{"id":11899,"date":"2026-05-05T09:21:02","date_gmt":"2026-05-05T09:21:02","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=11899"},"modified":"2026-05-05T10:07:33","modified_gmt":"2026-05-05T10:07:33","slug":"free-energy-gibbs-and-helmholtz","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/iit-jam\/free-energy-gibbs-and-helmholtz\/","title":{"rendered":"Free energy (Gibbs and Helmholtz): Master IIT JAM 2027"},"content":{"rendered":"<p><strong>Free energy (Gibbs and Helmholtz)<\/strong> For IIT JAM is a fundamental concept in physical chemistry, used to determine the spontaneity of a reaction and predict the direction of a process. It&#8217;s crucial for CSIR NET, IIT JAM, CUET PG, and GATE aspirants to grasp this concept.<\/p>\n<h2><strong>Syllabus: Thermodynamics and Kinetics (IIT JAM, CSIR NET)<\/strong><\/h2>\n<p>The topic of <strong>Free energy<\/strong> (Gibbs and Helmholtz) For IIT JAM is a crucial part of the syllabus for various competitive exams, including IIT JAM and CSIR NET. Specifically, it falls under the unit Chemical Thermodynamics in the <a href=\"https:\/\/jam2026.iitb.ac.in\/files\/syllabus_CY.pdf\" rel=\"nofollow noopener\" target=\"_blank\"><strong>IIT JAM syllabus<\/strong><\/a>, which is conducted by the National Testing Agency (NTA).<\/p>\n<p>In the context of IIT JAM, this topic is covered under the Thermodynamics and Kinetics section. Students preparing for these exams can refer to standard textbooks such as Atkins&#8217; Physical Chemistry and Levine&#8217;s Physical Chemistry, which comprehensively cover the concepts of Gibbs function, including Gibbs and Helmholtz <strong>free energy<\/strong>.<\/p>\n<ul>\n<li>CSIR NET: Physical Chemistry (Unit)<\/li>\n<li>IIT JAM: Thermodynamics and Kinetics (Section)<\/li>\n<\/ul>\n<p>These textbooks provide in-depth explanations and are widely recommended for students pursuing physical chemistry and related courses.<\/p>\n<h2><strong>Introduction to Free Energy (Gibbs and Helmholtz) For IIT JAM<\/strong><\/h2>\n<p>The concept of <strong>free energy<\/strong> is crucial in understanding the spontaneity of thermodynamic processes. Gibbs function is a measure of the maximum amount of work that can be extracted from a system at constant temperature and pressure. There are two types of<strong> free energy<\/strong> functions: <strong>Gibbs free energy<\/strong> (G)and <strong>Helmholtz free energy<\/strong> (A).<\/p>\n<p>The Gibbs Thermodynamic potential is defined as G = H &#8211; TS, where H is the enthalpy, T is the temperature, and S is the entropy. On the other hand, the Helmholtz Gibbs function is defined as A = U &#8211; TS, where U\u00a0 \u00a0 \u00a0is the internal energy. Both functions are essential in determining the spontaneity of a process.<\/p>\n<p>The importance of Thermodynamic potential lies in its ability to predict the spontaneity of a process. A negative change in Gibbs function (\u2206G&lt; 0or\u2206A&lt; 0) indicates a spontaneous process, while a positive change indicates a non-spontaneous process. The key factors influencing <strong>free energy<\/strong> are the enthalpy, entropy, and temperature of the system.<\/p>\n<p>Understanding Gibbs function (Gibbs and Helmholtz) For IIT JAM is vital for students preparing for CSIR NET, IIT JAM, and GATE exams. These concepts are fundamental to thermodynamics and are widely used to analyze the behavior of physical and chemical systems.<\/p>\n<h2><strong>Gibbs Free Energy and the Gibbs-Helmholtz Equation<\/strong><\/h2>\n<p>The Gibbs <strong>free energy<\/strong>(G) is a thermodynamic potential that measures the maximum amount of work that can be performed by a system at constant temperature and pressure. It is defined as G = H &#8211; TS, where H is the enthalpy, T is the temperature, and S is the entropy.<\/p>\n<p>The Gibbs-Helmholtz equation relates the change in Gibbs Gibbs function to the change in temperature : d(G\/T)\/dT = -H\/T^2. This equation is useful for understanding how the spontaneity of a reaction changes with temperature. For students preparing for <strong>Free energy<\/strong> (Gibbs and Helmholtz) For IIT JAM, it is essential to grasp this concept.<\/p>\n<p>The Gibbs Thermodynamic potential change(\u0394G) determines the spontaneity of a reaction. A negative\u0394Gindicates a spontaneous reaction, while a positive\u0394Gindicates a non-spontaneous reaction. At equilibrium,\u0394Gis zero. Understanding the relationship between Gibbs Gibbs function and spontaneity is crucial for<strong> Free energy<\/strong> (Gibbs and Helmholtz) For IIT JAM and other competitive exams.