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<span>Toggle Gay-Lussac's law subsection</span> </button> <ul id="toc-Gay-Lussac's_law-sublist" class="vector-toc-list"> <li id="toc-Statement_3" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Statement_3"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.1</span> <span>Statement</span> </div> </a> <ul id="toc-Statement_3-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Avogadro's_law" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Avogadro's_law"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Avogadro's law</span> </div> </a> <button aria-controls="toc-Avogadro's_law-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Avogadro's law subsection</span> </button> <ul id="toc-Avogadro's_law-sublist" class="vector-toc-list"> <li id="toc-Statement_4" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Statement_4"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.1</span> <span>Statement</span> </div> </a> <ul id="toc-Statement_4-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Combined_and_ideal_gas_laws" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Combined_and_ideal_gas_laws"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Combined and ideal gas laws</span> </div> </a> <ul id="toc-Combined_and_ideal_gas_laws-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_gas_laws" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Other_gas_laws"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>Other gas laws</span> </div> </a> <ul id="toc-Other_gas_laws-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>References</span> </div> </a> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>External links</span> </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" 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<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. Available in 30 languages" > <label id="p-lang-btn-label" for="p-lang-btn-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--action-progressive mw-portlet-lang-heading-30" aria-hidden="true" ><span class="vector-icon mw-ui-icon-language-progressive mw-ui-icon-wikimedia-language-progressive"></span> <span class="vector-dropdown-label-text">30 languages</span> </label> <div class="vector-dropdown-content"> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li class="interlanguage-link interwiki-am mw-list-item"><a href="https://am.wikipedia.org/wiki/%E1%8B%A8%E1%8A%A0%E1%8B%A8%E1%88%AD_%E1%88%85%E1%8C%8D%E1%8C%8B%E1%89%B5" title="የአየር ህግጋት – Amharic" lang="am" hreflang="am" data-title="የአየር ህግጋት" data-language-autonym="አማርኛ" data-language-local-name="Amharic" class="interlanguage-link-target"><span>አማርኛ</span></a></li><li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D9%82%D9%88%D8%A7%D9%86%D9%8A%D9%86_%D8%A7%D9%84%D8%BA%D8%A7%D8%B2%D8%A7%D8%AA" title="قوانين الغازات – Arabic" lang="ar" hreflang="ar" data-title="قوانين الغازات" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%97%E0%A7%8D%E0%A6%AF%E0%A6%BE%E0%A6%B8_%E0%A6%B8%E0%A7%82%E0%A6%A4%E0%A7%8D%E0%A6%B0%E0%A6%B8%E0%A6%AE%E0%A7%82%E0%A6%B9" title="গ্যাস সূত্রসমূহ – Bangla" lang="bn" hreflang="bn" data-title="গ্যাস সূত্রসমূহ" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target"><span>বাংলা</span></a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%93%D0%B0%D0%B7%D0%B0%D0%B2%D1%8B%D1%8F_%D0%B7%D0%B0%D0%BA%D0%BE%D0%BD%D1%8B" title="Газавыя законы – Belarusian" lang="be" hreflang="be" data-title="Газавыя законы" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target"><span>Беларуская</span></a></li><li class="interlanguage-link interwiki-be-x-old mw-list-item"><a href="https://be-tarask.wikipedia.org/wiki/%D0%93%D0%B0%D0%B7%D0%B0%D0%B2%D1%8B%D1%8F_%D0%B7%D0%B0%D0%BA%D0%BE%D0%BD%D1%8B" title="Газавыя законы – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Газавыя законы" data-language-autonym="Беларуская (тарашкевіца)" data-language-local-name="Belarusian (Taraškievica orthography)" class="interlanguage-link-target"><span>Беларуская (тарашкевіца)</span></a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Plinski_zakoni" title="Plinski zakoni – Bosnian" lang="bs" hreflang="bs" data-title="Plinski zakoni" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target"><span>Bosanski</span></a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Lleis_dels_gasos" title="Lleis dels gasos – Catalan" lang="ca" hreflang="ca" data-title="Lleis dels gasos" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target"><span>Català</span></a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Gasgesetze" title="Gasgesetze – German" lang="de" hreflang="de" data-title="Gasgesetze" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target"><span>Deutsch</span></a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%9D%CF%8C%CE%BC%CE%BF%CE%B9_%CF%84%CF%89%CE%BD_%CE%B1%CE%B5%CF%81%CE%AF%CF%89%CE%BD" title="Νόμοι των αερίων – Greek" lang="el" hreflang="el" data-title="Νόμοι των αερίων" 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/Leyes_de_los_gases" title="Leyes de los gases – Spanish" lang="es" hreflang="es" data-title="Leyes de los gases" 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%82%D9%88%D8%A7%D9%86%DB%8C%D9%86_%DA%AF%D8%A7%D8%B2" title="قوانین گاز – Persian" lang="fa" hreflang="fa" data-title="قوانین گاز" 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/G%C3%A1sdl%C3%ADthe" title="Gásdlíthe – Irish" lang="ga" hreflang="ga" data-title="Gásdlíthe" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target"><span>Gaeilge</span></a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EA%B8%B0%EC%B2%B4_%EB%B2%95%EC%B9%99" title="기체 법칙 – Korean" lang="ko" hreflang="ko" data-title="기체 법칙" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target"><span>한국어</span></a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%97%E0%A5%88%E0%A4%B8%E0%A5%8B%E0%A4%82_%E0%A4%95%E0%A5%87_%E0%A4%A8%E0%A4%BF%E0%A4%AF%E0%A4%AE" title="गैसों के नियम – Hindi" lang="hi" hreflang="hi" data-title="गैसों के नियम" 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/Plinski_zakoni" title="Plinski zakoni – Croatian" lang="hr" hreflang="hr" data-title="Plinski zakoni" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Hukum-hukum_gas" title="Hukum-hukum gas – Indonesian" lang="id" hreflang="id" data-title="Hukum-hukum gas" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target"><span>Bahasa