To calculate the enthalpy change for the oxidation of 2 moles of iron, we need to consider the balanced chemical equation for the reaction. The balanced equation for the oxidation of iron to form Fe2O3 is:4 Fe s + 3 O2 g 2 Fe2O3 s Now, we can use Hess's Law to calculate the enthalpy change for this reaction. Hess's Law states that the enthalpy change for a reaction is equal to the sum of the enthalpy changes for the formation of the products minus the sum of the enthalpy changes for the formation of the reactants.H_reaction = H_products - H_reactantsIn this case, the reactants are 4 moles of Fe s and 3 moles of O2 g , and the product is 2 moles of Fe2O3 s . The standard enthalpy of formation for Fe s and O2 g is 0 kJ/mol, as they are in their standard states. The standard enthalpy of formation for Fe2O3 s is given as -824 kJ/mol.H_reaction = [2 moles -824 kJ/mol ] - [4 moles 0 kJ/mol + 3 moles 0 kJ/mol]H_reaction = -1648 kJ - 0H_reaction = -1648 kJThe enthalpy change for the oxidation of 2 moles of iron to form Fe2O3 is -1648 kJ.