The enthalpies of combustion of carbon and carbon monoxide are $393.5$ and $- 283$ $k J {m o l}^{- 1}$ respectively. The enthalpy of formation of carbon monoxide per mole is:

- 676.9 k J

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676, 5 k J

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110.5 k J

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- 110.5 k J

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Solution

The correct option is B $- 110.5 k J$
$C (s) + O_{2} (g) ⟶ C O_{2} (g); Δ H = - 393.5 k J {m o l}^{- 1}$
$C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g); Δ H = - 283 k J {m o l}^{- 1}$
On subtracting equation (ii) from equation (i) we get
$C (s) + \frac{1}{2} O_{2} (g) ⟶ C O (g); Δ H = - 110.5 k J {m o l}^{- 1}$
The enthalpy of formation of carbon monoxide per mole $= - 110.5 k J {m o l}^{- 1}$

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The enthalpies of combustion of carbon and carbon monoxide are $- 393.5$ and $- 283 k J m o l^{- 1}$ respectively. The enthalpy of formation of carbon monoxide per mole is

The enthalpies of combustion of carbon and carbon monoxide are $- 393.5$ and $- 283$ kJ mol $^{- 1}$ respectively. The enthalpy of formation of carbon monoxide per mole is: