{"id":8360,"date":"2026-09-18T12:01:15","date_gmt":"2026-09-18T11:01:15","guid":{"rendered":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/bond-enthalpies\/"},"modified":"2026-09-18T12:09:27","modified_gmt":"2026-09-18T11:09:27","slug":"bond-enthalpies","status":"publish","type":"page","link":"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/bond-enthalpies\/","title":{"rendered":"Bond Enthalpies"},"content":{"rendered":"\n<section class=\"ols-revision-page ols-nature-of-covalent-bonding-9ch0-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      --soft-orange: #fff7ed;\n      --grey-text: #667085;\n      --body-text: #1f2937;\n      --border: rgba(28, 36, 75, 0.14);\n      --shadow: 0 18px 45px rgba(28, 36, 75, 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10px 0 0; font-size: 14px; color: #667085; text-align: center; }\n<\/style>\n\n  <aside class=\"ols-sidebar\">\n  <div class=\"ols-sidebar-header\">\n    <h3>Revision Notes<\/h3>\n    <p>A Level Chemistry<\/p>\n  <\/div>\n\n  <div class=\"ols-topic-group\">\n    <h4>3.1.4 Energetics<\/h4>\n\n    <ul class=\"ols-topic-list\">\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/\">3.1.4 Overview<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/enthalpy-changes-and-standard-conditions\/\">Enthalpy Changes and Standard Conditions<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/standard-enthalpy-changes\/\">Standard Enthalpy Changes<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/calorimetry-measuring-enthalpy-changes\/\">Calorimetry: Measuring Enthalpy Changes<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/hess-law-and-enthalpy-cycles\/\">Hess's Law and Enthalpy Cycles<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/bond-enthalpies\/\">Bond Enthalpies<\/a>\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\/aqa\/3-1-2-amount-of-substance\/\">3.1.2 Amount of Substance<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-3-bonding\/\">3.1.3 Bonding<\/a>\n      <\/li>\n      <li>\n        <a href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-2-1-periodicity\/\">3.2.1 Periodicity<\/a>\n      <\/li>\n    <\/ul>\n  <\/div>\n<\/aside>\n\n<script>\r\n(function() {\r\n  function normalisePath(path) {\r\n    return String(path || '')\r\n      .split('?')[0]\r\n      .split('#')[0]\r\n      .replace(\/\\\/+$\/, '')\r\n      .toLowerCase();\r\n  }\r\n\r\n  function highlightActive() {\r\n    var sidebar = document.querySelector('.ols-sidebar');\r\n    if (!sidebar) return false;\r\n\r\n    var currentPath = normalisePath(window.location.pathname);\r\n    var links = sidebar.querySelectorAll('a[href]');\r\n    var matched = null;\r\n    var matchedLength = 0;\r\n\r\n    sidebar.querySelectorAll('.active, .active-main, .parent-active').forEach(function(item) {\r\n      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 <p class=\"ols-page-intro\">A concise revision guide to bond enthalpies: what mean bond enthalpy means, why reactions are exothermic or endothermic, calculating \u0394H from bond enthalpies, and why the answers differ from Hess&#8217;s law values, for AQA A Level Chemistry.<\/p>\n\n        <div class=\"ols-badges\">\n<div class=\"ols-badge\">Paper 1 and 2 AQA<\/div>\n<div class=\"ols-badge\">3.1.4 Energetics<\/div>\n<div class=\"ols-badge\">7405\/1 and 7405\/2<\/div>\n<\/div>\n\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:<br><span>Dr. Mohammed Al-Fatah<\/span>\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 soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">1<\/div>\n<h2>What Bond Enthalpy Means<\/h2>\n<\/div>\n<p>The <strong>bond enthalpy<\/strong> is the energy needed to break one mole of a given covalent bond in molecules in the <strong>gaseous state<\/strong>. Breaking a bond always needs energy, so bond enthalpies are always positive; making the same bond releases the same amount of energy.<\/p>\n<p>For a diatomic molecule such as H\u2082 the value is exact. For bonds that appear in many compounds, such as C\u2013H, the value quoted is a <strong>mean bond enthalpy<\/strong>: the average energy needed to break that type of bond, taken over a range of compounds.