Final answer:
To determine the standard enthalpy of formation of glucose, one can apply Hess's Law by considering the enthalpies of formation for CO2 and H2O and the enthalpy of the combustion of glucose.
Step-by-step explanation:
The process for determining the standard enthalpy of formation of glucose starts with understanding that the standard enthalpy of formation of CO2(g) is −393.5 kJ/mol. This is relevant as it is directly related to the combustion of glucose. The reaction for the combustion of glucose, C6H12O6 (s) + 6 O2(g) → 6 CO2 (g) + 6 H2O(l) has an enthalpy of reaction (ΔH°) of −2803 kJ/mol, indicating an exothermic process. To calculate the enthalpy of formation of glucose, we would need to consider the enthalpies of formation of all reactants and products involved.
Using Hess's Law, the overall enthalpy change can be determined by the sum of the enthalpy changes for the formation of the products minus the enthalpy changes for the formation of the reactants. Given that the formation of O2(g) has an enthalpy change of zero, the calculation simplifies to focus on the CO2 and H2O produced. Table T1 provides the standard enthalpies of formation needed to perform these calculations.