{"id":203376,"date":"2025-03-19T16:54:45","date_gmt":"2025-03-19T16:54:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203376"},"modified":"2025-03-19T16:54:47","modified_gmt":"2025-03-19T16:54:47","slug":"calculate-the-molar-mass-of-sucrose","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/19\/calculate-the-molar-mass-of-sucrose\/","title":{"rendered":"Calculate the molar mass of sucrose"},"content":{"rendered":"\n<p>a) Calculate the molar mass of sucrose, C12H22O11.<\/p>\n\n\n\n<p>(b) How many moles of sucrose are present in:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(i) 1.00 gram;<\/li>\n\n\n\n<li>(ii) 1.00 pound;<\/li>\n\n\n\n<li>(iii) 1.00 kg of sucrose?<\/li>\n<\/ul>\n\n\n\n<p>(c) How many sucrose molecules are present in a 4.536-g sample of sucrose?<\/p>\n\n\n\n<p>(d) How many atoms of carbon, hydrogen, and oxygen, respectively, are present in 4.536 g of sucrose?<\/p>\n\n\n\n<p>(1 lb = 453.6 g; Avogadro&#8217;s number = 6.022 x 10<sup>23<\/sup>\/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-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Answers:<\/h3>\n\n\n\n<p>(a) The molar mass of sucrose (C\u2081\u2082H\u2082\u2082O\u2081\u2081) is <strong>342.296 g\/mol<\/strong>.<\/p>\n\n\n\n<p>(b) The number of moles of sucrose present in:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>(i) <strong>1.00 g<\/strong> of sucrose = <strong>0.00292 moles<\/strong><\/li>\n\n\n\n<li>(ii) <strong>1.00 lb (453.6 g)<\/strong> of sucrose = <strong>1.325 moles<\/strong><\/li>\n\n\n\n<li>(iii) <strong>1.00 kg (1000 g)<\/strong> of sucrose = <strong>2.921 moles<\/strong><\/li>\n<\/ul>\n\n\n\n<p>(c) The number of sucrose molecules in a <strong>4.536 g<\/strong> sample:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>7.98 \u00d7 10\u00b2\u00b9 molecules<\/strong><\/li>\n<\/ul>\n\n\n\n<p>(d) The number of atoms in <strong>4.536 g<\/strong> of sucrose:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon (C):<\/strong> <strong>9.58 \u00d7 10\u00b2\u00b2 atoms<\/strong><\/li>\n\n\n\n<li><strong>Hydrogen (H):<\/strong> <strong>1.76 \u00d7 10\u00b2\u00b3 atoms<\/strong><\/li>\n\n\n\n<li><strong>Oxygen (O):<\/strong> <strong>8.78 \u00d7 10\u00b2\u00b2 atoms<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Sucrose is composed of <strong>carbon (C), hydrogen (H), and oxygen (O)<\/strong> with a molecular formula of <strong>C\u2081\u2082H\u2082\u2082O\u2081\u2081<\/strong>. To determine its <strong>molar mass<\/strong>, we sum the atomic masses of its elements: (12\u00d712.01)+(22\u00d71.008)+(11\u00d716.00)=342.296&nbsp;g\/mol(12 \\times 12.01) + (22 \\times 1.008) + (11 \\times 16.00) = 342.296 \\text{ g\/mol}<\/p>\n\n\n\n<p>For part (b), the number of <strong>moles<\/strong> is found using the formula: Moles=MassMolar&nbsp;Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}<\/p>\n\n\n\n<p>This calculation is applied to different masses (1 g, 1 lb, and 1 kg) of sucrose.<\/p>\n\n\n\n<p>In part (c), we use <strong>Avogadro\u2019s number (6.022 \u00d7 10\u00b2\u00b3 molecules\/mol)<\/strong> to convert moles to molecules: Molecules=Moles\u00d76.022\u00d71023\\text{Molecules} = \\text{Moles} \\times 6.022 \\times 10^{23}<\/p>\n\n\n\n<p>Finally, for part (d), we determine the <strong>individual atom counts<\/strong> by multiplying the number of molecules by the number of atoms per sucrose molecule.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>a) Calculate the molar mass of sucrose, C12H22O11. (b) How many moles of sucrose are present in: (c) How many sucrose molecules are present in a 4.536-g sample of sucrose? (d) How many atoms of carbon, hydrogen, and oxygen, respectively, are present in 4.536 g of sucrose? (1 lb = 453.6 g; Avogadro&#8217;s number = [&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-203376","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203376","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=203376"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203376\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203376"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203376"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203376"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}