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Standard XII

Chemistry

Heat of Formation

The enthalpie...

Question

The enthalpies of formation of $C O$ and $C O$ $_{2}$ are $- 110.5 k J$ mol $^{- 1}$ and $- 393.5 k J$ mol $^{- 1}$ respectively. The enthalpy of combustion of carbon monoxide is

- 110.5 k J

mol

^{- 1}

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- 283.0 k J

mol

^{- 1}

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504.0 k J

mol

^{- 1}

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221.2 k J

mol

^{- 1}

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Solution

The correct option is A $- 283.0 k J$ mol $^{- 1}$
$C O + \frac{1}{2} O_{2} \to C O_{2}$
$Δ H = Δ H_{f} (C O_{2}) - Δ H_{f} (C O) - \frac{1}{2} Δ_{F} H (O_{2})$
$= (- 393.5) + 110.5$ kJ mol $^{- 1}$
$= - 283$ kJ mol $^{- 1}$

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Similar questions

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:

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The enthalpies of formation of CO and CO2 are −110.5 kJ mol−1 and −393.5 kJ mol−1 respectively. The enthalpy of combustion of carbon monoxide is

The correct option is A −283.0 kJ mol−1CO+12O2→CO2ΔH=ΔHf(CO2)−ΔHf(CO)−12ΔFH(O2)=(−393.5)+110.5 kJ mol−1 =−283 kJ mol−1

The enthalpies of formation of $C O$ and $C O$ $_{2}$ are $- 110.5 k J$ mol $^{- 1}$ and $- 393.5 k J$ mol $^{- 1}$ respectively. The enthalpy of combustion of carbon monoxide is

The correct option is A $- 283.0 k J$ mol $^{- 1}$
$C O + \frac{1}{2} O_{2} \to C O_{2}$
$Δ H = Δ H_{f} (C O_{2}) - Δ H_{f} (C O) - \frac{1}{2} Δ_{F} H (O_{2})$
$= (- 393.5) + 110.5$ kJ mol $^{- 1}$
$= - 283$ kJ mol $^{- 1}$