{"id":231140,"date":"2025-06-10T13:15:53","date_gmt":"2025-06-10T13:15:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=231140"},"modified":"2025-06-10T13:15:55","modified_gmt":"2025-06-10T13:15:55","slug":"calculate-the-density-of-co2-at-laboratory-conditions-at-stp","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/calculate-the-density-of-co2-at-laboratory-conditions-at-stp\/","title":{"rendered":"Calculate the density of CO2 at: Laboratory conditions At STP"},"content":{"rendered":"\n<p>Calculate the density of CO2 at: Laboratory conditions At STP<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the density of carbon dioxide (CO\u2082), we use the ideal gas law:<\/p>\n\n\n\n<p>Density(\u03c1)=PMRT\\text{Density} (\\rho) = \\frac{PM}{RT}<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>PP is pressure,<\/li>\n\n\n\n<li>MM is the molar mass of CO\u2082 (44.0144.01 g\/mol),<\/li>\n\n\n\n<li>RR is the gas constant (0.08210.0821 L\u00b7atm\/(mol\u00b7K)),<\/li>\n\n\n\n<li>TT is the temperature in Kelvin.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>Density at Laboratory Conditions<\/strong><\/h3>\n\n\n\n<p>Laboratory conditions vary, but assuming:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>T=25\u2218C=298T = 25^\\circ C = 298 K<\/li>\n\n\n\n<li>P=1P = 1 atm<\/li>\n<\/ul>\n\n\n\n<p>\u03c1=(1&nbsp;atm)(44.01&nbsp;g\/mol)(0.0821&nbsp;L\\cdotpatm\/(mol\\cdotpK))(298&nbsp;K)\\rho = \\frac{(1 \\text{ atm}) (44.01 \\text{ g\/mol})}{(0.0821 \\text{ L\u00b7atm\/(mol\u00b7K)}) (298 \\text{ K})}<\/p>\n\n\n\n<p>\u03c1\u22481.79&nbsp;g\/L\\rho \\approx 1.79 \\text{ g\/L}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>Density at Standard Temperature and Pressure (STP)<\/strong><\/h3>\n\n\n\n<p>STP is defined as:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>T=273T = 273 K<\/li>\n\n\n\n<li>P=1P = 1 atm<\/li>\n<\/ul>\n\n\n\n<p>\u03c1=(1&nbsp;atm)(44.01&nbsp;g\/mol)(0.0821&nbsp;L\\cdotpatm\/(mol\\cdotpK))(273&nbsp;K)\\rho = \\frac{(1 \\text{ atm}) (44.01 \\text{ g\/mol})}{(0.0821 \\text{ L\u00b7atm\/(mol\u00b7K)}) (273 \\text{ K})}<\/p>\n\n\n\n<p>\u03c1\u22481.96&nbsp;g\/L\\rho \\approx 1.96 \\text{ g\/L}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation<\/strong><\/h3>\n\n\n\n<p>The density of a gas is influenced by temperature and pressure. When temperature increases, the gas expands, lowering its density. Conversely, at lower temperatures, gas molecules occupy a smaller volume, increasing density. At STP, CO\u2082 has a density of <strong>1.96 g\/L<\/strong>, but in laboratory conditions (typically 25\u00b0C), the density reduces to <strong>1.79 g\/L<\/strong> due to thermal expansion.<\/p>\n\n\n\n<p>These calculations assume CO\u2082 behaves ideally. However, real gases exhibit minor deviations due to intermolecular forces, which can slightly affect density, especially at high pressures.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner6-184.jpeg\" alt=\"\" class=\"wp-image-231141\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the density of CO2 at: Laboratory conditions At STP The Correct Answer and Explanation is: To calculate the density of carbon dioxide (CO\u2082), we use the ideal gas law: Density(\u03c1)=PMRT\\text{Density} (\\rho) = \\frac{PM}{RT} where: 1. Density at Laboratory Conditions Laboratory conditions vary, but assuming: \u03c1=(1&nbsp;atm)(44.01&nbsp;g\/mol)(0.0821&nbsp;L\\cdotpatm\/(mol\\cdotpK))(298&nbsp;K)\\rho = \\frac{(1 \\text{ atm}) (44.01 \\text{ g\/mol})}{(0.0821 \\text{ L\u00b7atm\/(mol\u00b7K)}) [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-231140","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231140","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=231140"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231140\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231140"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231140"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231140"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}