{"id":55836,"date":"2015-10-24T16:00:13","date_gmt":"2015-10-24T14:00:13","guid":{"rendered":"http:\/\/wpcalc.com\/?p=55836"},"modified":"2026-10-15T08:22:44","modified_gmt":"2026-10-15T05:22:44","slug":"henrys-law","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/converters\/henrys-law\/","title":{"rendered":"Henry\u2019s Law Converter"},"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 Henry\u2019s Constant Between Units<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"55836\" data-favorite-title=\"Henry\u2019s Law\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/converters\/henrys-law\/\" data-favorite-excerpt=\"Convert a Henry\u2019s law constant between mol\/(L\u00b7atm), atm\u00b7L\/mol, mol\/(m\u00b3\u00b7Pa), mole-fraction forms, atm\u00b7m\u00b3\/mol and cm\u00b3\/cm\u00b3. Enter the value, pick the From and To units, and add a temperature when cm\u00b3\/cm\u00b3 is involved.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-physic\">\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\/converters\/henrys-law\/\" method=\"POST\" class=\"calculator\" id=\"calculator-55836\" data-post=\"55836\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field\" id=\"input-1\"><label for=\"field-1\">Henry\u2019s constant value<\/label><input type=\"text\" name=\"henrys_constant_value\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" min=\"0\" value=\"0.034\"\/><small id=\"calc-info-1\">Enter a value greater than zero.<\/small><\/div><div class=\"field\" id=\"input-2\"><label for=\"field-2\">From unit<\/label><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"from_unit\"><option value=\"mcp\" selected>mol\/(L\u00b7atm)<\/option><option value=\"lpc\">atm\u00b7L\/mol<\/option><option value=\"sicp\">mol\/(m\u00b3\u00b7Pa)<\/option><option value=\"pxatm\">atm\/mol fraction<\/option><option value=\"pxpa\">Pa\/mol fraction<\/option><option value=\"mpc\">atm\u00b7m\u00b3\/mol<\/option><option value=\"cc\">cm\u00b3\/cm\u00b3<\/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-3\"><label for=\"field-3\">To unit<\/label><div class=\"grid grid-cols-1\"><select id=\"field-3\" name=\"to_unit\"><option value=\"mcp\">mol\/(L\u00b7atm)<\/option><option value=\"lpc\">atm\u00b7L\/mol<\/option><option value=\"sicp\">mol\/(m\u00b3\u00b7Pa)<\/option><option value=\"pxatm\" selected>atm\/mol fraction<\/option><option value=\"pxpa\">Pa\/mol fraction<\/option><option value=\"mpc\">atm\u00b7m\u00b3\/mol<\/option><option value=\"cc\">cm\u00b3\/cm\u00b3<\/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-4\" hidden><label for=\"field-4\">Temperature<\/label><input type=\"text\" name=\"temperature\" id=\"field-4\" aria-describedby=\"calc-unit-4 calc-info-4\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" min=\"0\" value=\"298.15\"\/><div class=\"unit\" id=\"calc-unit-4\">K<\/div><small id=\"calc-info-4\">Required for conversions involving cm\u00b3\/cm\u00b3; 298.15 K is 25 \u00b0C.<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"55836\">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> Your Results<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Converted Henry\u2019s Constant<\/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><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=\"55836\" 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\">1<\/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>Henry\u2019s Law 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\\[ c = k_{c\/p}\\,p, \\qquad k_{p\/c} = \\frac{1}{k_{c\/p}}, \\qquad k_{p\/x} = \\frac{1}{k_{c\/p}\\,C_w}, \\qquad k_{\\mathrm{SI}} = k_{c\/p}\\cdot\\frac{1000}{101325} \\\\ k_{\\mathrm{atm\\,m^3\/mol}} = \\frac{1}{1000\\,k_{c\/p}}, \\qquad k_{cc} = \\frac{1}{1000\\,k_{c\/p}\\,RT} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(c\\) \u2014 dissolved-gas concentration (mol\/L).<\/li>\n<li>\\(p\\) \u2014 partial pressure of the gas above the liquid (atm; Pa forms use 1 atm = 101,325 Pa).<\/li>\n<li>\\(k_{c\/p}\\) \u2014 Henry\u2019s law constant in mol\/(L\u00b7atm), the base definition the calculator converts everything through.<\/li>\n<li>\\(k_{p\/c}\\) \u2014 the reciprocal constant in atm\u00b7L\/mol: \\(k_{p\/c}=1\/k_{c\/p}\\).<\/li>\n<li>\\(k_{p\/x}\\) \u2014 pressure per dissolved mole fraction, in atm\/mol fraction; the Pa\/mol fraction value is 101,325 times the atm\/mol fraction value.