Final answer:
The enthalpy of reaction (ΔHrxn) can be calculated using standard enthalpies of formation and applying Hess's Law. However, to provide a specific answer, the values for the enthalpies of formation for all reactants and products, including glucose and water, would be required.
Step-by-step explanation:
To calculate the enthalpy of reaction (ΔHrxn), we need to know the standard enthalpies of formation for the reactants and products in the balanced chemical equation C₆H₁₂O₆ (l) + 3O₂ (g) → 2CO₂ (g) + 3H₂O (g). Using these standard enthalpies of formation, we can apply Hess's Law to find ΔHrxn as follows:
ΔHrxn = ∑ ΔHf(products) - ∑ ΔHf(reactants)
For this example, let's assume that the standard enthalpy of formation of glucose, C₆H₁₂O₆, is X kJ/mol (as the exact value was not provided in the question). The information provided indicates that the standard enthalpy of formation for CO₂(g) is -393.5 kJ/mol and for H₂O(g) is Y kJ/mol (again, the exact value for water was not provided).
Therefore, the ΔHrxn calculation would be:
ΔHrxn = [2(-393.5 kJ/mol) + 3(Y kJ/mol)] - [1(X kJ/mol) + 3(0 kJ/mol)]
ΔHrxn = (2 * -393.5 kJ + 3Y kJ) - (X kJ)
We need the actual values of ΔHf for each substance to solve for ΔHrxn. Since we do not have the specific values for glucose and water's enthalpies of formation, we cannot complete this example without that information. Once these values are known, we substitute them into the equation to solve for the correct ΔHrxn value.