{"id":66522,"date":"2026-10-06T17:42:10","date_gmt":"2026-10-06T14:42:10","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66522"},"modified":"2026-10-06T17:42:10","modified_gmt":"2026-10-06T14:42:10","slug":"van-t-hoff-equation-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/","title":{"rendered":"Van 't Hoff Equation Calculator"},"content":{"rendered":"<section class=\"not-prose calculator-box\" aria-labelledby=\"calculator-title\"><div class=\"flex items-baseline sm:items-center justify-between gap-2 sm:gap-3\"><div class=\"flex flex-col sm:flex-row sm:items-center gap-2\"><span class=\"icon icon-calculator text-primary-700! text-base! dark:text-primary-300!\" aria-hidden=\"true\"><\/span><h2 id=\"calculator-title\" class=\"text-lg font-display font-bold\">Predict the Equilibrium Constant at a New Temperature<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66522\" data-favorite-title=\"Van &#039;t Hoff Equation\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\" data-favorite-excerpt=\"This calculator uses the Van &#039;t Hoff equation to predict how an equilibrium constant changes with temperature. Enter K at a reference temperature, the standard reaction enthalpy, and the two temperatures to get K at the new temperature, the change factor, and \u0394G\u00b0.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry-1\">\n    <span class=\"icon icon-shape-star-empty\" aria-hidden=\"true\"><\/span>\n  <\/button>\n  <div class=\"calcdash-favorite__tip\" aria-hidden=\"true\">\n   <span class=\"favorite-tooltip\" id=\"favorite-tooltip\"><\/span>\n  <\/div>\n  <span class=\"sr-only\" role=\"status\" id=\"favorite-status\"><\/span>\n<\/div><\/div><form action=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66522\" data-post=\"66522\"><fieldset class=\"fieldset-input is-2\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Equilibrium Constant at Reference Temperature<\/label><div class=\"term\">K\u2081<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"equilibrium_constant_at_reference_temperature\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1.0\" min=\"0\" value=\"1\"\/><small id=\"calc-info-1\">Dimensionless K (Kc or Kp) measured at the reference temperature<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Standard Reaction Enthalpy<\/label><div class=\"term\">\u0394H\u00b0<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"standard_reaction_enthalpy\" id=\"field-2\" aria-describedby=\"calc-info-2\" placeholder=\"e.g. 50\" step=\"any\" value=\"50\"\/><div class=\"grid grid-cols-1\"><select id=\"field-3\" name=\"unit\" aria-label=\"Unit\"><option value=\"kJ\" selected>kJ\/mol<\/option><option value=\"kcal\">kcal\/mol<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-2\">\u0394H\u00b0 of the reaction \u2014 positive for endothermic, negative for exothermic<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-4\">Reference Temperature<\/label><div class=\"term\">T\u2081<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"reference_temperature\" id=\"field-4\" aria-describedby=\"calc-info-4\" placeholder=\"e.g. 298.15\" step=\"any\" value=\"298.15\"\/><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"unit\" aria-label=\"Unit\"><option value=\"K\" selected>K<\/option><option value=\"C\">\u00b0C<\/option><option value=\"F\">\u00b0F<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-4\">Temperature at which K\u2081 was measured<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-6\">Target Temperature<\/label><div class=\"term\">T\u2082<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><div class=\"field-group\"><input type=\"number\" name=\"target_temperature\" id=\"field-6\" aria-describedby=\"calc-info-6\" placeholder=\"e.g. 373.15\" step=\"any\" value=\"373.15\"\/><div class=\"grid grid-cols-1\"><select id=\"field-7\" name=\"unit\" aria-label=\"Unit\"><option value=\"K\" selected>K<\/option><option value=\"C\">\u00b0C<\/option><option value=\"F\">\u00b0F<\/option><\/select><svg class=\"pointer-events-none col-start-1 row-start-1 mr-2 size-5 self-center justify-self-end text-gray-500 sm:size-4\" viewBox=\"0 0 16 16\" fill=\"currentColor\" aria-hidden=\"true\" data-slot=\"icon\">\n              <path fill-rule=\"evenodd\" d=\"M4.22 6.22a.75.75 0 0 1 1.06 0L8 8.94l2.72-2.72a.75.75 0 1 1 1.06 1.06l-3.25 3.25a.75.75 0 0 1-1.06 0L4.22 7.28a.75.75 0 0 1 0-1.06Z\" clip-rule=\"evenodd\" \/>\n            <\/svg><\/div><\/div><small id=\"calc-info-6\">Temperature at which you want to know K<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66522\">Calculate<\/button><button type=\"reset\">Reset<\/button><\/div><div class=\"field is-checkbox hidden!