{"id":135680,"date":"2022-03-04T16:56:13","date_gmt":"2022-03-04T11:26:13","guid":{"rendered":"https:\/\/infinitylearn.com\/surge\/?p=135680"},"modified":"2025-05-16T12:28:29","modified_gmt":"2025-05-16T06:58:29","slug":"blog-neet-relation-between-gibbs-energy-change-and-emf-of-a-cell","status":"publish","type":"post","link":"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/","title":{"rendered":"Relation between Gibbs energy change and EMF of a cell"},"content":{"rendered":"<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_37 counter-hierarchy ez-toc-counter ez-toc-grey ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title\">Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" style=\"display: none;\"><label for=\"item\" aria-label=\"Table of Content\"><span style=\"display: flex;align-items: center;width: 35px;height: 30px;justify-content: center;\"><svg style=\"fill: #999;color:#999\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #999;color:#999\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/label><input type=\"checkbox\" id=\"item\"><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1' style='display:block'><ul class='ez-toc-list-level-3'><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Introduction\" title=\"Introduction:\">Introduction:<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Overview\" title=\"Overview\">Overview<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Emf_of_a_cell\" title=\"Emf of a cell\">Emf of a cell<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Gibbs_free_energy\" title=\"Gibbs free energy \">Gibbs free energy <\/a><ul class='ez-toc-list-level-3'><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Standard_Gibbs_free_energy_formula\" title=\"Standard Gibb\u2019s free energy formula\">Standard Gibb\u2019s free energy formula<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/infinitylearn.com\/surge\/blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/#Relation_between_Gibbs_energy_change_and_EMF_of_a_cell\" title=\"Relation between Gibbs energy change and EMF of a cell\">Relation between Gibbs energy change and EMF of a cell<\/a><\/li><\/ul><\/li><\/ul><\/nav><\/div>\n<h3><span class=\"ez-toc-section\" id=\"Introduction\"><\/span><span style=\"color: #0000ff; font-size: 18pt;\"><strong>Introduction:<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p>Gibbs free energy, or simply Gibbs energy, is an important thermodynamic state function that describes the energy available for work in a thermodynamic system. It is the difference between the enthalpy and the product of the temperature and the entropy of the system. It is a measure of the potential for a chemical reaction to occur, with a negative value indicating a spontaneous reaction.<\/p>\n<p>Gibbs energy change is a measure of the change in Gibbs free energy from the start to the end of a chemical reaction. It is a function of the enthalpy and entropy changes that accompany the reaction. It can also be used to assess the spontaneity of a reaction. A positive Gibbs energy change indicates that the reaction is non-spontaneous and requires an input of energy to proceed. A negative Gibbs energy change indicates that the reaction is spontaneous and releases energy.<\/p>\n<p>Gibbs energy change can be used to calculate the equilibrium constants of a reaction and to determine the amount of energy released or absorbed by a reaction. It can also be used to evaluate reaction mechanisms and to determine the thermodynamic feasibility of a reaction.<\/p>\n<p>Gibbs energy change is an important concept in thermodynamics and is used to understand and predict the behavior of thermodynamic systems. It is also an important tool for scientists in the study of chemical systems and in the development of new materials.<\/p>\n<p><img loading=\"lazy\" class=\"aligncenter wp-image-136028 size-full\" src=\"https:\/\/infinitylearn.com\/surge\/wp-content\/uploads\/2022\/03\/Capture-8.png\" alt=\"emf of a cell\" width=\"483\" height=\"242\" srcset=\"https:\/\/infinitylearn.com\/surge\/wp-content\/uploads\/2022\/03\/Capture-8.png?v=1646392897 483w, https:\/\/infinitylearn.com\/surge\/wp-content\/uploads\/2022\/03\/Capture-8-300x150.png?v=1646392897 300w\" sizes=\"(max-width: 483px) 100vw, 483px\" \/><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Overview\"><\/span><span style=\"color: #000000;\"><strong>Overview<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Electrochemical cells are devices that use a chemical reaction to generate electricity. It is essentially a device that converts chemical energy into electrical energy. An electrochemical cell requires a chemical reaction that involves the exchange of electrons to function. These kinds of reactions are known as redox reactions.