The heats of combustion of carbon and carbon monoxide are $- 393.5$ and $- 283.5$ kJ mol $^{- 1}$ , 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

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+ 110.5

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Solution

The correct option is B $- 110$
The combustion reactions are as shown.
$C + O_{2} \to C O_{2} Δ H_{1} = - 393.5 k J / m o l$
$C O + 0.5 O_{2} \to C O_{2} Δ H_{2} = - 283.5 k J / m o l$
$C + 0.5 O_{2} \to C O Δ H_{3}$
$Δ H_{3} = Δ H_{1} - Δ H_{2}$
$Δ H_{3} = - 393.5 k J / m o l - (- 283.5 k J / m o l) = - 110 k J / m o l$

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The heats of combustion of carbon and carbon monoxide are −393.5 and −283.5 kJ mol−1, respectively. The heat of formation (in kJ) of carbon monoxide per mole is:

The correct option is B −110The combustion reactions are as shown.C+O2→CO2ΔH1=−393.5kJ/molCO+0.5O2→CO2ΔH2=−283.5kJ/molC+0.5O2→COΔH3ΔH3=ΔH1−ΔH2ΔH3=−393.5kJ/mol−(−283.5kJ/mol)=−110kJ/mol

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