Exothermic process

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Explosions are some of the most violent exothermic reactions.

In thermodynamics, an exothermic process (Template:Etymology)<ref>"Gate for the Greek language" on-line dictionary Template:Webarchive. greek-language.gr</ref> is a thermodynamic process or reaction that releases energy from the system to its surroundings,<ref name=":0">{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> usually in the form of heat, but also in a form of light (e.g. a spark, flame, or flash), electricity (e.g. a battery), or sound (e.g. explosion heard when burning hydrogen). The term exothermic was first coined by 19th-century French chemist Marcellin Berthelot.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

The opposite of an exothermic process is an endothermic process, one that absorbs energy, usually in the form of heat.<ref name=":0" /> The concept is frequently applied in the physical sciences to chemical reactions where chemical bond energy is converted to thermal energy (heat).

Two types of chemical reactionsEdit

Exothermic and endothermic describe two types of chemical reactions or systems found in nature, as follows:

ExothermicEdit

An exothermic reaction occurs when heat is released to the surroundings. According to the IUPAC, an exothermic reaction is "a reaction for which the overall standard enthalpy change ΔH⚬ is negative".<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> Some examples of exothermic process are fuel combustion, condensation and nuclear fission,<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> which is used in nuclear power plants to release large amounts of energy.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

EndothermicEdit

In an endothermic reaction or system, energy is taken from the surroundings in the course of the reaction, usually driven by a favorable entropy increase in the system.<ref>Template:Cite book</ref> An example of an endothermic reaction is a first aid cold pack, in which the reaction of two chemicals, or dissolving of one in another, requires calories from the surroundings, and the reaction cools the pouch and surroundings by absorbing heat from them.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

Photosynthesis, the process that allows plants to convert carbon dioxide and water to sugar and oxygen, is an endothermic process: plants absorb radiant energy from the sun and use it in an endothermic, otherwise non-spontaneous process. The chemical energy stored can be freed by the inverse (spontaneous) process: combustion of sugar, which gives carbon dioxide, water and heat (radiant energy).<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

Energy releaseEdit

Exothermic refers to a transformation in which a closed system releases energy (heat) to the surroundings, expressed by

When the transformation occurs at constant pressure and without exchange of electrical energy, heat Template:Mvar is equal to the enthalpy change, i.e.

<math>\Delta H < 0,</math><ref name="Oxtoby8th">Oxtoby, D. W; Gillis, H.P., Butler, L. J. (2015).Principles of Modern Chemistry, Brooks Cole. p. 617. Template:ISBN</ref>

while at constant volume, according to the first law of thermodynamics it equals internal energy (Template:Mvar) change, i.e.

<math>\Delta U = Q + 0 > 0.</math>

In an adiabatic system (i.e. a system that does not exchange heat with the surroundings), an otherwise exothermic process results in an increase in temperature of the system.<ref>Template:Cite book</ref>

In exothermic chemical reactions, the heat that is released by the reaction takes the form of electromagnetic energy or kinetic energy of molecules.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> The transition of electrons from one quantum energy level to another causes light to be released. This light is equivalent in energy to some of the stabilization energy of the energy for the chemical reaction, i.e. the bond energy. This light that is released can be absorbed by other molecules in solution to give rise to molecular translations and rotations, which gives rise to the classical understanding of heat. In an exothermic reaction, the activation energy (energy needed to start the reaction) is less than the energy that is subsequently released, so there is a net release of energy.<ref>Template:Cite book</ref>

ExamplesEdit

File:ThermiteReaction.jpg

An exothermic thermite reaction using iron(III) oxide. The sparks flying outwards are globules of molten iron trailing smoke in their wake.

Some examples of exothermic processes are:<ref>Exothermic – Endothermic examples Template:Webarchive. frostburg.edu</ref>

Combustion of fuels such as wood, coal and oil/petroleum
The thermite reaction<ref>{{#invoke:citation/CS1|citation

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The reaction of alkali metals and other highly electropositive metals with water
Condensation of rain from water vapor
Mixing water and strong acids or strong bases
The reaction of acids and bases
Dehydration of carbohydrates by sulfuric acid
The setting of cement and concrete
Some polymerization reactions such as the setting of epoxy resin
The reaction of most metals with halogens or oxygen
Nuclear fusion in hydrogen bombs and in stellar cores (to iron)
Nuclear fission of heavy elements
The reaction between zinc and hydrochloric acid
Respiration (breaking down of glucose to release energy in cells)

Implications for chemical reactionsEdit

{{#invoke:Labelled list hatnote|labelledList|Main article|Main articles|Main page|Main pages}} Chemical exothermic reactions are generally more spontaneous than their counterparts, endothermic reactions.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

In a thermochemical reaction that is exothermic, the heat may be listed among the products of the reaction.