\[ \text{CH}_3\text{OH}(l) + \dfrac{3}{2}\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\,\text{H}_2\text{O}(l) \quad \Delta H^\circ = -726\text{ kJ/mol}_{\text{rxn}} \]

Substance	\(\Delta H^\circ_f\ (\text{kJ/mol})\)
\(\text{CO}_2(g)\)	\(-394\)
\(\text{H}_2\text{O}(l)\)	\(-286\)

The combustion of methanol, \(\text{CH}_3\text{OH}(l)\), is represented by the thermochemical equation above. Based on the standard enthalpies of formation, \(\Delta H^\circ_f\), provided in the table, what is the standard enthalpy of formation of \(\text{CH}_3\text{OH}(l)\)?