The heats of combustion of carbon and carbon monoxide are $- 283.5 a n d - 283.5 k J m o l^{- 1}$ 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

$C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J m o l^{- 1}$
$C O + \frac{1}{2} O_{2} \to C O_{2} (g); Δ H = - 283.5 k J m o l^{- 1}$
On subtracting Eq. (ii) from Eq. (i), we get
$C (s) + \frac{1}{2} O_{2} (g) \to C O (g) Δ H = (- 393.5 + 283.5) k J m o l^{- 1} = - 110 k J m o l^{- 1}$ (approx)

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

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The heats of combustion of carbon and carbon monoxide are −283.5 and −283.5 kJ mol−1 respectively. The heat of formation (in kJ) of carbon monoxide per mole is

The correct option is C – 110.5 C(s)+O2(g)→CO2(g);ΔH=−393.5 kJ mol−1 CO+12O2→CO2(g); ΔH=−283.5 kJ mol−1 On subtracting Eq. (ii) from Eq. (i), we get C(s)+12 O2(g)→CO(g)ΔH=(−393.5+283.5)kJ mol−1=−110kJ mol−1 (approx)

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