{"id":12503,"date":"2026-05-15T12:19:08","date_gmt":"2026-05-15T12:19:08","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=12503"},"modified":"2026-05-15T12:26:23","modified_gmt":"2026-05-15T12:26:23","slug":"equilibrium-constant","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/iit-jam\/equilibrium-constant\/","title":{"rendered":"Equilibrium Constant (Kp, Kc, Kx): Master IIT JAM 2027"},"content":{"rendered":"<p><strong>Equilibrium constant<\/strong> (Kp, Kc, Kx) For IIT JAM is a crucial concept in physical chemistry that describes the equilibrium between reactants and products in a chemical reaction, with Kp and Kc representing different units of measurement.<\/p>\n<h2><strong>Chemical Equilibrium Syllabus for IIT JAM, CSIR NET, and GATE<\/strong><\/h2>\n<p data-path-to-node=\"5\">If you open up Chapter 2 of the <strong><a href=\"https:\/\/jam2026.iitb.ac.in\/files\/syllabus_CY.pdf\" rel=\"nofollow noopener\" target=\"_blank\">IIT JAM Physical Chemistry syllabus<\/a><\/strong>, you\u2019ll find chemical equilibrium sitting right there. It\u2019s a heavyweight topic. If you love flipping through classic textbooks, you\u2019ve probably seen this broken down beautifully in <i data-path-to-node=\"5\" data-index-in-node=\"250\">Physical Chemistry<\/i> by Atkins and De Paula, or McQuarrie and Simon\u2019s <i data-path-to-node=\"5\" data-index-in-node=\"318\">Physical Chemistry: A Molecular Approach<\/i>.<\/p>\n<p data-path-to-node=\"6\">These books do a great job with the deep theory, but when you&#8217;re in the exam hall, you need to know how to apply that theory fast. That&#8217;s why we at VedPrep love breaking these down into actionable shortcuts. At its core, the <strong>equilibrium constant<\/strong> is just a ratio that tells you if you\u2019ve got more products or reactants when the reaction finally settles down.<\/p>\n<h2><strong>Understanding Equilibrium Constant (Kp, Kc, Kx) For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"9\">Imagine a crowded coffee shop. People are walking in, and people are leaving. Equilibrium isn&#8217;t when the inside of the shop looks empty; it\u2019s when the rate of people entering perfectly matches the rate of people walking out. The total number of people inside stays constant.<\/p>\n<p data-path-to-node=\"10\">In chemistry, the <strong>equilibrium constant<\/strong> tracks this balance, but we use different versions depending on what state of matter we are dealing with:<\/p>\n<ul data-path-to-node=\"11\">\n<li>\n<p data-path-to-node=\"11,0,0\"><b data-path-to-node=\"11,0,0\" data-index-in-node=\"0\"><span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"0\">K<sub>c<\/sub><\/span>\u00a0(Concentration):<\/b> This is your go-to for aqueous solutions. We measure the species in molarity (moles per liter).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"11,1,0\"><b data-path-to-node=\"11,1,0\" data-index-in-node=\"0\"><span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"0\">K<sub>p<\/sub><\/span>\u00a0(Partial Pressure):<\/b> Used when gases are playing the main role. Instead of molarity, we track the individual pressure each gas exerts.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"11,2,0\"><b data-path-to-node=\"11,2,0\" data-index-in-node=\"0\"><span class=\"math-inline\" data-math=\"K_x\" data-index-in-node=\"0\">K<sub>x<\/sub><\/span>\u00a0(Mole Fraction):<\/b> This looks at the ratio of moles of one component to the total moles. It&#8217;s incredibly handy for mixtures and complex systems.<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"12\">A quick heads-up: while some older texts casually call these &#8220;dissociation constants,&#8221; they are all specific types of equilibrium constants. The one you choose simply depends on the units you have on hand.<\/p>\n<h2><strong>Worked Example: Equilibrium Constant (Kp, Kc, Kx) For IIT JAM<\/strong><\/h2>\n<p>Let\u2019s look at a classic problem you might encounter on exam day:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-16524 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium-Constant-300x55.png\" alt=\"Equilibrium Constant\" width=\"300\" height=\"55\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium-Constant-300x55.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium-Constant.png 362w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p>Imagine this reaction is trapped in a closed container at a total pressure of <span class=\"math-inline\" data-math=\"100\\text{ bar}\" data-index-in-node=\"78\">100 bar<\/span>. After things settle down, a sensor tells us the mole fractions (<span class=\"math-inline\" data-math=\"x_i\" data-index-in-node=\"158\">x<sub>i<\/sub><\/span>) for <span class=\"math-inline\" data-math=\"\\text{CO}\" data-index-in-node=\"167\">CO<\/span>, <span class=\"math-inline\" data-math=\"\\text{H}_2\" data-index-in-node=\"178\">H<sub>2<\/sub><\/span>, and <span class=\"math-inline\" data-math=\"\\text{CH}_3\\text{OH}\" data-index-in-node=\"194\">CH<sub>3<\/sub>OH<\/span> are <span class=\"math-inline\" data-math=\"0.2\" data-index-in-node=\"219\">0.2<\/span>, <span class=\"math-inline\" data-math=\"0.4\" data-index-in-node=\"224\">0.4<\/span>, and <span class=\"math-inline\" data-math=\"0.4\" data-index-in-node=\"233\">0.4<\/span>.