<\/li>\n<li>\\(C_w\\) \u2014 molar concentration of the liquid; the calculator uses \\(C_w \\approx 55.5\\) mol\/L, the value for water, with \\(x \\approx c\/C_w\\) for dilute solutions.<\/li>\n<li>\\(k_{\\mathrm{SI}}\\) \u2014 the same constant in mol\/(m\u00b3\u00b7Pa), obtained from 1 m\u00b3 = 1,000 L and 1 atm = 101,325 Pa.<\/li>\n<li>\\(k_{cc}\\) \u2014 dimensionless solubility in cm\u00b3\/cm\u00b3 (volume of gas, measured at the gas-phase conditions, per volume of liquid).<\/li>\n<li>\\(R = 8.2057\\times10^{-5}\\) atm\u00b7m\u00b3\/(mol\u00b7K) \u2014 the gas constant, and \\(T\\) \u2014 absolute temperature in kelvin.<\/li>\n<\/ul>\n<p>Henry\u2019s law itself is the first equation, \\(c = k_{c\/p}p\\): the dissolved concentration grows in proportion to the gas\u2019s partial pressure. The remaining relations convert one published definition of the constant into another, and the calculator applies them in two steps: first to mol\/(L\u00b7atm), then to the requested unit. Temperature enters only the cm\u00b3\/cm\u00b3 conversion.<\/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>Henry\u2019s Law \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> keep the default inputs \u2014 a Henry\u2019s constant value of 0.034 (a typical value for CO\u2082 in water at 25 \u00b0C), From unit mol\/(L\u00b7atm), To unit atm\/mol fraction. For a dilute aqueous solution, \\(x \\approx c\/55.5\\), so:<\/p>\n<p>\\[ k_{p\/x} = \\frac{1}{k_{c\/p}\\,C_w} = \\frac{55.5}{0.034} = 1632.353 \\ \\text{atm\/mol fraction} \\]<\/p>\n<p><strong>Result:<\/strong> 1632.353 atm\/mol fraction. As a cross-check, the Pa\/mol fraction form is 101,325 times larger, about \\(1.654\\times10^{8}\\) Pa\/mol fraction.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to use the calculator<\/h2>\n<ol>\n<li>Enter the number in <strong>Henry\u2019s constant value<\/strong>. It must be greater than zero, because several definitions are reciprocals of one another.<\/li>\n<li>Select <strong>From unit<\/strong> to match the definition under which your value was reported \u2014 concentration per pressure, pressure per concentration, pressure per mole fraction, or dimensionless. Do not match by name alone; check the source\u2019s units.<\/li>\n<li>Select the <strong>To unit<\/strong> you need.<\/li>\n<li>If either unit is <strong>cm\u00b3\/cm\u00b3<\/strong>, the <strong>Temperature<\/strong> field appears; enter the absolute temperature in kelvin (the default, 298.15 K, is 25 \u00b0C). This field is ignored for every other pair of units.<\/li>\n<li>Read the result under <strong>Converted Henry\u2019s Constant<\/strong>.<\/li>\n<\/ol>\n<h2>What a Henry\u2019s law constant tells you<\/h2>\n<p>Henry\u2019s law states that, at equilibrium and within a range where the relationship stays linear, the amount of a gas dissolved in a liquid is proportional to the partial pressure of that gas above the liquid. Written as \\(c = k_{c\/p}p\\), a larger constant means the gas dissolves more readily: oxygen dissolves in water more readily than nitrogen in the sense that its \\(k_{c\/p}\\) is larger. Written the other way, \\(p = k_{p\/c}c\\), a larger constant means a higher pressure is needed to hold a given concentration in solution \u2014 the same physical information, expressed as a reciprocal number.<\/p>\n<p>The constant is reported in many different forms because different fields measure different quantities. Environmental and aquatic-chemistry tables often use mol\/(L\u00b7atm); engineering references often use atm\u00b7m\u00b3\/mol; geochemistry and physical-chemistry compilations frequently use pressure per mole fraction, atm\/mol fraction or Pa\/mol fraction; gas-solubility tables may quote a dimensionless ratio in cm\u00b3 of gas per cm\u00b3 of liquid. The numbers differ by orders of magnitude even for the same gas at the same temperature, so a converter is essential when comparing values from different sources.<\/p>\n<p>The mole-fraction forms used here assume a dilute solution in water, where the mole fraction of dissolved gas is \\(x \\approx c\/55.5\\). The default example above illustrates the scale: 0.034 mol\/(L\u00b7atm) for CO\u2082 becomes about 1,632 atm\/mol fraction. If you also need to work with the pressure side of the equation in other units, the <a href=\"https:\/\/wpcalc.com\/en\/converters\/pressure\/\">Pressure converter<\/a> handles atm, Pa, bar and related units. For gas-phase properties that depend on conditions, the <a href=\"https:\/\/wpcalc.com\/en\/converters\/air-density-calculator\/\">Air Density calculator<\/a> can supply the density that appears alongside Henry\u2019s law in mass-transfer problems.