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| [[File:Exergonic Reaction.svg|thumbnail|An exergonic reaction (such as cellular respiration) is a reaction that loses energy during the process of the reaction. Activation energy (1) catalyzes the reaction to occur in a spontaneous manner. The progress of the reaction is shown by the line. The change of Gibbs free energy (ΔG) in an exergonic reaction (that takes place under constant pressure and temperature conditions) is a negative value because energy is lost (2). ]]
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| An '''exergonic reaction''' is a [[chemical reaction]] where the change in the [[thermodynamic free energy|free energy]] is negative,<ref>IUPAC [[Gold Book]] definition: [http://www.iupac.org/goldbook/E02262.pdf#search='Exergonic%20reaction' exergonic (exoergic) reaction]</ref> indicating a [[spontaneous reaction]]. For processes that take place under constant pressure and temperature conditions, the [[Gibbs free energy]] is used whereas the [[Helmholtz energy]] is used for processes that take place under constant volume and temperature conditions.
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| Symbolically, the release of free energy, ''G'', in an exergonic reaction (at constant pressure and temperature) is denoted as
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| :<math>\Delta G=G_{\rm{products}}-G_{\rm{reactants}}<0.\,</math>
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| Although exergonic reactions are said to occur ''spontaneously'', this does not imply that the reaction will take place at an observable [[Reaction rate|rate]]. For instance, the [[Catalysis#Background|disproportionation of hydrogen peroxide]] is very slow in the absence of a suitable catalyst. It has been suggested that ''eager'' would be a more intuitive term in this context.<ref>{{cite journal|doi=10.1021/ed061p710|last=Hamori|first=Eugene|coauthors=James E. Muldrey|year=1984|title=Use of the world "eager" instead of "spontaneous" for the description of exergonic reactions|journal=Journal of Chemical Education|volume=61|issue=8|pages=710|bibcode = 1984JChEd..61..710H }}</ref>
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| More generally, the terms [[exergonic]] and [[endergonic]] relate to the [[free energy]] change in any process, not just chemical reactions. An example of an exergonic reaction is cellular respiration.
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| The terms [[exothermic]] and [[endothermic]] relate to the overall exchange of [[heat]] during a process.
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| ==See also==
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| *[[Endergonic reaction]]
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| ==References==
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| {{reflist}}
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| [[Category:Thermochemistry]]
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| [[de:Exergon]]
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Revision as of 18:07, 15 February 2014
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