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class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Galvanic_corrosion" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Galvanic_corrosion"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Galvanic corrosion</span> </div> </a> <ul id="toc-Galvanic_corrosion-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Types" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Types"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Types</span> </div> </a> <ul id="toc-Types-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 class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>See also</span> </div> </a> <ul id="toc-See_also-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">6</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">7</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" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" ><span class="vector-icon mw-ui-icon-listBullet mw-ui-icon-wikimedia-listBullet"></span> <span class="vector-dropdown-label-text">Toggle the table of contents</span> </label> <div class="vector-dropdown-content"> <div id="vector-page-titlebar-toc-unpinned-container" class="vector-unpinned-container"> </div> </div> </div> </nav> <h1 id="firstHeading" class="firstHeading mw-first-heading"><span class="mw-page-title-main">Galvanic cell</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. Available in 60 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-60" 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">60 languages</span> </label> <div class="vector-dropdown-content"> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D8%AE%D9%84%D9%8A%D8%A9_%D8%BA%D9%84%D9%81%D8%A7%D9%86%D9%8A%D8%A9" title="خلية غلفانية – Arabic" lang="ar" hreflang="ar" data-title="خلية غلفانية" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/Qalvanik_element" title="Qalvanik element – Azerbaijani" lang="az" hreflang="az" data-title="Qalvanik element" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target"><span>Azərbaycanca</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%B2%E0%A6%AD%E0%A6%BE%E0%A6%A8%E0%A6%BF%E0%A6%95_%E0%A6%95%E0%A7%8B%E0%A6%B7" title="গ্যালভানিক কোষ – Bangla" lang="bn" hreflang="bn" data-title="গ্যালভানিক কোষ" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target"><span>বাংলা</span></a></li><li class="interlanguage-link interwiki-zh-min-nan mw-list-item"><a href="https://zh-min-nan.wikipedia.org/wiki/Galvani_ti%C4%81n-t%C3%AE" title="Galvani tiān-tî – Minnan" lang="nan" hreflang="nan" data-title="Galvani tiān-tî" data-language-autonym="閩南語 / Bân-lâm-gú" data-language-local-name="Minnan" class="interlanguage-link-target"><span>閩南語 / Bân-lâm-gú</span></a></li><li class="interlanguage-link interwiki-ba mw-list-item"><a href="https://ba.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D0%B8%D0%BA_%D1%8D%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Гальваник элемент – Bashkir" lang="ba" hreflang="ba" data-title="Гальваник элемент" data-language-autonym="Башҡортса" data-language-local-name="Bashkir" class="interlanguage-link-target"><span>Башҡортса</span></a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D1%96%D1%87%D0%BD%D1%8B_%D1%8D%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Гальванічны элемент – Belarusian" lang="be" hreflang="be" data-title="Гальванічны элемент" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target"><span>Беларуская</span></a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D0%B2%D0%B0%D0%BD%D0%B8%D1%87%D0%B5%D0%BD_%D0%B5%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Галваничен елемент – Bulgarian" lang="bg" hreflang="bg" data-title="Галваничен елемент" data-language-autonym="Български" data-language-local-name="Bulgarian" class="interlanguage-link-target"><span>Български</span></a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Cel%C2%B7la_galv%C3%A0nica" title="Cel·la galvànica – Catalan" lang="ca" hreflang="ca" data-title="Cel·la galvànica" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target"><span>Català</span></a></li><li class="interlanguage-link interwiki-cv mw-list-item"><a href="https://cv.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D0%B8_%D1%8D%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%87%C4%95" title="Гальвани элеменчĕ – Chuvash" lang="cv" hreflang="cv" data-title="Гальвани элеменчĕ" data-language-autonym="Чӑвашла" data-language-local-name="Chuvash" class="interlanguage-link-target"><span>Чӑвашла</span></a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/Galvanick%C3%BD_%C4%8Dl%C3%A1nek" title="Galvanický článek – Czech" lang="cs" hreflang="cs" data-title="Galvanický článek" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target"><span>Čeština</span></a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Galvanisk_celle" title="Galvanisk celle – Danish" lang="da" hreflang="da" data-title="Galvanisk celle" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target"><span>Dansk</span></a></li><li class="interlanguage-link interwiki-se mw-list-item"><a href="https://se.wikipedia.org/wiki/Galv%C3%A1nala%C5%A1_elemeanta" title="Galvánalaš elemeanta – Northern Sami" lang="se" hreflang="se" data-title="Galvánalaš elemeanta" data-language-autonym="Davvisámegiella" data-language-local-name="Northern Sami" class="interlanguage-link-target"><span>Davvisámegiella</span></a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Galvanische_Zelle" title="Galvanische Zelle – German" lang="de" hreflang="de" data-title="Galvanische Zelle" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target"><span>Deutsch</span></a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Galvaanielement" title="Galvaanielement – Estonian" lang="et" hreflang="et" data-title="Galvaanielement" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target"><span>Eesti</span></a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%93%CE%B1%CE%BB%CE%B2%CE%B1%CE%BD%CE%B9%CE%BA%CF%8C_%CF%83%CF%84%CE%BF%CE%B9%CF%87%CE%B5%CE%AF%CE%BF" title="Γαλβανικό στοιχείο – Greek" lang="el" hreflang="el" data-title="Γαλβανικό στοιχείο" 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/Celda_galv%C3%A1nica" title="Celda galvánica – Spanish" lang="es" hreflang="es" data-title="Celda galvánica" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target"><span>Español</span></a></li><li class="interlanguage-link interwiki-eo mw-list-item"><a href="https://eo.wikipedia.org/wiki/Galvana_pilo" title="Galvana pilo – Esperanto" lang="eo" hreflang="eo" data-title="Galvana pilo" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target"><span>Esperanto</span></a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Zelda_galvanikoa" title="Zelda galvanikoa – Basque" lang="eu" hreflang="eu" data-title="Zelda galvanikoa" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target"><span>Euskara</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D9%BE%DB%8C%D9%84_%DA%AF%D8%A7%D9%84%D9%88%D8%A7%D9%86%DB%8C" title="پیل گالوانی – Persian" lang="fa" hreflang="fa" data-title="پیل گالوانی" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target"><span>فارسی</span></a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Cellule_galvanique" title="Cellule galvanique – French" lang="fr" hreflang="fr" data-title="Cellule galvanique" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EA%B0%88%EB%B0%94%EB%8B%88_%EC%A0%84%EC%A7%80" title="갈바니 전지 – Korean" lang="ko" hreflang="ko" data-title="갈바니 전지" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target"><span>한국어</span></a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%B3%D5%A1%D5%AC%D5%BE%D5%A1%D5%B6%D5%A1%D5%AF%D5%A1%D5%B6_%D5%A7%D5%AC%D5%A5%D5%B4%D5%A5%D5%B6%D5%BF%D5%B6%D5%A5%D6%80" title="Գալվանական էլեմենտներ – Armenian" lang="hy" hreflang="hy" data-title="Գալվանական էլեմենտներ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target"><span>Հայերեն</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%B2%E0%A5%8D%E0%A4%B5%E0%A4%BE%E0%A4%A8%E0%A5%80_%E0%A4%B8%E0%A5%87%E0%A4%B2" title="गैल्वानी सेल – Hindi" lang="hi" hreflang="hi" data-title="गैल्वानी सेल" 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/Galvanski_elementi" title="Galvanski elementi – Croatian" lang="hr" hreflang="hr" data-title="Galvanski elementi" 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/Sel_Galvani" title="Sel Galvani – Indonesian" lang="id" hreflang="id" data-title="Sel Galvani" 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-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Cella_galvanica" title="Cella galvanica – Italian" lang="it" hreflang="it" data-title="Cella galvanica" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target"><span>Italiano</span></a></li><li class="interlanguage-link interwiki-he badge-Q70894304 mw-list-item" title=""><a href="https://he.wikipedia.org/wiki/%D7%AA%D7%90_%D7%92%D7%9C%D7%95%D7%95%D7%A0%D7%99" title="תא גלווני – Hebrew" lang="he" hreflang="he" data-title="תא גלווני" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target"><span>עברית</span></a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%92%E1%83%90%E1%83%9A%E1%83%95%E1%83%90%E1%83%9C%E1%83%A3%E1%83%A0%E1%83%98_%E1%83%94%E1%83%9A%E1%83%94%E1%83%9B%E1%83%94%E1%83%9C%E1%83%A2%E1%83%98" title="გალვანური ელემენტი – Georgian" lang="ka" hreflang="ka" data-title="გალვანური ელემენტი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target"><span>ქართული</span></a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D0%B8%D0%BA%D0%B0%D0%BB%D1%8B%D0%BA_%D1%8D%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82%D1%82%D0%B5%D1%80" title="Гальваникалык элементтер – Kyrgyz" lang="ky" hreflang="ky" data-title="Гальваникалык элементтер" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target"><span>Кыргызча</span></a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Galvaniskais_elements" title="Galvaniskais elements – Latvian" lang="lv" hreflang="lv" data-title="Galvaniskais elements" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target"><span>Latviešu</span></a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Galvaninis_elementas" title="Galvaninis elementas – Lithuanian" lang="lt" hreflang="lt" data-title="Galvaninis elementas" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target"><span>Lietuvių</span></a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Galv%C3%A1nelem" title="Galvánelem – Hungarian" lang="hu" hreflang="hu" data-title="Galvánelem" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target"><span>Magyar</span></a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D0%B2%D0%B0%D0%BD%D1%81%D0%BA%D0%B8_%D0%B5%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Галвански елемент – Macedonian" lang="mk" hreflang="mk" data-title="Галвански елемент" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target"><span>Македонски</span></a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%97%E0%B4%BE%E0%B5%BD%E0%B4%B5%E0%B4%A8%E0%B4%BF%E0%B4%95%E0%B5%8D_%E0%B4%B8%E0%B5%86%E0%B5%BD" title="ഗാൽവനിക് സെൽ – Malayalam" lang="ml" hreflang="ml" data-title="ഗാൽവനിക് സെൽ" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target"><span>മലയാളം</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Galvanisch_element" title="Galvanisch element – Dutch" lang="nl" hreflang="nl" data-title="Galvanisch element" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target"><span>Nederlands</span></a></li><li class="interlanguage-link interwiki-ne mw-list-item"><a href="https://ne.wikipedia.org/wiki/%E0%A4%97%E0%A5%8D%E0%A4%AF%E0%A4%BE%E0%A4%B2%E0%A5%8D%E0%A4%AD%E0%A4%BE%E0%A4%A8%E0%A4%BF%E0%A4%95_%E0%A4%B8%E0%A5%87%E0%A4%B2" title="ग्याल्भानिक सेल – Nepali" lang="ne" hreflang="ne" data-title="ग्याल्भानिक सेल" data-language-autonym="नेपाली" data-language-local-name="Nepali" class="interlanguage-link-target"><span>नेपाली</span></a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E3%82%AC%E3%83%AB%E3%83%90%E3%83%8B%E9%9B%BB%E6%B1%A0" title="ガルバニ電池 – Japanese" lang="ja" hreflang="ja" data-title="ガルバニ電池" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target"><span>日本語</span></a></li><li class="interlanguage-link interwiki-no mw-list-item"><a href="https://no.wikipedia.org/wiki/Galvanisk_element" title="Galvanisk element – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Galvanisk element" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target"><span>Norsk bokmål</span></a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Galvanisk_element" title="Galvanisk element – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Galvanisk element" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target"><span>Norsk nynorsk</span></a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Galvanik_hujayra" title="Galvanik hujayra – Uzbek" lang="uz" hreflang="uz" data-title="Galvanik hujayra" data-language-autonym="Oʻzbekcha / ўзбекча" data-language-local-name="Uzbek" class="interlanguage-link-target"><span>Oʻzbekcha / ўзбекча</span></a></li><li class="interlanguage-link interwiki-pa mw-list-item"><a href="https://pa.wikipedia.org/wiki/%E0%A8%97%E0%A9%88%E0%A8%B2%E0%A8%B5%E0%A9%88%E0%A8%A8%E0%A8%BF%E0%A8%95_%E0%A8%B8%E0%A9%88%E0%A9%B1%E0%A8%B2" title="ਗੈਲਵੈਨਿਕ ਸੈੱਲ – Punjabi" lang="pa" hreflang="pa" data-title="ਗੈਲਵੈਨਿਕ ਸੈੱਲ" data-language-autonym="ਪੰਜਾਬੀ" data-language-local-name="Punjabi" class="interlanguage-link-target"><span>ਪੰਜਾਬੀ</span></a></li><li class="interlanguage-link interwiki-pnb mw-list-item"><a href="https://pnb.wikipedia.org/wiki/%DA%AF%D9%84%D9%88%DB%8C%D9%86%DA%A9_%D8%B3%DB%8C%D9%84" title="گلوینک سیل – Western Punjabi" lang="pnb" hreflang="pnb" data-title="گلوینک سیل" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target"><span>پنجابی</span></a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Ogniwo_galwaniczne" title="Ogniwo galwaniczne – Polish" lang="pl" hreflang="pl" data-title="Ogniwo galwaniczne" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target"><span>Polski</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/C%C3%A9lula_galv%C3%A2nica" title="Célula galvânica – Portuguese" lang="pt" hreflang="pt" data-title="Célula galvânica" 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/Element_galvanic" title="Element galvanic – Romanian" lang="ro" hreflang="ro" data-title="Element galvanic" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D0%B8%D1%87%D0%B5%D1%81%D0%BA%D0%B8%D0%B9_%D1%8D%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Гальванический элемент – Russian" lang="ru" hreflang="ru" data-title="Гальванический элемент" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target"><span>Русский</span></a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B6%9C%E0%B7%90%E0%B6%BD%E0%B7%8A%E0%B7%80%E0%B7%8F%E0%B6%B1%E0%B7%92_%E0%B6%9A%E0%B7%9D%E0%B7%82%E0%B6%BA" title="ගැල්වානි කෝෂය – Sinhala" lang="si" hreflang="si" data-title="ගැල්වානි කෝෂය" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target"><span>සිංහල</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Chemical_cell" title="Chemical cell – Simple English" lang="en-simple" hreflang="en-simple" data-title="Chemical cell" 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-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Galvanick%C3%BD_%C4%8Dl%C3%A1nok" title="Galvanický článok – Slovak" lang="sk" hreflang="sk" data-title="Galvanický článok" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target"><span>Slovenčina</span></a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/Galvanski_%C4%8Dlen" title="Galvanski člen – Slovenian" lang="sl" hreflang="sl" data-title="Galvanski člen" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target"><span>Slovenščina</span></a></li><li class="interlanguage-link interwiki-ckb mw-list-item"><a href="https://ckb.wikipedia.org/wiki/%D8%AE%D8%A7%D9%86%DB%95%DB%8C_%DA%AF%DB%95%D9%84%DA%A4%D8%A7%D9%86%DB%8C" title="خانەی گەلڤانی – Central Kurdish" lang="ckb" hreflang="ckb" data-title="خانەی گەلڤانی" data-language-autonym="کوردی" data-language-local-name="Central Kurdish" class="interlanguage-link-target"><span>کوردی</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D0%B2%D0%B0%D0%BD%D1%81%D0%BA%D0%B8_%D0%B5%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Галвански елемент – Serbian" lang="sr" hreflang="sr" data-title="Галвански елемент" 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/Galvanski_element" title="Galvanski element – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Galvanski element" 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-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Galvaaninen_kenno" title="Galvaaninen kenno – Finnish" lang="fi" hreflang="fi" data-title="Galvaaninen kenno" data-language-autonym="Suomi" data-language-local-name="Finnish" class="interlanguage-link-target"><span>Suomi</span></a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Galvanisk_cell" title="Galvanisk cell – Swedish" lang="sv" hreflang="sv" data-title="Galvanisk cell" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target"><span>Svenska</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B9%80%E0%B8%8B%E0%B8%A5%E0%B8%A5%E0%B9%8C%E0%B8%81%E0%B8%B1%E0%B8%A5%E0%B8%A7%E0%B8%B2%E0%B8%99%E0%B8%B5" title="เซลล์กัลวานี – Thai" lang="th" hreflang="th" data-title="เซลล์กัลวานี" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target"><span>ไทย</span></a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%93%D0%B0%D0%BB%D1%8C%D0%B2%D0%B0%D0%BD%D1%96%D1%87%D0%BD%D0%B8%D0%B9_%D0%B5%D0%BB%D0%B5%D0%BC%D0%B5%D0%BD%D1%82" title="Гальванічний елемент – Ukrainian" lang="uk" hreflang="uk" data-title="Гальванічний елемент" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target"><span>Українська</span></a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Pin_Galvanic" title="Pin Galvanic – Vietnamese" lang="vi" hreflang="vi" data-title="Pin Galvanic" 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dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Electrochemical device</div><figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Galvanic_cell_with_no_cation_flow.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/310px-Galvanic_cell_with_no_cation_flow.svg.png" decoding="async" width="310" height="180" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/465px-Galvanic_cell_with_no_cation_flow.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/620px-Galvanic_cell_with_no_cation_flow.svg.png 2x" data-file-width="512" data-file-height="297" /></a><figcaption>Galvanic cell with no cation flow</figcaption></figure> <p>A <b>galvanic cell</b> or <b>voltaic cell</b>, named after the scientists <a href="/wiki/Luigi_Galvani" title="Luigi Galvani">Luigi Galvani</a> and <a href="/wiki/Alessandro_Volta" title="Alessandro Volta">Alessandro Volta</a>, respectively, is an <a href="/wiki/Electrochemical_cell" title="Electrochemical cell">electrochemical cell</a> in which an electric current is generated from <a href="/wiki/Spontaneous_reaction" class="mw-redirect" title="Spontaneous reaction">spontaneous</a> <a href="/wiki/Oxidation%E2%80%93reduction" class="mw-redirect" title="Oxidation–reduction">oxidation–reduction</a> reactions. An example of a galvanic cell consists of two different metals, each immersed in separate beakers containing their respective metal ions in solution that are connected by a <a href="/wiki/Salt_bridge" title="Salt bridge">salt bridge</a> or separated by a porous membrane.