{"id":66530,"date":"2026-10-15T09:20:33","date_gmt":"2026-10-15T06:20:33","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66530"},"modified":"2026-10-15T09:20:33","modified_gmt":"2026-10-15T06:20:33","slug":"henrys-law-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/henrys-law-calculator\/","title":{"rendered":"Henry's 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\">Find How Much Gas Dissolves at a Given Partial Pressure<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66530\" data-favorite-title=\"Henry&#039;s Law\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/henrys-law-calculator\/\" data-favorite-excerpt=\"Calculate how much gas dissolves in a liquid at a given partial pressure using Henry&#039;s law. Enter the pressure and Henry&#039;s law constant to get the dissolved concentration, or solve for the pressure instead.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-wind-2\">\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\/henrys-law-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66530\" data-post=\"66530\"><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\">Solve for<\/label><div class=\"grid grid-cols-1\"><select id=\"field-1\" name=\"solve_for\"><option value=\"C\" selected>Dissolved gas concentration (C)<\/option><option value=\"P\">Gas partial pressure (P)<\/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\">Partial pressure (P)<\/label><div class=\"term\">P<\/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=\"partial_pressure_p\" id=\"field-2\" aria-describedby=\"calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 1\" min=\"0\" value=\"1\"\/><div class=\"grid grid-cols-1\"><select id=\"field-3\" name=\"unit\" aria-label=\"Unit\"><option value=\"atm\" selected>atm<\/option><option value=\"bar\">bar<\/option><option value=\"kPa\">kPa<\/option><option value=\"mmHg\">mmHg<\/option><option value=\"Pa\">Pa<\/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-2\">Partial pressure of the gas above (or in contact with) the liquid<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-4\">Henry&#039;s law constant (k\u029c)<\/label><div class=\"term\">k\u029c<\/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=\"henrys_law_constant_k\" id=\"field-4\" aria-describedby=\"calc-info-4\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.033\" min=\"0\" value=\"0.033\"\/><div class=\"grid grid-cols-1\"><select id=\"field-5\" name=\"unit\" aria-label=\"Unit\"><option value=\"M_atm\" selected>mol\/(L\u00b7atm)<\/option><option value=\"M_bar\">mol\/(L\u00b7bar)<\/option><option value=\"M_kPa\">mol\/(L\u00b7kPa)<\/option><option value=\"mM_atm\">mmol\/(L\u00b7atm)<\/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\">Solubility form: k\u029c = C \/ P, e.g. CO\u2082 0.033, O\u2082 0.0013, N\u2082 0.00061 mol\/(L\u00b7atm) at 25 \u00b0C<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-6\">Dissolved concentration (C)<\/label><div class=\"term\">C<\/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=\"dissolved_concentration_c\" id=\"field-6\" aria-describedby=\"calc-info-6\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.033\" min=\"0\" value=\"0.033\"\/><div class=\"grid grid-cols-1\"><select id=\"field-7\" 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-6\">Concentration of the dissolved gas at equilibrium<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66530\">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> Henry&#039;s Law Results<\/h3><div class=\"result-box\"><div class=\"field-result is-column\" id=\"output-1\"><span class=\"field-title\"><span>Solution<\/span><span class=\"result-term\">\u2192<\/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>Dissolved Concentration<\/span><span class=\"result-term\">C<\/span><\/span><span class=\"field-value\" id=\"result-2\" data-unit=\"mol\/L\"><\/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>Partial Pressure<\/span><span class=\"result-term\">P<\/span><\/span><span class=\"field-value\" id=\"result-3\" data-unit=\"atm\"><\/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=\"66530\" 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>Henry's 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_H \\cdot P \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(C\\) \u2014 concentration of the dissolved gas at equilibrium (mol\/L)<\/li>\n<li>\\(k_H\\) \u2014 Henry's law constant in the solubility form (mol\/(L\u00b7atm))<\/li>\n<li>\\(P\\) \u2014 partial pressure of the gas above the liquid (atm)<\/li>\n<\/ul>\n<p>This is the solubility form of Henry's law: the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of that gas in contact with the liquid. The inverse relation, \\(P = C \/ k_H\\), gives the pressure needed to reach a target concentration.<\/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's Law \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> carbon dioxide gas is in contact with water at 25 \u00b0C, where \\(k_H = 0.033\\) mol\/(L\u00b7atm), at a partial pressure of 1 atm. How much CO\u2082 dissolves?<\/p>\n<p>\\[ C = k_H \\cdot P = 0.033 \\ \\text{mol\/(L\u00b7atm)} \\times 1 \\ \\text{atm} = 0.033 \\ \\text{mol\/L} \\]<\/p>\n<p><strong>Result:<\/strong> the water holds 0.033 mol\/L of dissolved CO\u2082 (33 mmol\/L) at equilibrium.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to use the calculator<\/h2>\n<ol>\n<li>Open the <strong>Solve for<\/strong> dropdown and choose whether you want the <strong>Dissolved gas concentration (C)<\/strong> or the <strong>Gas partial pressure (P)<\/strong>.