{"id":249718,"date":"2025-07-09T19:20:37","date_gmt":"2025-07-09T19:20:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249718"},"modified":"2025-07-09T19:20:39","modified_gmt":"2025-07-09T19:20:39","slug":"the-molecular-mass-of-octane-is-114-22-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/the-molecular-mass-of-octane-is-114-22-g-mol\/","title":{"rendered":"The molecular mass of octane is 114.22 g\/mol"},"content":{"rendered":"\n<p>The molecular mass of octane is 114.22 g\/mol. What is the mass of 22.05 mol of octane? 5.180 g 22.05 g 114.22 g 2,518 g<\/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 calculate the mass of 22.05 mol of octane (C8H18), we need to use the relationship between moles, molar mass, and mass: Mass=Moles\u00d7Molar&nbsp;Mass\\text{Mass} = \\text{Moles} \\times \\text{Molar Mass}Mass=Moles\u00d7Molar&nbsp;Mass<\/p>\n\n\n\n<p>From the problem:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The molar mass of octane is given as 114.22 g\/mol.<\/li>\n\n\n\n<li>The number of moles is 22.05 mol.<\/li>\n<\/ul>\n\n\n\n<p>Now, substitute these values into the formula: Mass=22.05\u2009mol\u00d7114.22\u2009g\/mol\\text{Mass} = 22.05 \\, \\text{mol} \\times 114.22 \\, \\text{g\/mol}Mass=22.05mol\u00d7114.22g\/mol Mass=2,518.5\u2009g\\text{Mass} = 2,518.5 \\, \\text{g}Mass=2,518.5g<\/p>\n\n\n\n<p>Therefore, the mass of 22.05 mol of octane is <strong>2,518 g<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The molar mass of a compound is the mass of one mole of that substance, measured in grams per mole (g\/mol). For octane, the molar mass is 114.22 g\/mol.<\/li>\n\n\n\n<li>When you multiply the number of moles (22.05 mol) by the molar mass (114.22 g\/mol), the units of moles cancel out, and you&#8217;re left with grams. This gives you the mass of the substance in grams.<\/li>\n\n\n\n<li>This approach is commonly used in chemistry to convert between moles and mass.<\/li>\n<\/ul>\n\n\n\n<p>In this case, <strong>2,518 g<\/strong> is the correct answer.<\/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-banner6-38.jpeg\" alt=\"\" class=\"wp-image-249719\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molecular mass of octane is 114.22 g\/mol. What is the mass of 22.05 mol of octane? 5.180 g 22.05 g 114.22 g 2,518 g The Correct Answer and Explanation is: To calculate the mass of 22.05 mol of octane (C8H18), we need to use the relationship between moles, molar mass, and mass: Mass=Moles\u00d7Molar&nbsp;Mass\\text{Mass} = [&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-249718","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249718","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=249718"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249718\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249718"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249718"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249718"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}