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<span>Toggle Two types of chemical reactions subsection</span> </button> <ul id="toc-Two_types_of_chemical_reactions-sublist" class="vector-toc-list"> <li id="toc-Exothermic" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Exothermic"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.1</span> <span>Exothermic</span> </div> </a> <ul id="toc-Exothermic-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Endothermic" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Endothermic"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.2</span> <span>Endothermic</span> </div> </a> <ul id="toc-Endothermic-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Energy_release" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Energy_release"> <div class="vector-toc-text"> <span class="vector-toc-numb">2</span> <span>Energy release</span> </div> </a> <ul id="toc-Energy_release-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Examples" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Examples"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Examples</span> </div> </a> <ul id="toc-Examples-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Implications_for_chemical_reactions" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Implications_for_chemical_reactions"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Implications for chemical reactions</span> </div> </a> <ul id="toc-Implications_for_chemical_reactions-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#See_also"> <div 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class="firstHeading mw-first-heading"><span class="mw-page-title-main">Exothermic process</span></h1> <div id="p-lang-btn" class="vector-dropdown mw-portlet mw-portlet-lang" > <input type="checkbox" id="p-lang-btn-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-p-lang-btn" class="vector-dropdown-checkbox mw-interlanguage-selector" aria-label="Go to an article in another language. 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class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Egzotermni_proces" title="Egzotermni proces – Bosnian" lang="bs" hreflang="bs" data-title="Egzotermni proces" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target"><span>Bosanski</span></a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Exoterm" title="Exoterm – Danish" lang="da" hreflang="da" data-title="Exoterm" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target"><span>Dansk</span></a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%95%CE%BE%CF%8E%CE%B8%CE%B5%CF%81%CE%BC%CE%B7_%CE%B4%CE%B9%CE%B5%CF%81%CE%B3%CE%B1%CF%83%CE%AF%CE%B1" title="Εξώθερμη διεργασία – Greek" lang="el" hreflang="el" data-title="Εξώθερμη διεργασία" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target"><span>Ελληνικά</span></a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Proceso_exot%C3%A9rmico" title="Proceso exotérmico – Spanish" lang="es" hreflang="es" data-title="Proceso exotérmico" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target"><span>Español</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D9%81%D8%B1%D8%A7%DB%8C%D9%86%D8%AF_%DA%AF%D8%B1%D9%85%D8%A7%D8%B2%D8%A7" title="فرایند گرمازا – Persian" lang="fa" hreflang="fa" data-title="فرایند گرمازا" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target"><span>فارسی</span></a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Pr%C3%B3iseas_eisiteirmeach" title="Próiseas eisiteirmeach – Irish" lang="ga" hreflang="ga" data-title="Próiseas eisiteirmeach" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target"><span>Gaeilge</span></a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%8A%E0%A4%B7%E0%A5%8D%E0%A4%AE%E0%A4%BE%E0%A4%95%E0%A5%8D%E0%A4%B7%E0%A5%87%E0%A4%AA%E0%A5%80_%E0%A4%AA%E0%A5%8D%E0%A4%B0%E0%A4%95%E0%A5%8D%E0%A4%B0%E0%A4%BF%E0%A4%AF%E0%A4%BE" title="ऊष्माक्षेपी प्रक्रिया – Hindi" lang="hi" hreflang="hi" data-title="ऊष्माक्षेपी प्रक्रिया" data-language-autonym="हिन्दी" data-language-local-name="Hindi" class="interlanguage-link-target"><span>हिन्दी</span></a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Egzotermni_proces" title="Egzotermni proces – Croatian" lang="hr" hreflang="hr" data-title="Egzotermni proces" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Processo_esotermico" title="Processo esotermico – Italian" lang="it" hreflang="it" data-title="Processo