{"id":66531,"date":"2026-10-07T08:28:56","date_gmt":"2026-10-07T05:28:56","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66531"},"modified":"2026-10-13T12:13:28","modified_gmt":"2026-10-13T09:13:28","slug":"raoults-law-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/raoults-law-calculator\/","title":{"rendered":"Raoult'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\">Vapor Pressure of an Ideal Liquid Mixture<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66531\" data-favorite-title=\"Raoult&#039;s Law\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/raoults-law-calculator\/\" data-favorite-excerpt=\"Calculate the total vapor pressure and vapor-phase composition of an ideal two-component liquid mixture using Raoult&#039;s law. Enter the mole fractions and the pure vapor pressures of both components.\" aria-label=\"Add to Favorites\" data-favorite-icon=\"icon icon-chemistry\">\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\/raoults-law-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66531\" data-post=\"66531\"><fieldset class=\"fieldset-input is-2\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field has-term\" id=\"input-1\"><label for=\"field-1\">Mole fraction of component 1<\/label><div class=\"term\">x\u2081<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"mole_fraction_of_component_1\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.4\" min=\"0\" max=\"1\" value=\"0.4\"\/><small id=\"calc-info-1\">Fraction of the liquid mixture that is component 1 (benzene in the default example)<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-2\">Mole fraction of component 2<\/label><div class=\"term\">x\u2082<\/div>  <div class=\"absolute bottom-0 left-16 top-8 w-2 h-0.5 bg-blue-500\"><\/div><input type=\"text\" name=\"mole_fraction_of_component_2\" id=\"field-2\" aria-describedby=\"calc-info-2\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 0.6\" min=\"0\" max=\"1\" value=\"0.6\"\/><small id=\"calc-info-2\">x\u2081 + x\u2082 must equal 1<\/small><\/div><div class=\"field has-term\" id=\"input-3\"><label for=\"field-3\">Pure vapor pressure of component 1<\/label><div class=\"term\">P\u2081\u00b0<\/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=\"pure_vapor_pressure_of_component_1\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 95.1\" min=\"0\" value=\"95.1\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"mmHg\" selected>mmHg<\/option><option value=\"kPa\">kPa<\/option><option value=\"atm\">atm<\/option><option value=\"bar\">bar<\/option><option value=\"psi\">psi<\/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\">Vapor pressure of pure component 1 at the mixture temperature (benzene at 25 \u00b0C)<\/small><\/div><div class=\"field has-term\" id=\"input-4\"><label for=\"field-5\">Pure vapor pressure of component 2<\/label><div class=\"term\">P\u2082\u00b0<\/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=\"pure_vapor_pressure_of_component_2\" id=\"field-5\" aria-describedby=\"calc-info-5\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 28.4\" min=\"0\" value=\"28.4\"\/><div class=\"grid grid-cols-1\"><select id=\"field-6\" name=\"unit\" aria-label=\"Unit\"><option value=\"mmHg\" selected>mmHg<\/option><option value=\"kPa\">kPa<\/option><option value=\"atm\">atm<\/option><option value=\"bar\">bar<\/option><option value=\"psi\">psi<\/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-5\">Vapor pressure of pure component 2 at the same temperature (toluene at 25 \u00b0C)<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66531\">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> Raoult&#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 is-column\" id=\"output-2\"><span class=\"field-title\"><span>Partial Pressure of Component 1<\/span><span class=\"result-term\">p\u2081<\/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>Partial Pressure of Component 2<\/span><span class=\"result-term\">p\u2082<\/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>Total Vapor Pressure<\/span><span class=\"result-term\">P<\/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\" id=\"output-5\"><span class=\"field-title\"><span>Vapor