<\/p>\n<p>The voltage of a cell defines it. Without considering the cell size, a specific cell type generates the same voltage. Given ideal operating conditions, the only thing that depends on cell voltage is the chemical composition of the cell.<\/p>\n<p>Usually, the cell voltage will deviate from this ideal value due to various factors such as temperature differences, concentration changes, and so on. Generally, the Nernst equation can be used to calculate the EMF value of a given cell if the cell&#8217;s standard cell potential is known.<\/p>\n<p>As per the second law of thermodynamics, there is a general natural tendency for systems reacting at standard conditions for temperature and pressure (or any other fixed temperature and pressure) to obtain a minimum of the Gibbs free energy. The phrase &#8220;free&#8221; was traditionally included in &#8220;Gibbs free energy&#8221; to mean &#8220;available in the form of useful work.&#8221; When we add the qualification that it is the energy available for non-pressure-volume work, the characterization becomes more precise. (For systems at a constant temperature, an analogous but slightly different meaning of &#8220;free&#8221; applies in conjunction with the Helmholtz free energy.)<\/p>\n<h2><span class=\"ez-toc-section\" id=\"Emf_of_a_cell\"><\/span><span style=\"color: #000000;\"><strong>Emf of a cell<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>In general, the electromotive force or emf of a cell is the maximum potential difference between two cell electrodes. This is also the net voltage between the reaction&#8217;s oxidation and reduction halves. We can say that a cell&#8217;s EMF is primarily used to determine whether or not an electrochemical cell is galvanic.<\/p>\n<p>When no current is drawn from a cell, the voltage or electric potential difference across its terminals, now, the emf is the net sum of the electric potential differences produced by charge separation (electrons or ions) at each phase boundary (or interface) in the cell. Each potential difference&#8217;s magnitude is determined by the chemical nature of the two contacting phases. As a result, some electrons will have moved from the metal with a higher free energy of electrons to the metal with a lower free energy of electrons at the interface between two different metals. The subsequent charge separation will generate a potential difference, similar to how charge separation generates a voltage across a capacitor; this exactly opposes further electron flow at equilibrium. Potential differences can also be produced when electrons partition across a metal solution or metal solid interface or when ions partition across a solution| membrane solution interface.<\/p>\n<h2><span class=\"ez-toc-section\" id=\"Gibbs_free_energy\"><\/span><span style=\"color: #000000;\"><strong>Gibbs free energy <\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p>Gibbs free energy, also identified as the Gibbs function, Gibb\u2019s energy, or free enthalpy, is a quantity used to calculate the maximum amount of work done in a thermodynamic system with constant temperature and pressure. The symbol &#8216;G&#8217; represents Gibbs&#8217;s free energy, and it is usually measured in Joules or Kilojoules. The maximum amount of work extracted from a closed system is defined as Gibbs&#8217;s free energy.<\/p>\n<p>One such property was discovered in 1876 by American scientist Josiah Willard Gibbs while conducting experiments to predict the behavior of systems when combined or whether a process could occur simultaneously and spontaneously. Gibbs&#8217;s free energy was previously referred to as &#8220;available energy.&#8221; It can be represented as the amount of useful energy present in a thermodynamic system that can be used to do some work.