Final answer:
The enthalpy change of a chemical reaction is calculated using standard enthalpies of formation, but the correct value from the given options cannot be determined without more details on the specific reaction involved.
Step-by-step explanation:
To determine the enthalpy change of a reaction, one usually uses the standard enthalpies of formation (ΔH°f) for each substance involved. These values are multiplied by the respective stoichiometric coefficients of the substances in the balanced chemical equation, then summed for both products and reactants. The enthalpy change for the reaction (ΔH°rxn) is found by subtracting the sum of the reactants' enthalpies from the sum of the products' enthalpies. However, the enthalpy changes presented in the student's question do not align with the examples provided. The values of ΔH° for the products and reactants and the stoichiometric coefficients must be known to perform the correct calculation. Without the proper values or a specified reaction, it's impossible to verify which of the given enthalpy changes (A) -170.38 kJ/mol, (B) -206.18 kJ/mol, (C) -447.28 kJ/mol, or (D) -393.58 kJ/mol is correct for the student's specific reaction.