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:

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

$C (s) + O_{2} (g) \to C O_{2} (g) Δ H = - 393.5 k J m o l^{- 1} C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g) Δ H = - 283.5 k J m o l^{- 1} - - - +$

$C (s) + \frac{1}{2} O_{2} (g) \to C O (g) Δ H = - 110.5 k J m o l^{- 1}$

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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

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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 C -110.5 C(s)+O2(g)→CO2(g)ΔH=−393.5 kJ mol−1CO(g)+12O2(g)→CO2(g)ΔH=−283.5 kJ mol−1− − − + C(s)+12O2(g)→CO(g)ΔH=−110.5 kJ mol−1

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:

The correct option is C
-110.5

$C (s) + O_{2} (g) \to C O_{2} (g) Δ H = - 393.5 k J m o l^{- 1} C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g) Δ H = - 283.5 k J m o l^{- 1} - - - +$

$C (s) + \frac{1}{2} O_{2} (g) \to C O (g) Δ H = - 110.5 k J m o l^{- 1}$