To calculate the bond dissociation energy BDE of the C-H bond in methane CH4 , we can use experimental data. The BDE is the energy required to break a bond and form two separate atoms. For methane, we can use the enthalpy of formation Hf of CH4 and the enthalpy of formation of the individual atoms C and H .The experimental data for the enthalpy of formation Hf of CH4 is -74.8 kJ/mol. The enthalpy of formation of atomic carbon C is 716.7 kJ/mol, and the enthalpy of formation of atomic hydrogen H is 218 kJ/mol.To calculate the BDE of the C-H bond in methane, we can use the following equation:BDE = Hf CH4 + 4 * Hf H - Hf C BDE = -74.8 kJ/mol + 4 * 218 kJ/mol - 716.7 kJ/mol BDE = -74.8 + 872 - 716.7 kJ/molBDE = 80.5 kJ/molThe bond dissociation energy of the C-H bond in methane CH4 is approximately 80.5 kJ/mol using experimental data.