To calculate the enthalpy change H for the combustion of 1 mole of propane, we need the enthalpies of formation Hf for all the reactants and products involved in the reaction. The enthalpy change for the reaction can be calculated using Hess's Law:H = Hf products - Hf reactants The standard enthalpies of formation for CO2, H2O, and C3H8 are as follows:Hf CO2 = -393.5 kJ/molHf H2O = -241.8 kJ/molHf C3H8 = -103.8 kJ/molHf O2 = 0 kJ/mol since O2 is in its elemental form Now, we can plug these values into Hess's Law equation:H = [3 Hf CO2 + 4 Hf H2O ] - [Hf C3H8 + 5 Hf O2 ]H = [3 -393.5 kJ/mol + 4 -241.8 kJ/mol ] - [ -103.8 kJ/mol + 5 0 kJ/mol ]H = -1180.5 kJ + -967.2 kJ - -103.8 kJ H = -2147.7 kJ + 103.8 kJH = -2043.9 kJ/molSo, the enthalpy change for the combustion of 1 mole of propane C3H8 is -2043.9 kJ/mol.