Composition of Component 1<\/span><span class=\"result-term\">y\u2081<\/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 class=\"field-result\" id=\"output-6\"><span class=\"field-title\"><span>Vapor Composition of Component 2<\/span><span class=\"result-term\">y\u2082<\/span><\/span><span class=\"field-value\" id=\"result-6\"><\/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-7\"><span class=\"field-title\"><span>Calculation Details<\/span><\/span><span class=\"field-value\" id=\"result-7\"><\/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=\"66531\" 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>Raoult'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\\[ p_1 = x_1 P_1\\degree, \\quad p_2 = x_2 P_2\\degree, \\quad P = p_1 + p_2 = x_1 P_1\\degree + x_2 P_2\\degree \\\\\\ y_1 = \\frac{p_1}{P}, \\quad y_2 = \\frac{p_2}{P} \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(p_1\\), \\(p_2\\) \u2014 partial vapor pressures of components 1 and 2 above the mixture<\/li>\n<li>\\(x_1\\), \\(x_2\\) \u2014 mole fractions of the components in the <em>liquid<\/em> phase (\\(x_1 + x_2 = 1\\))<\/li>\n<li>\\(P_1\\degree\\), \\(P_2\\degree\\) \u2014 vapor pressures of the pure components at the mixture temperature<\/li>\n<li>\\(P\\) \u2014 total vapor pressure above the solution<\/li>\n<li>\\(y_1\\), \\(y_2\\) \u2014 mole fractions of the components in the <em>vapor<\/em> phase<\/li>\n<\/ul>\n<p>Raoult's law states that each component's partial pressure equals its mole fraction in the liquid multiplied by the vapor pressure of the pure component at the same temperature. The total pressure is the sum of the partial pressures, and the vapor composition follows from Dalton's law.<\/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>Raoult's Law \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> a liquid mixture of benzene and toluene at 25 \u00b0C contains 40 mol% benzene and 60 mol% toluene. At 25 \u00b0C, pure benzene has a vapor pressure of 95.1 mmHg and pure toluene 28.4 mmHg. Find the total vapor pressure and the composition of the vapor.<\/p>\n<p>\\[ p_{\\text{benzene}} = x_1 P_1\\degree = 0.4 \\times 95.1 = 38.04 \\text{ mmHg} \\\\ p_{\\text{toluene}} = x_2 P_2\\degree = 0.6 \\times 28.4 = 17.04 \\text{ mmHg} \\\\ P = 38.04 + 17.04 = 55.08 \\text{ mmHg} \\\\ y_1 = \\frac{38.04}{55.08} = 0.6905, \\quad y_2 = 0.3095 \\<\/p>\n<p><strong>Result:<\/strong> the total vapor pressure is <strong>55.08 mmHg<\/strong> (7.34 kPa), and the vapor contains <strong>69.05 mol% benzene<\/strong> and <strong>30.95 mol% toluene<\/strong>. The vapor is richer in benzene than the liquid (40 mol%) because benzene is the more volatile component.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Mole fraction of component 1<\/strong> (\\(x_1\\)) as a number between 0 and 1. In the default example this is benzene with \\(x_1 = 0.4\\).<\/li>\n<li>Enter the <strong>Mole fraction of component 2<\/strong> (\\(x_2\\)). The two fractions must sum to 1; if you enter 0.4 for component 1, use 0.6 here.<\/li>\n<li>Enter the <strong>Pure vapor pressure of component 1<\/strong> (\\(P_1\\degree\\)) and pick its unit (mmHg, kPa, atm, bar, or psi) from the dropdown.<\/li>\n<li>Enter the <strong>Pure vapor pressure of component 2<\/strong> (\\(P_2\\degree\\)) at the <em>same temperature<\/em>, with its own unit selection.<\/li>\n<li>Read the results: the partial pressures \\(p_1\\) and \\(p_2\\), the total vapor pressure \\(P\\) (also converted to other units), and the vapor-phase mole fractions \\(y_1\\) and \\(y_2\\). The calculation details show every step.<\/li>\n<\/ol>\n<h2>What Is Raoult's Law?<\/h2>\n<p>Raoult's law, formulated by French chemist Fran\u00e7ois-Marie Raoult in 1887, describes the vapor pressure of an ideal solution. When two liquids mix to form an ideal solution, the presence of the other component dilutes each one, lowering its partial vapor pressure in direct proportion to its mole fraction in the liquid. This happens because fewer molecules of each component sit at the surface of the liquid, so fewer escape into the vapor phase per unit time.