{"id":235168,"date":"2025-06-15T02:48:41","date_gmt":"2025-06-15T02:48:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=235168"},"modified":"2025-06-15T02:48:43","modified_gmt":"2025-06-15T02:48:43","slug":"the-density-of-acetic-anhydride-is-1-08-g-ml-3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/15\/the-density-of-acetic-anhydride-is-1-08-g-ml-3\/","title":{"rendered":"The density of acetic anhydride is 1.08 g\/ml"},"content":{"rendered":"\n

The density of acetic anhydride is 1.08 g\/ml. What is the mass of 2.00 ml 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

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Correct Answers:<\/strong><\/p>\n\n\n\n

    \n
  1. Mass of 2.00 mL of acetic anhydride:<\/strong><\/li>\n<\/ol>\n\n\n\n

    Mass=Density\u00d7Volume=1.08\u2009g\/mL\u00d72.00\u2009mL=2.16\u2009g\\text{Mass} = \\text{Density} \\times \\text{Volume} = 1.08 \\, \\text{g\/mL} \\times 2.00 \\, \\text{mL} = \\boxed{2.16 \\, \\text{g}}Mass=Density\u00d7Volume=1.08g\/mL\u00d72.00mL=2.16g\u200b<\/p>\n\n\n\n

      \n
    1. Moles in 500.0 mL of acetic anhydride:<\/strong><\/li>\n<\/ol>\n\n\n\n

      First, calculate the mass: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}Mass=1.08g\/mL\u00d7500.0mL=540.0g<\/p>\n\n\n\n

      Molar mass of acetic anhydride (C\u2084H\u2086O\u2083):(4\u00d712.01)+(6\u00d71.008)+(3\u00d716.00)=102.09\u2009g\/mol(4 \\times 12.01) + (6 \\times 1.008) + (3 \\times 16.00) = 102.09 \\, \\text{g\/mol}(4\u00d712.01)+(6\u00d71.008)+(3\u00d716.00)=102.09g\/molMoles=MassMolar Mass=540.0\u2009g102.09\u2009g\/mol\u22485.29\u2009mol\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}} = \\frac{540.0 \\, \\text{g}}{102.09 \\, \\text{g\/mol}} \\approx \\boxed{5.29 \\, \\text{mol}}Moles=Molar MassMass\u200b=102.09g\/mol540.0g\u200b\u22485.29mol\u200b<\/p>\n\n\n\n

      \n\n\n\n

      Explanation<\/strong><\/p>\n\n\n\n

      Understanding the relationship between density, volume, and mass is essential in chemical calculations. Density is defined as mass per unit volume and is expressed in grams per milliliter (g\/mL). To determine the mass of a liquid when density and volume are known, multiplication of these two quantities gives the desired value.<\/p>\n\n\n\n

      In this case, acetic anhydride has a density of 1.08 g\/mL. When 2.00 mL of this compound is measured, the mass is obtained by multiplying the volume by the density, resulting in 2.16 grams.<\/p>\n\n\n\n

      To determine the number of moles in a specific volume of acetic anhydride, the process starts with calculating the total mass in grams. A 500.0 mL bottle contains 540.0 grams of the liquid based on its density. The number of moles is calculated by dividing this mass by the molar mass of the substance.<\/p>\n\n\n\n

      Acetic anhydride, with the molecular formula C\u2084H\u2086O\u2083, has a molar mass of approximately 102.09 g\/mol. This is calculated using the atomic masses of carbon (12.01 g\/mol), hydrogen (1.008 g\/mol), and oxygen (16.00 g\/mol). By dividing the total mass (540.0 g) by the molar mass (102.09 g\/mol), the resulting value indicates that the bottle contains approximately 5.29 moles of acetic anhydride.<\/p>\n\n\n\n

      This approach is commonly used in laboratory and industrial settings to convert between volume, mass, and moles, ensuring accurate measurements and effective reagent preparation in chemical processes.<\/p>\n\n\n\n

      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

      The density of acetic anhydride is 1.08 g\/ml. What is the mass of 2.00 ml 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: Correct Answers: Mass=Density\u00d7Volume=1.08\u2009g\/mL\u00d72.00\u2009mL=2.16\u2009g\\text{Mass} = \\text{Density} \\times \\text{Volume} = 1.08 \\, \\text{g\/mL} \\times 2.00 \\, \\text{mL} […]<\/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-235168","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235168","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=235168"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235168\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=235168"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=235168"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=235168"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}