<\/p>\n<h2><strong>Helmholtz Free Energy and its Significance<\/strong><\/h2>\n<p>The Helmholtz <strong>free energy<\/strong>, denoted by A, is a thermodynamic potential that measures the maximum amount of work that can be extracted from a system at constant temperature and volume. It is defined as A = U &#8211; TS, where U is the internal energy, T is the temperature, and S is the entropy.<\/p>\n<p>The relationship between Helmholtz Gibbs function and internal energy is given by the equation dA = dU &#8211; TdS. At constant temperature, the change in Helmholtz <strong>free energy<\/strong> is equal to the change in internal energy minus the product of temperature and change in entropy. This indicates that A is a measure of the internal energy that is available to do work.<\/p>\n<p>The Helmholtz Thermodynamic potential isothermal processes, where the temperature remains constant. In such processes, the change in Helmholtz Gibbs function dA is a measure of the maximum amount of work that can be done by the system. This makes A a useful quantity in the context of <strong>Free energy<\/strong> (Gibbs and Helmholtz) For IIT JAM and other related topics in thermodynamics. Understanding Helmholtz free energy is essential for students preparing for exams like CSIR NET, IIT JAM, and GATE.<\/p>\n<h2><strong>Common Misconceptions about Free Energy (Gibbs and Helmholtz) For IIT JAM<\/strong><\/h2>\n<p>Students often harbor misconceptions about <strong>free energy<\/strong>, specifically Gibbs and Helmholtz Gibbs function, which are crucial concepts in thermodynamics. One common misconception is that <strong>free energy<\/strong> is only related to temperature. This understanding is incorrect because <strong>free energy<\/strong>, particularly Gibb<strong>s free energy<\/strong>, is a function of both temperature and pressure.<\/p>\n<p>Gibbs Gibbs function is defined as \u0394G = \u0394H &#8211; T\u0394S, where \u0394H is the enthalpy change, T is the temperature in Kelvin, and \u0394S is the entropy change. This equation shows that \u0394G depends on both temperature and the enthalpy and entropy changes of a system. Helmholtz <strong>free energy<\/strong>, on the other hand, is defined as \u0394F = \u0394U &#8211; T\u0394S, where \u0394U is the internal energy change.<\/p>\n<p>Another misconception is that all reactions are spontaneous if their Gibbs function change (\u0394G or \u0394F) is negative. However, spontaneity is determined by the sign of \u0394G under specific conditions of temperature and pressure, not solely by the negative value of <strong>free energy<\/strong> change. A negative \u0394G indicates a thermodynamically favorable process, but kinetics also determining the rate of a reaction.<\/p>\n<p>It is also mistakenly believed that<strong> free energy<\/strong> is not important in kinetics. Gibbs function change provides essential information about the feasibility and spontaneity of a reaction. While kinetics tells us about the rate of a reaction, thermodynamics, through<strong> free energy<\/strong>, informs us about the reaction&#8217;s feasibility and equilibrium position. Understanding\u0394G = \u0394H &#8211; T\u0394Sand\u0394F = \u0394U &#8211; T\u0394Sequations helps in evaluating the thermodynamic stability and spontaneity, complementing kinetic studies.<\/p>\n<h2><strong>Practice Problems: Free Energy (Gibbs and Helmholtz) For IIT JAM<\/strong><\/h2>\n<p>Gibbs<strong> free energy<\/strong> is a measure of the energy available to do work in a system at constant temperature and pressure. It is defined as G = H &#8211; TS, where His the enthalpy, T is the temperature, and S is the entropy.<\/p>\n<p>Practice Problem 1:Calculate the Gibbs function change for the reaction CO(g) + 1\/2O2(g) \u2192 CO2(g)at 298 K, given that\u0394H= -283 kJ\/mol and\u0394S= -87 J\/(mol\u00b7K). Assume the reaction occurs at constant temperature and pressure.<\/p>\n<p>The Gibbs Thermodynamic potential change is given by \u0394G = \u0394H &#8211; T\u0394S. Substituting the given values, we get\u0394G = -283 kJ\/mol &#8211; (298 K)(-87 J\/(mol\u00b7K))= -283 kJ\/mol + 25.9 kJ\/mol = -257.1 kJ\/mol.<\/p>\n<p>Practice Problem 2:Determine the spontaneity of the reactionN2(g) + 3H2(g) \u2192 2NH3(g)at 298 K, given that\u0394G= 33 kJ\/mol. A negative\u0394Gindicates a spontaneous reaction.<\/p>\n<p>Since\u0394Gis positive (33 kJ\/mol), the reaction is non-spontaneous under standard conditions.<\/p>\n<p>Practice Problem 3:For a certain reaction,\u0394U= -100 kJ\/mol and\u0394S= 0.1 kJ\/(mol\u00b7K). At what temperature will\u0394G= 0? The relationship between\u0394G,\u0394U, and\u0394Sis given by\u0394G = \u0394U &#8211; T\u0394Sfor a reaction at constant volume or\u0394G = \u0394H &#8211; T\u0394Sat constant pressure.