Final answer:
The reaction is an exothermic reaction as it releases energy due to stronger bonds formed in the products compared to the energy required to break bonds in the reactants.
Step-by-step explanation:
If the energy gained by forming bonds is greater than the net energy required for breaking bonds, the reaction is an exothermic reaction. This type of reaction results when the bonds in the products are stronger than the bonds in the reactants, leading to a net release of energy. We can estimate the enthalpy change (ΔH) for a chemical reaction using bond energies, which involves adding together the energies required to break bonds in the reactants and the energies released from forming bonds in the products. The difference determines whether the reaction is exothermic (ΔH negative) or endothermic (ΔH positive).
During an exothermic reaction, the system releases energy to the surroundings, typically in the form of heat. Atoms in the products are in a lower energy, more stable state compared to the atoms in the reactants. In contrast, an endothermic reaction requires a net input of energy, meaning that the bonds formed in the products are weaker than those broken in the reactants, resulting in an overall absorption of energy (ΔH positive).