The enthalpies of combustion of Carbon and Carbon monoxide in excess of oxygen at $298 K$ and constant pressure are $- 393.5$ and $- 283.0 k J m o l^{- 1}$ , respectively. Calculate the heat of formation of Carbon monoxide at constant volume.

- 111.7 k J m o l^{- 1}

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+ 111.7 k J m o l^{- 1}

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- 100 k J m o l^{- 1}

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None of these

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Solution

The correct option is A $- 111.7 k J m o l^{- 1}$
Sol. $C (s) + \frac{1}{2} O_{2} (s) ⟶ C O_{(} S) . . . . . .$
$Δ H = ?$
Given: $C (g) + O_{2} (g) ⟶ C O_{2} (g); Δ H_{1} = - 393.5.....$
$(i)$ $C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (s);$ $Δ H_{2} = - 283.....$
$(i i)$ $Δ_{f} H = Δ H_{1} - Δ H_{2}$
$= 393.5 - (- 283)$
$= - 110.5 k J$
$Δ n_{g} = 1 - \frac{1}{2}$
$\frac{1}{2}$ $Δ U^{⊖} = Δ H - Δ n_{g} R T$ $- 11.05 - (- \frac{1}{2}) \times 8.314 \times 10^{- 3} \times 298$
$= - 111.7 k J m o l^{- 1}$

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