Standard enthalpies of formation are generally computed from the calorimetric data referring to reactions, which are easy to do in the laboratory. For numerous compounds, the enthalpy of the reaction with O2 (g) (combustion) is commonly utilized, together with the standard enthalpies of formation of the combustion products, to evaluate ΔHf°. For instance, sucrose C12H22O11, common table sugar, is found to have a standard enthalpy of combustion of -5640.9 kJ/mole. The standard enthalpies of formation of CO2 (g) and H2O (l) are, respectively, -393.51 and -285.83 kJ/mole. Evaluate the ΔHf°for sucrose from the standard enthalpies of formation for CO2 (g) and H2O (l). State the balanced equations representing the formation of each of the above compounds utilized in the formation of sucrose.