Indonesia</span></a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/G%C3%A1zt%C3%B6rv%C3%A9ny" title="Gáztörvény – Hungarian" lang="hu" hreflang="hu" data-title="Gáztörvény" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target"><span>Magyar</span></a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%B5%E0%B4%BE%E0%B4%A4%E0%B4%95_%E0%B4%A8%E0%B4%BF%E0%B4%AF%E0%B4%AE%E0%B4%99%E0%B5%8D%E0%B4%99%E0%B5%BE" title="വാതക നിയമങ്ങൾ – Malayalam" lang="ml" hreflang="ml" data-title="വാതക നിയമങ്ങൾ" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target"><span>മലയാളം</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Leis_dos_gases" title="Leis dos gases – Portuguese" lang="pt" hreflang="pt" data-title="Leis dos gases" 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/Legile_gazelor" title="Legile gazelor – Romanian" lang="ro" hreflang="ro" data-title="Legile gazelor" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B7%80%E0%B7%8F%E0%B6%BA%E0%B7%94_%E0%B6%B1%E0%B7%92%E0%B6%BA%E0%B6%B8" title="වායු නියම – Sinhala" lang="si" hreflang="si" data-title="වායු නියම" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target"><span>සිංහල</span></a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/Plinski_zakoni" title="Plinski zakoni – Slovenian" lang="sl" hreflang="sl" data-title="Plinski zakoni" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target"><span>Slovenščina</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/Gasni_zakoni" title="Gasni zakoni – Serbian" lang="sr" hreflang="sr" data-title="Gasni zakoni" 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-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Plinski_zakoni" title="Plinski zakoni – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Plinski zakoni" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target"><span>Srpskohrvatski / српскохрватски</span></a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%B5%E0%AE%B3%E0%AE%BF%E0%AE%AE_%E0%AE%B5%E0%AE%BF%E0%AE%A4%E0%AE%BF%E0%AE%95%E0%AE%B3%E0%AF%8D" title="வளிம விதிகள் – Tamil" lang="ta" hreflang="ta" data-title="வளிம விதிகள்" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target"><span>தமிழ்</span></a></li><li class="interlanguage-link interwiki-te mw-list-item"><a href="https://te.wikipedia.org/wiki/%E0%B0%B5%E0%B0%BE%E0%B0%AF%E0%B1%81_%E0%B0%A8%E0%B0%BF%E0%B0%AF%E0%B0%AE%E0%B0%BE%E0%B0%B2%E0%B1%81" title="వాయు నియమాలు – Telugu" lang="te" hreflang="te" data-title="వాయు నియమాలు" data-language-autonym="తెలుగు" data-language-local-name="Telugu" class="interlanguage-link-target"><span>తెలుగు</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%81%E0%B8%8E%E0%B8%82%E0%B8%AD%E0%B8%87%E0%B9%81%E0%B8%81%E0%B9%8A%E0%B8%AA" title="กฎของแก๊ส – Thai" lang="th" hreflang="th" data-title="กฎของแก๊ส" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target"><span>ไทย</span></a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/Gaz_yasalar%C4%B1" title="Gaz yasaları – Turkish" lang="tr" hreflang="tr" data-title="Gaz yasaları" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target"><span>Türkçe</span></a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%93%D0%B0%D0%B7%D0%BE%D0%B2%D1%96_%D0%B7%D0%B0%D0%BA%D0%BE%D0%BD%D0%B8" title="Газові закони – Ukrainian" lang="uk" hreflang="uk" data-title="Газові закони" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target"><span>Українська</span></a></li><li class="interlanguage-link interwiki-ur mw-list-item"><a href="https://ur.wikipedia.org/wiki/%DA%AF%DB%8C%D8%B3_%DA%A9%DB%92_%D9%82%D9%88%D8%A7%D9%86%DB%8C%D9%86" title="گیس کے قوانین – Urdu" lang="ur" hreflang="ur" data-title="گیس کے قوانین" data-language-autonym="اردو" data-language-local-name="Urdu" class="interlanguage-link-target"><span>اردو</span></a></li> </ul> <div class="after-portlet after-portlet-lang"><span class="wb-langlinks-edit wb-langlinks-link"><a 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<div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">List of physical laws relates to gases</div><style data-mw-deduplicate="TemplateStyles:r1251242444">.mw-parser-output .ambox{border:1px solid #a2a9b1;border-left:10px solid #36c;background-color:#fbfbfb;box-sizing:border-box}.mw-parser-output .ambox+link+.ambox,.mw-parser-output .ambox+link+style+.ambox,.mw-parser-output .ambox+link+link+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+style+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+link+.ambox{margin-top:-1px}html body.mediawiki .mw-parser-output .ambox.mbox-small-left{margin:4px 1em 4px 0;overflow:hidden;width:238px;border-collapse:collapse;font-size:88%;line-height:1.25em}.mw-parser-output .ambox-speedy{border-left:10px solid #b32424;background-color:#fee7e6}.mw-parser-output .ambox-delete{border-left:10px solid #b32424}.mw-parser-output .ambox-content{border-left:10px solid #f28500}.mw-parser-output .ambox-style{border-left:10px solid #fc3}.mw-parser-output .ambox-move{border-left:10px solid #9932cc}.mw-parser-output .ambox-protection{border-left:10px solid #a2a9b1}.mw-parser-output .ambox .mbox-text{border:none;padding:0.25em 0.5em;width:100%}.mw-parser-output .ambox .mbox-image{border:none;padding:2px 0 2px 0.5em;text-align:center}.mw-parser-output .ambox .mbox-imageright{border:none;padding:2px 0.5em 2px 0;text-align:center}.mw-parser-output .ambox .mbox-empty-cell{border:none;padding:0;width:1px}.mw-parser-output .ambox .mbox-image-div{width:52px}@media(min-width:720px){.mw-parser-output .ambox{margin:0 10%}}@media print{body.ns-0 .mw-parser-output .ambox{display:none!important}}</style><table class="box-More_citations_needed plainlinks metadata ambox ambox-content ambox-Refimprove" role="presentation"><tbody><tr><td class="mbox-image"><div class="mbox-image-div"><span typeof="mw:File"><a href="/wiki/File:Question_book-new.svg" class="mw-file-description"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/50px-Question_book-new.svg.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/75px-Question_book-new.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/100px-Question_book-new.svg.png 2x" data-file-width="512" data-file-height="399" /></a></span></div></td><td class="mbox-text"><div class="mbox-text-span">This article <b>needs additional citations for <a href="/wiki/Wikipedia:Verifiability" title="Wikipedia:Verifiability">verification</a></b>.