{"id":253655,"date":"2025-07-12T06:25:56","date_gmt":"2025-07-12T06:25:56","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=253655"},"modified":"2025-07-12T06:25:58","modified_gmt":"2025-07-12T06:25:58","slug":"determine-the-molecular-formula-of-a-compound-that-has-a-molar-mass-of-122-11-g-mol-and-an-empirical-formula-of-c2h5o2-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/12\/determine-the-molecular-formula-of-a-compound-that-has-a-molar-mass-of-122-11-g-mol-and-an-empirical-formula-of-c2h5o2-2\/","title":{"rendered":"Determine the molecular formula of a compound that has a molar mass of 122.11 g\/mol and an empirical formula of C2H5O2."},"content":{"rendered":"\n<p>122.11 g\/mol and an empirical formula of C2H5O2. Determine the molecular formula of a compound that has a molar mass of 122.11 g\/mol and an empirical formula of C2H5O2. C2H5O2 C8H20O8 C6H15O6 C4H10O4 C3H7O3<\/p>\n\n\n\n<p><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>To determine the molecular formula from the empirical formula and molar mass, we need to follow a few 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 given is C2H5O2. Let&#8217;s calculate its molar mass.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 12.01 g\/mol \u00d7 2 = 24.02 g\/mol<\/li>\n\n\n\n<li>Hydrogen (H): 1.008 g\/mol \u00d7 5 = 5.04 g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 16.00 g\/mol \u00d7 2 = 32.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>So, the molar mass of the empirical formula (C2H5O2) is:<\/p>\n\n\n\n<p><strong>24.02 + 5.04 + 32.00 = 61.06 g\/mol<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Compare the molar mass of the empirical formula with the given molar mass<\/h3>\n\n\n\n<p>The given molar mass is <strong>122.11 g\/mol<\/strong>.<\/p>\n\n\n\n<p>Now, divide the given molar mass by the molar mass of the empirical formula:<\/p>\n\n\n\n<p><strong>122.11 g\/mol \u00f7 61.06 g\/mol = 2<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Multiply the empirical formula by this factor<\/h3>\n\n\n\n<p>The factor we found is 2. This means the molecular formula contains 2 units of the empirical formula. So, we multiply each subscript in the empirical formula by 2:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 2 \u00d7 2 = 4<\/li>\n\n\n\n<li>Hydrogen (H): 2 \u00d7 5 = 10<\/li>\n\n\n\n<li>Oxygen (O): 2 \u00d7 2 = 4<\/li>\n<\/ul>\n\n\n\n<p>Thus, the molecular formula is <strong>C4H10O4<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Verify the molecular formula options<\/h3>\n\n\n\n<p>Looking at the given options:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>C2H5O2<\/li>\n\n\n\n<li>C8H20O8<\/li>\n\n\n\n<li>C6H15O6<\/li>\n\n\n\n<li>C4H10O4<\/li>\n\n\n\n<li>C3H7O3<\/li>\n<\/ul>\n\n\n\n<p>The correct answer is <strong>C4H10O4<\/strong>.<\/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>C4H10O4<\/strong>, which is derived by doubling the empirical formula (C2H5O2) to match the given molar mass of 122.11 g\/mol.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner9-150.jpeg\" alt=\"\" class=\"wp-image-253659\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>122.11 g\/mol and an empirical formula of C2H5O2. Determine the molecular formula of a compound that has a molar mass of 122.11 g\/mol and an empirical formula of C2H5O2. C2H5O2 C8H20O8 C6H15O6 C4H10O4 C3H7O3 The Correct Answer and Explanation is: To determine the molecular formula from the empirical formula and molar mass, we need to [&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-253655","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253655","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=253655"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253655\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=253655"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=253655"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=253655"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}