<sup id="cite_ref-:0_1-0" class="reference"><a href="#cite_note-:0-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </p><p>Volta was the inventor of the <a href="/wiki/Voltaic_pile" title="Voltaic pile">voltaic pile</a>, the first <a href="/wiki/Battery_(electricity)" class="mw-redirect" title="Battery (electricity)">electrical battery</a>. Common usage of the word <i>battery</i> has evolved to include a single Galvanic cell, but the first batteries had many Galvanic cells.<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> </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=Galvanic_cell&action=edit&section=1" title="Edit section: History"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>In 1780, <a href="/wiki/Luigi_Galvani" title="Luigi Galvani">Luigi Galvani</a> discovered that when two different metals (e.g., copper and zinc) are in contact and then both are touched at the same time to two different parts of a muscle of a frog leg, to close the circuit, the frog's leg contracts.<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> He called this "<a href="/wiki/Bioelectricity" class="mw-redirect" title="Bioelectricity">animal electricity</a>". The frog's leg, as well as being a detector of electrical current, was also the <a href="/wiki/Electrolyte" title="Electrolyte">electrolyte</a> (to use the language of modern chemistry). </p><p>A year after Galvani published his work (1790), <a href="/wiki/Alessandro_Volta" title="Alessandro Volta">Alessandro Volta</a> showed that the frog was not necessary, using instead a force-based detector and brine-soaked paper (as electrolyte). (Earlier Volta had established the law of capacitance <span class="nowrap"><i>C</i> = <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"><i>Q</i></span><span class="sr-only">/</span><span class="den"><i>V</i></span></span>⁠</span></span> with force-based detectors). In 1799 Volta invented the voltaic pile, which is a stack of galvanic cells each consisting of a metal disk, an electrolyte layer, and a disk of a different metal. He built it entirely out of non-biological material to challenge Galvani's (and the later experimenter <a href="/wiki/Leopoldo_Nobili" title="Leopoldo Nobili">Leopoldo Nobili</a>)'s animal electricity theory in favor of his own metal-metal contact electricity theory.<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> <a href="/wiki/Carlo_Matteucci" title="Carlo Matteucci">Carlo Matteucci</a> in his turn constructed a <a href="/wiki/Frog_battery" title="Frog battery">battery entirely out of biological material</a> in answer to Volta.<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> Volta's contact electricity view characterized each electrode with a number that we would now call the work function of the electrode. This view ignored the chemical reactions at the electrode-electrolyte interfaces, which include <a href="/wiki/Lemon_battery" title="Lemon battery">H<sub>2</sub> formation</a> on the more noble metal in Volta's pile. </p><p>Although Volta did not understand the operation of the battery or the galvanic cell, these discoveries paved the way for electrical batteries; Volta's cell was named an <a href="/wiki/List_of_IEEE_milestones" class="mw-redirect" title="List of IEEE milestones">IEEE Milestone</a> in 1999.<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><p>Some forty years later, Faraday (see <a href="/wiki/Faraday%27s_laws_of_electrolysis" title="Faraday's laws of electrolysis">Faraday's laws of electrolysis</a>) showed that the galvanic cell—now often called a voltaic cell—was chemical in nature. Faraday introduced new terminology to the language of chemistry: <a href="/wiki/Electrode" title="Electrode">electrode</a> (<a href="/wiki/Cathode" title="Cathode">cathode</a> and <a href="/wiki/Anode" title="Anode">anode</a>), <a href="/wiki/Electrolyte" title="Electrolyte">electrolyte</a>, and <a href="/wiki/Ion" title="Ion">ion</a> (<a href="/wiki/Cation" class="mw-redirect" title="Cation">cation</a> and <a href="/wiki/Anion" class="mw-redirect" title="Anion">anion</a>). Thus Galvani incorrectly thought the source of electricity (or source of <a href="/wiki/Electromotive_force" title="Electromotive force">electromotive force</a> (emf), or seat of emf) was in the animal, Volta incorrectly thought it was in the physical properties of the isolated electrodes, but Faraday correctly identified the source of emf as the chemical reactions at the two electrode-electrolyte interfaces. The authoritative work on the intellectual history of the voltaic cell remains that by Ostwald.<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> </p><p>It was suggested by <a href="/wiki/Wilhelm_K%C3%B6nig" title="Wilhelm König">Wilhelm König</a> in 1940 that the object known as the <a href="/wiki/Baghdad_battery" class="mw-redirect" title="Baghdad battery">Baghdad battery</a> might represent galvanic cell technology from ancient <a href="/wiki/Parthia" title="Parthia">Parthia</a>. Replicas filled with citric acid or grape juice have been shown to produce a voltage. However, it is far from certain that this was its purpose—other scholars have pointed out that it is very similar to vessels known to have been used for storing parchment scrolls.<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> <div class="mw-heading mw-heading2"><h2 id="Principles">Principles</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Galvanic_cell&action=edit&section=2" title="Edit section: Principles"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Galvanic_cell_labeled.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Galvanic_cell_labeled.svg/340px-Galvanic_cell_labeled.svg.png" decoding="async" width="340" height="306" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Galvanic_cell_labeled.svg/510px-Galvanic_cell_labeled.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Galvanic_cell_labeled.svg/680px-Galvanic_cell_labeled.svg.png 2x" data-file-width="545" data-file-height="491" /></a><figcaption>Schematic of Zn–Cu galvanic cell</figcaption></figure> <p>Galvanic cells are extensions of spontaneous <a href="/wiki/Redox" title="Redox">redox</a> reactions, but have been merely designed to harness the energy produced from said reaction.<sup id="cite_ref-:0_1-1" class="reference"><a href="#cite_note-:0-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> For example, when one immerses a strip of zinc metal (Zn) in an aqueous solution of copper sulfate (CuSO<sub>4</sub>), dark-colored solid deposits will collect on the surface of the zinc metal and the blue color characteristic of the Cu<sup>++</sup> ion disappears from the solution. The depositions on the surface of the zinc metal consist of copper metal, and the solution now contains zinc ions. This reaction is represented by </p> <dl><dd>Zn<sub>(s)</sub>   +   Cu<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">++</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">(aq)</sub></span></span>   <span class="texhtml">⟶</span>   Zn<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">++</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">(aq)</sub></span></span>   +   Cu<sub>(s)</sub></dd></dl> <p>In this <a href="/wiki/Redox" title="Redox">redox</a> reaction, Zn is oxidized to Zn<sup>++</sup> and Cu<sup>++</sup> is reduced to Cu. When electrons are transferred directly from Zn to Cu<sup>++</sup>, the <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> of reaction is lost to the surroundings as heat. However, the same reaction can be carried out in a galvanic cell, allowing some of the chemical energy released to be converted into electrical energy. In its simplest form, a <a href="/wiki/Half-cell" title="Half-cell">half-cell</a> consists of a solid metal (called an <a href="/wiki/Electrode" title="Electrode">electrode</a>) that is submerged in a solution; the solution contains <a href="/wiki/Cation" class="mw-redirect" title="Cation">cations</a> (+) of the electrode metal and <a href="/wiki/Anion" class="mw-redirect" title="Anion">anions</a> (−) to balance the charge of the cations.<sup id="cite_ref-:1_9-0" class="reference"><a href="#cite_note-:1-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> The full cell consists of two half-cells, usually connected by a <a href="/wiki/Semi-permeable_membrane" class="mw-redirect" title="Semi-permeable membrane">semi-permeable membrane</a> or by a <a href="/wiki/Salt_bridge" title="Salt bridge">salt bridge</a> that prevents the ions of the more noble metal from plating out at the other electrode.