{"id":66500,"date":"2026-10-06T17:35:46","date_gmt":"2026-10-06T14:35:46","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66500"},"modified":"2026-10-06T17:35:46","modified_gmt":"2026-10-06T14:35:46","slug":"kp-to-kc-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/kp-to-kc-calculator\/","title":{"rendered":"Kp to Kc 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\">Convert Between Pressure- and Concentration-Based Equilibrium Constants<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66500\" data-favorite-title=\"Kp to Kc\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/kp-to-kc-calculator\/\" data-favorite-excerpt=\"Convert an equilibrium constant between its pressure-based form (Kp) and concentration-based form (Kc). Enter the known constant, the temperature, and the change in moles of gas to get the result instantly.\" 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\/kp-to-kc-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66500\" data-post=\"66500\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field\" id=\"input-1\"><label for=\"field-1\">What to Calculate<\/label><div class=\"grid grid-cols-1\"><select id=\"field-1\" name=\"what_to_calculate\"><option value=\"kp\" selected>Kp (from a known Kc)<\/option><option value=\"kc\">Kc (from a known Kp)<\/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><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Known Equilibrium Constant<\/label><div class=\"term\">K<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"known_equilibrium_constant\" id=\"field-2\" aria-describedby=\"calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 4.0\" min=\"1.0E-6\" value=\"4\"\/><small id=\"calc-info-2\">The Kc value if you are finding Kp, or the Kp value if you are finding Kc<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-3\">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=\"text\" name=\"temperature\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 500\" min=\"0.01\" value=\"500\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"K\" selected>K<\/option><option value=\"C\">\u00b0C<\/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\">Temperature of the equilibrium mixture<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-5\">Change in Moles of Gas<\/label><div class=\"term\">\u0394n<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"number\" name=\"change_in_moles_of_gas\" id=\"field-5\" aria-describedby=\"calc-info-5\" placeholder=\"e.g. -1, 0, 1\" step=\"1\" value=\"-1\"\/><small id=\"calc-info-5\">\u0394n = (moles of gaseous products) \u2212 (moles of gaseous reactants); can be negative or zero<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66500\">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 Constant Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Kp (Pressure-Based Constant)<\/span><span class=\"result-term\">Kp<\/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>Kc (Concentration-Based Constant)<\/span><span class=\"result-term\">Kc<\/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>Conversion Factor (RT)^\u0394n<\/span><span class=\"result-term\">(RT)^\u0394n<\/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 class=\"field-result is-column\" id=\"output-4\"><span class=\"field-title\"><span>Calculation Details<\/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><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=\"66500\" 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>Kp to Kc 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\\[ K_p = K_c \\cdot (RT)^{\\Delta n} \\]\n\\[ K_c = \\frac{K_p}{(RT)^{\\Delta n}} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(K_p\\) \u2014 equilibrium constant based on partial pressures (atm)<\/li>\n<li>\\(K_c\\) \u2014 equilibrium constant based on molar concentrations (mol\/L)<\/li>\n<li>\\(R\\) \u2014 gas constant, 0.082057 L\u00b7atm\/(mol\u00b7K)<\/li>\n<li>\\(T\\) \u2014 absolute temperature (K)<\/li>\n<li>\\(\\Delta n\\) \u2014 change in moles of gas: \\(\\Delta n = \\) (moles of gaseous products) \\(-\\) (moles of gaseous reactants)<\/li>\n<\/ul>\n<p>The two constants describe the same equilibrium but are expressed in different units; the factor \\((RT)^{\\Delta n}\\) converts between them.<\/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>Kp to Kc \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> for the reaction \\(2SO_2(g) + O_2(g) \\rightleftharpoons 2SO_3(g)\\), the equilibrium constant is \\(K_c = 4.0\\) at 500 K. Find Kp.<\/p>\n<p>Count only gaseous species: \\(\\Delta n = 2 - (2 + 1) = -1\\)<\/p>\n<p>\\[ K_p = K_c \\cdot (RT)^{\\Delta n} = 4.0 \\times (0.082057 \\times 500)^{-1} = 4.0 \\times (41.0285)^{-1} \\]<\/p>\n<p>\\[ K_p = 4.0 \\times 0.024373 = 0.097494 \\]<\/p>\n<p><strong>Result:<\/strong> \\(K_p \\approx 0.0975\\) at 500 K.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Kp to Kc Calculator<\/h2>\n<ol>\n<li>Open the <strong>What to Calculate<\/strong> dropdown and choose whether you want <em>Kp (from a known Kc)<\/em> or <em>Kc (from a known Kp)<\/em>.<\/li>\n<li>Enter your value in <strong>Known Equilibrium Constant<\/strong> \u2014 the Kc if you are finding Kp, or the Kp if you are finding Kc.<\/li>\n<li>Type the temperature in <strong>Temperature<\/strong> and select the unit (K or \u00b0C) from the dropdown next to it. The calculator converts \u00b0C to kelvin automatically.<\/li>\n<li>Enter <strong>Change in Moles of Gas<\/strong>: subtract the total moles of gaseous reactants from the total moles of gaseous products. This value can be negative, zero, or positive.