esotermico" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target"><span>Italiano</span></a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%AD%D0%BA%D0%B7%D0%BE%D1%82%D0%B5%D1%80%D0%BC%D0%B8%D0%BA%D0%B0%D0%BB%D1%8B%D2%9B_%D0%BF%D1%80%D0%BE%D1%86%D0%B5%D1%81%D1%82%D0%B5%D1%80" title="Экзотермикалық процестер – Kazakh" lang="kk" hreflang="kk" data-title="Экзотермикалық процестер" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target"><span>Қазақша</span></a></li><li class="interlanguage-link interwiki-ht mw-list-item"><a href="https://ht.wikipedia.org/wiki/Egzot%C3%A8mik" title="Egzotèmik – Haitian Creole" lang="ht" hreflang="ht" data-title="Egzotèmik" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target"><span>Kreyòl ayisyen</span></a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Egzoterminis_procesas" title="Egzoterminis procesas – Lithuanian" lang="lt" hreflang="lt" data-title="Egzoterminis procesas" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target"><span>Lietuvių</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Exotherm_proces" title="Exotherm proces – Dutch" lang="nl" hreflang="nl" data-title="Exotherm proces" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target"><span>Nederlands</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Processo_exot%C3%A9rmico" title="Processo exotérmico – Portuguese" lang="pt" hreflang="pt" data-title="Processo exotérmico" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target"><span>Português</span></a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Proces_exoterm" title="Proces exoterm – Romanian" lang="ro" hreflang="ro" data-title="Proces exoterm" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Exothermic_reactions" title="Exothermic reactions – Simple English" lang="en-simple" hreflang="en-simple" data-title="Exothermic reactions" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target"><span>Simple English</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/Egzotermni_proces" title="Egzotermni proces – Serbian" lang="sr" hreflang="sr" data-title="Egzotermni proces" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target"><span>Српски / srpski</span></a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%B5%E0%AF%86%E0%AE%AA%E0%AF%8D%E0%AE%AA%E0%AE%AE%E0%AF%8D_%E0%AE%89%E0%AE%AE%E0%AE%BF%E0%AE%B4%E0%AF%8D_%E0%AE%9A%E0%AF%86%E0%AE%AF%E0%AE%B2%E0%AF%8D%E0%AE%AE%E0%AF%81%E0%AE%B1%E0%AF%88" title="வெப்பம் உமிழ் செயல்முறை – Tamil" lang="ta" hreflang="ta" data-title="வெப்பம் உமிழ் செயல்முறை" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target"><span>தமிழ்</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%81%E0%B8%A3%E0%B8%B0%E0%B8%9A%E0%B8%A7%E0%B8%99%E0%B8%81%E0%B8%B2%E0%B8%A3%E0%B8%84%E0%B8%B2%E0%B8%A2%E0%B8%84%E0%B8%A7%E0%B8%B2%E0%B8%A1%E0%B8%A3%E0%B9%89%E0%B8%AD%E0%B8%99_(%E0%B8%AD%E0%B8%B8%E0%B8%93%E0%B8%AB%E0%B8%9E%E0%B8%A5%E0%B8%A8%E0%B8%B2%E0%B8%AA%E0%B8%95%E0%B8%A3%E0%B9%8C)" title="กระบวนการคายความร้อน (อุณหพลศาสตร์) – Thai" lang="th" hreflang="th" data-title="กระบวนการคายความร้อน (อุณหพลศาสตร์)" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target"><span>ไทย</span></a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Qu%C3%A1_tr%C3%ACnh_t%E1%BB%8Fa_nhi%E1%BB%87t" title="Quá trình tỏa nhiệt – Vietnamese" lang="vi" hreflang="vi" data-title="Quá trình tỏa nhiệt" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target"><span>Tiếng Việt</span></a></li><li class="interlanguage-link interwiki-zh-yue 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data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">Not to be confused with <a href="/wiki/Ectothermic" class="mw-redirect" title="Ectothermic">Ectothermic</a>.</div> <figure class="mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Explosion1.JPG" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a3/Explosion1.JPG/300px-Explosion1.JPG" decoding="async" width="300" height="223" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a3/Explosion1.JPG/450px-Explosion1.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a3/Explosion1.JPG/600px-Explosion1.JPG 2x" data-file-width="743" data-file-height="552" /></a><figcaption><a href="/wiki/Explosion" title="Explosion">Explosions</a> are some of the most violent exothermic reactions.