$(Δ H - Δ U)$ for the formation of carbon monoxide ( $C O$ ) from its elements at $298 K$ is ( $R = 8.314 J K^{- 1} m o l^{- 1}$ )

$- 2477.57 J m o l^{- 1}$

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$2477.57 J m o l^{- 1}$

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$- 1238.78 J m o l^{- 1}$

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$1238.78 J m o l^{- 1}$

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Solution

The correct option is D
$1238.78 J m o l^{- 1}$

$C (s) + \frac{1}{2} O_{2} (g) \to C O$

$Δ H = Δ U + Δ n R T$ or $Δ H - Δ U = Δ n R T$ ;

$Δ n = 1 - \frac{1}{2} = \frac{1}{2}; Δ H - Δ U = \frac{1}{2} \times 8.314 \times 298$

= $1238.78 J m o l^{- 1}$

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