Calculate the values of \(\Delta H_{298}^{0}\) for the following reactions in the transformation of glucose in an organism:

\[ \begin{align*} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{~s}) & =2 \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{l})+2 \mathrm{CO}_{2}(\mathrm{~g}) \tag{A}\\ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{~s})+6 \mathrm{O}_{2}(\mathrm{~g}) & =6 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \tag{B} \end{align*} \]

Which of these reactions supplies more energy to the organism?

We are given that the heat of formation of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}=-1273.0 \mathrm{~kJ} / \mathrm{mol}\) the heat of formation of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{l})=-277.6 \mathrm{~kJ} / \mathrm{mol}\) the heat of formation of \(\mathrm{CO}_{2}(\mathrm{~g})=-393.5 \mathrm{~kJ} / \mathrm{mol}\) the heat of formation of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})=-285.8 \mathrm{~kJ} / \mathrm{mol}\)