In an endothermic process, the heat that a system absorbs is thermal energy transfer into the system. Thus, an endothermic reaction generally leads to a decrease in the temperature of the surroundings. [1] The term was coined by 19th-century French chemist Marcellin Berthelot. [3]
Endothermic and exothermic reactions can be thought of as having energy as either a reactant of the reaction or a product. Endothermic reactions require energy, so energy is a reactant.
Exothermic reactions release energy to their surroundings, while endothermic reactions absorb energy from their surroundings. That single distinction is the foundation for understanding how chemical reactions exchange energy with the world around them.
Endothermic reactions absorb energy from their surroundings, because the products are higher in energy than the reactants. What is an exothermic reaction? Exothermic reactions release energy to their surroundings, because the products are lower in energy than the reactants.
In the case of an endothermic reaction, the reactants are at a lower energy level compared to the products—as shown in the energy diagram below. In other words, the products are less stable than the reactants.
An endothermic reaction is a chemical or physical process defined by its absorption of energy, typically heat, from its immediate environment. The term combines the Greek prefix “endo-,” meaning inward, with “thermic,” relating to heat.
In this video, I explain why some reactions explode while others cool, exploring the root cause of chemical energy. I discuss the chemistry behind endothermic and exothermic reactions, which involves ...
An endothermic reaction feels cold because it absorbs heat from its surroundings. Examples of endothermic reactions include photosynthesis, dissolving salt in water, and chemical cold packs.