</figcaption></figure> <p>In <a href="/wiki/Thermodynamics" title="Thermodynamics">thermodynamics</a>, an <b>exothermic process</b> (from <a href="/wiki/Ancient_Greek_language" class="mw-redirect" title="Ancient Greek language">Ancient Greek</a> <i> </i><span lang="grc"><a href="https://en.wiktionary.org/wiki/%CE%AD%CE%BE%CF%89#Ancient_Greek" class="extiw" title="wikt:έξω">έξω</a></span><i> (<span title="Ancient Greek transliteration" lang="grc-Latn"><i>éxō</i></span>)</i> 'outward' and <i> </i><span lang="grc"><a href="https://en.wiktionary.org/wiki/%CE%B8%CE%B5%CF%81%CE%BC%CE%B9%CE%BA%CF%8C%CF%82#Ancient_Greek" class="extiw" title="wikt:θερμικός">θερμικός</a></span><i> (<span title="Ancient Greek transliteration" lang="grc-Latn"><i>thermikós</i></span>)</i> 'thermal')<sup id="cite_ref-1" class="reference"><a href="#cite_note-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> is a <a href="/wiki/Thermodynamic_process" title="Thermodynamic process">thermodynamic process</a> or <a href="/wiki/Chemical_reaction" title="Chemical reaction">reaction</a> that releases <a href="/wiki/Energy" title="Energy">energy</a> from the system to its <a href="/wiki/Environment_(systems)" title="Environment (systems)">surroundings</a>,<sup id="cite_ref-:0_2-0" class="reference"><a href="#cite_note-:0-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> usually in the form of <a href="/wiki/Heat" title="Heat">heat</a>, but also in a form of <a href="/wiki/Light" title="Light">light</a> (e.g. a spark, flame, or flash), <a href="/wiki/Electricity" title="Electricity">electricity</a> (e.g. a battery), or <a href="/wiki/Sound" title="Sound">sound</a> (e.g. explosion heard when burning hydrogen). The term <i>exothermic</i> was first coined by 19th-century French chemist <a href="/wiki/Marcellin_Berthelot" title="Marcellin Berthelot">Marcellin Berthelot</a>.<sup id="cite_ref-3" class="reference"><a href="#cite_note-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p><p>The opposite of an exothermic process is an <a href="/wiki/Endothermic" class="mw-redirect" title="Endothermic">endothermic</a> process, one that absorbs energy, usually in the form of heat.<sup id="cite_ref-:0_2-1" class="reference"><a href="#cite_note-:0-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> The concept is frequently applied in the <a href="/wiki/Outline_of_physical_science" title="Outline of physical science">physical sciences</a> to <a href="/wiki/Chemical_reaction" title="Chemical reaction">chemical reactions</a> where chemical <a href="/wiki/Bond_energy" title="Bond energy">bond energy</a> is converted to <a href="/wiki/Thermal_energy" title="Thermal energy">thermal energy</a> (heat). </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Two_types_of_chemical_reactions">Two types of chemical reactions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=1" title="Edit section: Two types of chemical reactions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Exothermic and endothermic describe two types of chemical reactions or systems found in nature, as follows: </p> <div class="mw-heading mw-heading3"><h3 id="Exothermic">Exothermic</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=2" title="Edit section: Exothermic"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>An exothermic reaction occurs when heat is released to the surroundings. According to the <a href="/wiki/International_Union_of_Pure_and_Applied_Chemistry" title="International Union of Pure and Applied Chemistry">IUPAC</a>, an exothermic reaction is "a reaction for which the overall standard <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> change Δ<i>H</i>⚬ is negative".<sup id="cite_ref-4" class="reference"><a href="#cite_note-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup> Some examples of exothermic process are fuel <a href="/wiki/Combustion" title="Combustion">combustion</a>, <a href="/wiki/Condensation" title="Condensation">condensation</a> and <a href="/wiki/Nuclear_fission" title="Nuclear fission">nuclear fission</a>,<sup id="cite_ref-5" class="reference"><a href="#cite_note-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> which is used in <a href="/wiki/Nuclear_power_plant" title="Nuclear power plant">nuclear power plants</a> to release large amounts of energy.<sup id="cite_ref-6" class="reference"><a href="#cite_note-6"><span class="cite-bracket">[</span>6<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Endothermic">Endothermic</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=3" title="Edit section: Endothermic"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>In an <a href="/wiki/Endothermic_process" title="Endothermic process">endothermic reaction</a> or system, energy is taken from the surroundings in the course of the reaction, usually driven by a favorable <a href="/wiki/Entropy" title="Entropy">entropy</a> increase in the system.