The given balanced chemical equation is for the complete combustion of ethanol to carbon dioxide and water, not for the oxidation of ethanol to acetic acid. To find the enthalpy change for the oxidation of 1 mole of ethanol to acetic acid, we need the balanced chemical equation for that reaction and the corresponding enthalpy change.The balanced chemical equation for the oxidation of ethanol to acetic acid is:C2H5OH + O2 CH3COOH + H2OTo find the enthalpy change for this reaction, we need the standard enthalpies of formation Hf for each compound involved. The standard enthalpies of formation are:Hf C2H5OH = -277.7 kJ/molHf O2 = 0 kJ/mol since O2 is an element in its standard state Hf CH3COOH = -483.8 kJ/molHf H2O = -285.8 kJ/molNow, we can calculate the enthalpy change for the reaction using the following equation:H = [Hf products - Hf reactants ]H = [ 1 mol -483.8 kJ/mol + 1 mol -285.8 kJ/mol ] - [ 1 mol -277.7 kJ/mol + 1 mol 0 kJ/mol ]H = -483.8 - 285.8 - -277.7 H = -769.6 + 277.7H = -491.9 kJ/molSo, the enthalpy change for the oxidation of 1 mole of ethanol to acetic acid is -491.9 kJ/mol.