{"id":66881,"date":"2026-10-13T10:05:23","date_gmt":"2026-10-13T07:05:23","guid":{"rendered":"https:\/\/wpcalc.com\/en\/?p=66881"},"modified":"2026-10-13T11:59:44","modified_gmt":"2026-10-13T08:59:44","slug":"molecular-speed-of-a-gas-calculator","status":"publish","type":"post","link":"https:\/\/wpcalc.com\/en\/chemistry\/molecular-speed-of-a-gas-calculator\/","title":{"rendered":"Molecular Speed of a Gas 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\">Molecular Speeds from Temperature and Molar Mass<\/h2><\/div><div class=\"calcdash-favorite group\">\n  <button type=\"button\" class=\"favorite\" id=\"favorite\" data-favorite-id=\"66881\" data-favorite-title=\"Molecular Speed of a Gas\" data-favorite-url=\"https:\/\/wpcalc.com\/en\/chemistry\/molecular-speed-of-a-gas-calculator\/\" data-favorite-excerpt=\"Calculate the root-mean-square, mean, and most probable speeds of gas molecules from the temperature and molar mass, plus the average translational energy per mole, using kinetic theory formulas.\" 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\/molecular-speed-of-a-gas-calculator\/\" method=\"POST\" class=\"calculator\" id=\"calculator-66881\" data-post=\"66881\"><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\">Absolute Temperature (T)<\/label><div class=\"term\">T<\/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=\"absolute_temperature_t\" id=\"field-1\" aria-describedby=\"calc-info-1\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 300\" min=\"0\" value=\"300\"\/><div class=\"grid grid-cols-1\"><select id=\"field-2\" name=\"unit\" aria-label=\"Unit\"><option value=\"K\" selected>K<\/option><option value=\"degC\">\u00b0C<\/option><option value=\"degF\">\u00b0F<\/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-1\">Temperature of the gas. Use kelvin for a true absolute temperature; \u00b0C and \u00b0F are converted automatically.<\/small><\/div><div class=\"field has-term\" id=\"input-2\"><label for=\"field-3\">Molar Mass (M)<\/label><div class=\"term\">M<\/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=\"molar_mass_m\" id=\"field-3\" aria-describedby=\"calc-info-3\" data-number inputmode=\"decimal\" autocomplete=\"off\" spellcheck=\"false\" placeholder=\"e.g. 32\" min=\"0\" value=\"32\"\/><div class=\"grid grid-cols-1\"><select id=\"field-4\" name=\"unit\" aria-label=\"Unit\"><option value=\"g_mol\" selected>g\/mol<\/option><option value=\"kg_mol\">kg\/mol<\/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\">Mass of one mole of the gas molecules, e.g. 2 for H\u2082, 28.97 for air, 32 for O\u2082, 44 for CO\u2082.<\/small><\/div><\/fieldset><div class=\"buttons\"><button type=\"submit\" data-text=\"Re-Calculate\" id=\"calculate-button\" data-post=\"66881\">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> Molecular Speeds (Kinetic Theory)<\/h3><div class=\"result-box\"><div class=\"field-result\" id=\"output-1\"><span class=\"field-title\"><span>Root-Mean-Square Speed<\/span><span class=\"result-term\">v_rms<\/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>Mean (Average) Speed<\/span><span class=\"result-term\">v\u0304<\/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\" id=\"output-3\"><span class=\"field-title\"><span>Most Probable Speed<\/span><span class=\"result-term\">v_p<\/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\" id=\"output-4\"><span class=\"field-title\"><span>Average Translational Energy per Mole<\/span><span class=\"result-term\">E\/mol<\/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>Calculation Details<\/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 is-column\" id=\"output-6\"><span class=\"field-title\"><span>About the Kinetic Theory of Gases<\/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><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=\"66881\" 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>Molecular Speed of a Gas 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\\[ v_{rms} = \\sqrt{\\frac{3RT}{M}} \\qquad \\bar{v} = \\sqrt{\\frac{8RT}{\\pi M}} \\qquad v_p = \\sqrt{\\frac{2RT}{M}} \\qquad E_{mol} = \\frac{3}{2}RT \\]\n<\/div>\r\n\t<\/figure>\r\n\t<\/p>\n<p><strong>Where:<\/strong><\/p>\n<ul>\n<li>\\(v_{rms}\\) \u2014 root-mean-square speed (m\/s)<\/li>\n<li>\\(\\bar{v}\\) \u2014 mean (average) speed (m\/s)<\/li>\n<li>\\(v_p\\) \u2014 most probable speed (m\/s)<\/li>\n<li>\\(E_{mol}\\) \u2014 average translational kinetic energy per mole (J\/mol)<\/li>\n<li>\\(R\\) \u2014 universal gas constant, \\(8.314\\ \\mathrm{J\/(mol\\cdot K)}\\)<\/li>\n<li>\\(T\\) \u2014 absolute temperature (K)<\/li>\n<li>\\(M\\) \u2014 molar mass (kg\/mol)<\/li>\n<\/ul>\n<p>The three speeds come from the Maxwell\u2013Boltzmann distribution of an ideal gas: \\(v_p\\) is the peak of the distribution, \\(\\bar{v}\\) is the average over all molecules, and \\(v_{rms}\\) follows from the average translational kinetic energy \\(\\frac{3}{2}kT\\) per molecule. Note that \\(E_{mol}\\) depends only on temperature, not on the type of gas.<\/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>Molecular Speed of a Gas \u2013 Calculation Example<\/h2><\/div>\r\n\r\n<\/p>\n<p><strong>Example:<\/strong> oxygen gas (O\u2082, molar mass 32 g\/mol) at 300 K \u2014 exactly the default values of the calculator.<\/p>\n<p>\\[ v_{rms} = \\sqrt{\\frac{3 \\times 8.314 \\times 300}{0.032}} = \\sqrt{233844} \\approx 483.6\\ \\mathrm{m\/s} \\\\ \\bar{v} = \\sqrt{\\frac{8 \\times 8.314 \\times 300}{\\pi \\times 0.032}} \\approx 445.5\\ \\mathrm{m\/s} \\\\ v_p = \\sqrt{\\frac{2 \\times 8.314 \\times 300}{0.032}} \\approx 394.8\\ \\mathrm{m\/s} \\\\ E_{mol} = \\tfrac{3}{2} \\times 8.314 \\times 300 \\approx 3741.5\\ \\mathrm{J\/mol} \\\\ \\\\ ]<\/p>\n<p><strong>Result:<\/strong> \\(v_{rms} \\approx\\) 483.6 m\/s (about 1740.8 km\/h), \\(\\bar{v} \\approx\\) 445.5 m\/s, \\(v_p \\approx\\) 394.8 m\/s, and an average translational energy of about 3741.5 J\/mol \u2014 roughly 0.064 eV (64 meV) per molecule.<\/p>\n<p>\n\r\n<\/section>\n<h2>How to Use the Calculator<\/h2>\n<ol>\n<li>Enter the <strong>Absolute Temperature (T)<\/strong> and choose its unit: K, \u00b0C or \u00b0F. The value is converted to kelvin automatically.<\/li>\n<li>Enter the <strong>Molar Mass (M)<\/strong> of the gas and select g\/mol or kg\/mol. Common values: 2 for H\u2082, 28.97 for air, 32 for O\u2082, 44 for CO\u2082.<\/li>\n<li>Read the results: <strong>Root-Mean-Square Speed<\/strong>, <strong>Mean (Average) Speed<\/strong> and <strong>Most Probable Speed<\/strong> are shown in m\/s and km\/h, and the <strong>Average Translational Energy per Mole<\/strong> in J\/mol.<\/li>\n<li>The <strong>Calculation Details<\/strong> section shows the substituted numbers, and <strong>About the Kinetic Theory of Gases<\/strong> summarizes the assumptions behind the formulas.<\/li>\n<\/ol>\n<h2>What Molecular Speed Means<\/h2>\n<p>Gas molecules are in constant, chaotic motion, colliding billions of times per second. Because collisions constantly redistribute energy, the speeds of individual molecules spread over a wide range described by the Maxwell\u2013Boltzmann distribution. Rather than tracking every molecule, it is useful to summarize the distribution with a few characteristic speeds \u2014 and that is exactly what this calculator does.<\/p>\n<p>The <strong>most probable speed<\/strong> \\(v_p\\) sits at the peak of the distribution: more molecules travel near this speed than any other. The <strong>mean speed<\/strong> \\(\\bar{v}\\) is the simple arithmetic average over all molecules, and it is the one relevant for quantities like collision frequency and effusion rates. The <strong>root-mean-square speed<\/strong> \\(v_{rms}\\) weights faster molecules more heavily (it is derived from the mean squared speed), which makes it the natural choice whenever energy or pressure is involved \u2014 pressure, for instance, follows from \\(PV = \\frac{1}{3}Nm\\overline{v^2}\\).<\/p>\n<p>The three speeds always appear in the fixed ratio \\(v_p : \\bar{v} : v_{rms} = \\sqrt{2} : \\sqrt{8\/\\pi} : \\sqrt{3} \\approx 1 : 1.128 : 1.225\\), regardless of the gas or temperature. Two simple scaling rules are worth remembering: doubling the absolute temperature multiplies every speed by \\(\\sqrt{2}\\), while doubling the molar mass divides every speed by \\(\\sqrt{2}\\). This is why light hydrogen molecules race around at nearly 2000 m\/s at room temperature, while heavy CO\u2082 molecules crawl along at about 400 m\/s at the same temperature.