The reaction for the metabolism of sucrose, C$12$H$22$O$11,$ in the body is the same as for its combustion in oxygen to yield CO$2($g$)$ and H$2$O$($l$).$ The standard enthalpy of formation of sucrose is $-2230$ kJ mol$-1.$ Use the following data to calculate the amount of energy released by metabolising $50\mathrm{.}0$ g of sucrose

$\backslash$Delta fHo$($CO$2($g$))=-393\mathrm{.}5$ kJ mol$-1$ and $\backslash$Delta fHo$($H$2$O$($l$))=-285\mathrm{.}9$ kJ mol$-1$