Calculate the enthalpy of combustion of benzene `(l)` on the basis of the following data:
a. Resonance energy of benzene `(l) =- 152 kJ// mol`
b. Enthalpy of hydrogenation of cyclohexene `(l) =- 119 kJ//mol`
c. `Delta_(f)H^(Theta)C_(6)H_(12)(l) =- 156 kJ mol^(-1)`
d. `Delta_(f)H^(Theta) of H_(2)O(l) =- 285.8 kJ mol^(-1)`
e. `Delta_(f)H^(Theta)of CO_(2)(g) =- 393.5 kJ mol^(-1)`

Explanation

`-357 = Delta_(t)^(@)("Products") - DeltaH_(t)^(@)("Reactant")`
`=-156 - DeltaH_(t)^(@)("Benzeene")`
`Delta_(t)^(@)("Benzene") = (-156 + 357) kJ mol^(-1) = 201 kJ mol^(-1)`
Resonance energy `(DeltaH_(t)^(@))("Benzene Alcohol") - DeltaH_(t)^(@) ("Benzene theoretical")`
`[DeltaH_(t)^(@) ("Benzene Alcohol")] = 49 kJ "mol"^(-1)`
`C_(6)H_(6) (i) + 15/2 O_(2)(g) to 6CO_(2)(g) + 3H_(2)O(l)`
`DeltaH_("reaction")^(@) = 6(DeltaH_(t)^(@))_(CO_(2)) + 3(DeltaH_(t)^(@))_(H_(2)O) - (DeltaH_(t)^(@))_("Benzene")`
`=6(-393.5) + 3(-285.8) - 49`
`=3267.4 kJ mol^(-1)`