\" id=\"field-auto-calc\"><input type=\"checkbox\" id=\"auto-calc\"><label for=\"auto-calc\">Calculate automatically<\/label><small>If enabled, the result will update automatically when you change any value.<\/small><\/div><div class=\"fieldset-result is-hidden\" aria-labelledby=\"result-title\" aria-live=\"polite\" role=\"region\"> <h3 class=\"result-title bg-gradient-to-r from-primary-50 to-gray-50 dark:from-primary-900 dark:to-gray-800\" id=\"result-title\"><span class=\"icon icon-s-pulse\" aria-hidden=\"true\"><\/span> Equilibrium at the Target Temperature<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Equilibrium Constant at Target Temperature<\/span><span class=\"result-term\">K\u2082<\/span><\/span><span class=\"field-value\" id=\"result-1\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-2\"><span class=\"field-title\"><span>Change Factor K\u2082 \/ K\u2081<\/span><span class=\"result-term\">K\u2082\/K\u2081<\/span><\/span><span class=\"field-value\" id=\"result-2\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result\" id=\"output-3\"><span class=\"field-title\"><span>\u0394G\u00b0 at Target Temperature<\/span><span class=\"result-term\">\u0394G\u00b0\u2082<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"kJ\/mol\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result is-column\" id=\"output-4\"><span class=\"field-title\"><span>Interpretation<\/span><\/span><span class=\"field-value\" id=\"result-4\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><div class=\"field-result is-column\" id=\"output-5\"><span class=\"field-title\"><span>Calculation Details<\/span><\/span><span class=\"field-value\" id=\"result-5\"><\/span><button type=\"button\" class=\"copy-result\" data-tooltip=\"Copy Result\" aria-label=\"Copy Result\"><span class=\"copy-icon icon icon-document-copy\" aria-hidden=\"true\"><\/span><\/button><\/div><\/div><div class=\"result-actions\"><button type=\"button\" class=\"copy-link\"><svg viewBox=\"0 0 20 20\" fill=\"currentColor\" aria-hidden=\"true\"><path d=\"M12.232 4.232a2.5 2.5 0 0 1 3.536 3.536l-1.225 1.224a.75.75 0 0 0 1.061 1.06l1.224-1.224a4 4 0 0 0-5.656-5.656l-3 3a4 4 0 0 0 .225 5.865.75.75 0 0 0 .977-1.138 2.5 2.5 0 0 1-.142-3.667l3-3Z\"\/><path d=\"M11.603 7.963a.75.75 0 0 0-.977 1.138 2.5 2.5 0 0 1 .142 3.667l-3 3a2.5 2.5 0 0 1-3.536-3.536l1.225-1.224a.75.75 0 0 0-1.061-1.06l-1.224 1.224a4 4 0 1 0 5.656 5.656l3-3a4 4 0 0 0-.225-5.865Z\"\/><\/svg><span class=\"copy-link__text\">Copy link to this calculation<\/span><\/button><span class=\"sr-only\" role=\"status\" id=\"copy-link-status\"><\/span><\/div><\/div><a href=\"#respond\" class=\"hidden transition-opacity duration-300 opacity-0 w-50 text-sm justify-center items-center gap-2 px-4 py-2 rounded bg-gray-200 text-gray-700 hover:bg-gray-300\" id=\"leave-comment\"><span class=\"icon icon-comments\" aria-hidden=\"true\"><\/span>Leave a Comment<\/a><\/form><\/section><section id=\"calc-reactions\" class=\"not-prose hidden my-12 bg-gradient-to-r from-primary-50 to-gray-50 border border-indigo-100 rounded-xl px-6 py-4 shadow-sm\" data-post=\"66522\" aria-live=\"polite\" aria-labelledby=\"calc-reactions-title\"><p id=\"calc-reactions-title\" class=\"text-sm text-gray-500 text-center mb-2\">How did this result make you feel?<\/p><div role=\"group\" aria-labelledby=\"calc-reactions-title\" class=\"grid grid-cols-3 sm:flex sm:flex-row sm:justify-around gap-4 sm:items-center sm:flex-wrap\"><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"like\"><span class=\"reaction-count\" data-reaction-count=\"like\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude00 <\/span><span class=\"reaction-description font-medium\">Like <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"helpful\"><span class=\"reaction-count\" data-reaction-count=\"helpful\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\udca1 <\/span><span class=\"reaction-description font-medium\">Helpful <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"confused\"><span class=\"reaction-count\" data-reaction-count=\"confused\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude15 <\/span><span class=\"reaction-description font-medium\">Confused <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"disappointed\"><span class=\"reaction-count\" data-reaction-count=\"disappointed\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\ud83d\ude1e <\/span><span class=\"reaction-description font-medium\">Disappointed <\/span><\/button><button type=\"button\" aria-pressed=\"false\" class=\"reaction-btn flex flex-col items-center gap-1 text-sm text-gray-700 hover:text-primary-600 cursor-pointer transition-transform hover:scale-105\" data-reaction=\"inaccurate\"><span class=\"reaction-count\" data-reaction-count=\"inaccurate\">0<\/span><span class=\"reaction text-3xl\" aria-hidden=\"true\">\u274c <\/span><span class=\"reaction-description font-medium\">Inaccurate <\/span><\/button><\/div><div id=\"reaction-message\" class=\"hidden mt-8 rounded-md border border-primary-100 bg-white\/50 backdrop-blur-sm px-4 py-2 text-sm text-center shadow-sm\"><\/div><\/section><div class=\"calcdash-ad not-prose calcdash-ad--calc_result calcdash-ad--in-article\"><ins class=\"adsbygoogle\" style=\"display:block\" data-ad-client=\"ca-pub-1721569815777345\" data-ad-slot=\"6317458308\" data-ad-layout=\"in-article\" data-ad-format=\"fluid\"><\/ins><script>(adsbygoogle = window.adsbygoogle || []).push({});<\/script><\/div>\n<style id=\"wpcoderpro-inline-1\">.formula-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section class=\"formula-box\" aria-labelledby=\"formula-title\">\r\n\t<div id=\"formula-title\" class=\"not-prose font-display mb-4\"><span class=\"icon icon-formula\" aria-hidden=\"true\"><\/span><h2>Van 't Hoff Equation Formula<\/h2><\/div>\r\n\t<figure class=\"not-prose formula\">\r\n\t\t<figcaption class=\"formula-title\">Formula<\/figcaption>\r\n\t\t<div class=\"text-base text-gray-800\" id=\"formula\">\n\\[ \\ln\\!\\left(\\frac{K_2}{K_1}\\right) = -\\frac{\\Delta H^\\circ}{R}\\left(\\frac{1}{T_2} - \\frac{1}{T_1}\\right) \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(K_1\\) \u2014 equilibrium constant at the reference temperature \\(T_1\\) (dimensionless)<\/li>\n<li>\\(K_2\\) \u2014 equilibrium constant at the target temperature \\(T_2\\)<\/li>\n<li>\\(\\Delta H^\\circ\\) \u2014 standard reaction enthalpy (J\/mol; positive for endothermic, negative for exothermic)<\/li>\n<li>\\(R\\) \u2014 gas constant, \\(8.314\\ \\text{J\/(mol\u00b7K)}\\)<\/li>\n<li>\\(T_1, T_2\\) \u2014 absolute temperatures in kelvin<\/li>\n<\/ul>\n<p>The equation tells you how strongly the equilibrium constant depends on temperature: the effect is driven by the reaction enthalpy and the difference between the reciprocals of the two temperatures.<\/p>\n<p>\r\n<\/section>\n<style id=\"wpcoderpro-inline-459\">.calculation-box {\r\n\tborder-bottom: none !important;\r\n}<\/style><section id=\"calculation\" class=\"calculation-box\" aria-labelledby=\"calculation-title\">\r\n\t<div id=\"calculation-title\" class=\"not-prose font-display\"><span class=\"icon icon-unordered-list\" aria-hidden=\"true\"><\/span><h2>Van 't Hoff Equation \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a reaction has an equilibrium constant \\(K_1 = 1\\) at \\(T_1 = 298.15\\ \\text{K}\\) (25 \u00b0C) and a standard reaction enthalpy of \\(\\Delta H^\\circ = +50\\ \\text{kJ\/mol}\\). What is \\(K\\) at \\(T_2 = 373.15\\ \\text{K}\\) (100 \u00b0C)?<\/p>\n<p>\\[ \\ln\\!\\left(\\frac{K_2}{K_1}\\right) = -\\frac{50{,}000}{8.314}\\left(\\frac{1}{373.15} - \\frac{1}{298.15}\\right) = -6013.9 \\times (-0.000674) = 4.054 \\]<\/p>\n<p>\\[ K_2 = K_1 \\cdot e^{4.054} = 1 \\times 57.6 \\]<\/p>\n<p><strong>Result:<\/strong> \\(K_2 \\approx 57.6\\) \u2014 the equilibrium constant grows by a factor of about 57.6. The calculator also gives \\(\\Delta G^\\circ_2 \\approx -12.57\\ \\text{kJ\/mol}\\), confirming the reaction becomes product-favoured at 100 \u00b0C.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Equilibrium Constant at Reference Temperature<\/strong> (K\u2081). It must be a positive, dimensionless number.<\/li>\n<li>Enter the <strong>Standard Reaction Enthalpy<\/strong> (\u0394H\u00b0) and choose its unit, kJ\/mol or kcal\/mol. Use a positive value for an endothermic reaction and a negative value for an exothermic one.<\/li>\n<li>Enter the <strong>Reference Temperature<\/strong> (T\u2081), the temperature at which K\u2081 was measured, and select K, \u00b0C or \u00b0F.<\/li>\n<li>Enter the <strong>Target Temperature<\/strong> (T\u2082), the temperature you want the new K for, with its unit.<\/li>\n<li>Read the results: K\u2082 at the target temperature, the change factor K\u2082\/K\u2081, \u0394G\u00b0 at the target temperature, plus an interpretation of the shift and a full calculation trace.