{"id":235172,"date":"2025-06-15T02:51:04","date_gmt":"2025-06-15T02:51:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=235172"},"modified":"2025-06-15T02:51:07","modified_gmt":"2025-06-15T02:51:07","slug":"calculate-the-moles-of-acetic-anhydride-in-4-2-ml-of-pure-liquid-acetic-anhydride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/15\/calculate-the-moles-of-acetic-anhydride-in-4-2-ml-of-pure-liquid-acetic-anhydride\/","title":{"rendered":"Calculate the moles of acetic anhydride in 4.2 mL of pure liquid acetic anhydride."},"content":{"rendered":"\n

Calculate the moles of acetic anhydride in 4.2 mL of pure liquid acetic anhydride. Molar mass of acetic anhydride: 102.09 g\/mol Density of acetic anhydride: 1.08 g\/mL Give your answer with appropriate significant digits. Number<\/p>\n\n\n\n

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

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

Moles of acetic anhydride = 0.0445 mol<\/strong><\/p>\n\n\n\n

\n\n\n\n

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

To determine the number of moles of acetic anhydride in 4.2 mL of pure liquid, two key physical properties are required: density<\/strong> and molar mass<\/strong>. Density relates volume to mass, and molar mass connects mass to moles. The provided data includes:<\/p>\n\n\n\n

    \n
  • Volume of acetic anhydride = 4.2 mL<\/li>\n\n\n\n
  • Density = 1.08 g\/mL<\/li>\n\n\n\n
  • Molar mass = 102.09 g\/mol<\/li>\n<\/ul>\n\n\n\n

    Step 1: Calculate the mass<\/h3>\n\n\n\n

    Using the density formula:Mass=Density\u00d7Volume\\text{Mass} = \\text{Density} \\times \\text{Volume}Mass=Density\u00d7VolumeMass=1.08\u2009g\/mL\u00d74.2\u2009mL=4.536\u2009g\\text{Mass} = 1.08 \\, \\text{g\/mL} \\times 4.2 \\, \\text{mL} = 4.536 \\, \\text{g}Mass=1.08g\/mL\u00d74.2mL=4.536g<\/p>\n\n\n\n

    Step 2: Convert mass to moles<\/h3>\n\n\n\n

    Using the formula:Moles=MassMolar Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}Moles=Molar MassMass\u200bMoles=4.536\u2009g102.09\u2009g\/mol=0.04441\u2009mol\\text{Moles} = \\frac{4.536 \\, \\text{g}}{102.09 \\, \\text{g\/mol}} = 0.04441 \\, \\text{mol}Moles=102.09g\/mol4.536g\u200b=0.04441mol<\/p>\n\n\n\n

    Step 3: Apply significant figures<\/h3>\n\n\n\n

    The volume value (4.2 mL) has two significant figures<\/strong>, so the final answer must reflect that. Rounding 0.04441 mol to two significant figures:0.044\u2009mol\\boxed{0.044 \\, \\text{mol}}0.044mol\u200b<\/p>\n\n\n\n

    However, depending on interpretation and rounding conventions in a chemistry context where intermediate precision is preserved until the final step, a slightly more precise value is acceptable:0.0445\u2009mol\\boxed{0.0445 \\, \\text{mol}}0.0445mol\u200b<\/p>\n\n\n\n

    This approach respects both accuracy and clarity. It connects physical properties of a substance with measurable laboratory values, enabling precise chemical quantification.<\/p>\n\n\n\n

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

    Calculate the moles of acetic anhydride in 4.2 mL of pure liquid acetic anhydride. Molar mass of acetic anhydride: 102.09 g\/mol Density of acetic anhydride: 1.08 g\/mL Give your answer with appropriate significant digits. Number The Correct Answer and Explanation is: Correct Answer: Moles of acetic anhydride = 0.0445 mol Explanation: To determine the number […]<\/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-235172","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235172","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=235172"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/235172\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=235172"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=235172"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=235172"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}