{"id":10714,"date":"2026-09-26T13:54:33","date_gmt":"2026-09-26T12:54:33","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/le-chateliers-principle\/"},"modified":"2026-10-04T23:03:20","modified_gmt":"2026-10-04T22:03:20","slug":"le-chateliers-principle","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/le-chateliers-principle\/","title":{"rendered":"Le Chatelier&#8217;s Principle"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-kinetics-equilibria-page\">\n  <style>\n    .ols-revision-page {\n      --navy: #1C244B;\n      --blue: #2563eb;\n      --soft-blue: #eef4ff;\n      --soft-red: #fff7f7;\n      --soft-purple: #f7f0ff;\n      --soft-green: #f0f7f1;\n      --gold: #c9973a;\n      --grey-text: #667085;\n   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href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9a-kinetics\/\">Topic 9A Kinetics<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9a-kinetics\/collision-theory-and-rates-of-reaction\/\">Collision Theory and Rates of Reaction<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9a-kinetics\/measuring-and-calculating-rates\/\">Measuring and Calculating Rates<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9a-kinetics\/maxwell-boltzmann-distribution\/\">The Maxwell\u2013Boltzmann Distribution<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9a-kinetics\/catalysts-and-reaction-profiles\/\">Catalysts and Reaction Profiles<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/core-practicals\/cp-9a-9b-iodine-propanone-and-clock-reaction-kinetics\/\">Core Practical 9A\/9B<\/a>\n          <\/li>\n        <\/ul>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/\">Topic 9B Equilibria<\/a>\n        <ul class=\"ols-subtopic-list\">\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/dynamic-equilibrium\/\">Dynamic Equilibrium<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/le-chateliers-principle\/\">Le Chatelier's Principle<\/a>\n          <\/li>\n          <li>\n            <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/equilibria-in-industry\/\">Equilibria in Industry<\/a>\n          <\/li>\n        <\/ul>\n      <\/li>\n    <\/ul>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>Other Topics<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-6-energetics\/\">Topic 6 Energetics<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-7-intermolecular-forces\/\">Topic 7 Intermolecular Forces<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-8-redox-chemistry-and-groups-1-2-and-7\/\">Topic 8 Redox &amp; Groups 1, 2 and 7<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/core-practicals\/\">Core Practicals<\/a>\n     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}\r\n})();\r\n<\/script>\r\n\n\n    <main class=\"ols-main\">\n\n      <!-- BREADCRUMBS - updated with full path and correct links -->\n      <nav class=\"ols-breadcrumbs\" aria-label=\"Breadcrumb\">\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/\">Revision Notes<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/\">A Level Chemistry<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/\">Edexcel International<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/\">Topic 9 Kinetics and Equilibria<\/a> \/\n<a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/\">Topic 9B Equilibria<\/a> \/\n<span>Le Chatelier&#8217;s Principle<\/span>\n<\/nav>\n\n      <header class=\"ols-title-card\">\n        <h1>Le Chatelier&#8217;s Principle<\/h1>\n        <p class=\"ols-page-intro\">A concise revision guide to Le Chatelier&#8217;s principle: predicting and justifying the effect of temperature, pressure and concentration changes on the position of a homogeneous equilibrium, and why a catalyst has no effect.<\/p>\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Exam board: Edexcel International<\/div>\n<div class=\"ols-badge\">Unit 2: WCH12\/01<\/div>\n<div class=\"ols-badge\">Topic 9B Equilibria<\/div>\n<\/div>\n        <div class=\"ols-author\">\n\n    <img decoding=\"async\"\n      class=\"ols-author-avatar-img\"\n      src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/05\/Author-Profile.jpeg\"\n      alt=\"Dr. Mohammed Al-Fatah\"\n    >\n\n    <div class=\"ols-author-content\">\n\n      <h2 class=\"ols-author-title\">\n        Written by: Dr. Mohammed Al-Fatah\n      <\/h2>\n\n      <p class=\"ols-author-description\">\n        Chemistry specialist revision notes for A Level Chemistry.\n      <\/p>\n\n      <a class=\"ols-linkedin-pill\" href=\"https:\/\/www.linkedin.com\/in\/doctormohammedfatah\/\" target=\"_blank\" rel=\"noopener noreferrer\">\n        <svg class=\"ols-linkedin-icon\" viewBox=\"0 0 24 24\" fill=\"currentColor\" aria-hidden=\"true\">\n          <path d=\"M4.98 3.5C4.98 4.88 3.86 6 2.48 6S0 4.88 0 3.5 1.12 1 2.48 1s2.5 1.12 2.5 2.5zM.5 8h4V24h-4V8zm7 0h3.8v2.2h.1c.5-.9 1.8-2.2 3.9-2.2 4.2 0 5 2.8 5 6.4V24h-4v-7.6c0-1.8 0-4.2-2.6-4.2s-3 2-3 4v7.8h-4V8z\"\/>\n        <\/svg>\n        View LinkedIn Profile\n      <\/a>\n\n    <\/div>\n\n  <\/div>\n      <\/header>\n\n      <article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>Le Chatelier&#8217;s Principle<\/h2>\n<\/div>\n<p><strong>Le Chatelier&#8217;s principle<\/strong> states that if a change is made to a system at dynamic equilibrium, the position of equilibrium moves in the direction that reduces the effect of the change.