A) \[-676.9\text{ }kJ\]
B) \[676.5\text{ }kJ\]
C) \[110.5\text{ }kJ\]
D) \[-110.5\text{ }kJ\]
Correct Answer: D
Solution :
\[C(s)+{{O}_{2}}(g)\xrightarrow[{}]{{}}C{{O}_{2}}(g)\] \[\Delta H=-\text{ }393.5\text{ }kJ\,mo{{l}^{-1}}\] \[CO(g)+\frac{1}{2}{{O}_{2}}(g)\to C{{O}_{2}}(g)\] \[\Delta H=-283\,kJ\,mo{{l}^{-1}}\] On subtracting equation (ii) from equation (i), we get \[C(s)+{{O}_{2}}(g)\to CO(g);\] \[\Delta H=-110.5\text{ }kJ\,mo{{l}^{-1}}\] The enthalpy of formation of carbon monoxide per mole\[=-110.5\text{ }kJ\,mo{{l}^{-1}}\]
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