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Question

The ΔfH0 for CO2 (g), CO(g) and H2O (g) are -393.5, -110.5 and -241.8 kJ mol1 respectively. The standard enthalpy change (in kJ mol1) for the reaction
CO2 (g)+H2 (g)CO (g)+H2O (g) is :

A
524.1
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B
+ 41.2
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C
-262.5
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D
- 41.2
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Solution

The correct option is B + 41.2
Given, ΔfH0(CO2)=393.5 kJmol1
ΔfH0(CO)=110.5 kJmol1
ΔfH0(H2)=241.8 kJmol1
CO2 (g)+H2 (g)CO (g)+H2 (g)
ΔrH is related to bond enthalpies of reactants and products in the gas phase reaction as
ΔrH= ΔfH0(products) ΔfH0(reactants)=ΔfH0(CO)+ΔfH0(H2)ΔfH0(CO2)ΔfH0(H2)=110.5241.8(393.5)=+ 41.20 kJ mol1
hence the standard enthalpy change for the given reaction is + 41.20 kJ mol1

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