<sup id="cite_ref-7" class="reference"><a href="#cite_note-7"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup> 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.<sup id="cite_ref-8" class="reference"><a href="#cite_note-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup> </p><p><a href="/wiki/Photosynthesis" title="Photosynthesis">Photosynthesis</a>, the process that allows plants to convert carbon dioxide and water to sugar and oxygen, is an endothermic process: plants absorb <a href="/wiki/Radiant_energy" title="Radiant energy">radiant energy</a> 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).<sup id="cite_ref-9" class="reference"><a href="#cite_note-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Energy_release">Energy release</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=4" title="Edit section: Energy release"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Exothermic refers to a transformation in which a closed system releases energy (heat) to the surroundings, expressed by </p> <dl><dd><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle Q>0.}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>Q</mi> <mo>></mo> <mn>0.</mn> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle Q>0.}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/632f244903cf3296756014fdc93e72d4b7995fd5" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:6.746ex; height:2.509ex;" alt="{\displaystyle Q>0.}"></span></dd></dl> <p>When the transformation occurs at <a href="/wiki/Isobaric_process" title="Isobaric process">constant pressure</a> and without exchange of <a href="/wiki/Electrical_energy" title="Electrical energy">electrical energy</a>, heat <span class="texhtml mvar" style="font-style:italic;">Q</span> is equal to the <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> change, i.e. </p> <dl><dd><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle \Delta H<0,}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi mathvariant="normal">Δ</mi> <mi>H</mi> <mo><</mo> <mn>0</mn> <mo>,</mo> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \Delta H<0,}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/0b882d1b8e6c6a7e3df490eb7aef3cbf633b898b" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:8.907ex; height:2.509ex;" alt="{\displaystyle \Delta H<0,}"></span><sup id="cite_ref-Oxtoby8th_10-0" class="reference"><a href="#cite_note-Oxtoby8th-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup></dd></dl> <p>while at <a href="/wiki/Constant_volume" class="mw-redirect" title="Constant volume">constant volume</a>, according to the <a href="/wiki/First_law_of_thermodynamics" title="First law of thermodynamics">first law of thermodynamics</a> it equals <a href="/wiki/Internal_energy" title="Internal energy">internal energy</a> (<span class="texhtml mvar" style="font-style:italic;">U</span>) change, i.e. </p> <dl><dd><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle \Delta U=Q+0>0.}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi mathvariant="normal">Δ</mi> <mi>U</mi> <mo>=</mo> <mi>Q</mi> <mo>+</mo> <mn>0</mn> <mo>></mo> <mn>0.</mn> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \Delta U=Q+0>0.}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/173761a4148a49fb6599e97518dc07cfa799bf47" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:17.566ex; height:2.509ex;" alt="{\displaystyle \Delta U=Q+0>0.}"></span></dd></dl> <p>In an <a href="/wiki/Adiabatic" class="mw-redirect" title="Adiabatic">adiabatic</a> 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.<sup id="cite_ref-11" class="reference"><a href="#cite_note-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> </p><p>In exothermic chemical reactions, the heat that is released by the reaction takes the form of electromagnetic energy or <a href="/wiki/Kinetic_energy" title="Kinetic energy">kinetic energy</a> of molecules.<sup id="cite_ref-12" class="reference"><a href="#cite_note-12"><span class="cite-bracket">[</span>12<span class="cite-bracket">]</span></a></sup> The transition of <a href="/wiki/Electron" title="Electron">electrons</a> from one quantum <a href="/wiki/Energy_level" title="Energy level">energy level</a> 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 <a href="/wiki/Bond_energy" title="Bond energy">bond energy</a>. This light that is released can be absorbed by other molecules in <a href="/wiki/Solution_(chemistry)" title="Solution (chemistry)">solution</a> to give rise to molecular translations and rotations, which gives rise to the classical understanding of heat. In an exothermic reaction, the <a href="/wiki/Activation_energy" title="Activation energy">activation energy</a> (energy needed to start the reaction) is less than the energy that is subsequently released, so there is a net release of energy.