<\/p>\n<p>According to Gibbs, the initial state of the body is such that &#8220;the body can be made to pass from it to states of dissipated energy by reversible processes.&#8221; He completely engaged his views on chemical-free energy in his magnum opus On the Equilibrium of Heterogeneous Substances, a graphical analysis of multi-phase chemical systems, published in 1876.<\/p>\n<h3><span class=\"ez-toc-section\" id=\"Standard_Gibbs_free_energy_formula\"><\/span><span style=\"color: #000000;\"><strong>Standard Gibb\u2019s free energy formula<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p>Gibb&#8217;s free energy is equivalent to the system&#8217;s enthalpy minus the product of temperature and entropy. The equation is as follows:<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>G = H \u2013 TS<\/strong><\/span><\/p>\n<p>Here,<\/p>\n<ul>\n<li>G = Gibbs free energy<\/li>\n<li>H = enthalpy<\/li>\n<li>T = temperature<\/li>\n<li>S = entropy<\/li>\n<\/ul>\n<p>OR<\/p>\n<p>or more completely as;<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>G = U + PV \u2013 TS<\/strong><\/span><\/p>\n<p>Here,<\/p>\n<ul>\n<li>U = the internal energy (SI unit: joule)<\/li>\n<li>P = pressure (SI unit: pascal)<\/li>\n<li>V = volume (SI unit: m<sup>3<\/sup>)<\/li>\n<li>T = temperature (SI unit: kelvin)<\/li>\n<li>S = entropy (SI unit: joule\/kelvin)<\/li>\n<\/ul>\n<p>The standard Gibbs free energy of formation of a compound is the change in Gibbs free energy that is followed by the formation of 1 mole of that substance from its component element available at their standard states or the most stable form of the element at 25 \u00b0C and 100 kPa. It has the symbol \u0394<sub>f<\/sub>G\u02da.<\/p>\n<p>Because there is no chance involved, all elements in their standard states (diatomic oxygen gas, graphite, etc.) have standard Gibbs free energy change of formation equal to zero.<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>\u0394<sub>f<\/sub>G = \u0394<sub>f<\/sub>G\u02da + RT ln Q<sub>f<\/sub>,<\/strong><\/span><\/p>\n<p>Here Q<sub>f<\/sub> is the reaction quotient.<\/p>\n<p>At equilibrium, \u0394<sub>f<\/sub>G = 0 and Q<sub>f<\/sub> = K, so the equation will be,<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>\u0394<sub>f<\/sub>G\u02da = \u2212RT ln K,<\/strong><\/span><\/p>\n<p>Here, K is said to be the equilibrium constant.<\/p>\n<h3><span class=\"ez-toc-section\" id=\"Relation_between_Gibbs_energy_change_and_EMF_of_a_cell\"><\/span><span style=\"color: #0000ff; font-size: 18pt;\"><strong>Relation between Gibbs energy change and EMF of a cell<\/strong><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<p>As in the case of galvanic cells, the Gibbs energy change is proportional to the cell&#8217;s electrical work.<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>\u0394G = -nFE(cell)<\/strong><\/span><\/p>\n<p>Here,<\/p>\n<ul style=\"list-style-type: square;\">\n<li>n = no. of moles of electrons involved<\/li>\n<li>F = the Faraday constant<\/li>\n<li>E = emf of the cell<\/li>\n<li>F=1 Faraday =96500 coulombs<\/li>\n<\/ul>\n<p>When reactants and products are in their standard states,<\/p>\n<p style=\"text-align: center;\"><span style=\"color: #ff0000;\"><strong>\u0394G\u00b0= \u2013nFE\u00b0cell<\/strong><\/span><\/p>\n<p><span style=\"color: #ff0000;\"><strong>Crack <span style=\"color: #0000ff;\"><a style=\"color: #0000ff;\" href=\"https:\/\/infinitylearn.com\/neet\" target=\"_blank\" rel=\"noopener\">NEET<\/a><\/span> with Result-Oriented Learning Program from Infinity Learn.<\/strong><\/span><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Introduction: Gibbs free energy, or simply Gibbs energy, is an important thermodynamic state function that describes the energy available for [&hellip;]<\/p>\n","protected":false},"author":7,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_yoast_wpseo_focuskw":"EMF of a cell","_yoast_wpseo_title":"","_yoast_wpseo_metadesc":"Gibbs energy change and emf of a cell, also identified as the Gibbs function, is a quantity used to calculate the maximum amount of work done.","custom_permalink":"blog\/neet\/relation-between-gibbs-energy-change-and-emf-of-a-cell\/"},"categories":[53,56],"tags":[],"table_tags":[],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v17.9 - 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