Answer :
Final answer:
An exothermic reaction results when the bonds formed in the products release more energy than what was consumed to break the bonds of the reactants. This results in a net release of energy (heat), hence the reaction is considered exothermic. Energy diagrams, showing energy differences between reactants and products, are often used to illustrate this.
Explanation:
A reaction is considered exothermic due to the nature of the energy changes during the process. In an exothermic reaction, the energy released when the bonds are formed in the products is greater than the energy absorbed to break the bonds in the reactants. This results in a net release of energy, hence it is considered exothermic.
This can be further explained using reaction diagrams where the enthalpy change of the reaction, denoted by ΔH, is the difference in energy between the reactants and products. If the ΔH of a reaction is negative, that signifies an exothermic reaction. That's because it indicates a decrease in system enthalpy as the system moves from reactants to products.
In the context of your question, without more specific information about what energy differences A, B, and C represent, it's difficult to directly relate these differences to why a reaction is exothermic. However, if B represented the energy of the reactants and C represented the energy of the products, for example, a larger B than C (choice c) could indicate an exothermic reaction, since the reactants would have more energy than the products, and the difference would be released as heat.
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