The question asks “What is the density of PF3 at STP”?<\/p>\n\n\n\n
Molar mass of PF3 is 87.9680 so just divide that by 22.4? Is the correct answer 3.92 g\/l?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n Yes, your approach is correct! At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 L<\/strong> of volume. To calculate the density of phosphorus trifluoride (PF\u2083)<\/strong> at STP, we use the formula:<\/p>\n\n\n\n [ Given:<\/p>\n\n\n\n Now, performing the calculation:<\/p>\n\n\n\n [ [ So, the correct answer is 3.93 g\/L<\/strong>, not 3.92 g\/L (a minor rounding difference).<\/p>\n\n\n\n The concept of gas density at STP is based on the ideal gas law<\/strong>, which states:<\/p>\n\n\n\n [ At STP (Standard Temperature = 273.15 K<\/strong>, Pressure = 1 atm<\/strong>), 1 mole of an ideal gas occupies 22.4 L<\/strong>. The density of a gas is given by:<\/p>\n\n\n\n [ Since 1 mole of PF\u2083<\/strong> weighs 87.9680 g<\/strong> and occupies 22.4 L<\/strong>, its density is simply the molar mass divided by the molar volume.<\/p>\n\n\n\n This method works for any ideal gas at STP and provides a quick way to determine its density. The slight difference in your calculation (3.92 g\/L) is likely due to rounding. Using more precise values, 3.93 g\/L<\/strong> is the most accurate answer.<\/p>\n","protected":false},"excerpt":{"rendered":" The question asks “What is the density of PF3 at STP”? Molar mass of PF3 is 87.9680 so just divide that by 22.4? Is the correct answer 3.92 g\/l? The Correct Answer and Explanation is : Yes, your approach is correct! At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 […]<\/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-187115","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187115","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=187115"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187115\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187115"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187115"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187115"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\\text{Density} = \\frac{\\text{Molar Mass}}{\\text{Molar Volume at STP}}
]<\/p>\n\n\n\n\n
\\text{Density} = \\frac{87.9680 \\text{ g\/mol}}{22.4 \\text{ L\/mol}}
]<\/p>\n\n\n\n
\\text{Density} = 3.93 \\text{ g\/L}
]<\/p>\n\n\n\nExplanation:<\/h3>\n\n\n\n
PV = nRT
]<\/p>\n\n\n\n
\\text{Density} = \\frac{\\text{Mass of Gas}}{\\text{Volume of Gas}}
]<\/p>\n\n\n\n