{"id":66533,"date":"2026-10-07T08:29:17","date_gmt":"2026-10-07T05:29:17","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66533"},"modified":"2026-10-07T08:29:17","modified_gmt":"2026-10-07T05:29:17","slug":"reaction-half-life-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/reaction-half-life-calculator\/","title":{"rendered":"Reaction Half-Life 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 the Half-Life of a Zero-, First- or Second-Order Reaction<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66533\" data-favorite-title=\"Reaction Half-Life\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/reaction-half-life-calculator\/\" data-favorite-excerpt=\"Calculate the half-life of a zero-, first- or second-order chemical reaction from the rate constant k and, where needed, the initial concentration. Results are shown in seconds and in your chosen time unit.\" 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\/reaction-half-life-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66533\" data-post=\"66533\"><fieldset class=\"fieldset-input is-2\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field is-single\" id=\"input-1\"><label for=\"field-1\">Reaction order<\/label><div class=\"grid grid-cols-1\"><select id=\"field-1\" name=\"reaction_order\"><option value=\"Zero order\">Zero order<\/option><option value=\"First order\">First order<\/option><option value=\"Second order\">Second order<\/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\">Rate constant (k)<\/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=\"rate_constant_k\" id=\"field-2\" aria-describedby=\"calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.05\" min=\"0\" value=\"0.05\"\/><small id=\"calc-info-2\">Expressed with the time unit chosen below: zero order in mol\u00b7L\u207b\u00b9\u00b7time\u207b\u00b9, first order in time\u207b\u00b9, second order in L\u00b7mol\u207b\u00b9\u00b7time\u207b\u00b9<\/small><\/div><div class=\"field\" id=\"input-3\"><label for=\"field-3\">Time unit of k<\/label><div class=\"grid grid-cols-1\"><select id=\"field-3\" name=\"time_unit_of_k\"><option value=\"s\">per second<\/option><option value=\"min\" selected>per minute<\/option><option value=\"h\">per hour<\/option><option value=\"d\">per day<\/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-4\"><label for=\"field-4\">Initial concentration (A\u2080)<\/label><div class=\"term\">A\u2080<\/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=\"initial_concentration_a\" id=\"field-4\" aria-describedby=\"calc-info-4\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.5\" min=\"0\" value=\"0.5\"\/><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"unit\" aria-label=\"Unit\"><option value=\"M\" selected>mol\/L<\/option><option value=\"mM\">mmol\/L<\/option><option value=\"uM\">\u00b5mol\/L<\/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\">Required for zero- and second-order reactions \u2014 a first-order half-life does not depend on it<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66533\">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> Half-Life Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Half-Life<\/span><span class=\"result-term\">t\u00bd<\/span><\/span><span class=\"field-value\" id=\"result-1\" data-unit=\"s\"><\/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>Half-Life in Your Time Unit<\/span><span class=\"result-term\">t\u00bd<\/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 is-column\" id=\"output-3\"><span class=\"field-title\"><span>Calculation Details<\/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=\"66533\" 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>Reaction Half-Life 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\\[ t_{1\/2} = \\frac{[A]_0}{2k} \\quad \\text{(zero order)} \\\\ t_{1\/2} = \\frac{\\ln 2}{k} \\quad \\text{(first order)} \\\\ t_{1\/2} = \\frac{1}{k[A]_0} \\quad \\text{(second order)} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(t_{1\/2}\\) \u2014 half-life, the time needed for the reactant concentration to drop to half of its initial value<\/li>\n<li>\\(k\\) \u2014 rate constant; its units depend on the order (see below)<\/li>\n<li>\\([A]_0\\) \u2014 initial concentration of the reactant (mol\/L)<\/li>\n<\/ul>\n<p>Each expression comes from integrating the rate law of the corresponding order. Notice that only the first-order half-life is independent of the starting concentration \u2014 this is the behaviour familiar from radioactive decay.<\/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>Reaction Half-Life \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a first-order decomposition has a rate constant of \\(k = 0.05\\ \\text{min}^{-1}\\) \u2014 the calculator's default values.<\/p>\n<p>\\[ t_{1\/2} = \\frac{\\ln 2}{k} = \\frac{0.6931}{0.05\\ \\text{min}^{-1}} = 13.86\\ \\text{min} \\]<\/p>\n<p><strong>Result:<\/strong> the half-life is <strong>13.86 minutes<\/strong> (about 831.8 seconds). Because the reaction is first order, no initial concentration is required \u2014 every half-life interval halves whatever concentration remains.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Open <strong>Reaction order<\/strong> and choose <em>Zero order<\/em>, <em>First order<\/em> or <em>Second order<\/em>. For a first-order reaction the initial-concentration field is hidden automatically.<\/li>\n<li>Enter the <strong>Rate constant (k)<\/strong>. Make sure its units match the order: mol\u00b7L\u207b\u00b9\u00b7time\u207b\u00b9 for zero order, time\u207b\u00b9 for first order, L\u00b7mol\u207b\u00b9\u00b7time\u207b\u00b9 for second order.