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Introduction
ΔH represents the difference in potential energy between products and reactants, indicating the amount of heat energy gained/lost in a reaction.
Exothermic Reactions
Energy flows out of the system into the surroundings, usually as heat or light.
The potential energy of reactants are higher than that of the products.
This means that the chemical bonds between reactants are weaker, making the reactants less stable compared to the products.
ΔH < 0 because the potential energy of products subtracted from that of reactants results in a negative value (decrease of overall energy due to release).
Endothermic Reactions
Energy flows into the system from the surroundings, usually in the form of heat.
The potential energy of products are higher than that of the products.
This means that the chemical bonds between products are weaker, making the products less stable compared to the reactants.
ΔH > 0 because the potential energy of products subtracted from that of reactants results in a positive value (increase of overall energy due to absorption).
ΔH is measured in KJ/mol.
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