<\/p><p>It predicts which way an equilibrium shifts when the temperature, pressure or a concentration is altered.<\/p><div class=\"ols-key-box\"><p><strong>Remember:<\/strong> the principle is a tool for prediction only. The reason a shift happens is always the change in the forward and reverse rates.<\/p><\/div>\n<p>The principle applies to <strong>homogeneous equilibria<\/strong>, where every substance is in the same phase, such as gases reacting to give gases or ions reacting in solution.<\/p><p>The examples below use the ammonia equilibrium, N\u2082(g) + 3H\u2082(g) \u21cc 2NH\u2083(g), \u0394H = \u221292 kJ mol\u207b\u00b9, because every kind of change can be shown on it.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Definition:<\/strong> If a change is made to a system at equilibrium, the position of equilibrium moves to minimise (oppose) the effect of that change.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>Changing the Temperature<\/h2>\n<\/div>\n<p>Raising the temperature favours the <strong>endothermic direction<\/strong>, because that direction absorbs heat and so reduces the temperature rise.<\/p><p>For the ammonia equilibrium the forward reaction is exothermic, so the reverse reaction is endothermic. Raising the temperature moves the position of equilibrium to the left, and the equilibrium yield of ammonia falls.<\/p><p>Lowering the temperature favours the exothermic forward reaction and the yield rises, but the rate falls, which is the industrial dilemma on the next page.<\/p>\n<p>The justification must name the direction and its sign. &#8220;The equilibrium moves in the endothermic direction, which is the reverse reaction, to absorb the extra heat&#8221; earns the marks; &#8220;it moves to the left&#8221; alone does not.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Rule:<\/strong> Increase temperature \u2192 shift in the endothermic direction. Decrease temperature \u2192 shift in the exothermic direction. Temperature is the only change that also changes the value of the equilibrium constant.<\/p>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Check: Temperature Changes<\/h2>\n<p>Predict and justify the effect of temperature on equilibria not used above.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-914\" class=\"h5p-iframe\" data-content-id=\"914\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Kinetics and Equilibria Quick Choice: Temperature Changes\"><\/iframe><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>Changing the Pressure<\/h2>\n<\/div>\n<p>Pressure only affects equilibria that involve gases, and only when the number of gas molecules is different on the two sides.<\/p><p>Increasing the pressure moves the position of equilibrium towards the side with <strong>fewer moles of gas<\/strong>, because fewer molecules in the same volume exert a lower pressure, which reduces the effect of the increase.<\/p><p>In the ammonia equilibrium there are four moles of gas on the left and two on the right, so a higher pressure moves the equilibrium to the right and raises the yield of ammonia.<\/p>\n<p>If the number of gas molecules is the same on both sides, as in H\u2082(g) + I\u2082(g) \u21cc 2HI(g), changing the pressure has no effect on the position of equilibrium, although it still increases the rate of both reactions.<\/p><p>Adding an inert gas at constant volume changes the total pressure but not the concentrations of the reacting gases, so it has no effect either.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam wording:<\/strong> Count the gas moles on each side and say so: &#8220;there are 4 moles of gas on the left and 2 on the right, so increasing the pressure moves the equilibrium to the right, the side with fewer gas molecules, to reduce the pressure&#8221;.<\/p>\n<\/div>\n<div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t9x-gasmoles.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t9x-gasmoles.jpg\" alt=\"Decision tree for the effect of pressure on equilibrium, with a table of four gas equilibria and their shifts.\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/t9x-gasmoles.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Increasing the pressure moves the position of equilibrium towards the side with fewer moles of gas, and has no effect when both sides have the same number.<\/p><\/div>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Changing a Concentration<\/h2>\n<\/div>\n<p>Adding more of a substance moves the position of equilibrium away from it, so that some of the extra is used up. Removing a substance moves the equilibrium towards it, so that some is replaced.<\/p><p>Adding more nitrogen to the ammonia equilibrium moves it to the right.<\/p><p>Removing ammonia as it forms, which is what happens in the industrial plant when the ammonia is condensed out, also moves it to the right and keeps the forward reaction going.<\/p>\n<p>In solution the classic demonstration is the chromate(VI)\u2013dichromate(VI) equilibrium, 2CrO\u2084\u00b2\u207b(aq) + 2H\u207a(aq) \u21cc Cr\u2082O\u2087\u00b2\u207b(aq) + H\u2082O(l), yellow \u21cc orange.<\/p><p>Adding acid raises [H\u207a] and the solution turns orange as the equilibrium moves right; adding alkali removes H\u207a and it turns yellow again.<\/p><p>Colour changes like this are how concentration and temperature effects are investigated in the laboratory: the mixture is prepared, the change is made, and the new colour is compared with the original.