The heat of combustion of carbon and carbon monoxide are $- 393.5$ and $- 283.5$ and $k J m o l^{- 1}$ , respectively. The heat of formation (in kJ) of carbon monoxide per mole is:

676.5

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-676.5

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-110.5

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110.5

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Solution

The correct option is C -110.5
Many enthalpy changes are difficult to measure directly under standard conditions.
Hess law states that the total enthalpy change of a reaction is independent of the route taken.
To find :

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

Given:- combustion of carbon
$C + O_{2} \to C O_{2} : △ H_{1} = - 393.5 K J m o l$

combination of carbon monoxide

$C O + \frac{1}{2} O_{2} \to C O_{2} : △ H_{2} = - 283.5 k J m o l^{- 1}$

Formation of carbon monoxide :

$△ H = △ H_{1} - △ H_{2} = - 393.5 - (- 283.5)$

$= 39.3.5 + 283.5 = - 110 k J / m o l$

Therefore, ans is C) $- 110 k J m o l^{- 1}$

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