<\/p>\n<div class=\"ols-zoom-card\">\n<div class=\"ols-zoom-card-image\">\n<a class=\"ols-lightbox-link\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/average-bond-enthalpies-of-common-covalent-bonds.jpg\" aria-label=\"Open image full screen\">\n<img decoding=\"async\" class=\"ols-zoomable-img ols-lightbox-target\" src=\"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-content\/uploads\/2026\/09\/average-bond-enthalpies-of-common-covalent-bonds.jpg\" alt=\"Bar chart of average bond enthalpies for common covalent bonds in kJ per mol\">\n<\/a>\n<\/div>\n<div class=\"ols-zoom-card-caption\"><p>Bond enthalpies for common bonds: multiple bonds are stronger than single bonds between the same atoms, and N\u2261N is the strongest shown.<\/p><\/div>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Definition:<\/strong> Mean bond enthalpy is the energy needed to break one mole of a given type of bond in gaseous molecules, averaged over a range of compounds.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">2<\/div>\n<h2>Why Reactions Are Exothermic or Endothermic<\/h2>\n<\/div>\n<p>Every reaction breaks some bonds and makes others. <strong>Bond breaking is endothermic<\/strong> and <strong>bond making is exothermic<\/strong>. The overall enthalpy change depends on which is larger:<\/p>\n<ul>\n<li>If more energy is released making the bonds in the products than is absorbed breaking the bonds in the reactants, the reaction is <strong>exothermic<\/strong>.<\/li>\n<li>If more energy is absorbed breaking bonds than is released making them, the reaction is <strong>endothermic<\/strong>.<\/li>\n<\/ul>\n<div class=\"ols-figure-card ols-figure-placeholder\">\n<div class=\"ols-figure-image\"><div class=\"ols-placeholder-box\">[3D MODEL NEEDED: Methane burning in oxygen, shown bond by bond: the C\u2013H and O=O bonds break, then the C=O and O\u2013H bonds form, with running totals of energy absorbed and released. SHARED CARD: generate once, used on all five boards.]<\/div><\/div>\n<div class=\"ols-figure-caption\"><p>Burning methane: breaking C\u2013H and O=O bonds absorbs less energy than forming C=O and O\u2013H bonds releases, so the reaction is exothermic.<\/p><\/div>\n<\/div>\n<!-- 3D PROMPT: Create an interactive 3D educational model of the bonds broken and made when methane burns, CH\u2084 + 2O\u2082 \u2192 CO\u2082 + 2H\u2082O. Stage 1 shows one CH\u2084 molecule (tetrahedral, black carbon, white hydrogens, bond angle 109.5\u00b0) beside two O\u2082 molecules (red spheres, double bond drawn as two parallel rods). * A \"break bonds\" button animates the four C\u2013H bonds and the two O=O bonds separating into free atoms, each broken bond flashing red, with a running counter \"energy absorbed: +2648 kJ\" built from 4 \u00d7 413 and 2 \u00d7 498. * A \"make bonds\" button animates the free atoms joining into one CO\u2082 molecule (linear, two C=O double bonds) and two H\u2082O molecules (bent, 104.5\u00b0), each new bond flashing green, with a running counter \"energy released: \u22123466 kJ\" built from 2 \u00d7 805 and 4 \u00d7 464. * A final panel shows \"\u0394H = +2648 \u2212 3466 = \u2212818 kJ mol\u207b\u00b9\" and an energy bar chart with the break bar going up and the make bar going down. * Labels on every bond type with its value in kJ mol\u207b\u00b9. * Buttons: reset, break bonds, make bonds, play all; toggles for labels and the energy bars. * Views: front, side, top. * Rotate and zoom; small x-y-z axis guide; white background; clear typography; restrained textbook styling. Title: Bonds broken and made when methane burns -->\n<div class=\"ols-key-box\">\n<p><strong>Key idea:<\/strong> \u0394H = energy absorbed breaking bonds \u2212 energy released making bonds. A negative answer means the products are held by stronger bonds overall.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card purple\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">3<\/div>\n<h2>Calculating \u0394H from Bond Enthalpies<\/h2>\n<\/div>\n<div class=\"ols-key-box\">\n<p><strong>Key equation:<\/strong> \u0394H = \u03a3(bond enthalpies of bonds broken) \u2212 \u03a3(bond enthalpies of bonds made)<\/p>\n<\/div>\n<p><strong>Worked example.<\/strong> Calculate the enthalpy change for the combustion of methane, CH\u2084(g) + 2O\u2082(g) \u2192 CO\u2082(g) + 2H\u2082O(g), using C\u2013H 413, O=O 498, C=O 805 and O\u2013H 464 kJ mol\u207b\u00b9.