<\/li>\n<li>Select the <strong>Time unit of k<\/strong> (per second, per minute, per hour or per day). The half-life is reported in the same unit.<\/li>\n<li>For zero- or second-order reactions, enter the <strong>Initial concentration (A\u2080)<\/strong> and pick its unit (mol\/L, mmol\/L or \u00b5mol\/L). The value is converted to mol\/L internally, so k must be referenced to mol\/L (e.g. L\u00b7mol\u207b\u00b9\u00b7min\u207b\u00b9, not L\u00b7mmol\u207b\u00b9\u00b7min\u207b\u00b9).<\/li>\n<li>Read the results: the <strong>Half-Life<\/strong> in seconds, the <strong>Half-Life in Your Time Unit<\/strong>, and the <strong>Calculation Details<\/strong> showing the formula used and the substitution step by step.<\/li>\n<\/ol>\n<h2>What Is the Half-Life of a Reaction?<\/h2>\n<p>The half-life \\(t_{1\/2}\\) is the time it takes for the concentration of a reactant to fall to one half of its value at the start of the interval. It is one of the most intuitive ways to describe how fast a reaction proceeds: a short half-life means the reactant disappears quickly, a long one means it lingers.<\/p>\n<p>Unlike radioactive decay, where the half-life is fixed, the half-life of a chemical reaction depends on the <em>order<\/em> of the reaction \u2014 that is, on how the rate depends on concentration. For a first-order reaction the rate is proportional to \\([A]\\), and the half-life comes out constant: \\(t_{1\/2} = \\ln 2 \/ k\\). Successive half-lives always halve what is left, so 75% of the reactant is gone after two half-lives, 87.5% after three, and so on. This is exactly the pattern our <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/radioactive-decay-calculator\/\">Radioactive Decay Calculator<\/a> uses.<\/p>\n<p>Zero- and second-order reactions behave differently. In a zero-order reaction the rate is constant regardless of concentration, so \\(t_{1\/2} = [A]_0\/2k\\): the half-life grows as the reactant is used up, and the reaction finishes completely at \\(t = [A]_0\/k\\), exactly twice the first half-life. In a second-order reaction \\(t_{1\/2} = 1\/(k[A]_0)\\), so each successive half-life <em>doubles<\/em> \u2014 doubling the initial concentration halves the half-life.<\/p>\n<table>\n<thead>\n<tr>\n<th>Order<\/th>\n<th>Half-life<\/th>\n<th>Units of k<\/th>\n<th>Dependence on \\([A]_0\\)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Zero<\/td>\n<td>\\(t_{1\/2} = [A]_0\/(2k)\\)<\/td>\n<td>mol\u00b7L\u207b\u00b9\u00b7time\u207b\u00b9<\/td>\n<td>Proportional<\/td>\n<\/tr>\n<tr>\n<td>First<\/td>\n<td>\\(t_{1\/2} = \\ln 2\/k\\)<\/td>\n<td>time\u207b\u00b9<\/td>\n<td>None<\/td>\n<\/tr>\n<tr>\n<td>Second<\/td>\n<td>\\(t_{1\/2} = 1\/(k[A]_0)\\)<\/td>\n<td>L\u00b7mol\u207b\u00b9\u00b7time\u207b\u00b9<\/td>\n<td>Inversely proportional<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Measuring how the half-life changes with concentration is in fact a classic experimental method for determining the order of a reaction: if \\(t_{1\/2}\\) is constant the reaction is first order; if it scales with \\([A]_0\\) it is zero order; if it is inversely proportional to \\([A]_0\\) it is second order.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>Single reactant, constant temperature.<\/strong> The formulas describe an isolated reactant whose integrated rate law holds over the whole concentration range. The rate constant \\(k\\) itself depends strongly on temperature, as described by the Arrhenius and <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\">Van 't Hoff equation<\/a>; if the temperature changes, so does the half-life.<\/li>\n<li><strong>Unit consistency matters.<\/strong> The concentration you enter is converted to mol\/L, so \\(k\\) must carry its concentration part in mol\u00b7L\u207b\u00b9 (for example L\u00b7mol\u207b\u00b9\u00b7s\u207b\u00b9). A constant quoted per mmol or per \u00b5mol must be rescaled before use.<\/li>\n<li><strong>Real reactions can change order.<\/strong> Many reactions follow simple kinetics only over a limited concentration range; near completion, side reactions, equilibria or depletion of a second reactant can alter the apparent order, so the calculated half-life is best treated as valid near the stated \\([A]_0\\).<\/li>\n<li><strong>Pseudo-orders are common.<\/strong> If one reactant is in large excess, its concentration stays nearly constant and the reaction may behave as first order in the tracked reactant even though the true molecularity is higher. The first-order formula still applies with the pseudo-first-order rate constant.<\/li>\n<li><strong>Successive half-lives.<\/strong> For zero order the reaction goes to completion at \\(t = [A]_0\/k\\); for first order the reactant never fully disappears, and for second order each successive half-life doubles \u2014 keep this in mind when extrapolating far beyond the first half-life.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the half-life of a zero-, first- or second-order chemical reaction from the rate constant k and, where needed, the initial concentration. Results are shown in seconds and in your chosen time unit.<\/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-66533","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\/66533","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=66533"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66533\/revisions"}],"predecessor-version":[{"id":66534,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66533\/revisions\/66534"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66533"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66533"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66533"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}