A) \[110.5\,\,kJ\]
B) \[676.5\,\,kJ\]
C) \[-676.5\,\,kJ\]
D) \[-110.5\,\,kJ\]
Correct Answer: D
Solution :
\[I:\,\,C(s)+{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta H=-393.5\,\,kJ\] \[II:\,\,CO(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}C{{O}_{2}}(g);\] \[\Delta H=-283.0\,\,kJ\] \[III:\,\,C(s)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}CO(g);\] \[\Delta H=-110.5\,\,kJ\] 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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