<\/p>\n<p data-path-to-node=\"18\">To find <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"8\">K<sub>p<\/sub><\/span>, we need partial pressures first. We get these by multiplying each mole fraction by the total pressure (<span class=\"math-inline\" data-math=\"p_i = x_i \\times P_{\\text{total}}\" data-index-in-node=\"116\">p<sub>i<\/sub> = x<sub>i<\/sub> \u00d7 P<sub>total<\/sub><\/span>:<\/p>\n<ul data-path-to-node=\"19\">\n<li>\n<p data-path-to-node=\"19,0,0\"><span class=\"math-inline\" data-math=\"p_{\\text{CO}} = 0.2 \\times 100 = 20\\text{ bar}\" data-index-in-node=\"0\">p<sub>CO<\/sub> = 0.2 \u00d7 100 = 20 bar<\/span><\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"19,1,0\"><span class=\"math-inline\" data-math=\"p_{\\text{H}_2} = 0.4 \\times 100 = 40\\text{ bar}\" data-index-in-node=\"0\">pH<sub>2<\/sub> = 0.4 \u00d7 100 = 40 bar<\/span><\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"19,2,0\"><span class=\"math-inline\" data-math=\"p_{\\text{CH}_3\\text{OH}} = 0.4 \\times 100 = 40\\text{ bar}\" data-index-in-node=\"0\">pCH<sub>3<\/sub>OH = 0.4 \u00d7 100 = 40 bar<\/span><\/p>\n<\/li>\n<\/ul>\n<p>Now, write out the expression for <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"34\">K<sub>p<\/sub><\/span>. Remember, products go on top, reactants on the bottom, and coefficients become exponents:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16527 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/coefficients.png\" alt=\"coefficients\" width=\"227\" height=\"96\" \/><\/p>\n<p>Plug in our numbers:<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-16529 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Plug-in-our-numbers-300x38.png\" alt=\"Plug in our numbers\" width=\"300\" height=\"38\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Plug-in-our-numbers-300x38.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Plug-in-our-numbers.png 691w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<h2><strong>Application of Equilibrium Constant (Kp, Kc, Kx) For IIT JAM in Real-World Scenarios<\/strong><\/h2>\n<p>To make this feel less like abstract math, let\u2019s look at a fictional scenario. Imagine a chemical engineer named Sarah who runs a massive industrial plant trying to make ammonia via the Haber-Bosch process:<\/p>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-16530 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium--300x60.png\" alt=\"Equilibrium\" width=\"300\" height=\"60\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium--300x60.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Equilibrium-.png 362w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p data-path-to-node=\"29\">If Sarah blindly mixes the gases without checking <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"50\">K<sub>p<\/sub><\/span>, she might end up wasting thousands of dollars producing almost nothing. By using the<strong> equilibrium constant<\/strong>, she knows exactly how much pressure to apply to force the reaction to favor ammonia.<\/p>\n<p data-path-to-node=\"30\">The same logic applies when creating methanol from carbon monoxide and hydrogen. Companies use <span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"95\">K<sub>c<\/sub><\/span>\u00a0to figure out the sweet spot for temperature and pressure so they don&#8217;t waste energy. From developing new pharmaceuticals to designing wastewater treatment filters, these constants give engineers a predictable blueprint of what a chemical system will do before they even turn on the machines.<\/p>\n<h2><strong>Exam Strategy: Equilibrium Constant (Kp, Kc, Kx) For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"33\">When you are prepping for IIT JAM, you can&#8217;t just memorize definitions. You need a game plan. The examiners love to test how you handle shifts and changes.<\/p>\n<p data-path-to-node=\"34\">Here are the absolute essentials you need to focus on:<\/p>\n<ul data-path-to-node=\"35\">\n<li>\n<p data-path-to-node=\"35,0,0\"><b data-path-to-node=\"35,0,0\" data-index-in-node=\"0\">Units matter:<\/b> Pay close attention to whether the question asks for <span class=\"math-inline\" data-math=\"\\text{bar}\" data-index-in-node=\"67\">bar<\/span>, <span class=\"math-inline\" data-math=\"\\text{atm}\" data-index-in-node=\"79\">atm<\/span>, or <span class=\"math-inline\" data-math=\"\\text{mol\/L}\" data-index-in-node=\"94\">mol\/L<\/span>.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"35,1,0\"><b data-path-to-node=\"35,1,0\" data-index-in-node=\"0\">The Interconversions:<\/b> You must know how to switch between constants effortlessly.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"35,2,0\"><b data-path-to-node=\"35,2,0\" data-index-in-node=\"0\">Le Chatelier\u2019s Principle:<\/b> Understand how changing temperature or pressure shifts the equilibrium position, and more importantly, how temperature is the <i data-path-to-node=\"35,2,0\" data-index-in-node=\"152\">only<\/i> thing that actually changes the value of <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"198\">K<sub>p<\/sub><\/span> and <span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"206\">K<sub>c<\/sub><\/span>.