<span class="hide-when-compact"> Please help <a href="/wiki/Special:EditPage/Gas_laws" title="Special:EditPage/Gas laws">improve this article</a> by <a href="/wiki/Help:Referencing_for_beginners" title="Help:Referencing for beginners">adding citations to reliable sources</a>. Unsourced material may be challenged and removed.<br /><small><span class="plainlinks"><i>Find sources:</i> <a rel="nofollow" class="external text" href="https://www.google.com/search?as_eq=wikipedia&q=%22Gas+laws%22">"Gas laws"</a> – <a rel="nofollow" class="external text" href="https://www.google.com/search?tbm=nws&q=%22Gas+laws%22+-wikipedia&tbs=ar:1">news</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?&q=%22Gas+laws%22&tbs=bkt:s&tbm=bks">newspapers</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?tbs=bks:1&q=%22Gas+laws%22+-wikipedia">books</a> <b>·</b> <a rel="nofollow" class="external text" href="https://scholar.google.com/scholar?q=%22Gas+laws%22">scholar</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.jstor.org/action/doBasicSearch?Query=%22Gas+laws%22&acc=on&wc=on">JSTOR</a></span></small></span> <span class="date-container"><i>(<span class="date">September 2024</span>)</i></span><span class="hide-when-compact"><i> (<small><a href="/wiki/Help:Maintenance_template_removal" title="Help:Maintenance template removal">Learn how and when to remove this message</a></small>)</i></span></div></td></tr></tbody></table><style 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">This article outlines the historical development of the laws describing ideal gases. For a detailed description of the ideal gas laws and their further development, see <a href="/wiki/Ideal_gas_law" title="Ideal gas law">ideal gas law</a>.</div> <p>The laws describing the behaviour of <a href="/wiki/Gas" title="Gas">gases</a> under fixed <a href="/wiki/Pressure" title="Pressure">pressure</a>, <a href="/wiki/Volume" title="Volume">volume</a>, amount of gas, and <a href="/wiki/Thermodynamic_temperature" title="Thermodynamic temperature">absolute</a> <a href="/wiki/Temperature" title="Temperature">temperature</a> conditions are called <b>gas laws</b>. The basic gas laws were discovered by the end of the 18th century when scientists found out that relationships between pressure, volume and temperature of a sample of gas could be obtained which would hold to approximation for all gases. The combination of several empirical gas laws led to the development of the <a href="/wiki/Ideal_gas_law" title="Ideal gas law">ideal gas law</a>. </p><p>The ideal gas law was later found to be consistent with <a href="/wiki/Atomic_theory" class="mw-redirect" title="Atomic theory">atomic</a> and <a href="/wiki/Kinetic_theory_of_gases" title="Kinetic theory of gases">kinetic theory</a>. </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="History">History</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=1" title="Edit section: History"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1251242444"><table class="box-Expand_section plainlinks metadata ambox mbox-small-left ambox-content" role="presentation"><tbody><tr><td class="mbox-image"><span typeof="mw:File"><a href="/wiki/File:Wiki_letter_w_cropped.svg" class="mw-file-description"><img alt="[icon]" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/20px-Wiki_letter_w_cropped.svg.png" decoding="async" width="20" height="14" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/30px-Wiki_letter_w_cropped.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/40px-Wiki_letter_w_cropped.svg.png 2x" data-file-width="44" data-file-height="31" /></a></span></td><td class="mbox-text"><div class="mbox-text-span">This section <b>needs expansion</b>. You can help by <a class="external text" href="https://en.wikipedia.org/w/index.php?title=Gas_laws&action=edit&section=">adding to it</a>. <span class="date-container"><i>(<span class="date">July 2023</span>)</i></span></div></td></tr></tbody></table> <p>In 1643, the Italian physicist and mathematician, <a href="/wiki/Evangelista_Torricelli" title="Evangelista Torricelli">Evangelista Torricelli</a>, who for a few months had acted as <a href="/wiki/Galileo_Galilei" title="Galileo Galilei">Galileo Galileo's</a> secretary, conducted a celebrated experiment in Florence.<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> He demonstrated that a column of mercury in an inverted tube can be supported by the pressure of air outside of the tube, with the creation of a small section of vacuum above the mercury.<sup id="cite_ref-2" class="reference"><a href="#cite_note-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> This experiment essentially paved the way towards the invention of the barometer, as well as drawing the attention of <a href="/wiki/Robert_Boyle" title="Robert Boyle">Robert Boyle</a>, then a "skeptical" scientist working in England. Boyle was inspired by Torricelli's experiment to investigate how the elasticity of air responds to varying pressure, and he did this through a series of experiments with a setup reminiscent of that used by Torricelli.<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> Boyle published his results in 1662. </p><p>Later on, in 1676, the French physicist <a href="/wiki/Edme_Mariotte" title="Edme Mariotte">Edme Mariotte</a>, independently arrived at the same conclusions of Boyle, while also noting some dependency of air volume on temperature.<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> However it took another century and a half for the development of thermometry and recognition of the absolute zero temperature scale, which eventually allowed the discovery of temperature-dependent gas laws. </p> <div class="mw-heading mw-heading2"><h2 id="Boyle's_law"><span id="Boyle.27s_law"></span>Boyle's law</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=2" title="Edit section: Boyle's law"><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/Boyle%27s_law" title="Boyle's law">Boyle's law</a></div> <p>In 1662, Robert Boyle systematically studied the relationship between the volume and pressure of a fixed amount of gas at a constant temperature. He observed that the volume of a given mass of a gas is inversely proportional to its pressure at a constant temperature. Boyle's law, published in 1662, states that, at a constant temperature, the product of the pressure and volume of a given mass of an <a href="/wiki/Ideal_gas" title="Ideal gas">ideal gas</a> in a <a href="/wiki/Closed_system" title="Closed