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Question

The enthalpy of combustion of carbon and carbon monoxide are $$-393.5$$ and $$-283\ kJ/mol$$ respectively. The enthalpy of formation of carbon monoxide per mole is:


A
110.5 kJ
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B
676.5 kJ
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C
676.5 kJ
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D
110.5 kJ
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Solution

The correct option is D $$-110.5\ kJ$$
I: $$C(s)+O_2(g)\rightarrow CO_2; \Delta H_1=-393.5\ kJ/mol$$

II: $$CO(g)+\displaystyle\frac{1}{2}O_2(g)\rightarrow CO_2(g); \Delta H_2=-283.0\ kJ/mol$$

On substracting II from I we get the formation reaction of carbon monoxide.

III: $$C(s)+\displaystyle\frac{1}{2}O_2(g)\rightarrow CO(g); \Delta H=\Delta H_1-\Delta H_2=-110.5\ kJ/mol$$

This equation III represents the formation of $$1$$ mole of $$CO$$ and thus enthalpy of formation of $$CO$$(g) is $$-110.5\ kJ/mol$$.

Chemistry

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