{"id":182648,"date":"2025-01-14T13:39:05","date_gmt":"2025-01-14T13:39:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182648"},"modified":"2025-01-14T13:39:07","modified_gmt":"2025-01-14T13:39:07","slug":"the-density-of-acetic-anhydride-is-1-08-g-ml","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/14\/the-density-of-acetic-anhydride-is-1-08-g-ml\/","title":{"rendered":"The density of acetic anhydride is 1.08 g\/ml"},"content":{"rendered":"\n<p>The density of acetic anhydride is 1.08 g\/ml. What is the mass of 2.00ml of acetic anhydride? How many moles of acetic anhydride are present in a 500.0 ml bottle of acetic anhydride?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>To calculate the mass of acetic anhydride in a 2.00 mL sample and the number of moles in a 500.0 mL bottle, we need to use the given density and the molar mass of acetic anhydride.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. Mass of Acetic Anhydride in 2.00 mL<\/h3>\n\n\n\n<p>We are given:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Density of acetic anhydride = 1.08 g\/mL<\/li>\n\n\n\n<li>Volume = 2.00 mL<\/li>\n<\/ul>\n\n\n\n<p>The formula to calculate mass from density is: Mass=Density\u00d7Volume\\text{Mass} = \\text{Density} \\times \\text{Volume}<\/p>\n\n\n\n<p>Substituting the known values: Mass=1.08\u2009g\/mL\u00d72.00\u2009mL=2.16\u2009g\\text{Mass} = 1.08 \\, \\text{g\/mL} \\times 2.00 \\, \\text{mL} = 2.16 \\, \\text{g}<\/p>\n\n\n\n<p>So, the mass of 2.00 mL of acetic anhydride is <strong>2.16 g<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">2. Moles of Acetic Anhydride in 500.0 mL<\/h3>\n\n\n\n<p>Next, we need to find the number of moles in a 500.0 mL bottle. To do this, we must first calculate the mass of acetic anhydride in 500.0 mL, then convert that mass to moles.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Volume = 500.0 mL<\/li>\n\n\n\n<li>Density = 1.08 g\/mL<\/li>\n<\/ul>\n\n\n\n<p>Using the mass formula again: Mass=1.08\u2009g\/mL\u00d7500.0\u2009mL=540.0\u2009g\\text{Mass} = 1.08 \\, \\text{g\/mL} \\times 500.0 \\, \\text{mL} = 540.0 \\, \\text{g}<\/p>\n\n\n\n<p>Now, to calculate moles, we use the molar mass of acetic anhydride, which is <strong>102.09 g\/mol<\/strong>. The formula to find moles is: Moles=MassMolar&nbsp;Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}<\/p>\n\n\n\n<p>Substituting the values: Moles=540.0\u2009g102.09\u2009g\/mol\u22485.29\u2009mol\\text{Moles} = \\frac{540.0 \\, \\text{g}}{102.09 \\, \\text{g\/mol}} \\approx 5.29 \\, \\text{mol}<\/p>\n\n\n\n<p>So, there are approximately <strong>5.29 moles<\/strong> of acetic anhydride in a 500.0 mL bottle.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Density<\/strong> describes how much mass is present in a given volume of substance. Using the density equation, we first calculate the mass of acetic anhydride in a specific volume.<\/li>\n\n\n\n<li>To convert mass to moles, we use the molar mass, which tells us how many grams of a substance are in one mole.<\/li>\n\n\n\n<li>By applying these two calculations, we can determine the mass in grams for any volume and the number of moles for that mass based on the substance&#8217;s molar mass.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>The density of acetic anhydride is 1.08 g\/ml. What is the mass of 2.00ml of acetic anhydride? How many moles of acetic anhydride are present in a 500.0 ml bottle of acetic anhydride? The Correct Answer and Explanation is : To calculate the mass of acetic anhydride in a 2.00 mL sample and the 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-182648","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182648","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=182648"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182648\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182648"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182648"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182648"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}