system">closed system</a> is always constant. It can be verified experimentally using a <a href="/wiki/Pressure_measurement" title="Pressure measurement">pressure gauge</a> and a variable volume container. It can also be derived from the <a href="/wiki/Kinetic_theory_of_gases" title="Kinetic theory of gases">kinetic theory of gases</a>: if a container, with a fixed number of <a href="/wiki/Molecule" title="Molecule">molecules</a> inside, is reduced in volume, more molecules will strike a given area of the sides of the container per unit time, causing a greater pressure. </p> <div class="mw-heading mw-heading3"><h3 id="Statement">Statement</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=3" title="Edit section: Statement"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Boyle's law states that: </p> <style data-mw-deduplicate="TemplateStyles:r996643573">.mw-parser-output .block-indent{padding-left:3em;padding-right:0;overflow:hidden}</style><div class="block-indent">The volume of a given mass of a gas is inversely related to its pressure when its temperature is kept constant.</div> <p>The concept can be represented with these formulae: </p> <ul><li><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 V\propto {\frac {1}{P}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>V</mi> <mo>∝</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mn>1</mn> <mi>P</mi> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle V\propto {\frac {1}{P}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/af5d27fb746798dd4fcbd49c72bd41c496b7a32b" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.838ex; width:7.467ex; height:5.176ex;" alt="{\displaystyle V\propto {\frac {1}{P}}}"></span>, meaning "Volume is inversely proportional to Pressure", or</li> <li><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 P\propto {\frac {1}{V}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mo>∝</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mn>1</mn> <mi>V</mi> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle P\propto {\frac {1}{V}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/36e185ae17420ddc45220bfc1572201e27f4131d" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.005ex; width:7.467ex; height:5.343ex;" alt="{\displaystyle P\propto {\frac {1}{V}}}"></span>, meaning "Pressure is inversely proportional to Volume", or</li> <li><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 PV=k_{1}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mi>V</mi> <mo>=</mo> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle PV=k_{1}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/376a5d33d1cb214ee04947f322227db1653138e2" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:8.897ex; height:2.509ex;" alt="{\displaystyle PV=k_{1}}"></span>, or</li></ul> <p><span class="mwe-math-element"><span class="mwe-math-mathml-display mwe-math-mathml-a11y" style="display: none;"><math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle P_{1}V_{1}=P_{2}V_{2}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <mo>=</mo> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle P_{1}V_{1}=P_{2}V_{2}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/522e50ea8f8539521eff96ee2eafe2f36872e79a" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:13.01ex; height:2.509ex;" alt="{\displaystyle P_{1}V_{1}=P_{2}V_{2}}"></span> where <span class="texhtml mvar" style="font-style:italic;">P</span> is the pressure, <span class="texhtml mvar" style="font-style:italic;">V</span> is the volume of a gas, and <span class="texhtml"><i>k</i><sub>1</sub></span> is the constant in this equation (and is not the same as the proportionality constants in the other equations). </p> <div class="mw-heading mw-heading2"><h2 id="Charles'_law"><span id="Charles.27_law"></span>Charles' law</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=4" title="Edit section: Charles' law"><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/Charles%27s_law" title="Charles's law">Charles's law</a></div> <p>Charles' law, or the law of volumes, was founded in 1787 by <a href="/wiki/Jacques_Charles" title="Jacques Charles">Jacques Charles</a>. It states that, for a given <a href="/wiki/Mass" title="Mass">mass</a> of an ideal gas at constant pressure, the volume is directly proportional to its <a href="/wiki/Absolute_temperature" class="mw-redirect" title="Absolute temperature">absolute temperature</a>, assuming in a closed system. The statement of Charles' law is as follows: the volume (V) of a given mass of a gas, at constant pressure (P), is directly proportional to its temperature (T). </p> <div class="mw-heading mw-heading3"><h3 id="Statement_2">Statement</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=5" title="Edit section: Statement"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Charles' law states that: </p> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">The volume of a given fixed mass of a dry gas is directly proportional to its absolute temperature at a constant pressure.</div> <p>Therefore, </p> <ul><li><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 V\propto T\,}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>V</mi> <mo>∝</mo> <mi>T</mi> <mspace width="thinmathspace" /> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle V\propto T\,}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/ba41100b3b1a370ee263b55d29724ac88eaa3556" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:6.909ex; height:2.176ex;" alt="{\displaystyle V\propto T\,}"></span>, or</li> <li><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 {V \over T}=k_{2}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mi>V</mi> <mi>T</mi> </mfrac> </mrow> <mo>=</mo> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {V \over T}=k_{2}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/af3d96a4fa90f1581fe82a68ce6d9cd7baca0b36" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.838ex; width:7.987ex; height:5.176ex;" alt="{\displaystyle {V \over T}=k_{2}}"></span>, or</li></ul> <dl><dd><span class="mwe-math-element"><span class="mwe-math-mathml-display mwe-math-mathml-a11y" style="display: none;"><math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {V_{1} \over T_{1}}={V_{2} \over T_{2}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mfrac> </mrow> <mo>=</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {V_{1} \over