<\/p>\n<p>The table below shows how all seven supported units relate to one another, using the default value \\(k_{c\/p} = 0.034\\) mol\/(L\u00b7atm) at 298.15 K:<\/p>\n<table>\n<thead>\n<tr>\n<th>Unit<\/th>\n<th>Definition<\/th>\n<th>Value for 0.034 mol\/(L\u00b7atm)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>mol\/(L\u00b7atm)<\/td>\n<td>concentration per pressure (base form)<\/td>\n<td>0.034<\/td>\n<\/tr>\n<tr>\n<td>atm\u00b7L\/mol<\/td>\n<td>pressure per concentration, \\(1\/k_{c\/p}\\)<\/td>\n<td>29.41176<\/td>\n<\/tr>\n<tr>\n<td>mol\/(m\u00b3\u00b7Pa)<\/td>\n<td>SI concentration per pressure<\/td>\n<td>0.000335553<\/td>\n<\/tr>\n<tr>\n<td>atm\/mol fraction<\/td>\n<td>pressure per dissolved mole fraction<\/td>\n<td>1632.353<\/td>\n<\/tr>\n<tr>\n<td>Pa\/mol fraction<\/td>\n<td>pressure per dissolved mole fraction (SI)<\/td>\n<td>\\(1.654\\times10^{8}\\)<\/td>\n<\/tr>\n<tr>\n<td>atm\u00b7m\u00b3\/mol<\/td>\n<td>pressure per concentration, volume in m\u00b3<\/td>\n<td>0.02941176<\/td>\n<\/tr>\n<tr>\n<td>cm\u00b3\/cm\u00b3<\/td>\n<td>gas volume per liquid volume, at 298.15 K<\/td>\n<td>1.202<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2>Assumptions and limitations<\/h2>\n<ul>\n<li><strong>Dilute aqueous solution.<\/strong> The mole-fraction and cm\u00b3\/cm\u00b3 conversions use \\(C_w = 55.5\\) mol\/L, the molar concentration of pure water, and \\(x \\approx c\/C_w\\). This is only valid for sparingly soluble gases in water. For other solvents, or concentrated solutions, use the solvent\u2019s actual molar concentration instead.<\/li>\n<li><strong>Reciprocal definitions.<\/strong> mol\/(L\u00b7atm) and atm\u00b7L\/mol are reciprocals, not equivalent units: 0.034 mol\/(L\u00b7atm) is 29.412 atm\u00b7L\/mol, not 0.034. Likewise atm\u00b7m\u00b3\/mol is the m\u00b3-based reciprocal, smaller by a factor of 1,000.<\/li>\n<li><strong>Temperature dependence.<\/strong> Henry\u2019s law constants change strongly with temperature (gases are generally less soluble at higher temperature). The temperature field affects only the cm\u00b3\/cm\u00b3 result; a constant quoted at one temperature is not valid at another.<\/li>\n<li><strong>Ideal-gas behavior.<\/strong> The cm\u00b3\/cm\u00b3 form assumes the dissolved-gas volume follows \\(pV = nRT\\) with the gas constant in atm\u00b7m\u00b3\/(mol\u00b7K), which is accurate at low pressures but degrades at high pressure.<\/li>\n<li><strong>Linearity range.<\/strong> Henry\u2019s law itself holds only at low partial pressures and low concentrations. At high pressures, chemical reactions of the gas with the liquid (for example CO\u2082 forming carbonic acid) can make the simple proportionality invalid.<\/li>\n<li><strong>Check the source convention.<\/strong> Published compilations use overlapping symbols (\\(k_H\\), \\(H\\), \\(K_H\\)) for different definitions. Always confirm the units attached to a value before entering it, and verify a converted value against the source\u2019s stated convention when accuracy matters.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Convert a Henry\u2019s law constant between mol\/(L\u00b7atm), atm\u00b7L\/mol, mol\/(m\u00b3\u00b7Pa), mole-fraction forms, atm\u00b7m\u00b3\/mol and cm\u00b3\/cm\u00b3. Enter the value, pick the From and To units, and add a temperature when cm\u00b3\/cm\u00b3 is involved.<\/p>\n","protected":false},"author":70,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[3],"tags":[34],"class_list":["post-55836","post","type-post","status-publish","format-standard","hentry","category-converters","tag-physics-units"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/55836","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\/70"}],"replies":[{"embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/comments?post=55836"}],"version-history":[{"count":3,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/55836\/revisions"}],"predecessor-version":[{"id":67114,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/55836\/revisions\/67114"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=55836"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=55836"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=55836"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}