<\/p>\n<div class=\"ols-table-wrap\">\n<table class=\"ols-table\">\n<thead>\n<tr><th>Bonds<\/th><th>Number<\/th><th>Energy \/ kJ<\/th><\/tr>\n<\/thead>\n<tbody>\n<tr><td><strong>Broken: C\u2013H<\/strong><\/td><td>4<\/td><td>4 \u00d7 413 = 1652<\/td><\/tr>\n<tr><td><strong>Broken: O=O<\/strong><\/td><td>2<\/td><td>2 \u00d7 498 = 996<\/td><\/tr>\n<tr><td><strong>Total broken<\/strong><\/td><td><\/td><td>+2648<\/td><\/tr>\n<tr><td><strong>Made: C=O<\/strong><\/td><td>2<\/td><td>2 \u00d7 805 = 1610<\/td><\/tr>\n<tr><td><strong>Made: O\u2013H<\/strong><\/td><td>4<\/td><td>4 \u00d7 464 = 1856<\/td><\/tr>\n<tr><td><strong>Total made<\/strong><\/td><td><\/td><td>3466<\/td><\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p>\u0394H = 2648 \u2212 3466 = <strong>\u2212818 kJ mol\u207b\u00b9<\/strong><\/p>\n<div class=\"ols-key-box\">\n<p><strong>Exam focus:<\/strong> Draw out the displayed formulae first and count every bond. Most lost marks come from missing a bond, not from the arithmetic.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">4<\/div>\n<h2>Why Bond Enthalpy Values Differ from Hess Values<\/h2>\n<\/div>\n<p>The data book enthalpy change of combustion of methane is \u2212890 kJ mol\u207b\u00b9, but the bond enthalpy calculation gives \u2212818 kJ mol\u207b\u00b9. There are two reasons:<\/p>\n<ol>\n<li><strong>Mean values are used.<\/strong> The C\u2013H value is an average over many compounds, not the exact value for methane, and the same is true of C=O and O\u2013H.<\/li>\n<li><strong>Everything is assumed to be gaseous.<\/strong> Bond enthalpies apply to gaseous molecules, but standard enthalpy changes of combustion form liquid water. Condensing the water releases extra energy that the calculation leaves out.<\/li>\n<\/ol>\n<div class=\"ols-key-box\">\n<p><strong>Exam sentence:<\/strong> Values calculated from bond enthalpies are less accurate than those from Hess&#8217;s law because bond enthalpies are averages over many compounds and apply only to substances in the gaseous state.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card soft\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">5<\/div>\n<h2>Finding a Mean Bond Enthalpy from \u0394H<\/h2>\n<\/div>\n<p>The same equation can be rearranged to find one unknown bond value when \u0394H and the others are known.<\/p>\n<p><strong>Worked example.<\/strong> H\u2082(g) + Cl\u2082(g) \u2192 2HCl(g), \u0394H = \u2212184 kJ mol\u207b\u00b9. Using H\u2013H 436 and Cl\u2013Cl 243 kJ mol\u207b\u00b9, find the H\u2013Cl value.<\/p>\n<ol>\n<li>\u0394H = (436 + 243) \u2212 2E(H\u2013Cl)<\/li>\n<li>\u2212184 = 679 \u2212 2E(H\u2013Cl)<\/li>\n<li>2E(H\u2013Cl) = 863, so E(H\u2013Cl) = <strong>432 kJ mol\u207b\u00b9<\/strong> (3 significant figures)<\/li>\n<\/ol>\n<div class=\"ols-key-box\">\n<p><strong>Remember:<\/strong> Two moles of HCl form, so two H\u2013Cl bonds are made. Divide by the number of bonds of the unknown type at the end.<\/p>\n<\/div>\n<\/article>\n<article class=\"ols-note-card\">\n<div class=\"ols-note-title\">\n<div class=\"ols-note-icon\">6<\/div>\n<h2>Common Exam Points<\/h2>\n<\/div>\n<h3>Define mean bond enthalpy<\/h3><p>The energy needed to break one mole of a given type of bond in gaseous molecules, averaged over a range of compounds.<\/p>\n<h3>Calculate \u0394H from bond enthalpies<\/h3><p>Bonds broken minus bonds made; count every bond from the displayed formulae.<\/p>\n<h3>Explain why the answer differs from the data book value<\/h3><p>Bond enthalpies are averages, and the calculation assumes all species are gases.<\/p>\n<h3>Do not say<\/h3><p>&#8220;Bond making needs energy&#8221;; &#8220;bond enthalpies are exact for every molecule&#8221;.<\/p>\n<\/article>\n<section class=\"ols-h5p-card\">\n<h2>Check Your Understanding<\/h2>\n<p>Calculate and explain using molecules other than those in the notes.<\/p>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-562\" class=\"h5p-iframe\" data-content-id=\"562\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Energetics Drag: bond breaking and making\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-563\" class=\"h5p-iframe\" data-content-id=\"563\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Energetics MCQ: hydrogenation of ethene\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-564\" class=\"h5p-iframe\" data-content-id=\"564\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Energetics MCQ: N\u2013H bond from \u0394H\"><\/iframe><\/div><\/div>\n<div class=\"ols-h5p-frame\"><div class=\"h5p-iframe-wrapper\"><iframe id=\"h5p-iframe-565\" class=\"h5p-iframe\" data-content-id=\"565\" style=\"height:1px\" src=\"about:blank\" frameBorder=\"0\" scrolling=\"no\" title=\"Energetics MCQ: ethanol combustion from bond data\"><\/iframe><\/div><\/div>\n<\/section>\n<section class=\"ols-faq-card\">\n<h2>FAQs<\/h2>\n<p>Use these quick answers to check the bond enthalpies ideas and calculations.