For complete combustion of methanol $\mathrm{CH}_3 \mathrm{OH}(1)+\frac{3}{2} \mathrm{O}_2(\mathrm{~g}) \rightarrow \mathrm{CO}_2(\mathrm{~g})+2 \mathrm{H}_2 \mathrm{O}(1)$ the amount of heat produced as measured by bomb calorimeter is $726 \mathrm{~kJ} \mathrm{~mol}^{-1}$ at $27^{\circ} \mathrm{C}$. The enthalpy of combustion for the reaction is $-x \mathrm{~kJ} \mathrm{~mol}^{-1}$, where x is $\_\_\_\_$ . (Nearest integer) (Given : $\mathrm{R}=8.3 \mathrm{JK}-1 \mathrm{~mol}-1$ )