T_{1}}={V_{2} \over T_{2}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/48b9aa62634216f32e702c039215ae9fbf8d7bad" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:9.594ex; height:5.509ex;" alt="{\displaystyle {V_{1} \over T_{1}}={V_{2} \over T_{2}}}"></span>,</dd></dl> <p><br /> where <i>"V"</i> is the volume of a gas, <i>"T"</i> is the absolute temperature and <i>k</i><sub>2</sub> is a proportionality constant (which is not the same as the proportionality constants in the other equations in this article). </p> <div class="mw-heading mw-heading2"><h2 id="Gay-Lussac's_law"><span id="Gay-Lussac.27s_law"></span>Gay-Lussac's law</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=6" title="Edit section: Gay-Lussac's law"><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/Gay-Lussac%27s_law" title="Gay-Lussac's law">Gay-Lussac's law</a></div> <p>Gay-Lussac's law, Amontons' law or the pressure law was founded by <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Joseph Louis Gay-Lussac</a> in 1808. </p> <div class="mw-heading mw-heading3"><h3 id="Statement_3">Statement</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=7" title="Edit section: Statement"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Gay-Lussac's law states that: </p> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">The pressure exerted by a given mass and constant volume of an ideal gas on the sides of its container is directly proportional to its absolute temperature.</div> <p>Therefore, </p> <ul><li><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 P\propto T\,}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mo>∝</mo> <mi>T</mi> <mspace width="thinmathspace" /> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle P\propto T\,}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/7f50857abc967ce5bf7c01c2acba5b708efb9fa3" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:6.867ex; height:2.176ex;" alt="{\displaystyle P\propto T\,}"></span>, or</li> <li><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 {P \over T}=k}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mi>P</mi> <mi>T</mi> </mfrac> </mrow> <mo>=</mo> <mi>k</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {P \over T}=k}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/c5bd649d1d43a2da546160cdbc496c59209f3a1c" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.838ex; width:6.891ex; height:5.176ex;" alt="{\displaystyle {P \over T}=k}"></span>, or</li></ul> <p><span class="mwe-math-element"><span class="mwe-math-mathml-display mwe-math-mathml-a11y" style="display: none;"><math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {P_{1} \over T_{1}}={P_{2} \over T_{2}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mfrac> </mrow> <mo>=</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {P_{1} \over T_{1}}={P_{2} \over T_{2}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/825980041e94f1a9b4fe5f8c7721643a16658a0b" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:9.864ex; height:5.509ex;" alt="{\displaystyle {P_{1} \over T_{1}}={P_{2} \over T_{2}}}"></span>, </p> <dl><dd>where <i>P</i> is the pressure, <i>T</i> is the absolute temperature, and <i>k</i> is another proportionality constant.</dd></dl> <div class="mw-heading mw-heading2"><h2 id="Avogadro's_law"><span id="Avogadro.27s_law"></span>Avogadro's law</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=8" title="Edit section: Avogadro's law"><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/Avogadro%27s_law" title="Avogadro's law">Avogadro's law</a></div> <p><b>Avogadro's law</b>, <b>Avogadro's hypothesis</b>, <b>Avogadro's principle</b> or <b>Avogadro-Ampère's hypothesis</b> is an experimental gas law which was hypothesized by <a href="/wiki/Amedeo_Avogadro" title="Amedeo Avogadro">Amedeo Avogadro</a> in 1811. It related the volume of a gas to the <a href="/wiki/Amount_of_substance" title="Amount of substance">amount of substance</a> of gas present.<sup id="cite_ref-Britannica_5-0" class="reference"><a href="#cite_note-Britannica-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Statement_4">Statement</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=9" title="Edit section: Statement"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Avogadro's law states that: </p> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">The volume occupied by an ideal gas at a constant temperature is directly proportional to the number of molecules of the gas present in the container.</div> <p>This statement gives rise to the <a href="/wiki/Molar_volume" title="Molar volume">molar volume</a> of a gas, which at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">STP</a> (273.15 K, 1 atm) is about 22.4 L. The relation is given 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 V\propto n\,}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>V</mi> <mo>∝</mo> <mi>n</mi> <mspace width="thinmathspace" /> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle V\propto n\,}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/c9f99343e99cb03010c68a0e77de2c9117c928e0" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:6.668ex; height:2.176ex;" alt="{\displaystyle V\propto n\,}"></span>, or<span class="mwe-math-element"><span class="mwe-math-mathml-display mwe-math-mathml-a11y" style="display: none;"><math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\frac {V_{1}}{n_{1}}}={\frac {V_{2}}{n_{2}}}\,}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <msub> <mi>n</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mfrac> </mrow> <mo>=</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <msub> <mi>n</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mfrac> </mrow> <mspace width="thinmathspace" /> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\frac {V_{1}}{n_{1}}}={\frac {V_{2}}{n_{2}}}\,}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/50f9d9fb325e1bd777e27d253691e02d6940d963" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:10.056ex; height:5.509ex;" alt="{\displaystyle {\frac {V_{1}}{n_{1}}}={\frac {V_{2}}{n_{2}}}\,}"></span>where <i>n</i> is equal to the number of molecules of gas (or the number of moles of gas).</dd></dl> <div class="mw-heading mw-heading2"><h2 id="Combined_and_ideal_gas_laws">Combined and ideal gas laws</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=10" title="Edit section: Combined and ideal gas laws"><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/Ideal_gas_law" title="Ideal gas law">Ideal gas law</a></div> <figure typeof="mw:File/Thumb"><a href="/wiki/File:Ideal_gas_law_relationships.