<\/li>\n<li>Enter the <strong>Partial pressure (P)<\/strong> and pick its unit (atm, bar, kPa, mmHg or Pa) \u2014 this is the value used when solving for concentration.<\/li>\n<li>Enter the <strong>Henry's law constant (k\u029c)<\/strong> in the solubility form \\(C\/P\\) and select its unit. For CO\u2082 at 25 \u00b0C use 0.033 mol\/(L\u00b7atm); for O\u2082 use 0.0013 mol\/(L\u00b7atm).<\/li>\n<li>If you are solving for pressure, enter the <strong>Dissolved concentration (C)<\/strong> and its unit (mol\/L, mmol\/L or \u00b5mol\/L) instead.<\/li>\n<li>Read the result: the main answer appears in your chosen units, with the dissolved concentration in mol\/L and the partial pressure in atm shown alongside the full calculation steps.<\/li>\n<\/ol>\n<h2>What Henry's law describes<\/h2>\n<p>Henry's law states that at a constant temperature, the concentration of a gas dissolved in a liquid is directly proportional to the partial pressure of that gas above the liquid. Doubling the partial pressure doubles the amount of gas that dissolves. The relationship only holds for gases that do not react with or dissociate in the solvent \u2014 the dissolved molecules must stay in their molecular form.<\/p>\n<p>The proportionality constant \\(k_H\\) is specific to each gas\u2013solvent pair and changes strongly with temperature: cold water holds noticeably more dissolved gas than warm water, which is why warm soda goes flat faster and fish prefer cool, oxygen-rich water. Typical \\(k_H\\) values in water at 25 \u00b0C range from about 0.00037 mol\/(L\u00b7atm) for helium (barely soluble) to 0.033 mol\/(L\u00b7atm) for CO\u2082 (highly soluble) and far higher for reactive gases such as ammonia.<\/p>\n<p>Interpreting the result: the calculated \\(C\\) is the equilibrium concentration \u2014 the level the dissolved gas eventually reaches if you wait long enough. If the liquid currently holds less gas than this, gas will keep dissolving; if it holds more, gas will bubble out until equilibrium is restored. This is the physics behind carbonated drinks (bottled under high CO\u2082 pressure), decompression sickness in divers, and the oxygen balance in lakes and aquariums. For temperature effects on equilibrium in general, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-t-hoff-equation-calculator\/\">Van 't Hoff equation calculator<\/a>.<\/p>\n<h2>Reference values of Henry's law constant at 25 \u00b0C<\/h2>\n<table>\n<thead>\n<tr>\n<th>Gas<\/th>\n<th>\\(k_H\\) in mol\/(L\u00b7atm)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Helium (He)<\/td>\n<td>0.00037<\/td>\n<\/tr>\n<tr>\n<td>Nitrogen (N\u2082)<\/td>\n<td>0.00061<\/td>\n<\/tr>\n<tr>\n<td>Hydrogen (H\u2082)<\/td>\n<td>0.00078<\/td>\n<\/tr>\n<tr>\n<td>Oxygen (O\u2082)<\/td>\n<td>0.0013<\/td>\n<\/tr>\n<tr>\n<td>Argon (Ar)<\/td>\n<td>0.0014<\/td>\n<\/tr>\n<tr>\n<td>Methane (CH\u2084)<\/td>\n<td>0.0014<\/td>\n<\/tr>\n<tr>\n<td>Carbon dioxide (CO\u2082)<\/td>\n<td>0.033<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>These constants apply to pure water at 25 \u00b0C. Values in other sources may differ slightly because of different measurement methods and temperature scales.<\/p>\n<h2>Assumptions, limitations and practical tips<\/h2>\n<ul>\n<li><strong>Watch out for the two conventions.<\/strong> This calculator uses the solubility form \\(k_H = C\/P\\) with units of mol\/(L\u00b7atm). Many textbooks and databases instead tabulate \\(k = P\/C\\) in L\u00b7atm\/mol \u2014 the exact reciprocal. If your constant is larger than about 1, you probably have the inverse form: take its reciprocal (1 \u00f7 value) before entering it.<\/li>\n<li><strong>Temperature must match.<\/strong> \\(k_H\\) increases as temperature drops, so a constant quoted at 25 \u00b0C will be wrong at 5 \u00b0C. Always check the temperature your \\(k_H\\) value refers to.<\/li>\n<li><strong>Reactive gases break the rule.<\/strong> Gases that chemically react with water \u2014 CO\u2082 forming carbonic acid, NH\u2083, SO\u2082, HCl \u2014 dissolve far more than Henry's law predicts for the molecular form alone, because the reaction removes dissolved molecules and pulls more gas into solution.<\/li>\n<li><strong>Dilute solutions and low pressures only.<\/strong> At very high pressures or high dissolved concentrations, deviations from proportionality appear and the simple law becomes inaccurate.<\/li>\n<li><strong>Use partial pressure, not total pressure.<\/strong> For air, the oxygen concentration is governed by the partial pressure of O\u2082 (about 0.21 atm in dry air), not by the 1 atm total. To compare how different gases distribute between phases, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/partition-coefficient-calculator\/\">partition coefficient calculator<\/a>.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Calculate how much gas dissolves in a liquid at a given partial pressure using Henry's law. Enter the pressure and Henry's law constant to get the dissolved concentration, or solve for the pressure instead.<\/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":[55],"class_list":["post-66530","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-gases"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66530","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=66530"}],"version-history":[{"count":1,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66530\/revisions"}],"predecessor-version":[{"id":67039,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66530\/revisions\/67039"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66530"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66530"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66530"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}