<sup id="cite_ref-:1_9-1" class="reference"><a href="#cite_note-:1-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> </p><p>A specific example is the <a href="/wiki/Daniell_cell" title="Daniell cell">Daniell cell</a> (see figure), with a <a href="/wiki/Zinc" title="Zinc">zinc</a> (Zn) half-cell containing a solution of ZnSO<sub>4</sub> (zinc sulfate) and a <a href="/wiki/Copper" title="Copper">copper</a> (Cu) half-cell containing a solution of CuSO<sub>4</sub> (copper sulfate). A salt bridge is used here to complete the electric circuit. </p><p>If an external electrical conductor connects the copper and zinc electrodes, zinc from the zinc electrode dissolves into the solution as Zn<sup>++</sup> ions (oxidation), releasing electrons that enter the external conductor. To compensate for the increased zinc ion concentration, via the salt bridge zinc ions (cations) leave and sulfate ions (anions) enter the zinc half-cell. In the copper half-cell, the copper ions plate onto the copper electrode (reduction), taking up electrons that leave the external conductor. Since the Cu<sup>++</sup> ions (cations) plate onto the copper electrode, the latter is called the <a href="/wiki/Cathode" title="Cathode">cathode</a>. Correspondingly the zinc electrode is the <a href="/wiki/Anode" title="Anode">anode</a>. The electrochemical reaction is </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 {\ce {Zn_{\mathsf {(s)}}\ +\ Cu_{\mathsf {(aq)}}^{++}\ ->\ Zn_{\mathsf {(aq)}}^{++}\ +\ Cu_{\mathsf {(s)}}}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <msubsup> <mtext>Zn</mtext> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo mathvariant="sans-serif" stretchy="false">(</mo> <mtext mathvariant="sans-serif">s</mtext> <mo mathvariant="sans-serif" stretchy="false">)</mo> </mrow> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mtext> </mtext> <mo>+</mo> <mtext> </mtext> <msubsup> <mtext>Cu</mtext> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo mathvariant="sans-serif" stretchy="false">(</mo> <mtext mathvariant="sans-serif">aq</mtext> <mo mathvariant="sans-serif" stretchy="false">)</mo> </mrow> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mo>+</mo> <mo>+</mo> </mrow> </msubsup> <mtext> </mtext> <mo stretchy="false">⟶</mo> <mtext> </mtext> <msubsup> <mtext>Zn</mtext> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo mathvariant="sans-serif" stretchy="false">(</mo> <mtext mathvariant="sans-serif">aq</mtext> <mo mathvariant="sans-serif" stretchy="false">)</mo> </mrow> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mo>+</mo> <mo>+</mo> </mrow> </msubsup> <mtext> </mtext> <mo>+</mo> <mtext> </mtext> <msubsup> <mtext>Cu</mtext> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mo mathvariant="sans-serif" stretchy="false">(</mo> <mtext mathvariant="sans-serif">s</mtext> <mo mathvariant="sans-serif" stretchy="false">)</mo> </mrow> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {Zn_{\mathsf {(s)}}\ +\ Cu_{\mathsf {(aq)}}^{++}\ ->\ Zn_{\mathsf {(aq)}}^{++}\ +\ Cu_{\mathsf {(s)}}}}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/cd7a2cf499427ae147db63bfab3f87d1260d663c" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.505ex; width:36.215ex; height:3.676ex;" alt="{\displaystyle {\ce {Zn_{\mathsf {(s)}}\ +\ Cu_{\mathsf {(aq)}}^{++}\ ->\ Zn_{\mathsf {(aq)}}^{++}\ +\ Cu_{\mathsf {(s)}}}}}"></span></dd></dl> <p>This is the same reaction as given in the previous example. In addition, electrons flow through the external conductor, which is the primary application of the galvanic cell. </p><p>As discussed under <a href="#Cell_voltage">cell voltage</a>, the <a href="/wiki/Electromotive_force" title="Electromotive force">electromotive force</a> of the cell is the difference of the half-cell potentials, a measure of the relative ease of dissolution of the two electrodes into the electrolyte. The emf depends on both the electrodes and on the electrolyte, an indication that the emf is chemical in nature. </p> <div class="mw-heading mw-heading3"><h3 id="Half_reactions_and_conventions">Half reactions and conventions</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Galvanic_cell&action=edit&section=3" title="Edit section: Half reactions and conventions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>A half-cell contains a metal in two <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation states</a>. Inside an isolated half-cell, there is an <a href="/wiki/Redox" title="Redox">oxidation-reduction</a> (redox) reaction that is in <a href="/wiki/Chemical_equilibrium" title="Chemical equilibrium">chemical equilibrium</a>, a condition written symbolically as follows (here, "M" represents a metal cation, an atom that has a charge imbalance due to the loss of <span class="texhtml mvar" style="font-style:italic;">n</span> electrons): </p> <dl><dd>M<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"> <span class="texhtml mvar" style="font-style:italic;">n</span>+</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"> (oxidized species)</sub></span></span>   +   <span class="texhtml mvar" style="font-style:italic;">n</span> e<sup>−</sup>   ⇌   M<sub> (reduced species)</sub></dd></dl> <p>A galvanic cell consists of two half-cells, such that the electrode of one half-cell is composed of metal A, and the electrode of the other half-cell is composed of metal B; the redox reactions for the two separate half-cells are thus: </p> <dl><dd>A<sup> <span class="texhtml mvar" style="font-style:italic;">n</span>+</sup>   +   <span class="texhtml mvar" style="font-style:italic;">n</span> e<sup>−</sup>   ⇌   A</dd> <dd>B<sup> <span class="texhtml mvar" style="font-style:italic;">m</span>+</sup>   +   <span class="texhtml mvar" style="font-style:italic;">m</span> e<sup>−</sup>   ⇌   B</dd></dl> <p>The overall balanced reaction is: </p> <dl><dd><span class="texhtml mvar" style="font-style:italic;">m</span> A   +   <span class="texhtml mvar" style="font-style:italic;">n</span> B<sup> <span class="texhtml mvar" style="font-style:italic;">m</span>+</sup>   ⇌   <span class="texhtml mvar" style="font-style:italic;">n</span> B   +   <span class="texhtml mvar" style="font-style:italic;">m</span> A<sup> <span class="texhtml mvar" style="font-style:italic;">n</span>+</sup></dd></dl> <p>In other words, the metal atoms of one half-cell are oxidized while the metal cations of the other half-cell are reduced. By separating the metals in two half-cells, their reaction can be controlled in a way that forces transfer of electrons through the external circuit where they can do useful <a href="/wiki/Work_(physics)" title="Work (physics)">work</a>. </p> <ul><li>The electrodes are connected with a metal wire in order <a href="/wiki/Electrical_conduction" class="mw-redirect" title="Electrical conduction">to conduct</a> the electrons that participate in the reaction.</li></ul> <p>In one half-cell, dissolved metal B cations combine with the free electrons that are available at the interface between the solution and the metal B electrode; these cations are thereby neutralized, causing them to <a href="/wiki/Precipitation_(chemistry)" title="Precipitation (chemistry)">precipitate</a> from solution as deposits on the metal B electrode, a process known as <a href="/wiki/Plating" title="Plating">plating</a>. </p><p>This reduction reaction causes the free electrons throughout the metal B electrode, the wire, and the metal A electrode to be pulled into the metal B electrode. Consequently, electrons are wrestled away from some of the atoms of the metal A electrode, as though the metal B cations were reacting directly with them; those metal A atoms become cations that dissolve into the surrounding solution. </p><p>As this reaction continues, the half-cell with the metal A electrode develops a positively charged solution (because the metal A cations dissolve into it), while the other half-cell develops a negatively charged solution (because the metal B cations precipitate out of it, leaving behind the anions); unabated, this imbalance in charge would stop the reaction. The solutions of the half-cells are connected by a salt bridge or a porous plate that allows ions to pass from one solution to the other, which balances the charges of the solutions and allows the reaction to continue. </p><p>By definition: </p> <ul><li>The <a href="/wiki/Anode" title="Anode">anode</a> is the electrode where oxidation (loss of electrons) takes place (metal A electrode); in a galvanic cell, it is the negative electrode, because when oxidation occurs, electrons are left behind on the electrode.<sup id="cite_ref-r1_10-0" class="reference"><a href="#cite_note-r1-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> These electrons then flow through the external circuit to the cathode (positive electrode) (while in electrolysis, an electric current drives electron flow in the opposite direction and the anode is the positive electrode).</li></ul> <ul><li>The <a href="/wiki/Cathode" title="Cathode">cathode</a> is the electrode where reduction (gain of electrons) takes place (metal B electrode); in a galvanic cell, it is the positive electrode, as ions get reduced by taking up electrons from the electrode and plate out (while in electrolysis, the cathode is the negative terminal and attracts positive ions from the solution). In both cases, the statement 'the <u>cat</u>hode attracts <u>cat</u>ions' is true.</li></ul> <p>By their nature, galvanic cells produce <a href="/wiki/Direct_current" title="Direct current">direct current</a>. </p><p>The <i><a href="/wiki/Weston_cell" title="Weston cell">Weston cell</a></i> has an anode composed of <a href="/wiki/Cadmium" title="Cadmium">cadmium</a> <a href="/wiki/Mercury_(element)" title="Mercury (element)">mercury</a> <a href="/wiki/Amalgam_(chemistry)" title="Amalgam (chemistry)">amalgam</a>, and a cathode composed of pure mercury. The electrolyte is a (saturated) solution of <a href="/wiki/Cadmium_sulfate" title="Cadmium sulfate">cadmium sulfate</a>. The <a href="/wiki/Depolarizer" title="Depolarizer">depolarizer</a> is a paste of mercurous sulfate. When the electrolyte solution is saturated, the voltage of the cell is very reproducible; hence, in 1911, it was adopted as an international standard for voltage. </p> <ul><li>In the strictest sense, a <i>battery</i> is a set of two or more galvanic cells that are connected <a href="/wiki/Series_circuits" class="mw-redirect" title="Series circuits">in series</a> to form a single source of voltage.