{"id":59575,"date":"2016-12-28T10:15:46","date_gmt":"2016-12-28T08:15:46","guid":{"rendered":"http:\/\/wpcalc.com\/?p=59575"},"modified":"2026-09-29T14:57:52","modified_gmt":"2026-09-29T11:57:52","slug":"daltons-law","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/daltons-law\/","title":{"rendered":"Dalton\u2019s 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\">Solve Dalton&#039;s Law Problems<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"59575\" data-favorite-title=\"Dalton\u2019s Law\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/daltons-law\/\" data-favorite-excerpt=\"Enter the moles of each gas, the temperature in kelvin, and the volume in liters to calculate mixture pressure. A unit-conversion error currently makes the displayed result 1,000 times too low.\" 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\/daltons-law\/\" method=\"POST\" class=\"calculator\" id=\"calculator-59575\" data-post=\"59575\"><fieldset class=\"fieldset-input is-1\"><legend class=\"sr-only\">Input Fields<\/legend><div class=\"field\" id=\"input-1\"><label for=\"field-1\">Moles of Gases (n\u2081, n\u2082, ...)<\/label><input type=\"text\" name=\"moles_of_gases_n_n_\" id=\"field-1\" aria-describedby=\"calc-info-1\" placeholder=\"e.g. 2.5,1.2,3.1\" step=\"any\" value=\"2.5,1.2,3.1\"\/><small id=\"calc-info-1\">Enter comma-separated values for moles of gases<\/small><\/div><div class=\"field\" id=\"input-2\"><label for=\"field-2\">Temperature (T)<\/label><input type=\"number\" name=\"temperature_t\" id=\"field-2\" aria-describedby=\"calc-unit-2\" placeholder=\"e.g. 298\" step=\"any\" value=\"298\"\/><div class=\"unit\" id=\"calc-unit-2\">K<\/div><\/div><div class=\"field\" id=\"input-3\"><label for=\"field-3\">Volume (V)<\/label><input type=\"number\" name=\"volume_v\" id=\"field-3\" aria-describedby=\"calc-unit-3\" placeholder=\"e.g. 10\" step=\"any\" value=\"10\"\/><div class=\"unit\" id=\"calc-unit-3\">L<\/div><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"59575\">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>Total Pressure (P)<\/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=\"59575\" 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>Dalton\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\\[P_{\\mathrm{total}}=\\sum_i p_i=\\frac{\\left(\\sum_i n_i\\right)RT}{V}\\\\P_{\\mathrm{shown}}=\\frac{\\left(\\sum_i n_i\\right)(8.314)T}{1000V}\\ \\mathrm{kPa}=\\frac{P_{\\mathrm{total}}}{1000}\\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(P_{\\mathrm{total}}\\) \u2014 total pressure of the gas mixture (kPa)<\/li>\n<li>\\(p_i\\) \u2014 partial pressure of gas \\(i\\) (kPa)<\/li>\n<li>\\(n_i\\) \u2014 amount of gas \\(i\\) (mol)<\/li>\n<li>\\(R\\) \u2014 ideal gas constant, approximately \\(8.314\\ \\mathrm{kPa\\cdot L\/(mol\\cdot K)}\\)<\/li>\n<li>\\(T\\) \u2014 absolute temperature (K)<\/li>\n<li>\\(V\\) \u2014 volume of the mixture (L)<\/li>\n<li>\\(P_{\\mathrm{shown}}\\) \u2014 value currently displayed by this calculator (kPa)<\/li>\n<\/ul>\n<p>Dalton\u2019s law adds the partial pressures of the gases. For an ideal gas mixture, total pressure also follows from the sum of their moles. The calculator divides that pressure by 1,000 unnecessarily, so its displayed value is 1,000 times too low.<\/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>Dalton\u2019s Law \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> The default entries describe three gases with 2.5, 1.2, and 3.1 mol in a 10 L container at 298 K.<\/p>\n<p>\\[n_{\\mathrm{total}}=2.5+1.2+3.1=6.8\\ \\mathrm{mol}\\]<\/p>\n<p>\\[P_{\\mathrm{total}}=\\frac{(6.8)(8.314)(298)}{10}=1684.74896\\ \\mathrm{kPa}\\]<\/p>\n<p>\\[P_{\\mathrm{shown}}=\\frac{1684.74896}{1000}=1.68474896\\ \\mathrm{kPa}\\]<\/p>\n<p><strong>Result:<\/strong> The calculator displays 1.6847 kPa. The ideal-gas pressure for these inputs is 1684.7490 kPa.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to use the calculator<\/h2>\n<ol>\n<li>In <strong>Moles of Gases (n\u2081, n\u2082, ...)<\/strong>, enter the amount of each gas in moles, separated by commas. For example, enter <code>2.5,1.2,3.1<\/code> for three gases.