Chapter 3, Problem 4P

The oxidation of glucose to CO₂ and water is a major source of energy in aerobic organisms. It is a reaction favored mainly by a large negative enthalpy change.
${\text{C}}_{\text{6}}{\text{H}}_{\text{12}}{\text{O}}_{\text{6}}\text{(s)}\text{+}{\text{6O}}_{\text{2}}\text{(g)}\to {\text{6CO}}_{\text{2}}\text{(g)}\text{+}{\text{6H}}_{\text{2}}\text{O(l)}$
$\Delta$ H^o = -2816 kJ/mol $\Delta$ S^o= +181 J/mol.K

a. At 37^o C, what is the value for $\Delta$ G^o?
b. In the overall reaction of aerobic metabolism of glucose, 32 moles of ATP are produced from ADP for every mole of glucose oxidized. Calculate the standard state free energy change for the overall reaction when glucose oxidation is coupled to the formation of ATP at 37^o C.
c. What is the efficiency of the process in terms of the percentage of the available free energy change captured in ATP?