<\/p>\n<\/li>\n<\/ul>\n<p>At <a href=\"https:\/\/www.vedprep.com\/online-courses\"><strong>VedPrep<\/strong><\/a>, we always tell students that practicing a wide variety of problems is the only way to build true speed. Working through mock tests helps you spot the tricks examiners hide in the question text before they catch you off guard.<\/p>\n<h2><strong>Important Equations and Formulas for Equilibrium Constant (Kp, Kc, Kx) For IIT JAM<\/strong><\/h2>\n<p>Let&#8217;s lay out the mathematical tools you need. For a standard hypothetical reaction:<\/p>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16535 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/hypothetical-reaction.png\" alt=\"hypothetical reaction\" width=\"271\" height=\"47\" \/><\/p>\n<p>Here are the formulas you should commit to memory:<\/p>\n<h3 data-path-to-node=\"42\">1. The Core Expressions<\/h3>\n<ul data-path-to-node=\"43\">\n<li>\n<p data-path-to-node=\"43,0,0\"><b data-path-to-node=\"43,0,0\" data-index-in-node=\"0\">For Concentration:<\/b><\/p>\n<\/li>\n<\/ul>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16537 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Concentration.png\" alt=\"Concentration\" width=\"197\" height=\"82\" \/><\/p>\n<ul>\n<li><strong>For Partial Pressure:<\/strong><\/li>\n<\/ul>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16541 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Partial-Pressure.png\" alt=\"Partial Pressure\" width=\"215\" height=\"86\" \/><\/p>\n<ul>\n<li><strong>For Mole Fraction:<\/strong><\/li>\n<\/ul>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16543 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Mole-Fraction.png\" alt=\"Mole Fraction\" width=\"210\" height=\"70\" \/><\/p>\n<h3 data-path-to-node=\"44\">2. The Bridge Equations<\/h3>\n<p data-path-to-node=\"45\">The real magic happens when you need to link these together.<\/p>\n<ul data-path-to-node=\"46\">\n<li>\n<p data-path-to-node=\"46,0,0\"><strong>Connecting <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"11\">K<sub>p<\/sub><\/span> and <span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"19\">K<sub>c<\/sub><\/span>:<\/strong><\/p>\n<\/li>\n<\/ul>\n<p><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16545 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Bridge-Equation.png\" alt=\"Bridge Equation\" width=\"205\" height=\"60\" \/><\/p>\n<ul>\n<li><strong>Connecting <span class=\"math-inline\" data-math=\"K_x\" data-index-in-node=\"11\">K<sub>x<\/sub><\/span> and <span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"19\">K<sub>c<\/sub><\/span>:<\/strong><\/li>\n<\/ul>\n<p style=\"text-align: center;\"><strong><img loading=\"lazy\" loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-16550\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Bridge-Equations.png\" alt=\"Bridge Equations\" width=\"227\" height=\"82\" \/><\/strong><\/p>\n<p><b data-path-to-node=\"47,0\" data-index-in-node=\"0\">Note on \u0394<span class=\"math-inline\" data-math=\"\\Delta n\" data-index-in-node=\"8\">n<\/span>:<\/b> This is just the number of moles of gaseous products minus the moles of gaseous reactants (\u0394<span class=\"math-inline\" data-math=\"\\Delta n = (c+d) - (a+b)\" data-index-in-node=\"109\">n = (c+d) &#8211; (a+b)<\/span>). If \u0394<span class=\"math-inline\" data-math=\"\\Delta n = 0\" data-index-in-node=\"139\">n = 0<\/span>, then <span class=\"math-inline\" data-math=\"K_p = K_c = K_x\" data-index-in-node=\"158\">K<sub>p<\/sub> = K<sub>c<\/sub> = K<sub>x<\/sub><\/span>, which is a favorite shortcut for exam setters!<\/p>\n<h2><strong>Final Thoughts<\/strong><\/h2>\n<p data-path-to-node=\"50\">Mastering the<strong> equilibrium constant<\/strong> for IIT JAM is less about mindless memorization and more about training your brain to think with analytical precision. Once you see how <span class=\"math-inline\" data-math=\"K_p\" data-index-in-node=\"171\">K<sub>p<\/sub><\/span>, <span class=\"math-inline\" data-math=\"K_c\" data-index-in-node=\"176\">K<sub>c<\/sub><\/span>, and <span class=\"math-inline\" data-math=\"K_x\" data-index-in-node=\"185\">K<sub>x<\/sub><\/span>\u00a0connect, the problems start solving themselves.<\/p>\n<p data-path-to-node=\"51\">We know how overwhelming exam prep can feel when you are balancing multiple subjects. That\u2019s exactly why we create targeted study materials and specific mock tests here at <a href=\"https:\/\/www.vedprep.com\/online-courses\/iit-jam\"><strong>VedPrep<\/strong><\/a>\u2014to help take the guesswork out of your routine. Keep working through the problems and get comfortable with the unit conversions, and you&#8217;ll find yourself cruising through the physical chemistry section with confidence.<\/p>\n<p data-path-to-node=\"51\">To know more in detail from our faculty, watch our YouTube video:<\/p>\n<p class=\"responsive-video-wrap clr\"><iframe title=\"\ud83d\udd25 Chemical Equilibrium Demo Class | Sanskar &amp; Super Batch Demo for IIT JAM, CSIR NET, GATE | VedPrep\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/N51YOEH-lLw?