How does the potential energy of the reactants compare to the potential energy of the products in an exothermic reaction, and where does the energy that is given off come from? Explain your answer in complete sentences.
The PE starts at a higher point than at the end, the difference is the amount of energy emitted.
In an exothermic reaction, the potential energy of the reactants is higher than the potential energy of the products. This means that the reactants possess more stored energy than the products.
To understand why energy is given off in an exothermic reaction, we need to look at the concept of potential energy and the formation or breaking of chemical bonds. Chemical reactions involve the rearrangement of atoms, which leads to the formation of new bonds and the breaking of old bonds. Breaking a chemical bond requires energy, while forming a bond releases energy.
In an exothermic reaction, more energy is released during bond formation than is required for bond breaking. This overall release of energy is what causes the reaction to be exothermic. The excess energy, or the difference in potential energy between the reactants and products, is released into the surroundings in the form of heat or other types of energy, such as light or sound.
Therefore, the energy that is given off in an exothermic reaction comes from the stored potential energy of the reactants. The breaking of existing bonds and the formation of new bonds result in the conversion of this stored energy into other forms of energy, which are then released into the surroundings.