{"id":66478,"date":"2026-10-06T17:20:22","date_gmt":"2026-10-06T14:20:22","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66478"},"modified":"2026-10-06T17:20:22","modified_gmt":"2026-10-06T14:20:22","slug":"gibbs-free-energy-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/gibbs-free-energy-calculator\/","title":{"rendered":"Gibbs Free Energy 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\">Find \u0394G and Check if the Reaction Is Spontaneous<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66478\" data-favorite-title=\"Gibbs Free Energy\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/gibbs-free-energy-calculator\/\" data-favorite-excerpt=\"Calculate the Gibbs free energy change (\u0394G) from enthalpy (\u0394H), entropy (\u0394S), and temperature, and instantly see whether the reaction is spontaneous under those conditions.\" 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\/gibbs-free-energy-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66478\" data-post=\"66478\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Enthalpy Change (\u0394H)<\/label><div class=\"term\">\u0394H<\/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=\"enthalpy_change_h\" id=\"field-1\" aria-describedby=\"calc-info-1\" placeholder=\"e.g. -92.2\" step=\"0.0001\" value=\"-92.2\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"kj_mol\" selected>kJ\/mol<\/option><option value=\"j_mol\">J\/mol<\/option><option value=\"kcal_mol\">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-1\">Negative = exothermic, positive = endothermic<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-3\">Entropy Change (\u0394S)<\/label><div class=\"term\">\u0394S<\/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=\"entropy_change_s\" id=\"field-3\" aria-describedby=\"calc-info-3\" placeholder=\"e.g. -198.75\" step=\"0.0001\" value=\"-198.75\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"j_molk\" selected>J\/(mol\u00b7K)<\/option><option value=\"kj_molk\">kJ\/(mol\u00b7K)<\/option><option value=\"cal_molk\">cal\/(mol\u00b7K)<\/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-3\">Positive = disorder increases, negative = disorder decreases<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-5\">Temperature<\/label><div class=\"term\">T<\/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=\"temperature\" id=\"field-5\" aria-describedby=\"calc-info-5\" placeholder=\"e.g. 25\" min=\"-273.15\" step=\"0.01\" value=\"25\"\/><div class=\"grid grid-cols-1\"><select id=\"field-6\" name=\"unit\" aria-label=\"Unit\"><option value=\"c\" selected>\u00b0C<\/option><option value=\"k\">K<\/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-5\">Temperature at which the reaction takes place<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66478\">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> Gibbs Free Energy Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Gibbs Free Energy Change<\/span><span class=\"result-term\">\u0394G<\/span><\/span><span class=\"field-value\" id=\"result-1\" 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\" id=\"output-2\"><span class=\"field-title\"><span>Gibbs Free Energy Change<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"kcal\/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-3\"><span class=\"field-title\"><span>Predicted Spontaneity<\/span><\/span><span class=\"field-value\" id=\"result-3\"><\/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=\"66478\" 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>Gibbs Free Energy 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\\[ \\Delta G = \\Delta H - T \\cdot \\Delta S \\\\ \\Delta G = \\Delta H - T \\Delta S \\quad \\text{(with } \\Delta H \\text{ in J\/mol, } \\Delta S \\text{ in J\/(mol\u00b7K), } T \\text{ in K)} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(\\Delta G\\) \u2014 Gibbs free energy change (J\/mol or kJ\/mol)<\/li>\n<li>\\(\\Delta H\\) \u2014 enthalpy change of the reaction (J\/mol)<\/li>\n<li>\\(T\\) \u2014 absolute temperature (kelvin)<\/li>\n<li>\\(\\Delta S\\) \u2014 entropy change of the reaction (J\/(mol\u00b7K))<\/li>\n<\/ul>\n<p>The formula combines the two driving forces of a chemical reaction \u2014 the release or absorption of heat (\\(\\Delta H\\)) and the change in disorder (\\(\\Delta S\\)) \u2014 into a single value that tells you whether the reaction can proceed on its own at the given temperature.<\/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>Gibbs Free Energy \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> the Haber reaction \\(N_2 + 3H_2 \\rightarrow 2NH_3\\) has \\(\\Delta H = -92.2\\) kJ\/mol and \\(\\Delta S = -198.75\\) J\/(mol\u00b7K). Is ammonia formation spontaneous at 25 \u00b0C?<\/p>\n<p>\\[ T = 25 + 273.15 = 298.15 \\text{ K} \\]<\/p>\n<p>\\[ \\Delta G = -92{,}200 - 298.15 \\times (-198.75) = -92{,}200 + 59{,}257.31 = -32{,}942.69 \\text{ J\/mol} \\]<\/p>\n<p><strong>Result:<\/strong> \\(\\Delta G \\approx -32.94\\) kJ\/mol (about \\(-7.87\\) kcal\/mol). Since \\(\\Delta G &lt; 0\\), the reaction is spontaneous at 25 \u00b0C \u2014 but the calculator also warns that spontaneity flips near 191 \u00b0C (464 K), so above that temperature ammonia formation stops being favorable.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Gibbs Free Energy Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Enthalpy Change (\u0394H)<\/strong> of the reaction and select its unit (kJ\/mol, J\/mol, or kcal\/mol). Use a negative value for exothermic reactions and a positive value for endothermic ones.<\/li>\n<li>Enter the <strong>Entropy Change (\u0394S)<\/strong> and choose the unit (J\/(mol\u00b7K), kJ\/(mol\u00b7K), or cal\/(mol\u00b7K)). Positive means disorder increases.