{"id":4367,"date":"2021-08-03T10:13:35","date_gmt":"2021-08-03T04:43:35","guid":{"rendered":"https:\/\/www.goseeko.com\/blog\/?p=4367"},"modified":"2021-10-30T07:40:32","modified_gmt":"2021-10-30T07:40:32","slug":"what-is-a-nernst-equation","status":"publish","type":"post","link":"https:\/\/www.goseeko.com\/blog\/what-is-a-nernst-equation\/","title":{"rendered":"What is a Nernst Equation?"},"content":{"rendered":"\n<p><a href=\"https:\/\/en.wikipedia.org\/wiki\/Nernst_equation\" target=\"_blank\" rel=\"noreferrer noopener\">Nernst Equation <\/a>corresponds to any change in the Gibbs free energy <em>G<\/em> directly correspond to changes in free energy for processes at constant temperature and pressure, change is the maximum non-expansion work obtainable under these conditions in a closed system; <em>\u0394G<\/em> is negative for spontaneous process, positive for nonspontaneous process, and zero for processes at equilibrium.<\/p>\n\n\n\n<p>It takes into consideration the values of the <a href=\"https:\/\/en.wikipedia.org\/wiki\/Standard_electrode_potential\" target=\"_blank\" rel=\"noreferrer noopener\">standard electrode potentials<\/a>, temperature, activity and the reaction quotient for the calculation of cell potential. For any cell reaction, that occurs Gibbs free energy can be related to standard electrode potential as:<\/p>\n\n\n\n<p>\u0394G =-nFE<\/p>\n\n\n\n<p>Where, n = number of electrons transferred in the reaction, \u0394G= Gibbs free energy, E= cell potential F = Faradays constant (96,500 C\/mol) and. Under standard conditions, the above equation we can write as follows<\/p>\n\n\n\n<p>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;\u0394G<sup>o<\/sup> =-nFE<sup>o<\/sup><\/p>\n\n\n\n<p>According to the theory of thermodynamics, Gibbs free energy under general conditions can be related to Gibbs free energy under standard condition and the reaction quotient as:<\/p>\n\n\n\n<p>\u0394G=\u0394G<sup>o <\/sup>+ RT lnQ<\/p>\n\n\n\n<p>Where, Q= reaction quotient, R= universal gas constant and T= temperature in Kelvin. Incorporating the value of \u0394G<sup>o<\/sup>&nbsp; and \u0394G, from the first two equations, we get the equation:<\/p>\n\n\n\n<p>-nFE = -nFE<sup>0<\/sup> + RT lnQ<\/p>\n\n\n\n<p>E = E<sup>0<\/sup> \u2013 (RT\/nF) lnQ<\/p>\n\n\n\n<p>By conversion of Natural log to log<sub>10<\/sub>, the above equation is called as the Nernst equation. Here, it shows the relation of the reaction quotient and the cell potential. Special cases of Nernst equation:<\/p>\n\n\n\n<p>E = E<sup>o<\/sup> &nbsp; \u2212 (2.303RT\/nF) log<sub>10<\/sub>Q<\/p>\n\n\n\n<p>At standard temperature, T= 298K:<\/p>\n\n\n\n<p>E = E<sup>o<\/sup> &nbsp; \u2212 (0.0592V\/n) log<sub>10<\/sub>Q<\/p>\n\n\n\n<p>At standard temperature T = 298 K, the 2.303RTF, term equals 0.0592 V.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Nernst Equation Under Equilibrium Condition<\/h2>\n\n\n\n<p>As the redox reaction in the cell progresses, the concentration of reactants decreases while the concentration of products increases. This process goes on until equilibrium is achieved. At equilibrium, \u0394G = 0. Hence, cell potential, E = 0. Thus, the Nernst equation can be modified to:<\/p>\n\n\n\n<p>E<sup>0 <\/sup>\u2013 (2.303RT\/nF) log<sub>10<\/sub>K<sub>eq <\/sub>= 0<\/p>\n\n\n\n<p>E<sup>0 <\/sup>= (2.303RT\/nF) log<sub>10<\/sub>K<sub>eq<\/sub><\/p>\n\n\n\n<p>Where, K<sub>eq<\/sub> = equilibrium constant and F= faradays constant. Therefore, the above equation gives us a relation between standard electrode potential of the cell where the reaction takes place and the equilibrium constant.<\/p>\n\n\n\n<p><strong>Interested in learning about similar topics? Here are a few hand-picked blogs for you!<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\"><li><a href=\"https:\/\/www.goseeko.com\/blog\/what-is-calorific-value\" target=\"_blank\" rel=\"noreferrer noopener\">What is Calorific value?<\/a><\/li><li><a rel=\"noreferrer noopener\" href=\"https:\/\/www.goseeko.com\/blog\/what-is-hunds-rule\" target=\"_blank\">What is Hund&#8217;s Rule?<\/a><\/li><li><a href=\"https:\/\/www.goseeko.com\/blog\/what-is-electron-affinity\" target=\"_blank\" rel=\"noreferrer noopener\">Electron affinity?<\/a><\/li><li><a href=\"https:\/\/www.goseeko.com\/blog\/what-is-kirchoffs-law\" target=\"_blank\" rel=\"noreferrer noopener\">Kirchoff&#8217;s law?<\/a><\/li><\/ol>\n","protected":false},"excerpt":{"rendered":"<p>At equilibrium Nernst equation is given by,<br \/>\n  E0 = (2.303RT\/nF) log10Keq<br \/>\nWhere, Keq = equilibrium constant and F= faradays constant, and gives a relation between standard electrode potential.<\/p>\n","protected":false},"author":28,"featured_media":4081,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_jetpack_memberships_contains_paid_content":false,"footnotes":""},"categories":[34],"tags":[],"class_list":["post-4367","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-chemistry"],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v25.3.1 - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>What is a Nernst Equation? - Goseeko blog<\/title>\n<meta name=\"description\" content=\"At equilibrium Nernst equation is given by E0 = (2.303RT\/nF) log10Keq Where, Keq = equilibrium constant and F= faradays constant,\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.goseeko.com\/blog\/what-is-a-nernst-equation\/\" \/>\n<meta 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