For the reaction CO_{(g)} + frac{1}{2}O_{2_{( | vedclass

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(A) The relationship between heat of reaction at constant pressure $(\Delta H)$ and constant volume $(\Delta U)$ is given by: $\Delta H = \Delta U + \

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$-68$

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(A) The relationship between heat of reaction at constant pressure $(\Delta H)$ and constant volume $(\Delta U)$ is given by: $\Delta H = \Delta U + \Delta n_g RT$. Here,$\Delta U = -67.71 \, K \, cal = -67710 \, cal$. Temperature $T = 17 + 273 = 290 \, K$. For the reaction $CO_{(g)} + \frac{1}{2}O_{2_{(g)}} ightarrow CO_{2_{(g)}}$,the change in number of moles of gaseous species is $\Delta n_g = 1 - (1 + 0.5) = -0.5$. Using $R = 2 \, cal \, K^{-1} \, mol^{-1}$: $\Delta H = -67710 + (-0.5 	imes 2 	imes 290) = -67710 - 290 = -68000 \, cal = -68 \, K \, cal$.

For the reaction $CO_{(g)} + \frac{1}{2}O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$ at $17^o C$ and constant volume,the heat of reaction is $-67.71 \, K \, cal$. What is the heat of reaction at constant pressure at $17^o C$ in $K \, cal$?

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