</li></ul> <p>For instance, a typical 12 V <a href="/wiki/Lead%E2%80%93acid_battery" title="Lead–acid battery">lead–acid battery</a> has six galvanic cells connected in series, with the anodes composed of lead and cathodes composed of lead dioxide, both immersed in <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>. </p><p>Large central office <a href="/wiki/Battery_room" title="Battery room">battery rooms</a> – in a <a href="/wiki/Telephone_exchange" title="Telephone exchange">telephone exchange</a> to provide power for subscribers' <a href="/wiki/Land-line" class="mw-redirect" title="Land-line">land-line</a> telephones, for instance – may have many cells, connected both in series and parallel: Individual cells are connected in series as a <i>battery</i> of cells with some standard voltage (<abbr title="circa">c.</abbr><span style="white-space:nowrap;"> 40 V</span>), and <i>banks</i> of such serial batteries, themselves connected in parallel, to provide adequate amperage to supply a typical peak demand for telephone connections. </p> <div class="mw-heading mw-heading3"><h3 id="Cell_voltage">Cell voltage</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Galvanic_cell&action=edit&section=4" title="Edit section: Cell voltage"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The voltage (<a href="/wiki/Electromotive_force" title="Electromotive force">electromotive force</a> <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup>) produced by a galvanic cell can be estimated from the standard <a href="/wiki/Gibbs_free_energy" title="Gibbs free energy">Gibbs free energy</a> change in the electrochemical reaction according to: </p><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 \ E_{\mathsf {cell}}^{\mathsf {\ \!o}}~~=\ -{\frac {\ \Delta _{r}G^{\mathsf {\ \!o}}\ }{\ \nu _{\mathsf {e}}F\ }}\ }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msubsup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msubsup> <mtext> </mtext> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <mo>−</mo> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <mtext> </mtext> <msub> <mi mathvariant="normal">Δ</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>r</mi> </mrow> </msub> <msup> <mi>G</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msup> <mtext> </mtext> </mrow> <mrow> <mtext> </mtext> <msub> <mi>ν</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">e</mi> </mrow> </mrow> </msub> <mi>F</mi> <mtext> </mtext> </mrow> </mfrac> </mrow> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \ E_{\mathsf {cell}}^{\mathsf {\ \!o}}~~=\ -{\frac {\ \Delta _{r}G^{\mathsf {\ \!o}}\ }{\ \nu _{\mathsf {e}}F\ }}\ }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/80510351e4085450c36add8a937b4974aba41dc2" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:21.018ex; height:5.676ex;" alt="{\displaystyle \ E_{\mathsf {cell}}^{\mathsf {\ \!o}}~~=\ -{\frac {\ \Delta _{r}G^{\mathsf {\ \!o}}\ }{\ \nu _{\mathsf {e}}F\ }}\ }"></span> </p><p>where <span class="texhtml mvar" style="font-style:italic;">ν</span><sub>e</sub> is the number of electrons transferred in the balanced half reactions, and <span class="texhtml mvar" style="font-style:italic;">F</span> is <a href="/wiki/Faraday%27s_constant" class="mw-redirect" title="Faraday's constant">Faraday's constant</a>. However, it can be determined more conveniently by the use of a <a href="/wiki/Table_of_standard_electrode_potentials" class="mw-redirect" title="Table of standard electrode potentials">standard potential table</a> for the two <a href="/wiki/Half_cell" class="mw-redirect" title="Half cell">half cells</a> involved. The first step is to identify the two metals and their ions reacting in the cell. Then one looks up the <a href="/wiki/Standard_electrode_potential" title="Standard electrode potential">standard electrode potential</a>, <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup>, in <a href="/wiki/Volt" title="Volt">volts</a>, for each of the two <a href="/wiki/Half-reaction" title="Half-reaction">half reactions</a>. The standard potential of the cell is equal to the more positive <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup> value minus the more negative <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup> value. </p><p>For example, in the figure above the solutions are CuSO<sub>4</sub> and ZnSO<sub>4</sub>. Each solution has a corresponding metal strip in it, and a salt bridge or porous disk connecting the two solutions and allowing <span class="chemf nowrap">SO<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">2−</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">4</sub></span></span></span> ions to flow freely between the copper and zinc solutions. To calculate the standard potential one looks up copper and zinc's half reactions and finds: </p> <dl><dd>Cu<sup>++</sup>   + 2 <span style="white-space:nowrap;"><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1.0em;font-size:80%;text-align:right"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span>e<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1.0em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">−</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span></span>   ⇌   Cu <span style="padding-left:2em;"> </span> : <span style="padding-left:2em;"> </span> <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup> = +0.34 V</dd> <dd>Zn<sup>++</sup>   + 2 <span style="white-space:nowrap;"><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1.0em;font-size:80%;text-align:right"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span>e<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1.0em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">−</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span></span>   ⇌   Zn <span style="padding-left:2em;"> </span> : <span style="padding-left:2em;"> </span> <span class="texhtml mvar" style="font-style:italic;">E</span><sup> o</sup> = −0.76 V</dd></dl> <p>Thus the overall reaction is: </p> <dl><dd>Cu<sup>++</sup> + Zn   ⇌   Cu + Zn<sup>++</sup></dd></dl> <p>The standard potential for the reaction is then <span class="nowrap">  +0.34 V − (−0.76 V) <span class="texhtml">=</span> +1.10 V .</span> The polarity of the cell is determined as follows. Zinc metal is more strongly reducing than copper metal because the standard (reduction) potential for zinc is more negative than that of copper. Thus, zinc metal will lose electrons to copper ions and develop a positive electrical charge. The <a href="/wiki/Equilibrium_constant" title="Equilibrium constant">equilibrium constant</a>, <span class="texhtml mvar" style="font-style:italic;">K</span>, for the cell is given by: </p><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 \ \log _{e}K~~=~~{\frac {~~~\nu _{\mathsf {e}}\;\!F\ E_{\mathsf {cell}}^{\mathsf {\ \!o}}\ }{\ R\ T\ }}\ }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msub> <mi>log</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>e</mi> </mrow> </msub> <mo>⁡</mo> <mi>K</mi> <mtext> </mtext> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <mtext> </mtext> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <mtext> </mtext> <mtext> </mtext> <mtext> </mtext> <msub> <mi>ν</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">e</mi> </mrow> </mrow> </msub> <mspace width="thickmathspace" /> <mspace width="negativethinmathspace" /> <mi>F</mi> <mtext> </mtext> <msubsup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msubsup> <mtext> </mtext> </mrow> <mrow> <mtext> </mtext> <mi>R</mi> <mtext> </mtext> <mi>T</mi> <mtext> </mtext> </mrow> </mfrac> </mrow> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \ \log _{e}K~~=~~{\frac {~~~\nu _{\mathsf {e}}\;\!F\ E_{\mathsf {cell}}^{\mathsf {\ \!o}}\ }{\ R\ T\ }}\ }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/f2e6ca7ab3930ddaa3955ca34719165956833eba" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.005ex; width:25.436ex; height:5.843ex;" alt="{\displaystyle \ \log _{e}K~~=~~{\frac {~~~\nu _{\mathsf {e}}\;\!F\ E_{\mathsf {cell}}^{\mathsf {\ \!o}}\ }{\ R\ T\ }}\ }"></span> </p><p>where </p> <dl><dd><span class="texhtml mvar" style="font-style:italic;">F</span>   is the <a href="/wiki/Faraday_constant" title="Faraday constant">Faraday constant</a>,</dd> <dd><span class="texhtml mvar" style="font-style:italic;">R</span>   is the <a href="/wiki/Gas_constant" title="Gas constant">gas constant</a>, and</dd> <dd><span class="texhtml mvar" style="font-style:italic;">T</span>   is the <a href="/wiki/Absolute_temperature" class="mw-redirect" title="Absolute temperature">absolute temperature</a> in <a href="/wiki/Kelvin_(unit)" class="mw-redirect" title="Kelvin (unit)">Kelvins</a>.</dd></dl> <p>For the Daniell cell <span class="nowrap">  <span class="texhtml"> <i>K</i> ≈ <span class="nowrap"><span data-sort-value="7037149999999999999♠"></span>1.5<span style="margin-left:0.25em;margin-right:0.15em;">×</span>10<sup>37</sup></span> </span>  .</span> Thus, at equilibrium, a few electrons are transferred, enough to cause the electrodes to be charged.