<\/p>\n<p>The average translational energy per mole, \\(E_{mol} = \\frac{3}{2}RT\\), is a direct consequence of the equipartition theorem: each of the three translational degrees of freedom carries \\(\\frac{1}{2}RT\\) per mole. It is identical for every ideal gas at the same temperature, so helium and uranium hexafluoride molecules carry the same average translational energy \u2014 they just move at very different speeds.<\/p>\n<h2>Assumptions, Limitations and Practical Tips<\/h2>\n<ul>\n<li><strong>Ideal gas behavior:<\/strong> the formulas assume point-like molecules with no intermolecular interactions. Real gases deviate at high pressure or near condensation \u2014 for those conditions use the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/van-der-waals-equation-calculator\/\">Van der Waals Equation Calculator<\/a>.<\/li>\n<li><strong>Equilibrium required:<\/strong> the Maxwell\u2013Boltzmann distribution only holds once the gas has reached thermal equilibrium. In strong flows, shock waves or very rarefied gases, the actual speed distribution can differ.<\/li>\n<li><strong>Use the right molar mass:<\/strong> enter the mass of the actual gas particles. For a mixture such as air, use the effective average molar mass (28.97 g\/mol). Monatomic species like He or Ar move as single atoms; for molecular gases like N\u2082 or O\u2082 the molar mass is that of the whole molecule.<\/li>\n<li><strong>Temperature must be absolute:<\/strong> the formulas need kelvin. The calculator converts \u00b0C and \u00b0F for you, but entering a value at or below absolute zero returns an error.<\/li>\n<li><strong>Only translational motion counts:<\/strong> \\(E_{mol}\\) covers translation only. Rotating polyatomic molecules and vibrating bonds store additional energy, which is why the molar heat capacity exceeds \\(\\frac{3}{2}R\\) for diatomic and polyatomic gases.<\/li>\n<\/ul>\n<h2>Typical Molecular Speeds at 300 K<\/h2>\n<table>\n<thead>\n<tr>\n<th>Gas<\/th>\n<th>Molar mass (g\/mol)<\/th>\n<th>\\(v_{rms}\\) (m\/s)<\/th>\n<th>\\(\\bar{v}\\) (m\/s)<\/th>\n<th>\\(v_p\\) (m\/s)<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>Hydrogen (H\u2082)<\/td>\n<td>2<\/td>\n<td>1934<\/td>\n<td>1781<\/td>\n<td>1578<\/td>\n<\/tr>\n<tr>\n<td>Helium (He)<\/td>\n<td>4<\/td>\n<td>1367<\/td>\n<td>1259<\/td>\n<td>1116<\/td>\n<\/tr>\n<tr>\n<td>Nitrogen (N\u2082)<\/td>\n<td>28<\/td>\n<td>517<\/td>\n<td>476<\/td>\n<td>422<\/td>\n<\/tr>\n<tr>\n<td>Air (average)<\/td>\n<td>28.97<\/td>\n<td>508<\/td>\n<td>468<\/td>\n<td>415<\/td>\n<\/tr>\n<tr>\n<td>Oxygen (O\u2082)<\/td>\n<td>32<\/td>\n<td>484<\/td>\n<td>445<\/td>\n<td>395<\/td>\n<\/tr>\n<tr>\n<td>Carbon dioxide (CO\u2082)<\/td>\n<td>44<\/td>\n<td>413<\/td>\n<td>380<\/td>\n<td>337<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Since molecular speeds depend directly on temperature, the same calculator is also useful when studying temperature\u2013pressure relationships such as <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/gay-lussacs-law-calculator\/\">Gay-Lussac's law<\/a>, or gas amount\u2013volume relationships like <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/avogadros-law-calculator\/\">Avogadro's law<\/a>. For reaction rates, where molecular collisions set the pace, the <a href=\"https:\/\/wpcalc.com\/en\/chemistry\/reaction-rate-law-calculator\/\">Reaction Rate Law Calculator<\/a> is a natural companion tool.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the root-mean-square, mean, and most probable speeds of gas molecules from the temperature and molar mass, plus the average translational energy per mole, using kinetic theory formulas.<\/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":[55],"class_list":["post-66881","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\/66881","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=66881"}],"version-history":[{"count":2,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66881\/revisions"}],"predecessor-version":[{"id":67094,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/posts\/66881\/revisions\/67094"}],"wp:attachment":[{"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/media?parent=66881"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/categories?post=66881"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/wpcalc.com\/en\/wp-json\/wp\/v2\/tags?post=66881"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}