<\/p>\n<p>At\u0394G= 0,0 = \u0394U &#8211; T\u0394SorT = \u0394U \/ \u0394S. However, to use this equation directly,\u0394Hshould be used instead of\u0394Ufor constant pressure processes. Assuming\u0394H\u2248\u0394Ufor simplicity and given\u0394Sin kJ,T = -100 kJ\/mol \/ 0.1 kJ\/(mol\u00b7K) = 1000 K. <strong>Free energy<\/strong> (Gibbs and Helmholtz) For IIT JAM problems often test understanding of these relationships.<\/p>\n<h2><strong>Final Thoughts\u00a0<\/strong><\/h2>\n<p>mastering the concepts of Gibbs and Helmholtz <strong>free energy<\/strong> is a strategic necessity for any serious chemistry aspirant. Moving beyond rote memorization of formulas to truly understanding the thermodynamic implications of spontaneity will give you a significant competitive edge in exams like the IIT JAM. As you navigate these complex principles, remember that consistent practice with numerical problems is just as critical as achieving conceptual clarity. For structured guidance and expert-curated practice materials that simplify these challenging thermodynamic topics, <a href=\"https:\/\/www.vedprep.com\/online-courses\/iit-jam\"><strong>VedPrep<\/strong> <\/a>offers the comprehensive resources you need to excel in your upcoming examinations. Stay consistent, keep analyzing those energy relationships, and you will undoubtedly strengthen your physical chemistry foundation for success.<\/p>\n<p>To know more in detail from our faculty, watch our YouTube video:<\/p>\n<p class=\"responsive-video-wrap clr\"><iframe title=\"Thermodynamics | Gibbs Free Energy | Criteria of Spontaneity | CSIR NET | GATE |  IIT JAM\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/Offgp2BmK1c?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe><\/p>\n<section>\n<h2><strong>Frequently Asked Questions<\/strong><\/h2>\n<\/section>\n<style>#sp-ea-14875 .spcollapsing { height: 0; overflow: hidden; transition-property: height;transition-duration: 300ms;}#sp-ea-14875.sp-easy-accordion>.sp-ea-single {margin-bottom: 10px; border: 1px solid #e2e2e2; }#sp-ea-14875.sp-easy-accordion>.sp-ea-single>.ea-header a {color: #444;}#sp-ea-14875.sp-easy-accordion>.sp-ea-single>.sp-collapse>.ea-body {background: #fff; color: #444;}#sp-ea-14875.sp-easy-accordion>.sp-ea-single {background: #eee;}#sp-ea-14875.sp-easy-accordion>.sp-ea-single>.ea-header a .ea-expand-icon { float: left; color: #444;font-size: 16px;}<\/style><div id=\"sp_easy_accordion-1777973003\">\n<div id=\"sp-ea-14875\" class=\"sp-ea-one sp-easy-accordion\" data-ea-active=\"ea-click\" data-ea-mode=\"vertical\" data-preloader=\"\" data-scroll-active-item=\"\" data-offset-to-scroll=\"0\">\n\n<!-- Start accordion card div. -->\n<div class=\"ea-card ea-expand sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148750\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148750\" aria-controls=\"collapse148750\" href=\"#\"  aria-expanded=\"true\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-minus\"><\/i> What is Free energy (Gibbs and Helmholtz) in physical chemistry?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse collapsed show\" id=\"collapse148750\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148750\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Free energy (Gibbs and Helmholtz) represents thermodynamic potentials that measure the maximum amount of \"useful\" work a system can perform at constant temperature and pressure (Gibbs) or constant temperature and volume (Helmholtz).<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148751\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148751\" aria-controls=\"collapse148751\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is understanding Free energy (Gibbs and Helmholtz) important for IIT JAM 2027?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148751\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148751\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It is a cornerstone of the Chemical Thermodynamics unit. IIT JAM examiners frequently test the ability to predict reaction spontaneity using these functions, making it a high-weightage topic.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148752\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148752\" aria-controls=\"collapse148752\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the fundamental difference between Gibbs and Helmholtz free energy?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148752\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148752\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Gibbs free energy (<span class=\"math-inline\" data-math=\"G = H - TS\" data-index-in-node=\"98\">G = H - TS<\/span>) is used for processes at constant temperature and pressure, whereas Helmholtz free energy (<span class=\"math-inline\" data-math=\"A = U - TS\" data-index-in-node=\"201\">A = U - TS<\/span>) is applied to processes at constant temperature and volume.