A) \[-219.0\text{ }kJ\text{ }mo{{l}^{-1}}\]
B) \[-109.5\text{ }kJ\text{ }mo{{l}^{-1}}\]
C) \[-175.0\text{ }kJ\text{ }mo{{l}^{-1}}\]
D) \[-87.5\text{ }kJ\text{ }mo{{l}^{-1}}\]
Correct Answer: B
Solution :
Given, reactions are \[C+{{O}_{2}}\xrightarrow{{}}C{{O}_{2}};\] \[\Delta H=-394kJ/mol\] ...(i) \[2CO+{{O}_{2}}\to 2C{{O}_{2}};\] \[\Delta H=-569kJ/mol\]...(ii) We obtained reaction \[C+\frac{1}{2}{{O}_{2}}\xrightarrow{{}}CO;\] \[\Delta H=?\] Divide Eq. (ii) by 2, take its reciprocal and add the obtained equation in Eq. (i) \[C{{O}_{2}}\xrightarrow{{}}CO+\frac{1}{2}{{O}_{2}},\] \[\Delta H=+284.5kJ/mol\] \[\frac{C+{{O}_{2}}\xrightarrow{{}}C{{O}_{2}},\,\,\,\,\,\,\,\,\Delta H=-394kJ/mol}{C+\frac{1}{2}{{O}_{2}}\xrightarrow{{}}CO,\,\,\,\,\,\,\Delta H=-109.5kJ/mol}\] \[\Delta H(CO)=-109.5kJ/mol\]
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