The heat of carbon combustion with the ${C O}_{2}$ formation, is $- 393.5 K J / m o l$ , and the heat of $C O$ combustion with the formation of ${C O}_{2}$ , is $- 283 K J / m o l$ . calculate the heat of combustion of carbon there in $C O$ .

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Solution

Given:-
$C + O_{2} ⟶ C O_{2}; Δ H = - 393.5 k J / m o l . . . . . (1)$
$C O + \frac{1}{2} O_{2} ⟶ C O_{2}; Δ H = - 283 k J / m o l$
$C O_{2} ⟶ C O + \frac{1}{2} O_{2}; Δ H = 283 k J / m o l . . . . . (2)$
Adding ${e q}^{n} (1) & (2)$ , we have
$C + O_{2} + C O_{2} ⟶ C O_{2} + C O + \frac{1}{2} O_{2}; Δ H = [(- 393.5) + 283] k J / m o l$
$C + \frac{1}{2} O_{2} ⟶ C O; Δ H = - 110.5 k J / m o l$
Hence, the heat of combustion of carbon there in $C O$ is $- 110.5 k J / m o l$ .

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