{"id":66873,"date":"2026-10-13T10:02:09","date_gmt":"2026-10-13T07:02:09","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66873"},"modified":"2026-10-13T10:02:09","modified_gmt":"2026-10-13T07:02:09","slug":"reaction-rate-law-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/reaction-rate-law-calculator\/","title":{"rendered":"Reaction Rate Law 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\">Calculate Reaction Rate from the Rate Law<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66873\" data-favorite-title=\"Reaction Rate Law\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/reaction-rate-law-calculator\/\" data-favorite-excerpt=\"Calculate the instantaneous reaction rate from the rate law v = k[A]^a[B]^b\u2026 Enter the rate constant, the concentration and order of each reactant, and get the rate, overall order and correct unit of k.\" 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-rate-law-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66873\" data-post=\"66873\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"is-single field\" id=\"input-1\"><span class=\"font-semibold\">Rate Constant<\/span><\/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=\"number\" name=\"rate_constant_k\" id=\"field-2\" aria-describedby=\"calc-info-2\" step=\"any\" value=\"0.042\"\/><small id=\"calc-info-2\">Experimental value of k at the reaction temperature, entered in units consistent with the concentration and time units chosen below (the correct unit of k is shown in the results).<\/small><\/div><div class=\"is-single field\" id=\"input-3\"><span class=\"font-semibold\">Units<\/span><\/div><div class=\"field\" id=\"input-4\"><label for=\"field-4\">Concentration unit<\/label><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"concentration_unit\"><option value=\"M\" selected>mol\/L (M)<\/option><option value=\"mM\">mmol\/L (mM)<\/option><option value=\"uM\">\u00b5mol\/L (\u00b5M)<\/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\" id=\"input-5\"><label for=\"field-5\">Time unit<\/label><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"time_unit\"><option value=\"s\" selected>seconds (s)<\/option><option value=\"min\">minutes (min)<\/option><option value=\"h\">hours (h)<\/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=\"is-single field\" id=\"input-6\"><span class=\"font-semibold\">Reactants<\/span><\/div><div class=\"field is-single\" id=\"input-7\"><label for=\"field-7\">Concentration \u00d7 Order<\/label><textarea id=\"field-7\" name=\"concentration_order\">0.50 \u00d7 1; 0.20 \u00d7 2<\/textarea><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66873\">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> Reaction Rate<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Reaction Rate<\/span><span class=\"result-term\">v<\/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>Rate in mol\/(L\u00b7s)<\/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>Rate Law<\/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>Reactant Contributions<\/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>Overall Order and Unit of k<\/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=\"66873\" 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>Rate Law<\/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\\[ v = k\\,[A]^a [B]^b [C]^c \\cdots \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(v\\) \u2014 reaction rate, the change in concentration per unit time (mol\/L\u00b7s or the chosen units)<\/li>\n<li>\\(k\\) \u2014 rate constant, a temperature-dependent experimental value<\/li>\n<li>\\([A], [B], [C]\\) \u2014 molar concentrations of the reactants<\/li>\n<li>\\(a, b, c\\) \u2014 reaction orders with respect to each reactant (determined experimentally)<\/li>\n<\/ul>\n<p>The overall reaction order is the sum of the exponents: \\(n = a + b + c + \\cdots\\). The rate constant carries units that depend on \\(n\\): \\(k\\) has units of \\((\\text{concentration})^{1-n}\\,(\\text{time})^{-1}\\).<\/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>Rate Law \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a reaction with rate law \\(v = k[A][B]^2\\), where \\(k = 0.042\\;\\mathrm{M^{-2}\\,s^{-1}}\\), \\([A] = 0.50\\;\\mathrm{M}\\) and \\([B] = 0.20\\;\\mathrm{M}\\).<\/p>\n<p>\\[ v = 0.042 \\times (0.50)^{1} \\times (0.20)^{2} = 0.042 \\times 0.50 \\times 0.040 \\]<\/p>\n<p>\\[ v = 8.4 \\times 10^{-4}\\;\\mathrm{M\/s} \\]<\/p>\n<p><strong>Result:<\/strong> \\(v = 8.4 \\times 10^{-4}\\) mol\/(L\u00b7s). The overall order is \\(n = 1 + 2 = 3\\), so the unit of \\(k\\) is \\(\\mathrm{M^{-2}\\,s^{-1}}\\) (equivalently \\(\\mathrm{L^{2}\\,mol^{-2}\\,s^{-1}}\\)).<\/p>\n<p>\n\r\n<\/section>\n<h2>How to use the calculator<\/h2>\n<ol>\n<li>Enter the <strong>Rate constant (k)<\/strong> \u2014 the experimental value of \\(k\\) at the reaction temperature. Use the units that match your concentration and time choices; the correct unit of \\(k\\) is shown in the results.<\/li>\n<li>Choose the <strong>Concentration unit<\/strong> (M, mM or \u00b5M) and the <strong>Time unit<\/strong> (s, min or h) for your data.<\/li>\n<li>List the reactants in <strong>Concentration \u00d7 Order<\/strong>, one per line or separated by semicolons \u2014 for example <code>0.50 \u00d7 1; 0.20 \u00d7 2<\/code> for a rate law \\(v = k[A][B]^2\\). A plain concentration without an order counts as first order; zero, fractional and negative orders are all accepted.