<sup id="cite_ref-13" class="reference"><a href="#cite_note-13"><span class="cite-bracket">[</span>13<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Examples">Examples</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=5" title="Edit section: Examples"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:ThermiteReaction.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5b/ThermiteReaction.jpg/220px-ThermiteReaction.jpg" decoding="async" width="220" height="244" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5b/ThermiteReaction.jpg/330px-ThermiteReaction.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/5b/ThermiteReaction.jpg/440px-ThermiteReaction.jpg 2x" data-file-width="2095" data-file-height="2322" /></a><figcaption>An exothermic <a href="/wiki/Thermite" title="Thermite">thermite</a> reaction using iron(III) oxide. The sparks flying outwards are globules of molten iron trailing smoke in their wake.</figcaption></figure> <p>Some examples of exothermic processes are:<sup id="cite_ref-14" class="reference"><a href="#cite_note-14"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup> </p> <ul><li><a href="/wiki/Combustion" title="Combustion">Combustion</a> of <a href="/wiki/Fuel" title="Fuel">fuels</a> such as <a href="/wiki/Wood" title="Wood">wood</a>, <a href="/wiki/Coal" title="Coal">coal</a> and <a href="/wiki/Oil" title="Oil">oil</a>/<a href="/wiki/Petroleum" title="Petroleum">petroleum</a></li> <li>The thermite reaction<sup id="cite_ref-15" class="reference"><a href="#cite_note-15"><span class="cite-bracket">[</span>15<span class="cite-bracket">]</span></a></sup></li> <li>The reaction of <a href="/wiki/Alkali_metal" title="Alkali metal">alkali metals</a> and other highly <a href="/wiki/Electropositive" class="mw-redirect" title="Electropositive">electropositive</a> metals with water</li> <li><a href="/wiki/Condensation" title="Condensation">Condensation</a> of rain from water vapor</li> <li>Mixing water and <a href="/wiki/Strong_acid" class="mw-redirect" title="Strong acid">strong acids</a> or <a href="/wiki/Strong_base" class="mw-redirect" title="Strong base">strong bases</a></li> <li>The reaction of <a href="/wiki/Acid" title="Acid">acids</a> and <a href="/wiki/Base_(chemistry)" title="Base (chemistry)">bases</a></li> <li>Dehydration of <a href="/wiki/Carbohydrate" title="Carbohydrate">carbohydrates</a> by <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a></li> <li>The setting of <a href="/wiki/Cement" title="Cement">cement</a> and <a href="/wiki/Concrete" title="Concrete">concrete</a></li> <li>Some <a href="/wiki/Polymerisation" class="mw-redirect" title="Polymerisation">polymerization</a> reactions such as the setting of <a href="/wiki/Epoxy_resin" class="mw-redirect" title="Epoxy resin">epoxy resin</a></li> <li>The reaction of most metals with halogens or oxygen</li> <li><a href="/wiki/Nuclear_fusion" title="Nuclear fusion">Nuclear fusion</a> in hydrogen bombs and in stellar cores (to iron)</li> <li><a href="/wiki/Nuclear_fission" title="Nuclear fission">Nuclear fission</a> of heavy elements</li> <li>The reaction between zinc and <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a></li> <li><a href="/wiki/Cellular_respiration" title="Cellular respiration">Respiration</a> (breaking down of glucose to release energy in cells)</li></ul> <div class="mw-heading mw-heading2"><h2 id="Implications_for_chemical_reactions">Implications for chemical reactions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=6" title="Edit section: Implications for chemical reactions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Exothermic_reaction" title="Exothermic reaction">Exothermic reaction</a></div> <p>Chemical exothermic reactions are generally more spontaneous than their counterparts, <a href="/wiki/Endothermic_reaction" class="mw-redirect" title="Endothermic reaction">endothermic reactions</a>.