The combustion of one mole of benzene takes place at 298 K and 1 atm. After combustion, CO₂(g) and H₂O (l) 
are produced and 3267.0 kJ of heat is liberated.
The standard enthalpy of formation, ∆_fH^⊖ of benzene is:
(Standard enthalpies of formation of CO₂(g) and ${\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$ are –393.5 kJ mol^–1 and – 285.83 kJ mol^–1 respectively.)

1. 54. 24 kJ mol^–1
2. 48. 51 kJ mol^–1
3. 66. 11 kJ mol^–1
4. 15. 21 kJ mol^–1

Given

\(\begin{aligned} &\mathrm{C}_{\text {(graphite) }}+\mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) \\ &\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-393.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ &H_{2}(g) + \frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\ &\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-285.8 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ &\mathrm{CO}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \\ &\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=+890.3 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}\)

Based on the above thermochemical equations, the value of Δ_rH° at 298 K for the reaction

${\mathrm{C}}_{\left(\mathrm{graphite}\right)}+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{CH}}_4\left(\mathrm{g}\right)\hspace{0.17em}\mathrm{will} \mathrm{be}:$

1. –74.8 kJ mol^–1

2. –144.0 kJ mol^–1

3. +74.8 kJ mol^–1

4. +144.0 kJ mol^–1