<\/li>\n<\/ol>\n<h2>What the Van 't Hoff Equation Tells You<\/h2>\n<p>Chemical equilibria respond to temperature, and the direction of that response is fixed by the sign of the reaction enthalpy. Heat an endothermic reaction (\u0394H\u00b0 &gt; 0) and the equilibrium shifts towards the products, so K increases; heat an exothermic reaction (\u0394H\u00b0 &lt; 0) and K decreases. This is Le Chatelier's principle made quantitative: the Van 't Hoff equation converts a qualitative rule into a number you can act on.<\/p>\n<p>The result is easiest to read through the change factor \\(K_2\/K_1\\). A factor of 57.6 means the product-to-reactant ratio at equilibrium becomes 57.6 times larger \u2014 a dramatic shift. A factor near 1 means the temperature change barely matters, which typically happens when \u0394H\u00b0 is small or the two temperatures are close together. Because the equation works with \\(1\/T\\), the same temperature jump has a much bigger effect at low temperatures than at high ones.<\/p>\n<p>The calculator also reports \\(\\Delta G^\\circ\\) at the target temperature, derived from the relation \\(\\Delta G^\\circ = -RT\\ln K\\) together with the assumption that \\(\\Delta S^\\circ\\) stays constant. A negative \u0394G\u00b0 means the reaction is product-favoured under standard conditions (K &gt; 1); a positive value means reactants dominate. If you work the other way around \u2014 from \u0394G\u00b0 to K \u2014 the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/gibbs-free-energy-calculator\/\">Gibbs Free Energy calculator<\/a> and the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/equilibrium-constant-calculator\/\">Equilibrium Constant calculator<\/a> are useful companions.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>\u0394H\u00b0 is treated as constant.<\/strong> In reality it drifts with temperature because of heat capacity differences between reactants and products. Over a range of 50\u2013100 K the error is usually small; over hundreds of kelvin it can become significant.<\/li>\n<li><strong>Temperatures must be absolute.<\/strong> The equation requires kelvin. The calculator converts \u00b0C and \u00b0F automatically, but if you use the formula by hand, convert first.<\/li>\n<li><strong>K must be dimensionless.<\/strong> Use the thermodynamic equilibrium constant (activities or the properly standardised Kc\/Kp), not a ratio with units. If you need to convert between pressure and concentration constants, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/kp-to-kc-calculator\/\">Kp to Kc calculator<\/a>.<\/li>\n<li><strong>Watch the exponential behaviour.<\/strong> Because \\(K_2 = K_1 e^{\\ln(K_2\/K_1)}\\), large enthalpies or big temperature gaps can shift K by many orders of magnitude. A prediction of K = 10<sup>12<\/sup> is mathematically correct but practically meaningless if the reaction becomes diffusion-limited or a competing pathway takes over.<\/li>\n<li><strong>The equation says nothing about rate.<\/strong> A favourable K does not guarantee a fast reaction; kinetics and thermodynamics are separate questions.<\/li>\n<\/ul>\n<p>A related temperature-dependence tool is the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/clausius-clapeyron-calculator\/\">Clausius\u2013Clapeyron calculator<\/a>, which applies the same mathematics to vapour pressures instead of equilibrium constants.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>This calculator uses the Van 't Hoff equation to predict how an equilibrium constant changes with temperature. Enter K at a reference temperature, the standard reaction enthalpy, and the two temperatures to get K at the new temperature, the change factor, and \u0394G\u00b0.<\/p>\n","protected":false},"author":3168,"featured_media":0,"comment_status":"open","ping_status":"","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[57],"class_list":["post-66522","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-reactions"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66522","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/users\/3168"}],"replies":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/comments?post=66522"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66522\/revisions"}],"predecessor-version":[{"id":66523,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66522\/revisions\/66523"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66522"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66522"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66522"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}