{"id":217568,"date":"2025-05-22T05:50:41","date_gmt":"2025-05-22T05:50:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=217568"},"modified":"2025-05-22T05:50:43","modified_gmt":"2025-05-22T05:50:43","slug":"what-is-the-molar-mass-of-acetaminophen-c8h9no2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/22\/what-is-the-molar-mass-of-acetaminophen-c8h9no2\/","title":{"rendered":"What is the molar mass of acetaminophen, C8H9NO2"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">What is the molar mass of acetaminophen, C8H9NO2?<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">A. 43 g\/mol<br>B. 76 g\/mol<br>C. 151 g\/mol<br>D. 162 g\/mol<br>E. 125 g\/mol<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">The correct answer is: <strong>D. 162 g\/mol<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation:<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">To determine the <strong>molar mass<\/strong> of acetaminophen (<strong>C\u2088H\u2089NO\u2082<\/strong>), you need to sum the molar masses of each atom in the molecular formula. Here&#8217;s a step-by-step calculation using the atomic masses of each element:<\/p>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th><strong>Element<\/strong><\/th><th><strong>Number of Atoms<\/strong><\/th><th><strong>Atomic Mass (g\/mol)<\/strong><\/th><th><strong>Total Contribution (g\/mol)<\/strong><\/th><\/tr><\/thead><tbody><tr><td>Carbon (C)<\/td><td>8<\/td><td>12.01<\/td><td>8 \u00d7 12.01 = 96.08<\/td><\/tr><tr><td>Hydrogen (H)<\/td><td>9<\/td><td>1.008<\/td><td>9 \u00d7 1.008 = 9.072<\/td><\/tr><tr><td>Nitrogen (N)<\/td><td>1<\/td><td>14.01<\/td><td>1 \u00d7 14.01 = 14.01<\/td><\/tr><tr><td>Oxygen (O)<\/td><td>2<\/td><td>16.00<\/td><td>2 \u00d7 16.00 = 32.00<\/td><\/tr><tr><td><\/td><td><\/td><td><\/td><td><strong>Total = 151.16 g\/mol<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<p class=\"wp-block-paragraph\">Wait \u2014 that total seems to be <strong>151.16 g\/mol<\/strong>, which might suggest answer <strong>C (151 g\/mol)<\/strong>. But let\u2019s double-check our numbers with a bit more precision and compare again:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon (C)<\/strong>: 12.01 \u00d7 8 = <strong>96.08 g\/mol<\/strong><\/li>\n\n\n\n<li><strong>Hydrogen (H)<\/strong>: 1.008 \u00d7 9 = <strong>9.072 g\/mol<\/strong><\/li>\n\n\n\n<li><strong>Nitrogen (N)<\/strong>: 14.01 \u00d7 1 = <strong>14.01 g\/mol<\/strong><\/li>\n\n\n\n<li><strong>Oxygen (O)<\/strong>: 16.00 \u00d7 2 = <strong>32.00 g\/mol<\/strong><\/li>\n\n\n\n<li><strong>Total<\/strong> = 96.08 + 9.072 + 14.01 + 32.00 = <strong>151.162 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Thus, the correct molar mass of acetaminophen is <strong>approximately 151.16 g\/mol<\/strong>, which <strong>rounds to 151 g\/mol<\/strong>.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">So, <strong>the correct answer is actually:<\/strong><\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p class=\"wp-block-paragraph\">\u2705 <strong>C. 151 g\/mol<\/strong><\/p>\n<\/blockquote>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Key Concepts:<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Molar mass<\/strong> is the mass of one mole of a substance and is calculated by adding together the atomic masses of all atoms in a molecule.<\/li>\n\n\n\n<li>Atomic masses (in g\/mol) are taken from the periodic table:\n<ul class=\"wp-block-list\">\n<li><strong>C = 12.01<\/strong><\/li>\n\n\n\n<li><strong>H = 1.008<\/strong><\/li>\n\n\n\n<li><strong>N = 14.01<\/strong><\/li>\n\n\n\n<li><strong>O = 16.00<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Acetaminophen (also known as paracetamol) is a common over-the-counter pain reliever and fever reducer.<\/li>\n<\/ol>\n\n\n\n<p class=\"wp-block-paragraph\">By using correct atomic masses and accurate arithmetic, we see the most precise and correct answer is <strong>C. 151 g\/mol<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the molar mass of acetaminophen, C8H9NO2? A. 43 g\/molB. 76 g\/molC. 151 g\/molD. 162 g\/molE. 125 g\/mol The Correct Answer and Explanation is: The correct answer is: D. 162 g\/mol Explanation: To determine the molar mass of acetaminophen (C\u2088H\u2089NO\u2082), you need to sum the molar masses of each atom in the molecular formula. [&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-217568","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217568","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=217568"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217568\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=217568"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=217568"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=217568"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}