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Question: The heat of formations of \(CO(g)\) and \(CO_{2}(g)\) are –26.4 kcal and \(- 94.0\)kcal respectively...

The heat of formations of CO(g)CO(g) and CO2(g)CO_{2}(g) are –26.4 kcal and −94.0- 94.0kcal respectively. The heat of combustion of carbon monoxide will be

A
  • 26.4 kcal
B

– 67.6 kcal

C

–120.6 kcal

D
  • 52.8 kcal
Answer

– 67.6 kcal

Explanation

Solution

CO+12O2→CO2CO + \frac{1}{2}O_{2} \rightarrow CO_{2}; ΔH=?\Delta H = ?

ΔHCO2=−94.0kcal\mathbf{\Delta}\mathbf{H}_{\mathbf{C}\mathbf{O}_{\mathbf{2}}}\mathbf{= - 94.0kcal}, ΔHCO=−26.4kcal\mathbf{\Delta}\mathbf{H}_{\mathbf{CO}}\mathbf{=}\mathbf{-}\mathbf{26.4kcal}

ΔH=ΔH(CO2)−ΔH(CO)\mathbf{\Delta H = \Delta}\mathbf{H}_{\mathbf{(C}\mathbf{O}_{\mathbf{2}}\mathbf{)}}\mathbf{- \Delta}\mathbf{H}_{\mathbf{(CO)}} =−94.0−(−26.4)=−67.6kcal\mathbf{= - 94.0 - ( - 26.4)}\mathbf{=}\mathbf{-}\mathbf{67.6kcal}