<\/li>\n<li>In <strong>Temperature (T)<\/strong>, enter the mixture\u2019s absolute temperature in kelvin. Convert from Celsius by adding 273.15.<\/li>\n<li>In <strong>Volume (V)<\/strong>, enter the volume occupied by the mixture in liters. All the gases must occupy this same volume.<\/li>\n<li>Read <strong>Total Pressure (P)<\/strong> in kPa. <strong>Multiply the displayed number by 1,000<\/strong> to obtain the ideal-gas pressure implied by your entries. This correction is necessary because of the calculator\u2019s current unit-conversion error.<\/li>\n<\/ol>\n<h2>What Dalton\u2019s law tells you<\/h2>\n<p>Dalton\u2019s law of partial pressures states that the pressure of an ideal gas mixture equals the sum of the pressures its components would each exert alone at the mixture\u2019s temperature and volume. Each component\u2019s contribution is its <em>partial pressure<\/em>. If a mixture has three gases, its total pressure is \\(p_1+p_2+p_3\\).<\/p>\n<p>For an ideal mixture, a component\u2019s partial pressure is \\(p_i=n_iRT\/V\\). Adding these contributions gives \\(P_{\\mathrm{total}}=(\\sum_i n_i)RT\/V\\): total pressure depends on the total amount of gas, temperature, and volume. At fixed temperature and volume, adding more moles raises the pressure, regardless of which ideal gas is added.<\/p>\n<p>The share of pressure due to one gas is its mole fraction times the total pressure: \\(p_i=(n_i\/n_{\\mathrm{total}})P_{\\mathrm{total}}\\). This relationship can help interpret a mixture even though this calculator reports only a total, not separate partial pressures. For other calculations using moles, temperature, volume, and pressure, see the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/ideal-gas-law\/\">Ideal Gas Law calculator<\/a>.<\/p>\n<h2>Assumptions and practical limits<\/h2>\n<p>The calculation assumes the gases behave ideally, are thoroughly mixed, and share one temperature and volume. Real gases can depart from ideal behavior, especially at high pressures or low temperatures. A gas that reacts, condenses, or dissolves may no longer contribute pressure according to the amount originally entered.<\/p>\n<p>Enter positive temperature and volume values and enough valid mole entries to give a positive total. The calculator skips comma-separated entries it cannot read as numbers; check your list carefully rather than assuming every entry was included. It does not accept partial pressures as inputs, despite what a general description of Dalton\u2019s law might suggest.<\/p>\n<p><strong>Unit caution:<\/strong> Using \\(R=8.314\\ \\mathrm{kPa\\cdot L\/(mol\\cdot K)}\\) with liters gives pressure directly in kPa. The calculator then divides by 1,000, causing the error noted above. Do not use its displayed number as a physical pressure without correcting it. If you are comparing how pressure changes with temperature or volume, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/combined-gas-law\/\">Combined Gas Law calculator<\/a> and <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/boyles-law\/\">Boyle\u2019s Law calculator<\/a> cover those relationships.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Enter the moles of each gas, the temperature in kelvin, and the volume in liters to calculate mixture pressure. A unit-conversion error currently makes the displayed result 1,000 times too low.<\/p>\n","protected":false},"author":70,"featured_media":0,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":""},"categories":[54],"tags":[55],"class_list":["post-59575","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\/59575","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=59575"}],"version-history":[{"count":4,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/59575\/revisions"}],"predecessor-version":[{"id":65580,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/59575\/revisions\/65580"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=59575"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=59575"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=59575"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}