{"id":252566,"date":"2025-07-11T10:56:57","date_gmt":"2025-07-11T10:56:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=252566"},"modified":"2025-07-11T10:57:01","modified_gmt":"2025-07-11T10:57:01","slug":"how-many-moles-are-in-2-7-ml-of-acetic-anhydride-density-of-1-082","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/11\/how-many-moles-are-in-2-7-ml-of-acetic-anhydride-density-of-1-082\/","title":{"rendered":"How many moles are in 2.7 mL of acetic anhydride, density of 1.082"},"content":{"rendered":"\n

molecular weight of Acetic Anhydride = 102 How many moles are in 2.7 mL of acetic anhydride, density of 1.082? Use the molecular weights that you have already calculated. Give two significant figures.<\/p>\n\n\n\n

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

To calculate the number of moles in 2.7 mL of acetic anhydride, we can break the calculation into two parts:<\/p>\n\n\n\n

    \n
  1. Convert the volume to mass using the density<\/strong>:
    The formula to find mass is: Mass=Density\u00d7Volume\\text{Mass} = \\text{Density} \\times \\text{Volume}Mass=Density\u00d7Volume We are given:
    • Density of acetic anhydride = 1.082 g\/mL<\/li>
    • Volume = 2.7 mL<\/li><\/ul>Mass=1.082\u2009g\/mL\u00d72.7\u2009mL=2.9214\u2009g\\text{Mass} = 1.082 \\, \\text{g\/mL} \\times 2.7 \\, \\text{mL} = 2.9214 \\, \\text{g}Mass=1.082g\/mL\u00d72.7mL=2.9214g<\/li>\n\n\n\n
    • Convert mass to moles<\/strong>:
      To convert mass to moles, use the formula: Moles=MassMolar\u00a0Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}Moles=Molar\u00a0MassMass\u200b The molecular weight of acetic anhydride is given as 102 g\/mol. Moles=2.9214\u2009g102\u2009g\/mol=0.0286\u2009mol\\text{Moles} = \\frac{2.9214 \\, \\text{g}}{102 \\, \\text{g\/mol}} = 0.0286 \\, \\text{mol}Moles=102g\/mol2.9214g\u200b=0.0286mol When rounded to two significant figures, the number of moles is: Moles=0.029\u2009mol\\text{Moles} = 0.029 \\, \\text{mol}Moles=0.029mol<\/li>\n<\/ol>\n\n\n\n

      Conclusion<\/strong>: There are 0.029 moles<\/strong> of acetic anhydride in 2.7 mL, considering the density and molecular weight provided.<\/p>\n\n\n\n

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

      molecular weight of Acetic Anhydride = 102 How many moles are in 2.7 mL of acetic anhydride, density of 1.082? Use the molecular weights that you have already calculated. Give two significant figures. The Correct Answer and Explanation is: To calculate the number of moles in 2.7 mL of acetic anhydride, we can break the […]<\/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-252566","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/252566","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=252566"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/252566\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=252566"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=252566"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=252566"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}