To calculate the bond energy required to break the H-O bond in water, we can use the concept of bond dissociation energy. Bond dissociation energy is the energy required to break a bond and form individual atoms. We can use Hess's Law to solve this problem.Hess's Law states that the total enthalpy change for a reaction is the same, regardless of the pathway taken. In this case, we can consider the formation of water from its elements H2 and O2 and then calculate the bond energy of the H-O bond.The formation of water can be represented by the following equation:H2 g + 1/2 O2 g H2O g The bond energy of the H-H bond is given as 436 kJ/mol, and the bond energy of the O=O bond is given as 495 kJ/mol. We can use these values to calculate the energy required to break the bonds in the reactants:Energy required to break H-H bond: 436 kJ/molEnergy required to break 1/2 O=O bond: 495 kJ/mol * 1/2 = 247.5 kJ/molNow, let's assume that the energy required to break one H-O bond is x kJ/mol. Since there are two H-O bonds in a water molecule, the energy required to break both H-O bonds would be 2x kJ/mol.According to Hess's Law, the energy required to break the bonds in the reactants should be equal to the energy required to break the bonds in the product water .So, 436 kJ/mol + 247.5 kJ/mol = 2x683.5 kJ/mol = 2xx = 341.75 kJ/molTherefore, the bond energy required to break the H-O bond in water is 341.75 kJ/mol.