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-14898 .spcollapsing { height: 0; overflow: hidden; transition-property: height;transition-duration: 300ms;}#sp-ea-14898.sp-easy-accordion>.sp-ea-single {margin-bottom: 10px; border: 1px solid #e2e2e2; }#sp-ea-14898.sp-easy-accordion>.sp-ea-single>.ea-header a {color: #444;}#sp-ea-14898.sp-easy-accordion>.sp-ea-single>.sp-collapse>.ea-body {background: #fff; color: #444;}#sp-ea-14898.sp-easy-accordion>.sp-ea-single {background: #eee;}#sp-ea-14898.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-1777982609\">\n<div id=\"sp-ea-14898\" 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-148980\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148980\" aria-controls=\"collapse148980\" 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 the equilibrium constant?\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=\"collapse148980\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148980\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant is a value that describes the ratio of the concentrations of products to reactants at equilibrium in a reversible chemical reaction.<\/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-148981\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148981\" aria-controls=\"collapse148981\" 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 Kp, Kc, and Kx?\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=\"collapse148981\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148981\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">Kp, Kc, and Kx are equilibrium constants expressed in terms of partial pressures, concentrations, and mole fractions, respectively.<\/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-148982\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148982\" aria-controls=\"collapse148982\" 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 is Kc related to Kp?\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=\"collapse148982\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148982\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">Kp and Kc are related by the equation Kp = Kc(RT)<sup>\u0394n<\/sup>, where \u0394n is the difference in the number of moles of gas between products and reactants.<\/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-148983\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148983\" aria-controls=\"collapse148983\" 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 significance of Kx?\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=\"collapse148983\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148983\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">Kx is the equilibrium constant expressed in terms of mole fractions, which is useful for reactions involving gases or non-ideal solutions.<\/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-148984\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148984\" aria-controls=\"collapse148984\" 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 is equilibrium constant related to reaction quotient?\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=\"collapse148984\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148984\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The reaction quotient (Q) is the ratio of product concentrations to reactant concentrations at any point in the reaction, while the equilibrium constant (K) is the value of Q at equilibrium.<\/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-148985\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148985\" aria-controls=\"collapse148985\" 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 units of equilibrium constant?\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=\"collapse148985\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148985\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The units of Kc depend on the reaction, while Kp is unitless. Kx is also unitless.<\/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-148986\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148986\" aria-controls=\"collapse148986\" 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 equilibrium constant be negative?\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=\"collapse148986\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148986\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">No, the equilibrium constant is always positive.<\/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-148987\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148987\" aria-controls=\"collapse148987\" 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 to calculate Kp from Kc?\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=\"collapse148987\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148987\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">To calculate Kp from Kc, use the equation Kp = Kc(RT)<sup>\u0394n<\/sup> and ensure that the units are consistent.