Calculate the standard enthalpy of formation of CH\(_{3}\)OH(l) from the following data:
\[
\text{CH}_{3}\text{OH(l)} + \frac{3}{2} \text{O}_{2} (\text{g}) \rightarrow \text{CO}_{2} (\text{g}) + 2\text{H}_{2}\text{O(l)}, \quad \Delta H = -726 \, \text{kJ mol}^{-1},
\]
\[
\text{C(graphite)} + \text{O}_{2} (\text{g}) \rightarrow \text{CO}_{2} (\text{g}), \quad \Delta H = -393 \, \text{kJ mol}^{-1},
\]
\[
\text{H}_{2} (\text{g}) + \frac{1}{2} \text{O}_{2} \rightarrow \text{H}_{2}\text{O(l)}, \quad \Delta H = -286 \, \text{kJ mol}^{-1}.
\]