Bond dissociation energy BDE is the energy required to break a chemical bond homolytically, i.e., to separate the bonded atoms into individual atoms with one electron each. It is an important parameter to evaluate the bond strength of a molecule.For methane CH4 , there are four C-H bonds. The average bond dissociation energy for a C-H bond in methane is approximately 439 kJ/mol. Since there are four such bonds, the total bond dissociation energy for methane is approximately 4 x 439 kJ/mol = 1756 kJ/mol.For carbon monoxide CO , there is one CO triple bond. The bond dissociation energy for the CO bond in CO is approximately 1072 kJ/mol.For ammonia NH3 , there are three N-H bonds. The average bond dissociation energy for an N-H bond in ammonia is approximately 391 kJ/mol. Since there are three such bonds, the total bond dissociation energy for ammonia is approximately 3 x 391 kJ/mol = 1173 kJ/mol.Comparing the bond strengths using bond dissociation energies:Methane CH4 has a total bond dissociation energy of 1756 kJ/mol, which is higher than that of carbon monoxide CO at 1072 kJ/mol and ammonia NH3 at 1173 kJ/mol. This indicates that the C-H bonds in methane are relatively strong compared to the CO bond in CO and the N-H bonds in NH3. However, it is important to note that this comparison is for the total bond dissociation energy of the molecules, not the individual bond strengths. The CO triple bond in CO is stronger than a single C-H bond in methane or an N-H bond in ammonia, but methane and ammonia have more bonds contributing to their total bond dissociation energies.