<\/li>\n<li>Read the results: Kp, Kc, the conversion factor \\((RT)^{\\Delta n}\\), and a step-by-step calculation trail showing exactly how the answer was obtained.<\/li>\n<\/ol>\n<h2>What Are Kp and Kc?<\/h2>\n<p>Chemical equilibria involving gases can be described in two equivalent ways. \\(K_c\\) is built from the equilibrium molar concentrations of the species (mol\/L), while \\(K_p\\) is built from their partial pressures (atm). Textbooks and exam problems use both, and it is common to be given one form and asked for the other.<\/p>\n<p>The link between them comes from the ideal gas law, \\(PV = nRT\\), which relates a gas's partial pressure to its concentration: \\(P = (n\/V)RT\\). When you substitute this into the equilibrium expression, every gaseous species contributes a factor of \\(RT\\), and these factors collect into \\((RT)^{\\Delta n}\\), where \\(\\Delta n\\) is the change in the number of moles of gas between products and reactants.<\/p>\n<p>The sign of \\(\\Delta n\\) controls the direction of the conversion. If the reaction produces more gas molecules than it consumes (\\(\\Delta n &gt; 0\\)), then \\(K_p &gt; K_c\\) at typical temperatures. If it consumes gas (\\(\\Delta n &lt; 0\\)), then \\(K_p &lt; K_c\\). If the number of gas molecules is unchanged (\\(\\Delta n = 0\\)), the two constants are numerically equal \u2014 for example, for \\(H_2(g) + I_2(g) \\rightleftharpoons 2HI(g)\\).<\/p>\n<p>Keep in mind that neither constant is truly dimensionless in this elementary treatment; they are conventionally reported as plain numbers. The conversion factor \\((RT)^{\\Delta n}\\) carries the units, which is why the numerical value of the constant changes between the two forms.<\/p>\n<h2>Assumptions, Limitations, and Tips<\/h2>\n<ul>\n<li><strong>Count only gaseous species.<\/strong> Pure solids and liquids do not appear in equilibrium expressions, so they must be excluded when computing \\(\\Delta n\\). For \\(CaCO_3(s) \\rightleftharpoons CaO(s) + CO_2(g)\\), \\(\\Delta n = 1\\), not 2 \u2212 1 = 1 from all species counted.<\/li>\n<li><strong>The gas constant must match the units.<\/strong> This calculator uses \\(R = 0.082057\\) L\u00b7atm\/(mol\u00b7K), which is the correct choice when pressures are in atm and concentrations in mol\/L. If a problem quotes pressures in bar or kPa, convert them to atm first or use the corresponding value of R.<\/li>\n<li><strong>Temperature must be absolute.<\/strong> The formula requires kelvin. If you enter \u00b0C, the calculator adds 273.15 for you, but double-check that you selected the right unit.<\/li>\n<li><strong>\u0394n must be a whole number.<\/strong> Count the stoichiometric coefficients of gaseous products and reactants from the balanced equation; do not use the actual amounts present at equilibrium.<\/li>\n<li><strong>Ideal behavior is assumed.<\/strong> At very high pressures or low temperatures, real gases deviate from ideality and the simple \\((RT)^{\\Delta n}\\) relationship becomes approximate.<\/li>\n<li>Double-check your balanced equation first \u2014 a wrong \\(\\Delta n\\) is the most common source of error in these conversions.<\/li>\n<\/ul>\n<h2>Quick Reference: \u0394n for Common Reaction Types<\/h2>\n<table>\n<thead>\n<tr>\n<th>Reaction (gases only counted)<\/th>\n<th>\\(\\Delta n\\)<\/th>\n<th>Relation at 500 K<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>\\(N_2 + 3H_2 \\rightleftharpoons 2NH_3\\)<\/td>\n<td>\\(-2\\)<\/td>\n<td>\\(K_p = K_c \/ (RT)^2 \\approx K_c \/ 1683\\)<\/td>\n<\/tr>\n<tr>\n<td>\\(2SO_2 + O_2 \\rightleftharpoons 2SO_3\\)<\/td>\n<td>\\(-1\\)<\/td>\n<td>\\(K_p \\approx K_c \/ 41.03\\)<\/td>\n<\/tr>\n<tr>\n<td>\\(H_2 + I_2 \\rightleftharpoons 2HI\\)<\/td>\n<td>\\(0\\)<\/td>\n<td>\\(K_p = K_c\\)<\/td>\n<\/tr>\n<tr>\n<td>\\(N_2O_4 \\rightleftharpoons 2NO_2\\)<\/td>\n<td>\\(+1\\)<\/td>\n<td>\\(K_p \\approx K_c \\times 41.03\\)<\/td>\n<\/tr>\n<tr>\n<td>\\(PCl_5 \\rightleftharpoons PCl_3 + Cl_2\\)<\/td>\n<td>\\(+1\\)<\/td>\n<td>\\(K_p \\approx K_c \\times 41.03\\)<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>To explore the equilibrium concept further, try our <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/equilibrium-constant-calculator\/\">Equilibrium Constant calculator<\/a>, or connect \\(K\\) to thermodynamics with the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/gibbs-free-energy-calculator\/\">Gibbs Free Energy calculator<\/a>. For equilibria at electrodes, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/nernst-equation-calculator\/\">Nernst Equation calculator<\/a> is another useful tool.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Convert an equilibrium constant between its pressure-based form (Kp) and concentration-based form (Kc). Enter the known constant, the temperature, and the change in moles of gas to get the result instantly.<\/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-66500","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\/66500","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=66500"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66500\/revisions"}],"predecessor-version":[{"id":66501,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66500\/revisions\/66501"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66500"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66500"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66500"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}