The reaction for the metabolism of sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$, is the same as for its combustion in oxygen to yield $\mathrm{CO}_{2}(g)$ and $\mathrm{H}_{2} \mathrm{O}(l)$. The standard heat of formation of sucrose is $-2230 \mathrm{~kJ} \mathrm{~mol}^{-1}$. Use the data in Table $7.2$ to compute the amount of energy (in $\mathrm{kJ}$ ) released by metabolizing $1 \mathrm{oz}$ $(28.4 \mathrm{~g})$ of sucrose.