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148753\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148753\" aria-controls=\"collapse148753\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Is Free energy (Gibbs and Helmholtz) a state function?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148753\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148753\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, both Gibbs and Helmholtz free energy are state functions, meaning their values depend only on the current state of the system (temperature, pressure, volume, composition), not on the path taken to reach that state.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148754\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148754\" aria-controls=\"collapse148754\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can Helmholtz free energy be used to predict spontaneity?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148754\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148754\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, at constant temperature and volume, a decrease in Helmholtz free energy (\u0394<span class=\"math-inline\" data-math=\"\\Delta A &lt; 0\" data-index-in-node=\"139\">A &lt; 0<\/span>) indicates a spontaneous process.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148755\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148755\" aria-controls=\"collapse148755\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What are the key variables that influence Gibbs free energy?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148755\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148755\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Gibbs free energy is influenced by enthalpy (\u0394<span class=\"math-inline\" data-math=\"\\Delta H\" data-index-in-node=\"109\">H<\/span>), entropy (\u0394<span class=\"math-inline\" data-math=\"\\Delta S\" data-index-in-node=\"129\">S<\/span>), and temperature (<span class=\"math-inline\" data-math=\"T\" data-index-in-node=\"157\">T<\/span>), as defined by the relation \u0394<span class=\"math-inline\" data-math=\"\\Delta G = \\Delta H - T\\Delta S\" data-index-in-node=\"188\">G = \u0394H - T\u0394S<\/span>.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148756\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148756\" aria-controls=\"collapse148756\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the role of Free energy (Gibbs and Helmholtz) in kinetics?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148756\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148756\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>While thermodynamics (via free energy) tells us if a reaction is <i data-path-to-node=\"11\" data-index-in-node=\"136\">feasible<\/i> (spontaneous), it does not determine the <i data-path-to-node=\"11\" data-index-in-node=\"186\">rate<\/i> of the reaction; that is the domain of chemical kinetics.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148757\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148757\" aria-controls=\"collapse148757\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Does temperature affect the spontaneity of a reaction?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148757\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148757\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes. In the equation \u0394<span class=\"math-inline\" data-math=\"\\Delta G = \\Delta H - T\\Delta S\" data-index-in-node=\"80\">G = \u0394H - T\u0394S<\/span>, the temperature <span class=\"math-inline\" data-math=\"T\" data-index-in-node=\"129\">T<\/span>\u00a0can change the sign of \u0394<span class=\"math-inline\" data-math=\"\\Delta G\" data-index-in-node=\"154\">G<\/span>, meaning a reaction can be spontaneous at high temperatures but non-spontaneous at low temperatures (or vice versa).<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148758\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148758\" aria-controls=\"collapse148758\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What does \"Free\" mean in Free energy?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148758\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148758\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>\"Free\" refers to the portion of the system's total internal energy that is \"free\" or available to be converted into useful work, rather than being \"bound\" as heat (<span class=\"math-inline\" data-math=\"TS\" data-index-in-node=\"206\">TS<\/span>).<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-148759\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148759\" aria-controls=\"collapse148759\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Are these concepts covered in the IIT JAM 2027 syllabus?