<\/p>\n<p>The law is the foundation of much of vapor\u2013liquid equilibrium chemistry. It explains why adding a solute lowers the vapor pressure of a solvent \u2014 the basis of <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/boiling-point-elevation-calculator\/\">boiling point elevation<\/a> and <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/freezing-point-depression-calculator\/\">freezing point depression<\/a> \u2014 and it underlies the design of distillation columns, where mixtures are separated by repeatedly vaporizing and condensing them.<\/p>\n<p>A key insight from the results is the difference between liquid and vapor composition. The vapor above a mixture is always richer in the <strong>more volatile<\/strong> component (the one with the higher pure vapor pressure). In the benzene\u2013toluene example, the liquid is 40% benzene but the vapor is about 69% benzene. This enrichment is exactly what makes distillation work: each vaporization step concentrates the more volatile component further.<\/p>\n<p>Note that the pure vapor pressures themselves depend strongly on temperature. If your mixture is not at 25 \u00b0C, look up (or estimate with the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/clausius-clapeyron-calculator\/\">Clausius\u2013Clapeyron equation<\/a>) the vapor pressures of each pure component at your actual temperature before using this calculator.<\/p>\n<h2>Assumptions, Limitations and Tips<\/h2>\n<ul>\n<li><strong>Ideal solution:<\/strong> Raoult's law assumes the two components interact with each other exactly as strongly as with themselves. It works best for chemically similar liquids, such as benzene\/toluene, hexane\/heptane, or close isomers.<\/li>\n<li><strong>Positive deviation:<\/strong> if unlike molecules attract each other <em>less<\/em> than like molecules (e.g. ethanol\/water), the actual total pressure is <em>higher<\/em> than Raoult's law predicts, and the mixture may form a minimum-boiling azeotrope.<\/li>\n<li><strong>Negative deviation:<\/strong> if unlike molecules attract each other <em>more<\/em> strongly (e.g. acetone\/chloroform), the actual pressure is <em>lower<\/em> than predicted, possibly giving a maximum-boiling azeotrope.<\/li>\n<li><strong>Same temperature:<\/strong> both pure vapor pressures must be taken at the temperature of the mixture. Mixing values measured at different temperatures gives meaningless results.<\/li>\n<li><strong>Nonvolatile solutes:<\/strong> if component 2 is nonvolatile (\\(P_2\\degree \\approx 0\\)), the total pressure reduces to \\(P = x_1 P_1\\degree\\) \u2014 the dilution form used in colligative property calculations.<\/li>\n<li><strong>Extension to multicomponent mixtures:<\/strong> for more than two components, simply sum \\(x_i P_i\\degree\\) over all of them; the two-component form here is the most common case.<\/li>\n<\/ul>\n<p>For related equilibrium calculations, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/partition-coefficient-calculator\/\">partition coefficient calculator<\/a> or the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/equilibrium-constant-calculator\/\">equilibrium constant calculator<\/a>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the total vapor pressure and vapor-phase composition of an ideal two-component liquid mixture using Raoult's law. Enter the mole fractions and the pure vapor pressures of both components.<\/p>\n","protected":false},"author":3168,"featured_media":0,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[56],"class_list":["post-66531","post","type-post","status-publish","format-standard","hentry","category-chemistry","tag-stoichiometry"],"acf":[],"_links":{"self":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66531","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=66531"}],"version-history":[{"count":3,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66531\/revisions"}],"predecessor-version":[{"id":67109,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66531\/revisions\/67109"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66531"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66531"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66531"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}