To calculate the molar mass of acetaminophen (C8H9NO2), we need to add the atomic masses of all the atoms in the chemical formula:<\/p>\n\n\n\n
- \n
- Carbon (C)<\/strong>: There are 8 carbon atoms in the formula. The atomic mass of carbon is approximately 12.01 g\/mol. 8\u00d712.01=96.08\u2009g\/mol8 \\times 12.01 = 96.08 \\, \\text{g\/mol}8\u00d712.01=96.08g\/mol<\/li>\n\n\n\n
- Hydrogen (H)<\/strong>: There are 9 hydrogen atoms in the formula. The atomic mass of hydrogen is approximately 1.008 g\/mol. 9\u00d71.008=9.072\u2009g\/mol9 \\times 1.008 = 9.072 \\, \\text{g\/mol}9\u00d71.008=9.072g\/mol<\/li>\n\n\n\n
- Nitrogen (N)<\/strong>: There is 1 nitrogen atom in the formula. The atomic mass of nitrogen is approximately 14.01 g\/mol. 1\u00d714.01=14.01\u2009g\/mol1 \\times 14.01 = 14.01 \\, \\text{g\/mol}1\u00d714.01=14.01g\/mol<\/li>\n\n\n\n
- Oxygen (O)<\/strong>: There are 2 oxygen atoms in the formula. The atomic mass of oxygen is approximately 16.00 g\/mol. 2\u00d716.00=32.00\u2009g\/mol2 \\times 16.00 = 32.00 \\, \\text{g\/mol}2\u00d716.00=32.00g\/mol<\/li>\n<\/ul>\n\n\n\n
Now, we add all these contributions together: 96.08+9.072+14.01+32.00=151.162\u2009g\/mol96.08 + 9.072 + 14.01 + 32.00 = 151.162 \\, \\text{g\/mol}96.08+9.072+14.01+32.00=151.162g\/mol<\/p>\n\n\n\n
Therefore, the molar mass of acetaminophen (C8H9NO2) is 151.16 g\/mol<\/strong>.<\/p>\n\n\n\n
Explanation:<\/h3>\n\n\n\n
The molar mass is calculated by multiplying the number of atoms of each element in the compound by the atomic mass of the element and then summing up all the individual masses. This gives us the molar mass of the entire compound, which represents the mass of one mole of acetaminophen. It\u2019s an essential quantity for understanding how much of a substance is involved in chemical reactions, helping us to convert between grams and moles for stoichiometric calculations.<\/p>\n\n\n\n
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<\/figure>\n","protected":false},"excerpt":{"rendered":"What is the molar mass of acetaminophen, C8H9NO2? The Correct Answer and Explanation is: To calculate the molar mass of acetaminophen (C8H9NO2), we need to add the atomic masses of all the atoms in the chemical formula: Now, we add all these contributions together: 96.08+9.072+14.01+32.00=151.162\u2009g\/mol96.08 + 9.072 + 14.01 + 32.00 = 151.162 \\, \\text{g\/mol}96.08+9.072+14.01+32.00=151.162g\/mol […]<\/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-259892","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259892","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=259892"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259892\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259892"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259892"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259892"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- Hydrogen (H)<\/strong>: There are 9 hydrogen atoms in the formula. The atomic mass of hydrogen is approximately 1.008 g\/mol. 9\u00d71.008=9.072\u2009g\/mol9 \\times 1.008 = 9.072 \\, \\text{g\/mol}9\u00d71.008=9.072g\/mol<\/li>\n\n\n\n