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)`.

Explanation

To calculate the standard enthalpy of formation (Δ_fH^Θ) of benzene (C₆H₆) from the given combustion data, we can follow these steps:

### Step 1: Write the balanced chemical equation for the combustion of benzene.

The balanced equation for the combustion of benzene is:
\[ C_6H_6 + \frac{15}{2} O_2 \rightarrow 6 CO_2 + 3 H_2O \]
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