{"id":249700,"date":"2025-07-09T19:06:36","date_gmt":"2025-07-09T19:06:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249700"},"modified":"2025-07-09T19:06:38","modified_gmt":"2025-07-09T19:06:38","slug":"the-molecular-formula-for-octane-is-c8h18-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/the-molecular-formula-for-octane-is-c8h18-2\/","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-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the molar mass of the empirical formula of octane (C8H18), we first need to find the empirical formula itself. The empirical formula represents the simplest whole-number ratio of the elements in a compound.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the empirical formula of octane<\/h3>\n\n\n\n<p>Octane&#8217;s molecular formula is <strong>C8H18<\/strong>, which shows there are 8 carbon (C) atoms and 18 hydrogen (H) atoms. To find the empirical formula, we divide both the number of carbon atoms and the number of hydrogen atoms by their greatest common divisor (GCD).<\/p>\n\n\n\n<p>The GCD of 8 and 18 is <strong>2<\/strong>.<\/p>\n\n\n\n<p>Thus, divide the subscripts of both elements by 2:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 8 \/ 2 = 4<\/li>\n\n\n\n<li>Hydrogen (H): 18 \/ 2 = 9<\/li>\n<\/ul>\n\n\n\n<p>Therefore, the <strong>empirical formula<\/strong> of octane is <strong>C4H9<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the molar mass of the empirical formula (C4H9)<\/h3>\n\n\n\n<p>To find the molar mass, we sum the atomic masses of the elements in the empirical formula:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The atomic mass of carbon (C) is <strong>12.01 g\/mol<\/strong>.<\/li>\n\n\n\n<li>The atomic mass of hydrogen (H) is <strong>1.008 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>So, the molar mass of <strong>C4H9<\/strong> is calculated as:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>4 carbon atoms \u00d7 12.01 g\/mol = 48.04 g\/mol<\/li>\n\n\n\n<li>9 hydrogen atoms \u00d7 1.008 g\/mol = 9.072 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Total molar mass = 48.04 g\/mol + 9.072 g\/mol = <strong>57.112 g\/mol<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Answer<\/h3>\n\n\n\n<p>The molar mass of the empirical formula of octane (C4H9) is approximately <strong>57.116 g\/mol<\/strong>. Thus, the correct answer is:<\/p>\n\n\n\n<p><strong>57.116 g\/mol<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<p>The empirical formula of a compound represents its simplest form, which helps simplify the calculation of molar masses. The molecular formula of octane (C8H18) corresponds to a more complex version of this empirical formula, but the molar mass of the empirical formula C4H9 is about <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-banner6-33.jpeg\" alt=\"\" class=\"wp-image-249701\"\/><\/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 determine the molar mass of the empirical formula of octane (C8H18), we first need to find the empirical formula itself. The empirical formula [&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-249700","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249700","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=249700"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249700\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249700"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249700"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249700"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}