Question

During a reaction, the energy for reactants is -750 kJ/mole, and the energy for products is 920 kJ/mole. Which statement correctly compares energy in bonds?

Answer 1

The enthalpy change of the reaction indicates that the reaction is exothermic as the bonds in the products are stronger than those in the reactants.

Step-by-step explanation:

The enthalpy change (AH) of the reaction is approximately -111 kcal/mol. This means that bonds in the products (440 kcal) are stronger than the bonds in the reactants (329 kcal) by about 111 kcal/mol. Because the bonds in the products are stronger than those in the reactants, the reaction releases more energy than it absorbs. This excess energy is released as heat, so the reaction is exothermic.