{"id":201753,"date":"2025-03-15T22:14:44","date_gmt":"2025-03-15T22:14:44","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=201753"},"modified":"2025-03-15T22:14:46","modified_gmt":"2025-03-15T22:14:46","slug":"what-is-the-molecular-formula-of-a-compound-with-the-empirical-formula-ch2-if-the-molecular-mass-of-the-compound-is-56-10-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/15\/what-is-the-molecular-formula-of-a-compound-with-the-empirical-formula-ch2-if-the-molecular-mass-of-the-compound-is-56-10-g-mol\/","title":{"rendered":"What is the molecular formula of a compound with the empirical formula CH2 if the molecular mass of the compound is 56.10 g\/mol"},"content":{"rendered":"\n<p>What is the molecular formula of a compound with the empirical formula CH2 if the molecular mass of the compound is 56.10 g\/mol?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To determine the molecular formula of a compound from its empirical formula and molecular mass, we can follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Calculate the molar mass of the empirical formula.<\/h3>\n\n\n\n<p>The empirical formula is CH\u2082, so we need to find its molar mass by summing the atomic masses of carbon (C) and hydrogen (H):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has an atomic mass of approximately 12.01 g\/mol.<\/li>\n\n\n\n<li>Hydrogen (H) has an atomic mass of approximately 1.008 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>For the empirical formula CH\u2082:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Molar mass = (1 \u00d7 12.01 g\/mol) + (2 \u00d7 1.008 g\/mol) = 12.01 g\/mol + 2.016 g\/mol = 14.026 g\/mol.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Determine the ratio of the molecular mass to the empirical formula mass.<\/h3>\n\n\n\n<p>The molecular mass of the compound is given as 56.10 g\/mol. Now, we calculate the ratio of the molecular mass to the empirical formula mass:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Ratio = Molecular mass \/ Empirical formula mass<\/li>\n\n\n\n<li>Ratio = 56.10 g\/mol \/ 14.026 g\/mol \u2248 4.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Find the molecular formula.<\/h3>\n\n\n\n<p>The ratio tells us that the molecular formula is 4 times the empirical formula. Therefore, to get the molecular formula, multiply each element in the empirical formula by 4:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Empirical formula: CH\u2082<\/li>\n\n\n\n<li>Molecular formula: (CH\u2082)\u2084 = C\u2084H\u2088.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>The molecular formula of the compound with the empirical formula CH\u2082 and a molecular mass of 56.10 g\/mol is <strong>C\u2084H\u2088<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The empirical formula represents the simplest whole-number ratio of atoms in a compound. In this case, the empirical formula CH\u2082 suggests a ratio of 1 carbon atom to 2 hydrogen atoms. The molecular formula represents the actual number of atoms in the compound, which can be a multiple of the empirical formula. By comparing the molecular mass to the empirical formula mass, we find that the molecular formula is a multiple (in this case, 4) of the empirical formula. Therefore, the molecular formula is C\u2084H\u2088.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular formula of a compound with the empirical formula CH2 if the molecular mass of the compound is 56.10 g\/mol? The correct answer and explanation is : To determine the molecular formula of a compound from its empirical formula and molecular mass, we can follow these steps: Step 1: Calculate the molar [&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-201753","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201753","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=201753"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201753\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201753"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201753"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201753"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}