A) \[110.5\,kJ\]
B) \[676.5\,kJ\]
C) \[-676.5\,kJ\]
D) \[-110.5\,kJ\]
Correct Answer: D
Solution :
(i) \[C(s)+{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta \Eta =-393.5\,kJ\] (ii) \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta H=-283.0\,kJ\] (i) and (ii) gives (iii) \[C(s)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}CO(g);\] \[\Delta H=-110.5\,kJ\] Equation III also represents the enthalpy of formation of 1 mole of CO and thus, enthalpy change is the heat of formation of \[CO(g).\]
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