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse148759\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-148759\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, Free energy (Gibbs and Helmholtz) is a core component of the \"Thermodynamics and Kinetics\" section in the official IIT JAM Chemistry syllabus.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-1487510\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1487510\" aria-controls=\"collapse1487510\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is Gibbs free energy more commonly used than Helmholtz in chemistry?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse1487510\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-1487510\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Most chemical reactions occur under conditions of constant atmospheric pressure rather than constant volume, making Gibbs free energy a more practical tool for laboratory and industrial chemistry.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-1487511\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1487511\" aria-controls=\"collapse1487511\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does entropy affect Free energy (Gibbs and Helmholtz)?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse1487511\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-1487511\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Entropy represents the degree of disorder. A higher entropy change (\u0394<span class=\"math-inline\" data-math=\"\\Delta S &gt; 0\" data-index-in-node=\"131\">S &gt; 0<\/span>) generally contributes to a more negative \u0394<span class=\"math-inline\" data-math=\"\\Delta G\" data-index-in-node=\"186\">G<\/span>, favoring spontaneity, especially at higher temperatures.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-1487512\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1487512\" aria-controls=\"collapse1487512\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can a non-spontaneous reaction be made spontaneous?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse1487512\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-1487512\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, by coupling a non-spontaneous reaction with a highly spontaneous one, or by changing the experimental conditions like temperature or concentration to alter the sign of \u0394<span class=\"math-inline\" data-math=\"\\Delta G\" data-index-in-node=\"229\">G<\/span>.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-1487513\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1487513\" aria-controls=\"collapse1487513\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Which textbooks are best for studying Free energy (Gibbs and Helmholtz) for IIT JAM?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse1487513\" data-parent=\"#sp-ea-14875\" role=\"region\" aria-labelledby=\"ea-header-1487513\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Atkins' Physical Chemistry and Levine's Physical Chemistry are highly recommended for mastering these concepts for competitive exams like IIT JAM and CSIR NET.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<\/div>\n<\/div>\n\n","protected":false},"excerpt":{"rendered":"<p>Understanding Free Energy (Gibbs and Helmholtz) For IIT JAM is crucial for CSIR NET, IIT JAM, CUET PG, and GATE aspirants. It determines the spontaneity of a reaction and predicts the direction of a process.<\/p>\n","protected":false},"author":12,"featured_media":11898,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","rank_math_seo_score":85},"categories":[23],"tags":[2923,6586,6587,6588,861,2922],"class_list":["post-11899","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-iit-jam","tag-competitive-exams","tag-free-energy-gibbs-and-helmholtz-for-iit-jam","tag-free-energy-gibbs-and-helmholtz-for-iit-jam-notes","tag-free-energy-gibbs-and-helmholtz-for-iit-jam-questions","tag-physical-chemistry","tag-vedprep","entry","has-media"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/11899","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=11899"}],"version-history":[{"count":8,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/11899\/revisions"}],"predecessor-version":[{"id":14886,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/11899\/revisions\/14886"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/11898"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=11899"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=11899"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=11899"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}