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/62/Ideal_gas_law_relationships.svg/200px-Ideal_gas_law_relationships.svg.png" decoding="async" width="200" height="133" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/62/Ideal_gas_law_relationships.svg/300px-Ideal_gas_law_relationships.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/62/Ideal_gas_law_relationships.svg/400px-Ideal_gas_law_relationships.svg.png 2x" data-file-width="512" data-file-height="341" /></a><figcaption>Relationships between <a href="/wiki/Boyle%27s_law" title="Boyle's law">Boyle's</a>, <a href="/wiki/Charles%27s_law" title="Charles's law">Charles's</a>, <a href="/wiki/Gay-Lussac%27s_law" title="Gay-Lussac's law">Gay-Lussac's</a>, <a href="/wiki/Avogadro%27s_law" title="Avogadro's law">Avogadro's</a>, <a href="/wiki/Combined_gas_law" class="mw-redirect" title="Combined gas law">combined</a> and <span class="nowrap"><a href="/wiki/Ideal_gas_law" title="Ideal gas law">ideal gas laws</a></span>, with the <a href="/wiki/Boltzmann_constant" title="Boltzmann constant">Boltzmann constant</a> <span class="texhtml"><var style="padding-right: 1px;">k</var><sub><var style="padding-right: 1px;"></var></sub> = <style data-mw-deduplicate="TemplateStyles:r1214402035">.mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num{display:block;line-height:1em;margin:0.0em 0.1em;border-bottom:1px solid}.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0.1em 0.1em}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style><span class="sfrac">⁠<span class="tion"><span class="num"><var style="padding-right: 1px;">R</var></span><span class="sr-only">/</span><span class="den"><var style="padding-right: 1px;">N</var><sub><var style="padding-right: 1px;">A</var></sub></span></span>⁠</span> = <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035"><span class="sfrac">⁠<span class="tion"><span class="num"><var style="padding-right: 1px;">n</var> <var style="padding-right: 1px;">R</var></span><span class="sr-only">/</span><span class="den"><var style="padding-right: 1px;">N</var></span></span>⁠</span></span> (in each law, <a href="/wiki/Physical_property" title="Physical property">properties</a> circled are variable and properties not circled are held constant)</figcaption></figure> <p>The <a href="/wiki/Combined_gas_law" class="mw-redirect" title="Combined gas law">combined gas law</a> or general gas equation is obtained by combining Boyle's law, Charles's law, and Gay-Lussac's law. It shows the relationship between the pressure, volume, and temperature for a fixed mass of gas: </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 PV=k_{5}T}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mi>V</mi> <mo>=</mo> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>5</mn> </mrow> </msub> <mi>T</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle PV=k_{5}T}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/9cf2a30cd6b1bd93ebabac67f9c54c029d799242" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:10.533ex; height:2.509ex;" alt="{\displaystyle PV=k_{5}T}"></span></dd></dl> <p>This can also be written as: </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 {\frac {P_{1}V_{1}}{T_{1}}}={\frac {P_{2}V_{2}}{T_{2}}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mrow> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> </mfrac> </mrow> <mo>=</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mrow> <msub> <mi>T</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mfrac> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\frac {P_{1}V_{1}}{T_{1}}}={\frac {P_{2}V_{2}}{T_{2}}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/171a1e95810f86795f3393fdd717a7eb1925fb67" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:14.683ex; height:5.509ex;" alt="{\displaystyle {\frac {P_{1}V_{1}}{T_{1}}}={\frac {P_{2}V_{2}}{T_{2}}}}"></span></dd></dl> <p>With the addition of <a href="/wiki/Avogadro%27s_law" title="Avogadro's law">Avogadro's law</a>, the <a href="/wiki/Combined_gas_law" class="mw-redirect" title="Combined gas law">combined gas law</a> develops into the <a href="/wiki/Ideal_gas_law" title="Ideal gas law">ideal gas law</a>: </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 PV=nRT}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mi>V</mi> <mo>=</mo> <mi>n</mi> <mi>R</mi> <mi>T</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle PV=nRT}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/934032db2ac1f12624f85a90eeba651dcf4af377" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:11.426ex; height:2.176ex;" alt="{\displaystyle PV=nRT}"></span></dd> <dd>where <i>P</i> is the pressure, <i>V</i> is volume, <i>n</i> is the number of moles, <i>R</i> is the universal gas constant and <i>T</i> is the absolute temperature.</dd> <dd>The proportionality constant, now named R, is the <a href="/wiki/Universal_gas_constant" class="mw-redirect" title="Universal gas constant">universal gas constant</a> with a value of 8.3144598 (kPa∙L)/(mol∙K).</dd></dl> <p>An equivalent formulation of this law is: </p> <dl><dd><span class="mwe-math-element"><span class="mwe-math-mathml-display mwe-math-mathml-a11y" style="display: none;"><math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle PV=Nk_{\text{B}}T}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>P</mi> <mi>V</mi> <mo>=</mo> <mi>N</mi> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mtext>B</mtext> </mrow> </msub> <mi>T</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle PV=Nk_{\text{B}}T}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/87c1466fa2e15cc9d0dc7362c34835e18026296c" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:12.938ex; height:2.509ex;" alt="{\displaystyle PV=Nk_{\text{B}}T}"></span></dd> <dd>where <i>P</i> is the pressure, <i>V</i> is the volume, <i>N</i> is the number of gas molecules, <i>k</i><sub>B</sub> is the <a href="/wiki/Boltzmann_constant" title="Boltzmann constant">Boltzmann constant</a> (1.381×10<sup>−23</sup>J·K<sup>−1</sup> in SI units) and T is the absolute temperature.