<sup id="cite_ref-Atkins-dePala-2006_11-0" class="reference"><a href="#cite_note-Atkins-dePala-2006-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Location: ch. 7, "Equilibrium electrochemistry" §§">(ch. 7, "Equilibrium electrochemistry" §§)</span></sup> </p><p>Actual half-cell potentials must be calculated by using the <a href="/wiki/Nernst_equation" title="Nernst equation">Nernst equation</a> as the solutes are unlikely to be in their standard states: </p><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 \ E_{\mathsf {\;\!half-cell}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}\ F\ }}\ \log _{e}Q\ }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mspace width="thickmathspace" /> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">h</mi> <mi mathvariant="sans-serif">a</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">f</mi> <mo mathvariant="sans-serif">−</mo> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> </msub> <mtext> </mtext> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <mtext> </mtext> <msup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msup> <mtext> </mtext> <mo>−</mo> <mtext> </mtext> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <mtext> </mtext> <mi>R</mi> <mtext> </mtext> <mi>T</mi> <mtext> </mtext> </mrow> <mrow> <mtext> </mtext> <msub> <mi>ν</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">e</mi> </mrow> </mrow> </msub> <mtext> </mtext> <mi>F</mi> <mtext> </mtext> </mrow> </mfrac> </mrow> <mtext> </mtext> <msub> <mi>log</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>e</mi> </mrow> </msub> <mo>⁡</mo> <mi>Q</mi> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \ E_{\mathsf {\;\!half-cell}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}\ F\ }}\ \log _{e}Q\ }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/c175d3c9c1e4fd06dbb8976b9b5340157b967425" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:35.554ex; height:5.509ex;" alt="{\displaystyle \ E_{\mathsf {\;\!half-cell}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}\ F\ }}\ \log _{e}Q\ }"></span> </p><p>where <span class="texhtml mvar" style="font-style:italic;">Q</span> is the <a href="/wiki/Reaction_quotient" title="Reaction quotient">reaction quotient</a>. When the charges of the ions in the reaction are equal, this simplifies to: </p><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 \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ 2.303\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}F\ }}\ \log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mspace width="thickmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">h</mi> <mi mathvariant="sans-serif">a</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">f</mi> <mo mathvariant="sans-serif">−</mo> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> </mrow> </msub> <mtext> </mtext> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <mtext> </mtext> <msup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msup> <mtext> </mtext> <mo>−</mo> <mtext> </mtext> <mn>2.303</mn> <mtext> </mtext> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <mtext> </mtext> <mi>R</mi> <mtext> </mtext> <mi>T</mi> <mtext> </mtext> </mrow> <mrow> <mtext> </mtext> <msub> <mi>ν</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">e</mi> </mrow> </mrow> </msub> <mi>F</mi> <mtext> </mtext> </mrow> </mfrac> </mrow> <mtext> </mtext> <msub> <mi>log</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>10</mn> </mrow> </msub> <mo>⁡</mo> <mrow> <mo>{</mo> <mrow> <mtext> </mtext> <mtext> </mtext> <msup> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">M</mi> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> <mo>+</mo> </mrow> </msup> </mrow> <mo>}</mo> </mrow> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ 2.303\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}F\ }}\ \log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/d189db92d459cf8f5cc67e6082bc7ae74a2839d8" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:48.035ex; height:5.509ex;" alt="{\displaystyle \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ 2.303\ {\frac {\ R\ T\ }{\ \nu _{\mathsf {e}}F\ }}\ \log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }"></span> </p><p>where M<sup> <span class="texhtml mvar" style="font-style:italic;">n</span>+</sup> is the <a href="/wiki/Activity_(chemistry)" class="mw-redirect" title="Activity (chemistry)">activity</a> of the metal ion in solution. In practice concentration in <span style="font-size:85%;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035"><span class="sfrac">⁠<span class="tion"><span class="num"> mol </span><span class="sr-only">/</span><span class="den"> L </span></span>⁠</span></span> is used in place of activity. The metal electrode is in its standard state so by definition has unit activity. The potential of the whole cell is obtained as the difference between the potentials for the two half-cells, so it depends on the concentrations of both dissolved metal ions. If the concentrations are the same the Nernst equation is not needed, and <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 ~E_{\mathsf {cell}}~=~E_{\mathsf {cell}}^{\mathsf {\;\!o}}~~}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> </msub> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <msubsup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mspace width="thickmathspace" /> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msubsup> <mtext> </mtext> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle ~E_{\mathsf {cell}}~=~E_{\mathsf {cell}}^{\mathsf {\;\!o}}~~}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/4e7d7db503441d4720f856d152edb82267736193" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.005ex; width:14.39ex; height:2.843ex;" alt="{\displaystyle ~E_{\mathsf {cell}}~=~E_{\mathsf {cell}}^{\mathsf {\;\!o}}~~}"></span> under the conditions assumed here. </p><p>The value of <span class="nowrap">  <span class="texhtml"> 2.303 <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035"><span class="sfrac">⁠<span class="tion"><span class="num"> <i>R</i> </span><span class="sr-only">/</span><span class="den"> <i>F</i> </span></span>⁠</span> </span>  </span> is <span class="nowrap">  <span class="texhtml">1.9845<span style="font-size:85%;">×</span>10<sup><span class="nowrap"><span data-sort-value="2999600000000000000♠"></span>−4</span></sup> </span> <span style="font-size:85%;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035"><span class="sfrac">⁠<span class="tion"><span class="num"> V </span><span class="sr-only">/</span><span class="den"> K </span></span>⁠</span></span> ,</span> so at <span class="texhtml">  <i>T</i> = </span> 25 °C (298.15 K)   the half-cell potential will change by only <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035"><span class="sfrac">⁠<span class="tion"><span class="num">  0.05918 V  </span><span class="sr-only">/</span><span class="den"> <span class="texhtml mvar" style="font-style:italic;">ν</span><sub>e</sub> </span></span>⁠</span> if the concentration of a metal ion is increased or decreased by a <span class="nowrap">factor of <span class="texhtml">10</span> .</span> </p><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 \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ 0.05918\ {\mathsf {V}}\ }{\ \nu _{\mathsf {e}}\ }}\log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mtext> </mtext> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mspace width="thickmathspace" /> <mspace width="negativethinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">h</mi> <mi mathvariant="sans-serif">a</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">f</mi> <mo mathvariant="sans-serif">−</mo> <mi mathvariant="sans-serif">c</mi> <mi mathvariant="sans-serif">e</mi> <mi mathvariant="sans-serif">l</mi> <mi mathvariant="sans-serif">l</mi> </mrow> </mrow> </mrow> </msub> <mtext> </mtext> <mtext> </mtext> <mo>=</mo> <mtext> </mtext> <mtext> </mtext> <msup> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mtext mathvariant="sans-serif"> </mtext> <mspace width="negativethinmathspace" /> <mi mathvariant="sans-serif">o</mi> </mrow> </mrow> </msup> <mtext> </mtext> <mo>−</mo> <mtext> </mtext> <mrow class="MJX-TeXAtom-ORD"> <mfrac> <mrow> <mtext> </mtext> <mn>0.05918</mn> <mtext> </mtext> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">V</mi> </mrow> </mrow> <mtext> </mtext> </mrow> <mrow> <mtext> </mtext> <msub> <mi>ν</mi> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">e</mi> </mrow> </mrow> </msub> <mtext> </mtext> </mrow> </mfrac> </mrow> <msub> <mi>log</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>10</mn> </mrow> </msub> <mo>⁡</mo> <mrow> <mo>{</mo> <mrow> <mtext> </mtext> <mtext> </mtext> <msup> <mrow class="MJX-TeXAtom-ORD"> <mrow class="MJX-TeXAtom-ORD"> <mi mathvariant="sans-serif">M</mi> </mrow> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mi>n</mi> <mo>+</mo> </mrow> </msup> </mrow> <mo>}</mo> </mrow> <mtext> </mtext> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ 0.05918\ {\mathsf {V}}\ }{\ \nu _{\mathsf {e}}\ }}\log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/90cdb8ccb8790e21d1012c68c28fedb97daa4328" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -2.171ex; width:47.348ex; height:5.676ex;" alt="{\displaystyle \ E_{\;\!{\mathsf {half-cell}}}~~=~~E^{\mathsf {\ \!o}}\ -\ {\frac {\ 0.05918\ {\mathsf {V}}\ }{\ \nu _{\mathsf {e}}\ }}\log _{10}\left\{~~{\mathsf {M}}^{n+}\right\}\ }"></span> </p><p>These calculations are based on the assumption that all chemical reactions are in equilibrium. When a current flows in the circuit, equilibrium conditions are not achieved and the cell voltage will usually be reduced by various mechanisms, such as the development of <a href="/wiki/Overpotential" title="Overpotential">overpotentials</a>.