<\/p>\n<div class=\"ols-figure-card ols-zoom-pop\">\n<div class=\"ols-figure-image\">\n<a class=\"ols-image-fullscreen-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/kinetics-equilibria-le-chatelier-table.jpg\" target=\"_blank\" rel=\"noopener\" aria-label=\"Open image fullscreen\">\n<img decoding=\"async\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/kinetics-equilibria-le-chatelier-table.jpg\" alt=\"Le Chatelier summary for N\u2082 + 3H\u2082 \u21cc 2NH\u2083: the effect of temperature, pressure, concentration and a catalyst\" data-fullscreen-src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/kinetics-equilibria-le-chatelier-table.jpg\">\n<\/a>\n<\/div>\n<div class=\"ols-figure-caption\"><p>Le Chatelier applied to the ammonia equilibrium: each change, the direction of the shift and the reason.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> Add a substance \u2192 equilibrium moves away from it. Remove a substance \u2192 equilibrium moves towards it.<\/p>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Check: Pressure and Concentration<\/h2>\n<p>Predict the shift for equilibria with different gas-mole counts and concentration changes.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-content\" data-content-id=\"915\"><\/div><\/div>\n<\/section>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Catalysts and Equilibrium<\/h2>\n<\/div>\n<p>A catalyst has <strong>no effect on the position of equilibrium<\/strong> and no effect on the equilibrium yield. It lowers the activation energy of the forward and reverse reactions by the same amount, so it speeds up both reactions equally.<\/p><p>What it does change is the time taken: equilibrium is reached much sooner.<\/p><p>In industry this is exactly what is wanted, because it allows an acceptable rate at a lower temperature, where the yield of an exothermic reaction is higher.<\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam wording:<\/strong> &#8220;A catalyst increases the rates of the forward and reverse reactions equally, so the position of equilibrium is unchanged but equilibrium is reached faster.&#8221;<\/p>\n<\/div>\n<\/article>\n<section class=\"ols-h5p-card ols-h5p-inline\">\n<span class=\"ols-h5p-kicker\">Check your understanding<\/span>\n<h2>Check: Putting It Together<\/h2>\n<p>Combine temperature, pressure, concentration and catalyst effects for an unfamiliar equilibrium.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-916\" class=\"h5p-iframe\" data-content-id=\"916\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Kinetics and Equilibria Explain: An Unfamiliar Equilibrium\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check Le Chatelier&#8217;s principle.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>Which way does the equilibrium move when I heat it?<\/h3>\n<p>In the endothermic direction, because that absorbs some of the added heat. For an exothermic forward reaction that means to the left.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>What if the number of gas moles is the same on both sides?<\/h3>\n<p>Then changing the pressure has no effect on the position of equilibrium, although both rates increase.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why does removing a product move the equilibrium to the right?<\/h3>\n<p>The system responds by making more of the removed product to replace some of what was lost, so more reactant is converted.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Does a catalyst increase the yield?<\/h3>\n<p>No. It speeds up the forward and reverse reactions equally, so the position of equilibrium and the yield are unchanged; equilibrium is just reached sooner.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Does Le Chatelier explain why the equilibrium moves?<\/h3>\n<p>It predicts the direction. The explanation is that the change alters the forward and reverse rates unequally until they become equal again at a new position.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"ols-related-card\">\n<h2>Related Topic 9B Equilibria Pages<\/h2>\n<p>Use these pages to connect the ideas across equilibria and the rest of Topic 9.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/dynamic-equilibrium\/\">Dynamic Equilibrium<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/equilibria-in-industry\/\">Equilibria in Industry<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/edexcel-international\/topic-9-kinetics-and-equilibria\/9b-equilibria\/\">Topic 9B Equilibria Overview<\/a>\n<\/div>\n<\/section>\n<section class=\"ols-attribution-card\">\n        <p><strong>Copyright notice:<\/strong> This OLS revision content, including the explanations, layout, diagrams, tables and embedded learning structure, is authored for Online Learning System by Dr. Mohammed Al-Fatah. 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Notes \/ A Level Chemistry \/ Edexcel International \/ Topic 9 Kinetics and Equilibria \/ Topic 9B Equilibria \/ Le Chatelier&#8217;s Principle Le Chatelier&#8217;s Principle A concise revision guide to Le Chatelier&#8217;s principle: predicting and justifying the effect of temperature, pressure and concentration changes on the position of a homogeneous equilibrium, and why a 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