + \frac{1}{2} O_{2(g)} \longrightarrow CO_{2(g)}$ The change in

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$\Delta H < \Delta U$

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(C) The balanced chemical equation for the combustion of carbon monoxide is: $CO_{(g)} + \frac{1}{2} O_{2(g)} \longrightarrow CO_{2(g)}$ The change in the number of gaseous moles is given by: $\Delta n_g = \sum n_{g(products)} - \sum n_{g(reactants)}$ $\Delta n_g = 1 - (1 + 0.5) = 1 - 1.5 = -0.5$ We know the relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is: $\Delta H = \Delta U + \Delta n_g RT$ Since $\Delta n_g = -0.5$ (which is negative),the term $\Delta n_g RT$ will be negative. Therefore,$\Delta H = \Delta U - 0.5 RT$. This implies that $\Delta H < \Delta U$.

$A$ mixture of $2 \ mol$ of $CO_{(g)}$ and $1 \ mol$ of $O_{2(g)}$ is ignited to convert $CO$ to $CO_2$. Which of the following relations is correct?

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