<sup id="cite_ref-16" class="reference"><a href="#cite_note-16"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup> </p><p>In a thermochemical reaction that is exothermic, the heat may be listed among the products of the reaction. </p> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=7" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1184024115">.mw-parser-output .div-col{margin-top:0.3em;column-width:30em}.mw-parser-output .div-col-small{font-size:90%}.mw-parser-output .div-col-rules{column-rule:1px solid #aaa}.mw-parser-output .div-col dl,.mw-parser-output .div-col ol,.mw-parser-output .div-col ul{margin-top:0}.mw-parser-output .div-col li,.mw-parser-output .div-col dd{page-break-inside:avoid;break-inside:avoid-column}</style><div class="div-col" style="column-width: 22em;"> <ul><li><a href="/wiki/Calorimetry" title="Calorimetry">Calorimetry</a></li> <li><a href="/wiki/Chemical_thermodynamics" title="Chemical thermodynamics">Chemical thermodynamics</a></li> <li><a href="/wiki/Differential_scanning_calorimetry" title="Differential scanning calorimetry">Differential scanning calorimetry</a></li> <li><a href="/wiki/Endergonic" class="mw-redirect" title="Endergonic">Endergonic</a></li> <li><a href="/wiki/Endergonic_reaction" title="Endergonic reaction">Endergonic reaction</a></li> <li><a href="/wiki/Exergonic" class="mw-redirect" title="Exergonic">Exergonic</a></li> <li><a href="/wiki/Exergonic_reaction" title="Exergonic reaction">Exergonic reaction</a></li> <li><a href="/wiki/Endothermic_reaction" class="mw-redirect" title="Endothermic reaction">Endothermic reaction</a></li></ul> </div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Exothermic_process&action=edit&section=8" title="Edit section: References"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-1"><span class="mw-cite-backlink"><b><a href="#cite_ref-1">^</a></b></span> <span class="reference-text"><a rel="nofollow" class="external text" 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Retrieved <span class="nowrap">2024-06-26</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=Chemistry+LibreTexts&rft.atitle=Potential+Energy&rft.date=2013-10-02&rft_id=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FPhysical_and_Theoretical_Chemistry_Textbook_Maps%2FSupplemental_Modules_%28Physical_and_Theoretical_Chemistry%29%2FThermodynamics%2FEnergies_and_Potentials%2FPotential_Energy&rfr_id=info%3Asid%2Fen.wikipedia.org%3AExothermic+process" class="Z3988"></span></span> </li> <li id="cite_note-13"><span class="mw-cite-backlink"><b><a href="#cite_ref-13">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation book cs1">"Chapter 2 - Carbon-based fuels". <i>Heinemann Chemistry</i>. Vol. 2 (6 ed.). <a href="/wiki/Pearson_Education" title="Pearson Education">Pearson</a>. pp. 64–65. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780655700098" title="Special:BookSources/9780655700098"><bdi>9780655700098</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Chapter+2+-+Carbon-based+fuels&rft.btitle=Heinemann+Chemistry&rft.pages=64-65&rft.edition=6&rft.pub=Pearson&rft.isbn=9780655700098&rfr_id=info%3Asid%2Fen.wikipedia.org%3AExothermic+process" class="Z3988"></span></span> </li> <li id="cite_note-14"><span class="mw-cite-backlink"><b><a href="#cite_ref-14">^</a></b></span> <span class="reference-text"><a rel="nofollow" class="external text" href="http://antoine.frostburg.edu/chem/senese/101/thermo/faq/exothermic-endothermic-examples.shtml">Exothermic – Endothermic examples</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20060901100540/http://antoine.frostburg.edu/chem/senese/101/thermo/faq/exothermic-endothermic-examples.shtml">Archived</a> 2006-09-01 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a>. frostburg.edu</span> </li> <li id="cite_note-15"><span class="mw-cite-backlink"><b><a href="#cite_ref-15">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.colorado.edu/lab/lecture-demo-manual/t510-exothermic-reaction-thermite">"T510: Exothermic Reaction – Thermite"</a>. 23 December 2015.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=T510%3A+Exothermic+Reaction+%E2%80%93+Thermite&rft.date=2015-12-23&rft_id=https%3A%2F%2Fwww.colorado.edu%2Flab%2Flecture-demo-manual%2Ft510-exothermic-reaction-thermite&rfr_id=info%3Asid%2Fen.wikipedia.org%3AExothermic+process" class="Z3988"></span></span> </li> <li id="cite_note-16"><span class="mw-cite-backlink"><b><a href="#cite_ref-16">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.chemicool.com/examples/spontaneous-endothermic-reactions.html#:~:text=Hence%20reactions%20are%20spontaneous%20only,in%20free%20energy,%20is%20negative.&text=Exothermic%20reactions%20have%20negative%20values,with%20positive%20values%20of%20%CE%94H.">"Examples of Spontaneous Endothermic Reactions - Chemistry Examples"</a>. <i>www.chemicool.com</i><span class="reference-accessdate">. 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