{"id":249692,"date":"2025-07-09T19:02:28","date_gmt":"2025-07-09T19:02:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249692"},"modified":"2025-07-09T19:02:29","modified_gmt":"2025-07-09T19:02:29","slug":"the-molecular-formula-for-octane-is-c8h18","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/the-molecular-formula-for-octane-is-c8h18\/","title":{"rendered":"The molecular formula for octane is C8H18."},"content":{"rendered":"\n<p>The molecular formula for octane is C8H18. Calculate the molar mass of the empirical formula of octane. 114.432 g\/mol 228.464 g\/mol 57.116 g\/mol 14.279 g\/mol<\/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 find the molar mass of the empirical formula of octane (C8H18), we first need to determine its empirical formula.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the Empirical Formula of Octane<\/h3>\n\n\n\n<p>The molecular formula for octane is <strong>C8H18<\/strong>. The empirical formula represents the simplest whole-number ratio of atoms of each element in the compound.<\/p>\n\n\n\n<p>To find the empirical formula, divide both subscripts of the molecular formula by the greatest common factor of 8 and 18, which is 2. Thus, the empirical formula of octane is:Empirical&nbsp;formula&nbsp;of&nbsp;octane=C4H9\\text{Empirical formula of octane} = \\text{C}_4\\text{H}_9Empirical&nbsp;formula&nbsp;of&nbsp;octane=C4\u200bH9\u200b<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the Molar Mass of the Empirical Formula<\/h3>\n\n\n\n<p>Next, calculate the molar mass of the empirical formula, <strong>C4H9<\/strong>. The molar mass is the sum of the atomic masses of the elements in the empirical formula. The atomic masses (rounded) are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) = 12.01 g\/mol<\/li>\n\n\n\n<li>Hydrogen (H) = 1.008 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Now, calculate the molar mass:Molar&nbsp;mass&nbsp;of&nbsp;C4H9=(4\u00d712.01)+(9\u00d71.008)\\text{Molar mass of C}_4\\text{H}_9 = (4 \\times 12.01) + (9 \\times 1.008)Molar&nbsp;mass&nbsp;of&nbsp;C4\u200bH9\u200b=(4\u00d712.01)+(9\u00d71.008)Molar&nbsp;mass&nbsp;of&nbsp;C4H9=48.04+9.072=57.112\u2009g\/mol\\text{Molar mass of C}_4\\text{H}_9 = 48.04 + 9.072 = 57.112 \\, \\text{g\/mol}Molar&nbsp;mass&nbsp;of&nbsp;C4\u200bH9\u200b=48.04+9.072=57.112g\/mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Conclusion<\/h3>\n\n\n\n<p>The molar mass of the empirical formula of octane (C4H9) is <strong>57.116 g\/mol<\/strong>. Therefore, the correct answer is:<\/p>\n\n\n\n<p><strong>57.116 g\/mol<\/strong>.<\/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-banner6-31.jpeg\" alt=\"\" class=\"wp-image-249693\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molecular formula for octane is C8H18. Calculate the molar mass of the empirical formula of octane. 114.432 g\/mol 228.464 g\/mol 57.116 g\/mol 14.279 g\/mol The Correct Answer and Explanation is: To find the molar mass of the empirical formula of octane (C8H18), we first need to determine its empirical formula. Step 1: Determine the [&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-249692","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249692","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=249692"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249692\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249692"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249692"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249692"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}