SEP Use Mathematics Using the table of average bond energies estimate the energy needed to break the bonds of the reactants and the energy released when the products form for the reaction N_(2)+O_(2)arrow 2NO Note: N_(2) has a triple bond and O_(2) and NO have double bonds.

To estimate the energy needed to break the bonds of the reactants and the energy released when the products form for the reaction , we can use the table of average bond energies.First, let's calculate the energy needed to break the bonds of the reactants:1. Breaking the triple bond in : The average bond energy for a triple bond is 941 kJ/mol. Since there is only one molecule, we need to break one triple bond. Therefore, the energy needed to break the bond in is 941 kJ/mol.2. Breaking the double bond in : The average bond energy for a double bond is 498 kJ/mol. Since there is only one molecule, we need to break one double bond. Therefore, the energy needed to break the bond in is 498 kJ/mol.Now, let's calculate the energy released when the products form:1. Forming the double bonds in 2 molecules: The average bond energy for a double bond is 607 kJ/mol. Since there are two molecules, we need to form two double bonds. Therefore, the energy released when the products form is 2 * 607 kJ/mol = 1214 kJ/mol.Now, let's calculate the overall energy change for the reaction:Energy needed to break bonds = 941 kJ/mol + 498 kJ/mol = 1439 kJ/molEnergy released when products form = 1214 kJ/molOverall energy change = Energy released when products form - Energy needed to break bondsOverall energy change = 1214 kJ/mol - 1439 kJ/mol = -225 kJ/molTherefore, the energy needed to break the bonds of the reactants is 1439 kJ/mol, and the energy released when the products form is 1214 kJ/mol. The overall energy change for the reaction is -225 kJ/mol, indicating that the reaction is exothermic.