The heats of combustion of carbon and carbon monoxide are –393.5 and –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
$C + O_{2} \to C O_{2}; Δ H_{1} = - 393.5 k J / m o l . . . . . (1)$

$C O + \frac{1}{2} O_{2} \to C O_{2}; Δ H_{2} = - 283.5 k J / m o l . . . (2)$

From equation (1) and (2),
$C + \frac{1}{2} O_{2} \to C O; Δ_{f} H_{(C O, g)} = Δ H_{1} - Δ H_{2}$

$Δ_{f} H_{(C O, g)} = - 393.5 - (- 283.5) k J / m o l$

$= - 393.5 + 283.5$

$= - 110 k J / m o l$

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

The correct option is C - 110.5C+O2→CO2 ; ΔH1=−393.5 kJ/mol .....(1) CO+12O2→CO2 ; ΔH2=−283.5 kJ/mol ...(2) From equation (1) and (2), C+12O2→CO ; ΔfH(CO, g)=ΔH1−ΔH2 ΔfH(CO, g)=−393.5−(−283.5) kJ/mol =−393.5+283.5 =−110 kJ/mol

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