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

1238.78 J {mol}^{- 1}

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- 2477.57 J {mol}^{- 1}

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2477.57 J {mol}^{- 1}

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- 1238.78 J {mol}^{- 1}

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Solution

The correct option is A $1238.78 J {mol}^{- 1}$
$Δ H - Δ U = Δ n_{g} R T$
$C (s) + \frac{1}{2} O_{2} (g) \to C O (g)$
$Δ n_{g} = 1 - \frac{1}{2} = + \frac{1}{2} Δ H - Δ U = \frac{1}{2} \times 8.314 \times 298 = 1238.78 J {mol}^{- 1}$

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Similar questions

(Δ H - Δ U)

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