Compare endothermic and exothermic reactions in terms of potential energy, heat flow, and observed temperature changes. Explain your answer in complete sentences.
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I just wanted to compare my answer with the answer that i will be getting.. This is what I have:
Exothermic reaction starts at a higher energy value and ends at a lower energy value. In an exothermic reaction, we know that energy is given off in the form of heat. This energy comes from the stored energy of the unbroken bonds between atoms, which is the potential energy of the molecules. When these bonds break, energy is released in the form of heat. Therefore we would expect the potential energy of reactants to be larger than the products.
can you add to this?
Exothermic reaction starts at a higher energy value and ends at a lower energy value. In an exothermic reaction, we know that energy is given off in the form of heat. This energy comes from the stored energy of the unbroken bonds between atoms, which is the potential energy of the molecules. When these bonds break, energy is released in the form of heat. Therefore we would expect the potential energy of reactants to be larger than the products.
can you add to this?
I might add that the excess heat (but light also may be involved) is absorbed by the surroundings in exothermic reactions.
Next, you need to talk about endothermic reactions and how the heat needed to make the reaction go is supplied by the surroundings.
Next, you need to talk about endothermic reactions and how the heat needed to make the reaction go is supplied by the surroundings.
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