<\/li>\n<li>Read the <strong>Reaction Rate<\/strong> in your units and converted to mol\/(L\u00b7s), together with the substituted rate law, each reactant's contribution, the overall order and the unit of \\(k\\).<\/li>\n<\/ol>\n<h2>What the rate law describes<\/h2>\n<p>The rate law expresses how the instantaneous rate of a chemical reaction depends on the concentrations of its reactants. For a general reaction, the rate is proportional to each concentration raised to a power: \\(v = k[A]^a[B]^b \\cdots\\). Importantly, the exponents (the orders) <em>cannot<\/em> be read off the balanced equation \u2014 except for elementary steps \u2014 they must be determined experimentally, classically from initial-rate measurements.<\/p>\n<p>Each order tells you how sensitively the rate responds to that reactant. If \\([A]\\) doubles and the rate stays the same, the reaction is zero order in A. If the rate doubles, it is first order (rate \\(\\propto [A]\\)). If the rate quadruples, it is second order (rate \\(\\propto [A]^2\\)). The calculator's contribution table shows exactly this effect for each reactant you enter, including fractional and negative orders, where an inhibitor slows the reaction as its concentration rises.<\/p>\n<p>The rate constant \\(k\\) absorbs everything else: temperature, catalyst and medium. Its numerical value is meaningless without its units, which follow from the overall order \\(n\\). For a first-order reaction \\(k\\) has units of s\u207b\u00b9; for second order, M\u207b\u00b9\u00b7s\u207b\u00b9; for third order, M\u207b\u00b2\u00b7s\u207b\u00b9. This is why the calculator reports the unit of \\(k\\) alongside the rate \u2014 it lets you check that the \\(k\\) you entered is consistent with the orders you assumed.<\/p>\n<p>Keep in mind that the result is the <em>instantaneous<\/em> rate at the concentrations entered. As the reaction proceeds, reactants are consumed and the rate falls. This is why chemists usually work with initial rates, measured before concentrations change appreciably.<\/p>\n<h2>Assumptions, limitations and tips<\/h2>\n<ul>\n<li><strong>Fixed temperature:<\/strong> \\(k\\) and the orders are valid only at the temperature at which they were measured. The rate constant rises strongly with temperature (Arrhenius behaviour); to compare \\(k\\) at two temperatures, use our <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\">Van 't Hoff Equation Calculator<\/a>.<\/li>\n<li><strong>Not for equilibrium mixtures:<\/strong> the rate law describes the forward kinetics, not the equilibrium composition. For gas-phase equilibria, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/kp-to-kc-calculator\/\">Kp to Kc Calculator<\/a>.<\/li>\n<li><strong>First-order reactions only:<\/strong> simple half-life formulas apply only when the overall order is 1. For other orders the half-life depends on the starting concentration \u2014 the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/reaction-half-life-calculator\/\">Reaction Half-Life Calculator<\/a> handles those cases.<\/li>\n<li><strong>Units of k must be consistent:<\/strong> if you enter concentrations in mM, the rate is returned in mM per time unit and \\(k\\) must correspondingly use mM. When in doubt, convert everything to M and s \u2014 the calculator also shows the rate in mol\/(L\u00b7s).<\/li>\n<li><strong>Orders need not be integers:<\/strong> complex or chain mechanisms often give fractional orders, and catalysts or inhibitors can give negative ones. Both are handled correctly here.<\/li>\n<\/ul>\n<h2>Quick reference: order and the effect of doubling a concentration<\/h2>\n<table>\n<thead>\n<tr>\n<th>Order in reactant X<\/th>\n<th>Rate law term<\/th>\n<th>Rate change if [X] doubles<\/th>\n<th>Typical unit of k (n = this order only)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>0<\/td>\n<td>\\([X]^0 = 1\\)<\/td>\n<td>no change<\/td>\n<td>M\u00b7s\u207b\u00b9<\/td>\n<\/tr>\n<tr>\n<td>1<\/td>\n<td>\\([X]\\)<\/td>\n<td>\u00d7 2<\/td>\n<td>s\u207b\u00b9<\/td>\n<\/tr>\n<tr>\n<td>2<\/td>\n<td>\\([X]^2\\)<\/td>\n<td>\u00d7 4<\/td>\n<td>M\u207b\u00b9\u00b7s\u207b\u00b9<\/td>\n<\/tr>\n<tr>\n<td>3<\/td>\n<td>\\([X]^3\\)<\/td>\n<td>\u00d7 8<\/td>\n<td>M\u207b\u00b2\u00b7s\u207b\u00b9<\/td>\n<\/tr>\n<tr>\n<td>0.5<\/td>\n<td>\\([X]^{0.5}\\)<\/td>\n<td>\u00d7 1.41<\/td>\n<td>M<sup>0.5<\/sup>\u00b7s\u207b\u00b9<\/td>\n<\/tr>\n<tr>\n<td>\u22121 (inhibitor)<\/td>\n<td>\\([X]^{-1}\\)<\/td>\n<td>\u00d7 0.5 (rate halves)<\/td>\n<td>M\u00b2\u00b7s\u207b\u00b9<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>For a multi-reactant rate law, the effects multiply: in the example above, doubling both \\([A]\\) and \\([B]\\) increases the rate by \\(2^1 \\times 2^2 = 8\\).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the instantaneous reaction rate from the rate law v = k[A]^a[B]^b\u2026 Enter the rate constant, the concentration and order of each reactant, and get the rate, overall order and correct unit of k.<\/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-66873","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\/66873","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=66873"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66873\/revisions"}],"predecessor-version":[{"id":66874,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66873\/revisions\/66874"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66873"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66873"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66873"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}