<sup id="cite_ref-Atkins-dePala-2006_11-1" class="reference"><a href="#cite_note-Atkins-dePala-2006-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Location: § 25.12 "Working galvanic cells"">(§ 25.12 "Working galvanic cells")</span></sup> Also, since chemical reactions occur when the cell is producing power, the electrolyte concentrations change and the cell voltage is reduced. A consequence of the temperature dependency of standard potentials is that the voltage produced by a galvanic cell is also temperature dependent. </p> <div class="mw-heading mw-heading2"><h2 id="Galvanic_corrosion">Galvanic corrosion</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Galvanic_cell&action=edit&section=5" title="Edit section: Galvanic corrosion"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <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">Main article: <a href="/wiki/Galvanic_corrosion" title="Galvanic corrosion">Galvanic corrosion</a></div> <p>Galvanic corrosion is the <a href="/wiki/Electrochemical" class="mw-redirect" title="Electrochemical">electrochemical</a> erosion of metals. <a href="/wiki/Corrosion" title="Corrosion">Corrosion</a> occurs when two dissimilar metals are in contact with each other in the presence of an <a href="/wiki/Electrolyte" title="Electrolyte">electrolyte</a>, such as salt water. This forms a galvanic cell, with hydrogen gas forming on the more noble (less active) metal. The resulting electrochemical potential then develops an electric current that electrolytically dissolves the less noble material. A <a href="/wiki/Concentration_cell" title="Concentration cell">concentration cell</a> can be formed if the same metal is exposed to two different concentrations of electrolyte. </p> <div class="mw-heading mw-heading2"><h2 id="Types">Types</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Galvanic_cell&action=edit&section=6" title="Edit section: Types"><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: 10em;"> <ul><li><a href="/wiki/Concentration_cell" title="Concentration cell">Concentration cell</a></li> <li><a href="/wiki/Electrolytic_cell" title="Electrolytic cell">Electrolytic cell</a></li> <li><a href="/wiki/Electrochemical_cell" title="Electrochemical cell">Electrochemical cell</a></li> <li><a href="/wiki/Lemon_battery" title="Lemon battery">Lemon battery</a></li> <li><a href="/wiki/Thermogalvanic_cell" title="Thermogalvanic cell">Thermogalvanic cell</a></li></ul> </div> <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=Galvanic_cell&action=edit&section=7" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1184024115"><div class="div-col" style="column-width: 15em;"> <ul><li><a href="/wiki/Bioelectrochemical_reactor" title="Bioelectrochemical reactor">Bioelectrochemical reactor</a></li> <li><a href="/wiki/Resting_potential" title="Resting potential">Resting potential</a></li> <li><a href="/wiki/Bio-nano_generator" class="mw-redirect" title="Bio-nano generator">Bio-nano generator</a></li> <li><a href="/wiki/Cell_notation" title="Cell notation">Cell notation</a></li> <li><a href="/wiki/Desulfation" class="mw-redirect" title="Desulfation">Desulfation</a></li> <li><a href="/wiki/Electrochemical_engineering" title="Electrochemical engineering">Electrochemical engineering</a></li> <li><a href="/wiki/Electrode_potential" title="Electrode potential">Electrode potential</a></li> <li><a href="/wiki/Electrohydrogenesis" title="Electrohydrogenesis">Electrohydrogenesis</a></li> <li><a href="/wiki/Electrosynthesis" title="Electrosynthesis">Electrosynthesis</a></li> <li><a href="/wiki/Enzymatic_biofuel_cell" title="Enzymatic biofuel cell">Enzymatic biofuel cell</a></li> <li><a href="/wiki/Galvanic_series" title="Galvanic series">Galvanic series</a></li> <li><a href="/wiki/Isotope_electrochemistry" title="Isotope electrochemistry">Isotope electrochemistry</a></li> <li><a href="/wiki/List_of_battery_types" title="List of battery types">List of battery types</a></li> <li><a href="/wiki/Sacrificial_anode" class="mw-redirect" title="Sacrificial anode">Sacrificial anode</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=Galvanic_cell&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 reflist-columns references-column-width" style="column-width: 25em;"> <ol class="references"> <li id="cite_note-:0-1"><span class="mw-cite-backlink">^ <a href="#cite_ref-:0_1-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-:0_1-1"><sup><i><b>b</b></i></sup></a></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 .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite id="CITEREFMcMurryFayRobinson2015" class="citation book cs1">McMurry, John; Fay, Robert C.; Robinson, Jill K. (2015). <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/889577526"><i>Chemistry</i></a> (7th ed.). Boston: Pearson. p. 762. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-321-94317-0" title="Special:BookSources/978-0-321-94317-0"><bdi>978-0-321-94317-0</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/889577526">889577526</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry&rft.place=Boston&rft.pages=762&rft.edition=7th&rft.pub=Pearson&rft.date=2015&rft_id=info%3Aoclcnum%2F889577526&rft.isbn=978-0-321-94317-0&rft.aulast=McMurry&rft.aufirst=John&rft.au=Fay%2C+Robert+C.&rft.au=Robinson%2C+Jill+K.&rft_id=https%3A%2F%2Fwww.worldcat.org%2Foclc%2F889577526&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" 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"><a rel="nofollow" class="external text" href="http://www.merriam-webster.com/dictionary/battery">"battery" (def. 4b)</a>, <i>Merriam-Webster Online Dictionary</i> (2008). Retrieved 6 August 2008.</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="CITEREFKeithley1999" class="citation book cs1">Keithley, Joseph F (1999). <i>Daniell Cell</i>. John Wiley and Sons. pp. 49–51. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-7803-1193-0" title="Special:BookSources/978-0-7803-1193-0"><bdi>978-0-7803-1193-0</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Daniell+Cell&rft.pages=49-51&rft.pub=John+Wiley+and+Sons&rft.date=1999&rft.isbn=978-0-7803-1193-0&rft.aulast=Keithley&rft.aufirst=Joseph+F&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" 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">Kipnis, Nahum (2003) <a rel="nofollow" class="external text" href="http://ppp.unipv.it/Collana/Pages/Libri/Saggi/Nuova%20Voltiana5_PDF/p__143-162.pdf">"Changing a theory: the case of Volta's contact electricity"</a>, <i>Nuova Voltiana</i>, Vol. 5. 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Retrieved <span class="nowrap">26 July</span> 2011</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=IEEE+Global+History+Network&rft.atitle=Milestones%3AVolta%27s+Electrical+Battery+Invention%2C+1799&rft_id=http%3A%2F%2Fwww.ieeeghn.org%2Fwiki%2Findex.php%2FMilestones%3AVolta%2527s_Electrical_Battery_Invention%2C_1799&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" class="Z3988"></span></span> </li> <li id="cite_note-7"><span class="mw-cite-backlink"><b><a href="#cite_ref-7">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFOstwald1980" class="citation book cs1">Ostwald, Wilhelm (1980). <i>Electrochemistry: History and Theory</i>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Electrochemistry%3A+History+and+Theory&rft.date=1980&rft.aulast=Ostwald&rft.aufirst=Wilhelm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" class="Z3988"></span></span> </li> <li id="cite_note-8"><span class="mw-cite-backlink"><b><a href="#cite_ref-8">^</a></b></span> <span class="reference-text">Haughton, Brian (2007) <i>Hidden History: Lost Civilizations, Secret Knowledge, and Ancient Mysteries</i>. Career Press. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/1564148971" title="Special:BookSources/1564148971">1564148971</a>. pp. 129–132</span> </li> <li id="cite_note-:1-9"><span class="mw-cite-backlink">^ <a href="#cite_ref-:1_9-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-:1_9-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFPetrucciHerringMaduraBissonnette2017" class="citation book cs1">Petrucci, Ralph H.; Herring, F. Geoffrey; Madura, Jeffry D.; Bissonnette, Carey (2017). <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/951078429"><i>General chemistry: principles and modern applications</i></a> (11th ed.). Toronto: Pearson. p. 869. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-13-293128-1" title="Special:BookSources/978-0-13-293128-1"><bdi>978-0-13-293128-1</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/951078429">951078429</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=General+chemistry%3A+principles+and+modern+applications&rft.place=Toronto&rft.pages=869&rft.edition=11th&rft.pub=Pearson&rft.date=2017&rft_id=info%3Aoclcnum%2F951078429&rft.isbn=978-0-13-293128-1&rft.aulast=Petrucci&rft.aufirst=Ralph+H.&rft.au=Herring%2C+F.+Geoffrey&rft.au=Madura%2C+Jeffry+D.&rft.au=Bissonnette%2C+Carey&rft_id=https%3A%2F%2Fwww.worldcat.org%2Foclc%2F951078429&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" class="Z3988"></span></span> </li> <li id="cite_note-r1-10"><span class="mw-cite-backlink"><b><a href="#cite_ref-r1_10-0">^</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="http://www.chemguide.co.uk/physical/redoxeqia/introduction.html#top">"An introduction to redox equilibria"</a>. <i>Chemguide (chemguide.co.uk)</i><span class="reference-accessdate">. Retrieved <span class="nowrap">20 July</span> 2014</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=Chemguide+%28chemguide.co.uk%29&rft.atitle=An+introduction+to+redox+equilibria&rft_id=http%3A%2F%2Fwww.chemguide.co.uk%2Fphysical%2Fredoxeqia%2Fintroduction.html%23top&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" class="Z3988"></span></span> </li> <li id="cite_note-Atkins-dePala-2006-11"><span class="mw-cite-backlink">^ <a href="#cite_ref-Atkins-dePala-2006_11-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Atkins-dePala-2006_11-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFAtkinsde_Paula2006" class="citation book cs1">Atkins, P.; de Paula, J. (2006). <i>Physical Chemistry</i> (8th ed.). Oxford University Press. Ch. 7 and Ch. 25, § 25.12. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-19-870072-2" title="Special:BookSources/978-0-19-870072-2"><bdi>978-0-19-870072-2</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Physical+Chemistry&rft.pages=Ch.-7+and+Ch.-25%2C+%C2%A7-25.12&rft.edition=8th&rft.pub=Oxford+University+Press&rft.date=2006&rft.isbn=978-0-19-870072-2&rft.aulast=Atkins&rft.aufirst=P.&rft.au=de+Paula%2C+J.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AGalvanic+cell" class="Z3988"></span></span> </li> </ol></div> <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=Galvanic_cell&action=edit&section=9" title="Edit section: External links"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20141124233113/http://www.miniscience.com/link/Airbattery.htm">How to build a galvanic cell battery</a> from MiniScience.com</li> <li><a rel="nofollow" class="external text" href="http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/galvan5.swf">Galvanic Cell</a>, an animation</li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20110719210759/http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/electroChem/voltaicCell20.html">Interactive animation of Galvanic Cell</a>. Chemical Education Research Group, Iowa State University.</li> <li><a rel="nofollow" class="external text" href="https://av.tib.eu/media/34660?pag=1">Electron transfer reactions and redox potentials in GALVANIc cells - what happens to the ions at the phase boundary (NERNST, FARADAY)</a> (Video by SciFox on TIB AV-Portal)</li></ul> <div class="navbox-styles"><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline ol,.mw-parser-output .hlist.inline ul,.mw-parser-output .hlist dl dl,.mw-parser-output .hlist dl ol,.mw-parser-output .hlist dl ul,.mw-parser-output .hlist ol dl,.mw-parser-output .hlist ol ol,.mw-parser-output .hlist ol ul,.mw-parser-output .hlist ul dl,.mw-parser-output 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href="/wiki/Fuel_cell" title="Fuel cell">Fuel cell</a></li> <li><a href="/wiki/Thermogalvanic_cell" title="Thermogalvanic cell">Thermogalvanic cell</a></li> <li><a href="/wiki/Voltaic_pile" title="Voltaic pile">Voltaic pile</a></li></ul> </div></td><td class="noviewer navbox-image" rowspan="5" style="width:1px;padding:0 0 0 2px"><div><span typeof="mw:File"><a href="/wiki/File:Galvanic_Cell.svg" class="mw-file-description" title="Galvanic cell"><img alt="Galvanic cell" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Galvanic_Cell.svg/150px-Galvanic_Cell.svg.png" decoding="async" width="150" height="159" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Galvanic_Cell.svg/225px-Galvanic_Cell.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Galvanic_Cell.svg/300px-Galvanic_Cell.svg.png 2x" data-file-width="376" data-file-height="399" /></a></span></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Primary_battery" title="Primary battery">Primary cell</a><br /><span class="nobold">(non-rechargeable)</span></div></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Alkaline_battery" title="Alkaline battery">Alkaline</a></li> <li><a href="/wiki/Aluminium%E2%80%93air_battery" title="Aluminium–air battery">Aluminium–air</a></li> <li><a href="/wiki/Bunsen_cell" title="Bunsen cell">Bunsen</a></li> <li><a href="/wiki/Chromic_acid_cell" title="Chromic acid cell">Chromic acid</a></li> <li><a href="/wiki/Clark_cell" title="Clark cell">Clark</a></li> <li><a href="/wiki/Daniell_cell" title="Daniell cell">Daniell</a></li> <li><a href="/wiki/Dry_cell" title="Dry cell">Dry</a></li> <li><a href="/wiki/Edison%E2%80%93Lalande_cell" title="Edison–Lalande cell">Edison–Lalande</a></li> <li><a href="/wiki/Grove_cell" title="Grove cell">Grove</a></li> <li><a href="/wiki/Leclanch%C3%A9_cell" title="Leclanché cell">Leclanché</a></li> <li><a href="/wiki/Lithium_metal_battery" title="Lithium metal battery">Lithium metal</a></li> <li><a href="/wiki/Lithium%E2%80%93air_battery" title="Lithium–air battery">Lithium–air</a></li> <li><a href="/wiki/Mercury_battery" title="Mercury battery">Mercury</a></li> <li><a href="/wiki/Metal%E2%80%93air_electrochemical_cell" title="Metal–air electrochemical cell">Metal–air electrochemical</a></li> <li><a href="/wiki/Nickel_oxyhydroxide_battery" title="Nickel oxyhydroxide battery">Nickel oxyhydroxide</a></li> <li><a href="/wiki/Silicon%E2%80%93air_battery" title="Silicon–air battery">Silicon–air</a></li> <li><a href="/wiki/Silver_oxide_battery" title="Silver oxide battery">Silver oxide</a></li> <li><a href="/wiki/Weston_cell" title="Weston cell">Weston</a></li> <li><a href="/wiki/Zamboni_pile" title="Zamboni pile">Zamboni</a></li> <li><a href="/wiki/Zinc%E2%80%93air_battery" title="Zinc–air battery">Zinc–air</a></li> <li><a href="/wiki/Zinc%E2%80%93carbon_battery" title="Zinc–carbon battery">Zinc–carbon</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Rechargeable_battery" title="Rechargeable battery">Secondary cell</a><br /><span class="nobold">(rechargeable)</span></div></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Automotive_battery" title="Automotive battery">Automotive</a></li> <li><a href="/wiki/Lead%E2%80%93acid_battery" title="Lead–acid battery">Lead–acid</a> <ul><li><a href="/wiki/VRLA_battery" title="VRLA battery">gel–VRLA</a></li></ul></li> <li><a href="/wiki/Lithium%E2%80%93air_battery" title="Lithium–air battery">Lithium–air</a></li> <li><a href="/wiki/Lithium-ion_battery" title="Lithium-ion battery">Lithium ion</a> <ul><li><a href="/wiki/Dual_carbon_battery" title="Dual carbon battery">Dual carbon</a></li> <li><a href="/wiki/Lithium_iron_phosphate_battery" title="Lithium iron phosphate battery">Lithium–iron–phosphate</a></li> <li><a href="/wiki/Lithium_polymer_battery" title="Lithium polymer battery">Lithium–polymer</a></li> <li><a href="/wiki/Lithium%E2%80%93sulfur_battery" title="Lithium–sulfur battery">Lithium–sulfur</a></li> <li><a href="/wiki/Lithium-titanate_battery" title="Lithium-titanate battery">Lithium–titanate</a></li></ul></li> <li><a href="/wiki/Metal%E2%80%93air_electrochemical_cell" title="Metal–air electrochemical cell">Metal–air</a></li> <li><a href="/wiki/Molten-salt_battery" title="Molten-salt battery">Molten salt</a></li> <li><a href="/wiki/Nanopore_battery" title="Nanopore battery">Nanopore</a></li> <li><a href="/wiki/Nanowire_battery" title="Nanowire battery">Nanowire</a></li> <li><a href="/wiki/Nickel%E2%80%93cadmium_battery" title="Nickel–cadmium battery">Nickel–cadmium</a></li> <li><a href="/wiki/Nickel%E2%80%93hydrogen_battery" title="Nickel–hydrogen battery">Nickel–hydrogen</a></li> <li><a href="/wiki/Nickel%E2%80%93iron_battery" title="Nickel–iron battery">Nickel–iron</a></li> <li><a href="/wiki/Nickel%E2%80%93lithium_battery" title="Nickel–lithium battery">Nickel–lithium</a></li> <li><a href="/wiki/Nickel%E2%80%93metal_hydride_battery" title="Nickel–metal hydride battery">Nickel–metal hydride</a></li> <li><a href="/wiki/Nickel%E2%80%93zinc_battery" title="Nickel–zinc battery">Nickel–zinc</a></li> <li><a href="/wiki/Polysulfide%E2%80%93bromide_battery" title="Polysulfide–bromide battery">Polysulfide–bromide</a></li> <li><a href="/wiki/Potassium-ion_battery" title="Potassium-ion battery">Potassium ion</a></li> <li><a href="/wiki/Rechargeable_alkaline_battery" title="Rechargeable alkaline battery">Rechargeable alkaline</a></li> <li><a href="/wiki/Silver%E2%80%93cadmium_battery" title="Silver–cadmium battery">Silver–cadmium</a></li> <li><a href="/wiki/Silver_zinc_battery" title="Silver zinc battery">Silver–zinc</a></li> <li><a href="/wiki/Sodium-ion_battery" title="Sodium-ion battery">Sodium ion</a></li> <li><a href="/wiki/Sodium%E2%80%93sulfur_battery" title="Sodium–sulfur battery">Sodium–sulfur</a></li> <li><a href="/wiki/Solid-state_battery" title="Solid-state battery">Solid state</a></li> <li><a href="/wiki/Vanadium_redox_battery" title="Vanadium redox battery">Vanadium redox</a></li> <li><a href="/wiki/Zinc%E2%80%93bromine_battery" title="Zinc–bromine battery">Zinc–bromine</a></li> <li><a href="/wiki/Zinc%E2%80%93cerium_battery" title="Zinc–cerium battery">Zinc–cerium</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Other cell</div></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Atomic_battery" title="Atomic battery">Atomic battery</a></li> <li><a href="/wiki/Fuel_cell" title="Fuel cell">Fuel cell</a></li> <li><a href="/wiki/Solar_cell" title="Solar cell">Solar cell</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Cell parts</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Anode" title="Anode">Anode</a></li> <li><a href="/wiki/Binder_(material)" title="Binder (material)">Binder</a></li> <li><a href="/wiki/Catalysis" title="Catalysis">Catalyst</a></li> <li><a href="/wiki/Cathode" title="Cathode">Cathode</a></li> <li><a href="/wiki/Electrode" title="Electrode">Electrode</a></li> <li><a href="/wiki/Electrolyte" title="Electrolyte">Electrolyte</a></li> <li><a href="/wiki/Half-cell" title="Half-cell">Half-cell</a></li> <li><a href="/wiki/Ion" title="Ion">Ions</a></li> <li><a href="/wiki/Salt_bridge" title="Salt bridge">Salt bridge</a></li> <li><a href="/wiki/Semipermeable_membrane" title="Semipermeable membrane">Semipermeable membrane</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style></div><div role="navigation" class="navbox authority-control" aria-label="Navbox" style="padding:3px"><table class="nowraplinks hlist navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Help:Authority_control" title="Help:Authority control">Authority control databases</a>: National <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a 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