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Question
The ΔfH∘ for CO2(g),CO(g)andH2O(g) are −393.5,−110.5 and −241.8kJmol−1 respectively. The standard enthalpy change (in kJ) for the reaction is:
CO2(g)+H2(g)⟶CO(g)+H2O(g)
The ΔfH∘ for CO2(g),CO(g)andH2O(g) are −393.5,−110.5 and −241.8kJmol−1 respectively. The standard enthalpy change (in kJ) for the reaction is:
CO2(g)+H2(g)⟶CO(g)+H2O(g)
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Solution
The correct option is C 41.2
First write the balanced chemical reactions for the formation of carbon dioxide, carbon monoxide and water.
C+O2⟶CO2;ΔH∘=−393.5kJ ... (i)
C+12O2⟶CO;ΔH∘=−110.5kJ ...(ii)
H2+12O2⟶H2O;ΔH∘=−241.8kJ ...(iii)
Then obtain the required equation by equating (ii)+(iii)−(i):
CO2+H2⟶CO+H2O;ΔH∘=+41.2
Hence, the standard enthalpy change for the reaction is 41.2 kJ/mol.
First write the balanced chemical reactions for the formation of carbon dioxide, carbon monoxide and water.
C+O2⟶CO2;ΔH∘=−393.5kJ ... (i)
C+12O2⟶CO;ΔH∘=−110.5kJ ...(ii)
H2+12O2⟶H2O;ΔH∘=−241.8kJ ...(iii)
Then obtain the required equation by equating (ii)+(iii)−(i):
CO2+H2⟶CO+H2O;ΔH∘=+41.2
Hence, the standard enthalpy change for the reaction is 41.2 kJ/mol.
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