<\/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-148988\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148988\" aria-controls=\"collapse148988\" 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 applications of equilibrium constant 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 \" id=\"collapse148988\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148988\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant has numerous applications in Physical Chemistry, including predicting reaction spontaneity and calculating concentrations at equilibrium.<\/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-148989\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse148989\" aria-controls=\"collapse148989\" 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 to determine the equilibrium constant experimentally?\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=\"collapse148989\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-148989\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant can be determined experimentally by measuring the concentrations of reactants and products at equilibrium and then calculating K.<\/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-1489810\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1489810\" aria-controls=\"collapse1489810\" 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 factors affecting equilibrium constant?\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=\"collapse1489810\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-1489810\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant is affected by temperature, but not by concentration or pressure.<\/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-1489811\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1489811\" aria-controls=\"collapse1489811\" 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 a common mistake when calculating equilibrium constant?\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=\"collapse1489811\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-1489811\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">A common mistake is to confuse the reaction quotient (Q) with the equilibrium constant (K).<\/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-1489812\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1489812\" aria-controls=\"collapse1489812\" 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 to avoid errors in calculating Kp and Kc?\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=\"collapse1489812\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-1489812\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">Ensure that the units are consistent and that \u0394n is calculated correctly.<\/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-1489813\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1489813\" aria-controls=\"collapse1489813\" 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 relationship between equilibrium constant and 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=\"collapse1489813\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-1489813\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant is related to the Gibbs free energy change by \u0394G = -RT ln(K).<\/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-1489814\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse1489814\" aria-controls=\"collapse1489814\" 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 to derive the equilibrium constant expression?\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=\"collapse1489814\" data-parent=\"#sp-ea-14898\" role=\"region\" aria-labelledby=\"ea-header-1489814\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p><span style=\"font-weight: 400\">The equilibrium constant expression can be derived from the law of mass action and the definition of equilibrium.<\/span><\/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>Equilibrium Constant (Kp, Kc, Kx) For IIT JAM is a crucial concept in physical chemistry that describes the equilibrium between reactants and products in a chemical reaction, with Kp and Kc representing different units of measurement. This topic falls under Physical Chemistry in the syllabi of IIT JAM, CSIR NET, and GATE.<\/p>\n","protected":false},"author":11,"featured_media":12502,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","rank_math_seo_score":89},"categories":[23],"tags":[2923,11252,7260,11253,11254,11255,11256,2922],"class_list":["post-12503","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-iit-jam","tag-competitive-exams","tag-equilibrium-constant-kp","tag-iit-jam-physical-chemistry","tag-kc","tag-kx-for-iit-jam","tag-kx-for-iit-jam-notes","tag-kx-for-iit-jam-questions","tag-vedprep","entry","has-media"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12503","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\/11"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=12503"}],"version-history":[{"count":7,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12503\/revisions"}],"predecessor-version":[{"id":16557,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12503\/revisions\/16557"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/12502"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=12503"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=12503"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=12503"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}