Using $\Delta _{f}G_{298}^{\circ}$ Data Given Below Calculate the Standard Gibbs Energy Change

Multiple Choice

Using $\Delta _{f}G_{298}^{\circ}$ data given below:
$\begin{array}{|c|c|c|c|c|}\hline & \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(\mathrm{~s}) & \mathrm{O}_{2}(\mathrm{~g}) & \mathrm{CO}_{2}(\mathrm{~g}) & \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \\\hline \Delta_{\mathrm{f}} G_{298}^{\circ} / \mathrm{kJ} \mathrm{mol}^{-1} & -1543 & 0 & -394.4 & -237.1 \\\hline\end{array}$
Calculate the standard Gibbs energy change, $\Delta _{T}G_{298}^{\circ}$ (kJ mol^-1) , for the following reaction:
C₁₂H₂₂O₁₁ (s) + 12 O₂ (g) → 12 CO₂ (g) + 11 H₂O (l)

A) + 911.5.
B) - 5797.9.
C) + 5797.9.
D) - 911.5.