To calculate the bond dissociation energy BDE of the H-Cl bond in a hydrogen chloride molecule, we can use the following equation:BDE = 1/2 * h * vwhere h is the Planck's constant 6.626 x 10^-34 Js , and v is the vibrational frequency 8.8 x 10^13 Hz .BDE = 1/2 * 6.626 x 10^-34 Js * 8.8 x 10^13 Hz BDE = 1/2 * 6.626 x 10^-34 Js * 8.8 x 10^13 s^-1 BDE = 1/2 * 5.831 x 10^-20 J Now, we need to convert the energy from Joules to kJ/mol. To do this, we can use the following conversion factors:1 J = 0.239006 kcal/mol1 kcal = 4.184 kJBDE = 1/2 * 5.831 x 10^-20 J * 0.239006 kcal/J * 4.184 kJ/kcal BDE = 1/2 * 5.831 x 10^-20 J * 0.239006 mol/kcal * 4.184 kJ/kcal BDE = 1/2 * 5.831 x 10^-20 J * 1.000 kcal/mol * 4.184 kJ/kcal BDE = 1/2 * 5.831 x 10^-20 J * 4.184 kJ/kcal BDE = 1/2 * 2.439 x 10^-19 kJ Now, we need to convert the energy from kJ to kJ/mol. To do this, we can use Avogadro's number 6.022 x 10^23 mol^-1 :BDE = 1/2 * 2.439 x 10^-19 kJ * 6.022 x 10^23 mol^-1 BDE = 1/2 * 1.468 x 10^5 kJ/mol Finally, we can calculate the bond dissociation energy:BDE = 1/2 * 1.468 x 10^5 kJ/mol BDE = 7.34 x 10^4 kJ/molThe bond dissociation energy of the H-Cl bond in a hydrogen chloride molecule is approximately 73,400 kJ/mol.