<\/li>\n<li>Enter the <strong>Temperature<\/strong> and pick \u00b0C, K, or \u00b0F. The calculator converts everything to consistent units automatically.<\/li>\n<li>Read the <strong>Gibbs Free Energy Change<\/strong> in both kJ\/mol and kcal\/mol, plus the <strong>Predicted Spontaneity<\/strong> of the reaction under those exact conditions.<\/li>\n<\/ol>\n<h2>What Is Gibbs Free Energy?<\/h2>\n<p>Gibbs free energy, named after Josiah Willard Gibbs, is a thermodynamic quantity that measures the maximum amount of useful work a reaction can perform at constant temperature and pressure. Its change during a reaction, \\(\\Delta G\\), is the single most convenient indicator of whether a process is thermodynamically favorable: a reaction can proceed spontaneously only if it lowers the Gibbs free energy of the system.<\/p>\n<p>The sign of \\(\\Delta G\\) carries all the meaning. If \\(\\Delta G  0\\), the forward reaction is non-spontaneous (endergonic), and energy must be supplied to drive it; the reverse reaction is then the spontaneous one. If \\(\\Delta G = 0\\), the system is at equilibrium and no net reaction occurs in either direction.<\/p>\n<p>Temperature plays a decisive role because the entropy term is multiplied by \\(T\\). When \\(\\Delta H\\) and \\(\\Delta S\\) have opposite signs, the outcome is the same at every temperature. When they have the same sign, temperature decides: an endothermic reaction with a positive entropy change (like melting ice) becomes spontaneous only above a certain temperature, while an exothermic reaction with negative entropy change (like the Haber example above) is spontaneous only below a crossover temperature given by \\(T = \\Delta H \/ \\Delta S\\).<\/p>\n<p>One important caveat: spontaneity is about thermodynamics, not speed. A reaction can have a strongly negative \\(\\Delta G\\) and still be extremely slow \u2014 diamond converting to graphite is the classic example. For rates and activation barriers, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/arrhenius-equation-2\/\">Arrhenius Equation calculator<\/a>.<\/p>\n<h2>Sign Combinations at a Glance<\/h2>\n<table>\n<thead>\n<tr>\n<th>\u0394H<\/th>\n<th>\u0394S<\/th>\n<th>\u0394G = \u0394H \u2212 T\u0394S<\/th>\n<th>Outcome<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>\u2212<\/td>\n<td>+<\/td>\n<td>always negative<\/td>\n<td>Spontaneous at all temperatures<\/td>\n<\/tr>\n<tr>\n<td>+<\/td>\n<td>\u2212<\/td>\n<td>always positive<\/td>\n<td>Never spontaneous<\/td>\n<\/tr>\n<tr>\n<td>\u2212<\/td>\n<td>\u2212<\/td>\n<td>negative at low T<\/td>\n<td>Spontaneous below the crossover temperature<\/td>\n<\/tr>\n<tr>\n<td>+<\/td>\n<td>+<\/td>\n<td>negative at high T<\/td>\n<td>Spontaneous above the crossover temperature<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions and Practical Tips<\/h2>\n<ul>\n<li><strong>Standard vs. actual values:<\/strong> tabulated \\(\\Delta H\\) and \\(\\Delta S\\) values usually refer to standard conditions (298.15 K, 1 bar). The calculator applies them at any temperature you enter, which assumes both quantities are roughly temperature-independent \u2014 a good approximation over moderate ranges.<\/li>\n<li><strong>Constant conditions:<\/strong> the formula is strictly valid at constant temperature and pressure; that covers most bench-top chemistry and biological processes.<\/li>\n<li><strong>Concentrations matter:<\/strong> this calculator uses the simple \\(\\Delta G = \\Delta H - T\\Delta S\\) form. If reactant and product concentrations differ from standard values, the actual \\(\\Delta G\\) will shift (the full expression involves the reaction quotient \\(Q\\)).<\/li>\n<li><strong>Check your units:<\/strong> the classic mistake is mixing kJ with J. If you enter \\(\\Delta H\\) in kJ\/mol but \\(\\Delta S\\) in J\/(mol\u00b7K), let the unit selectors handle the conversion \u2014 the calculator always converts internally before applying the formula.<\/li>\n<li><strong>Per mole:<\/strong> values must refer to the reaction as written (per mole of reaction). If you double the stoichiometric coefficients, \\(\\Delta H\\) and \\(\\Delta S\\) double too.<\/li>\n<\/ul>\n<p>Once you know a reaction is thermodynamically favorable, you can plan the rest of your stoichiometry: use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/limiting-reactant-calculator\/\">Limiting Reactant calculator<\/a> to find how much product the available reagents can make, and the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/percent-yield-calculator\/\">Percent Yield calculator<\/a> to compare your actual output with the theoretical maximum. For solutions chemistry, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/molarity-calculator\/\">Molarity calculator<\/a> is a natural next step.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the Gibbs free energy change (\u0394G) from enthalpy (\u0394H), entropy (\u0394S), and temperature, and instantly see whether the reaction is spontaneous under those conditions.<\/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-66478","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\/66478","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=66478"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66478\/revisions"}],"predecessor-version":[{"id":66479,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66478\/revisions\/66479"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66478"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66478"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66478"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}