</dd></dl> <p>These equations are exact only for an <a href="/wiki/Ideal_gas" title="Ideal gas">ideal gas</a>, which neglects various intermolecular effects (see <a href="/wiki/Real_gas" title="Real gas">real gas</a>). However, the ideal gas law is a good approximation for most gases under moderate pressure and temperature. </p><p>This law has the following important consequences: </p> <ol><li>If temperature and pressure are kept constant, then the volume of the gas is directly proportional to the number of molecules of gas.</li> <li>If the temperature and volume remain constant, then the pressure of the gas changes is directly proportional to the number of molecules of gas present.</li> <li>If the number of gas molecules and the temperature remain constant, then the pressure is inversely proportional to the volume.</li> <li>If the temperature changes and the number of gas molecules are kept constant, then either pressure or volume (or both) will change in direct proportion to the temperature.</li></ol> <div class="mw-heading mw-heading2"><h2 id="Other_gas_laws">Other gas laws</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=11" title="Edit section: Other gas laws"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <dl><dt><a href="/wiki/Graham%27s_law" title="Graham's law">Graham's law</a></dt> <dd>This law states that the rate at which gas molecules <a href="/wiki/Diffusion" title="Diffusion">diffuse</a> is inversely proportional to the square root of the gas density at a constant temperature. Combined with Avogadro's law (i.e. since equal volumes have an equal number of molecules) this is the same as being inversely proportional to the root of the molecular weight.</dd> <dt><a href="/wiki/Dalton%27s_law" title="Dalton's law">Dalton's law</a> of <a href="/wiki/Partial_pressure" title="Partial pressure">partial pressures</a></dt> <dd>This law states that the pressure of a mixture of gases simply is the sum of the <a href="/wiki/Partial_pressures" class="mw-redirect" title="Partial pressures">partial pressures</a> of the individual components. Dalton's law is as follows:</dd> <dd></dd> <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 P_{\textrm {total}}=P_{1}+P_{2}+P_{3}+\cdots +P_{n}\equiv \sum _{i=1}^{n}P_{i},}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext>total</mtext> </mrow> </mrow> </msub> <mo>=</mo> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <mo>+</mo> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>3</mn> </mrow> </msub> <mo>+</mo> <mo>⋯</mo> <mo>+</mo> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> </mrow> </msub> <mo>≡</mo> <munderover> <mo>∑</mo> <mrow class="MJX-TeXAtom-ORD"> <mi>i</mi> <mo>=</mo> <mn>1</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> </mrow> </munderover> <msub> <mi>P</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>i</mi> </mrow> </msub> <mo>,</mo> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle P_{\textrm {total}}=P_{1}+P_{2}+P_{3}+\cdots +P_{n}\equiv \sum _{i=1}^{n}P_{i},}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/407c5750ae8230b72126c4de549ee36b669c91f6" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -3.005ex; width:42.418ex; height:6.843ex;" alt="{\displaystyle P_{\textrm {total}}=P_{1}+P_{2}+P_{3}+\cdots +P_{n}\equiv \sum _{i=1}^{n}P_{i},}"></span></dd> <dd></dd> <dd>and all component gases and the mixture are at the same temperature and volume</dd> <dd>where <i>P</i><sub>total</sub> is the total pressure of the gas mixture</dd> <dd><i>P</i><sub>i</sub> is the partial pressure or pressure of the component gas at the given volume and temperature.</dd> <dd></dd> <dt><a href="/wiki/Amagat%27s_law" title="Amagat's law">Amagat's law</a> of <a href="/wiki/Partial_gas_volume" class="mw-redirect" title="Partial gas volume">partial volumes</a></dt> <dd>This law states that the volume of a mixture of gases (or the volume of the container) simply is the sum of the partial volumes of the individual components. Amagat's law is as follows:</dd> <dd></dd> <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 V_{\textrm {total}}=V_{1}+V_{2}+V_{3}+\cdots +V_{n}\equiv \sum _{i=1}^{n}V_{i},}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext>total</mtext> </mrow> </mrow> </msub> <mo>=</mo> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>1</mn> </mrow> </msub> <mo>+</mo> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>3</mn> </mrow> </msub> <mo>+</mo> <mo>⋯</mo> <mo>+</mo> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> </mrow> </msub> <mo>≡</mo> <munderover> <mo>∑</mo> <mrow class="MJX-TeXAtom-ORD"> <mi>i</mi> <mo>=</mo> <mn>1</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> </mrow> </munderover> <msub> <mi>V</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>i</mi> </mrow> </msub> <mo>,</mo> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle V_{\textrm {total}}=V_{1}+V_{2}+V_{3}+\cdots +V_{n}\equiv \sum _{i=1}^{n}V_{i},}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/3410affea69a855c7f24384942c2f2b89ae753fd" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -3.005ex; width:41.596ex; height:6.843ex;" alt="{\displaystyle V_{\textrm {total}}=V_{1}+V_{2}+V_{3}+\cdots +V_{n}\equiv \sum _{i=1}^{n}V_{i},}"></span></dd> <dd></dd> <dd>and all component gases and the mixture are at the same temperature and pressure</dd> <dd>where <i>V</i><sub>total</sub> is the total volume of the gas mixture or the volume of the container,</dd> <dd><i>V</i><sub>i</sub> is the partial volume, or volume of the component gas at the given pressure and temperature.</dd> <dd></dd> <dt><a href="/wiki/Henry%27s_law" title="Henry's law">Henry's law</a></dt> <dd>This states that at constant temperature, the amount of a given gas dissolved in a given type and volume of liquid is directly proportional to the <a href="/wiki/Partial_pressure" title="Partial pressure">partial pressure</a> of that gas in equilibrium with that liquid. The equation is as follows:</dd> <dd></dd> <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 p=k_{\rm {H}}\,c}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>p</mi> <mo>=</mo> <msub> <mi>k</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="normal">H</mi> </mrow> </mrow> </msub> <mspace width="thinmathspace" /> <mi>c</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle p=k_{\rm {H}}\,c}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/737f69fe6bc0df679796308faa937ba7b68ad7f5" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; margin-left: -0.089ex; width:8.427ex; height:2.509ex;" alt="{\displaystyle p=k_{\rm {H}}\,c}"></span></dd> <dd></dd> <dt><a href="/wiki/Real_gas_law" class="mw-redirect" title="Real gas law">Real gas law</a></dt> <dd>This was formulated by <a href="/wiki/Johannes_Diderik_van_der_Waals" title="Johannes Diderik van der Waals">Johannes Diderik van der Waals</a> in 1873.