{"id":264901,"date":"2025-07-21T16:54:48","date_gmt":"2025-07-21T16:54:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=264901"},"modified":"2025-07-21T16:54:57","modified_gmt":"2025-07-21T16:54:57","slug":"a-compound-with-the-empirical-formula-ch2-has-a-molar-mass-of-84-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/21\/a-compound-with-the-empirical-formula-ch2-has-a-molar-mass-of-84-g-mol\/","title":{"rendered":"A compound with the empirical formula CH2 has a molar mass of 84 g\/mol"},"content":{"rendered":"\n<p>A compound with the empirical formula CH2 has a molar mass of 84 g\/mol. What is the molecular formula for this compound?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the molecular formula of a compound given its empirical formula and molar mass, follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the molar mass of the empirical formula<\/h3>\n\n\n\n<p>The empirical formula is CH\u2082, which means it contains one carbon (C) atom and two hydrogen (H) atoms. The atomic masses of carbon and hydrogen are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 12 g\/mol<\/li>\n\n\n\n<li>Hydrogen (H): 1 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>The molar mass of the empirical formula CH\u2082 is calculated by adding the atomic masses of each element: Molar&nbsp;mass&nbsp;of&nbsp;CH2=(12\u2009g\/mol)+(2\u00d71\u2009g\/mol)=12\u2009g\/mol+2\u2009g\/mol=14\u2009g\/mol\\text{Molar mass of CH}_2 = (12 \\, \\text{g\/mol}) + (2 \\times 1 \\, \\text{g\/mol}) = 12 \\, \\text{g\/mol} + 2 \\, \\text{g\/mol} = 14 \\, \\text{g\/mol}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Divide the molar mass of the compound by the molar mass of the empirical formula<\/h3>\n\n\n\n<p>The given molar mass of the compound is 84 g\/mol. To find how many empirical formula units are present in the molecular formula, divide the molar mass of the compound by the molar mass of the empirical formula: Number&nbsp;of&nbsp;units=Molar&nbsp;mass&nbsp;of&nbsp;the&nbsp;compoundMolar&nbsp;mass&nbsp;of&nbsp;the&nbsp;empirical&nbsp;formula=84\u2009g\/mol14\u2009g\/mol=6\\text{Number of units} = \\frac{\\text{Molar mass of the compound}}{\\text{Molar mass of the empirical formula}} = \\frac{84 \\, \\text{g\/mol}}{14 \\, \\text{g\/mol}} = 6<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Multiply the empirical formula by the number of units<\/h3>\n\n\n\n<p>Now that we know there are 6 empirical formula units in the molecular formula, multiply each element in the empirical formula by 6: Molecular&nbsp;formula=(CH2)\u00d76=C6H12\\text{Molecular formula} = (C H_2) \\times 6 = C_6 H_{12}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<p>The molecular formula of the compound is <strong>C\u2086H\u2081\u2082<\/strong>.<\/p>\n\n\n\n<p>This means the compound consists of 6 carbon atoms and 12 hydrogen atoms. The empirical formula (CH\u2082) represents the simplest ratio of elements in the compound, and the molecular formula shows the actual number of atoms in one molecule of the compound.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>A compound with the empirical formula CH2 has a molar mass of 84 g\/mol. What is the molecular formula for this compound? The correct answer and explanation is: To find the molecular formula of a compound given its empirical formula and molar mass, follow these steps: Step 1: Determine the molar mass of the empirical [&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-264901","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/264901","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=264901"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/264901\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=264901"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=264901"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=264901"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}