(Originais Teachy 2023) - Question Hard of Chemistry

Consider the complete combustion reaction of methane (CH4) under standard conditions, producing carbon dioxide (CO2) and gaseous water (H2O). The standard formation enthalpy of methane is -74.8 kJ/mol, of carbon dioxide is -393.5 kJ/mol, and of water is -285.8 kJ/mol. Additionally, the bond energy for C-H bonds is 413 kJ/mol, for C=O bonds is 799 kJ/mol, and for O-H bonds is 459 kJ/mol. Based on this information, calculate the change in enthalpy for the complete combustion reaction of methane under standard conditions. Consider that methane has four C-H bonds, carbon dioxide has two C=O bonds, and water has two O-H bonds. Justify the step-by-step calculation, including the application of the formula that relates the reaction enthalpy to the bond energies of the reactants and products.