<\/p>\n\n<div class=\"ols-faq-list\">\n<div class=\"ols-faq-item\">\n<h3>Why are bond enthalpies always positive?<\/h3>\n<p>They are defined for breaking bonds, and breaking a bond always needs energy.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>How do I calculate \u0394H from bond values?<\/h3>\n<p>Add up the bond enthalpies of all the bonds broken, add up those of all the bonds made, and subtract: bonds broken minus bonds made.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Why is my answer different from the data book value?<\/h3>\n<p>The bond enthalpies are averages over many compounds, and the method assumes every substance is a gas, whereas standard values may involve liquids.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>What makes a reaction exothermic in terms of bonds?<\/h3>\n<p>More energy is released making the bonds in the products than is absorbed breaking the bonds in the reactants.<\/p>\n<\/div>\n\n<div class=\"ols-faq-item\">\n<h3>Are any bond values exact?<\/h3>\n<p>Yes, for diatomic molecules such as H\u2082 or Cl\u2082, where there is only one bond in one environment. Bonds found in many compounds, such as C\u2013H, have average values.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<section class=\"ols-related-card\">\n<h2>Related Energetics Pages<\/h2>\n<p>Use these pages to connect enthalpy definitions, measurement and calculation methods across the topic.<\/p>\n<div class=\"ols-related-grid\">\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/enthalpy-changes-and-standard-conditions\/\">Enthalpy Changes and Standard Conditions<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/standard-enthalpy-changes\/\">Standard Enthalpy Changes<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/calorimetry-measuring-enthalpy-changes\/\">Calorimetry: Measuring Enthalpy Changes<\/a>\n<a class=\"ols-related-item\" href=\"https:\/\/www.onlinelearningsystem.net\/xyz\/revision-notes\/a-level-chemistry\/aqa\/3-1-4-energetics\/hess-law-and-enthalpy-cycles\/\">Hess&#8217;s Law and Enthalpy Cycles<\/a>\n<\/div>\n<\/section>\n<section class=\"ols-attribution-card\">\n        <p><strong>Copyright and author footprint:<\/strong> This OLS revision page was written for Online Learning System by <strong>Dr. Mohammed Al-Fatah<\/strong>. It is designed for A Level Chemistry revision and should not be copied or redistributed without permission.<\/p>\n      <\/section>\n\n      <div class=\"ols-image-lightbox\" id=\"olsImageLightboxNatureCovalentBonding9ch0\" aria-hidden=\"true\" role=\"dialog\" aria-modal=\"true\" aria-label=\"Expanded revision image\">\n        <div class=\"ols-image-lightbox-inner\">\n          <button class=\"ols-image-lightbox-close\" type=\"button\" aria-label=\"Close enlarged image\">\u00d7<\/button>\n          <img decoding=\"async\" class=\"ols-image-lightbox-img\" src=\"\" alt=\"\">\n        <\/div>\n      <\/div>\n\n      <script>\n        (function(){\n          var page = document.querySelector(\".ols-nature-of-covalent-bonding-9ch0-page\");\n          if (!page) { return; }\n          var lightbox = page.querySelector(\"#olsImageLightboxNatureCovalentBonding9ch0\");\n          if (!lightbox) { return; }\n          var lightboxImage = lightbox.querySelector(\".ols-image-lightbox-img\");\n    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Paper 1 [&hellip;]<\/p>\n","protected":false},"author":12,"featured_media":0,"parent":8355,"menu_order":4,"comment_status":"closed","ping_status":"closed","template":"","meta":{"footnotes":""},"class_list":["post-8360","page","type-page","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/8360","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/users\/12"}],"replies":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/comments?post=8360"}],"version-history":[{"count":0,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/8360\/revisions"}],"up":[{"embeddable":true,"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/pages\/8355"}],"wp:attachment":[{"href":"https:\/\/www.onlinelearningsystem.net\/xyz\/wp-json\/wp\/v2\/media?parent=8360"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}