1. The molar mass of oleic acid is 282.5 g\/mol and its density is 0.895 g\/cm? Use this information to calculate the molar volume of oleic acid. (Use the appropriate units, those associated with the two numbers given here.)<\/p>\n\n\n\n
2. Figure out a way to estimate the number of molecules in one mole of oleic acid. (This is Avogadro's number.) Report the result to the appropriate number of significant figures.<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The molar volume is the volume occupied by one mole of a substance, and it can be calculated using the formula:<\/p>\n\n\n\n [ Given:<\/p>\n\n\n\n Now, let’s plug in the values:<\/p>\n\n\n\n [ [ Thus, the molar volume of oleic acid is 316.3 cm\u00b3\/mol<\/strong>.<\/p>\n\n\n\n Avogadro’s number is a fundamental constant in chemistry, which is the number of atoms, ions, or molecules in one mole of a substance. To estimate the number of molecules in one mole of oleic acid, we can use the following approach:<\/p>\n\n\n\n We know that 1 mole of any substance contains 6.022 \u00d7 10\u00b2\u00b3<\/strong> entities (atoms or molecules), which is Avogadro\u2019s number. This value is universal for any substance, whether it is oleic acid or any other compound.<\/p>\n\n\n\n So, the number of molecules in one mole of oleic acid is:<\/p>\n\n\n\n [ This is the most accurate estimate of the number of molecules in one mole of oleic acid, based on Avogadro\u2019s number. Therefore, the result is:<\/p>\n\n\n\n 6.022 \u00d7 10\u00b2\u00b3 molecules\/mol<\/strong><\/p>\n\n\n\n Molar Volume Calculation:<\/strong><\/p>\n\n\n\n To calculate the molar volume, we divide the molar mass by the density. The units of g\/mol (molar mass) and g\/cm\u00b3 (density) cancel the grams, leaving cm\u00b3\/mol as the unit for molar volume. This calculation gives us the volume occupied by one mole of oleic acid at its given density.<\/p>\n\n\n\n Avogadro’s Number:<\/strong><\/p>\n\n\n\n Avogadro\u2019s number is a universal constant that defines how many entities (atoms or molecules) are present in one mole of a substance. This number is fixed, and for every mole of any substance, the number of molecules will always be 6.022 \u00d7 10\u00b2\u00b3. In the case of oleic acid, the number of molecules in one mole of oleic acid is exactly the same.<\/p>\n","protected":false},"excerpt":{"rendered":" 1. The molar mass of oleic acid is 282.5 g\/mol and its density is 0.895 g\/cm? Use this information to calculate the molar volume of oleic acid. (Use the appropriate units, those associated with the two numbers given here.) 2. Figure out a way to estimate the number of molecules in one mole of oleic […]<\/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-185452","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185452","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=185452"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185452\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185452"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185452"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185452"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}1. Molar Volume of Oleic Acid<\/h3>\n\n\n\n
\\text{Molar Volume} = \\frac{\\text{Molar Mass}}{\\text{Density}}
]<\/p>\n\n\n\n\n
\\text{Molar Volume} = \\frac{282.5 \\, \\text{g\/mol}}{0.895 \\, \\text{g\/cm}^3}
]<\/p>\n\n\n\n
\\text{Molar Volume} = 316.3 \\, \\text{cm}^3\/\\text{mol}
]<\/p>\n\n\n\n2. Estimating the Number of Molecules in One Mole of Oleic Acid (Avogadro’s Number)<\/h3>\n\n\n\n
6.022 \\times 10^{23} \\, \\text{molecules\/mol}
]<\/p>\n\n\n\nExplanation of the Calculations<\/h3>\n\n\n\n