The combustion of `1 mol` of benzene takes place at `298 K` and `1 atm`. After combustion, `CO_(2)(g)` and `H_(2)O(l)` are produced and `3267.0 kJ` of heat is librated. Calculate the standard entalpy of formation, `Delta_(f)H^(Θ)` of benzene
Given: `Delta_(f)H^(Θ)CO_(2)(g) = -393.5 kJ mol^(-1)`
`Delta_(f)H^(Θ)H_(2)O(l) = -285.83 kJ mol^(-1)`.

Options

A. `-48.51` kJ/Mole
B. `48.51` kJ/Mole
C. `-24.5 kJ`
D. `24.5 kJ`

Answer

B

Explanation

`DeltaH=H_(p)-H_(R)`
`6C+3H_(2) rarr C_(6)H_(6)" "DeltaH= ?`