</dd></dl> <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=Gas_laws&action=edit&section=12" 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"><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"><style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output 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class="citation web cs1">Lagouge, Michel. <a rel="nofollow" class="external text" href="https://lagouge.ecole-alsacienne.org/14-15/cahier_texte_1S/Documents/Doc%20C4/History%20of%20Gas%20Laws.pdf">"History of Gas Laws"</a> <span class="cs1-format">(PDF)</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=History+of+Gas+Laws&rft.aulast=Lagouge&rft.aufirst=Michel&rft_id=https%3A%2F%2Flagouge.ecole-alsacienne.org%2F14-15%2Fcahier_texte_1S%2FDocuments%2FDoc%2520C4%2FHistory%2520of%2520Gas%2520Laws.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></span> </li> <li id="cite_note-2"><span class="mw-cite-backlink"><b><a href="#cite_ref-2">^</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://brunelleschi.imss.fi.it/itineraries/multimedia/TorricellisBarometricExperiment.html#:~:text=Torricelli%20filled%20a%20glass%20tube,height%20of%20around%2076%20cm.">"Torricelli's barometric experiment"</a>. <i>brunelleschi.imss.fi.it</i>. 2008-01-23<span class="reference-accessdate">. Retrieved <span class="nowrap">2024-03-21</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=brunelleschi.imss.fi.it&rft.atitle=Torricelli%27s+barometric+experiment&rft.date=2008-01-23&rft_id=https%3A%2F%2Fbrunelleschi.imss.fi.it%2Fitineraries%2Fmultimedia%2FTorricellisBarometricExperiment.html%23%3A~%3Atext%3DTorricelli%2520filled%2520a%2520glass%2520tube%2Cheight%2520of%2520around%252076%2520cm.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></span> </li> <li id="cite_note-3"><span class="mw-cite-backlink"><b><a href="#cite_ref-3">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFPurdue_University" class="citation web cs1">Purdue University. <a rel="nofollow" class="external text" href="https://chemed.chem.purdue.edu/genchem/topicreview/bp/ch4/gaslaws3.html">"Gas Laws"</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Gas+Laws&rft.au=Purdue+University&rft_id=https%3A%2F%2Fchemed.chem.purdue.edu%2Fgenchem%2Ftopicreview%2Fbp%2Fch4%2Fgaslaws3.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></span> </li> <li id="cite_note-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-4">^</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.britannica.com/biography/Edme-Mariotte">"Edme Mariotte | Experimental Physics, Pressure Law & Hydrostatics | Britannica"</a>. <i>www.britannica.com</i><span class="reference-accessdate">. Retrieved <span class="nowrap">2024-03-21</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=www.britannica.com&rft.atitle=Edme+Mariotte+%7C+Experimental+Physics%2C+Pressure+Law+%26+Hydrostatics+%7C+Britannica&rft_id=https%3A%2F%2Fwww.britannica.com%2Fbiography%2FEdme-Mariotte&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></span> </li> <li id="cite_note-Britannica-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-Britannica_5-0">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation encyclopaedia cs1"><a rel="nofollow" class="external text" href="http://www.britannica.com/science/Avogadros-law">"Avogadro's law"</a>. <i><a href="/wiki/Encyclop%C3%A6dia_Britannica" title="Encyclopædia Britannica">Encyclopædia Britannica</a></i><span class="reference-accessdate">. Retrieved <span class="nowrap">3 February</span> 2016</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Avogadro%27s+law&rft.btitle=Encyclop%C3%A6dia+Britannica&rft_id=http%3A%2F%2Fwww.britannica.com%2Fscience%2FAvogadros-law&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></span> </li> </ol></div></div> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFCastka,_Joseph_F.Metcalfe,_H._ClarkDavis,_Raymond_E.Williams,_John_E.2002" class="citation book cs1">Castka, Joseph F.; Metcalfe, H. Clark; Davis, Raymond E.; Williams, John E. (2002). <i>Modern Chemistry</i>. Holt, Rinehart and Winston. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-03-056537-5" title="Special:BookSources/0-03-056537-5"><bdi>0-03-056537-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Modern+Chemistry&rft.pub=Holt%2C+Rinehart+and+Winston&rft.date=2002&rft.isbn=0-03-056537-5&rft.au=Castka%2C+Joseph+F.&rft.au=Metcalfe%2C+H.+Clark&rft.au=Davis%2C+Raymond+E.&rft.au=Williams%2C+John+E.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGuch,_Ian2003" class="citation book cs1">Guch, Ian (2003). <a rel="nofollow" class="external text" href="https://archive.org/details/completeidiotsgu00guch"><i>The Complete Idiot's Guide to Chemistry</i></a>. Alpha, Penguin Group Inc. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/1-59257-101-8" title="Special:BookSources/1-59257-101-8"><bdi>1-59257-101-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Complete+Idiot%27s+Guide+to+Chemistry&rft.pub=Alpha%2C+Penguin+Group+Inc.&rft.date=2003&rft.isbn=1-59257-101-8&rft.au=Guch%2C+Ian&rft_id=https%3A%2F%2Farchive.org%2Fdetails%2Fcompleteidiotsgu00guch&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFZumdahl,_Steven_S1998" class="citation book cs1">Zumdahl, Steven S (1998). <a rel="nofollow" class="external text" href="https://archive.org/details/chemicalprincipl00zumd_1"><i>Chemical Principles</i></a>. Houghton Mifflin Company. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-395-83995-5" title="Special:BookSources/0-395-83995-5"><bdi>0-395-83995-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemical+Principles&rft.pub=Houghton+Mifflin+Company&rft.date=1998&rft.isbn=0-395-83995-5&rft.au=Zumdahl%2C+Steven+S&rft_id=https%3A%2F%2Farchive.org%2Fdetails%2Fchemicalprincipl00zumd_1&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGas+laws" class="Z3988"></span></li> <li><a rel="nofollow" class="external text" href="https://www.chem.fsu.edu/chemlab/chm1045/gas_laws.html">FSU(Florida State University)</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Gas_laws&action=edit&section=13" title="Edit section: 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