1.80 g of E-Stilbene (molar mass: 180 g\/mol) reacts with 3.25 g of pyridinium tribromide (molar mass: 320 g\/mol) in acetic acid to give 2.55 g of pure meso-1,2-dibromo-1,2-diphenylethane (molar mass: 340 g\/mol). What is the percentage yield of this reaction?
A 50.0%
B 65.0%
C 75.0%
D 80.0%<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine the percentage yield of this reaction, we need to calculate the theoretical yield of meso-1,2-dibromo-1,2-diphenylethane based on the limiting reagent and compare it to the actual yield.<\/p>\n\n\n\n First, we need to calculate the number of moles of both E-Stilbene and pyridinium tribromide.<\/p>\n\n\n\n Since the reaction involves a 1:1 molar ratio between E-Stilbene and pyridinium tribromide, E-Stilbene<\/strong> is the limiting reagent because it has fewer moles (0.010 mol).<\/p>\n\n\n\n In this reaction, 1 mole of E-Stilbene reacts with 1 mole of pyridinium tribromide to give 1 mole of meso-1,2-dibromo-1,2-diphenylethane. Since E-Stilbene is the limiting reagent, the theoretical yield of meso-1,2-dibromo-1,2-diphenylethane is based on the number of moles of E-Stilbene:<\/p>\n\n\n\n [ The molar mass of meso-1,2-dibromo-1,2-diphenylethane is 340 g\/mol. Therefore, the theoretical yield is: The actual yield is given as 2.55 g. The percentage yield is calculated as: The percentage yield of the reaction is 75.0%<\/strong>, which corresponds to answer choice C<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" 1.80 g of E-Stilbene (molar mass: 180 g\/mol) reacts with 3.25 g of pyridinium tribromide (molar mass: 320 g\/mol) in acetic acid to give 2.55 g of pure meso-1,2-dibromo-1,2-diphenylethane (molar mass: 340 g\/mol). What is the percentage yield of this reaction?A 50.0%B 65.0%C 75.0%D 80.0% The correct answer and explanation is : To determine 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-209317","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209317","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=209317"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/209317\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=209317"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=209317"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=209317"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Identify the limiting reagent<\/h3>\n\n\n\n
\n
The molar mass of E-Stilbene is given as 180 g\/mol. The number of moles of E-Stilbene is calculated as:
[
\\text{moles of E-Stilbene} = \\frac{\\text{mass of E-Stilbene}}{\\text{molar mass of E-Stilbene}} = \\frac{1.80 \\, \\text{g}}{180 \\, \\text{g\/mol}} = 0.010 \\, \\text{mol}
]<\/li>\n\n\n\n
The molar mass of pyridinium tribromide is 320 g\/mol. The number of moles of pyridinium tribromide is calculated as:
[
\\text{moles of pyridinium tribromide} = \\frac{\\text{mass of pyridinium tribromide}}{\\text{molar mass of pyridinium tribromide}} = \\frac{3.25 \\, \\text{g}}{320 \\, \\text{g\/mol}} = 0.01016 \\, \\text{mol}
]<\/li>\n<\/ol>\n\n\n\nStep 2: Calculate the theoretical yield<\/h3>\n\n\n\n
\\text{moles of meso-1,2-dibromo-1,2-diphenylethane} = \\text{moles of E-Stilbene} = 0.010 \\, \\text{mol}
]<\/p>\n\n\n\n
[
\\text{theoretical yield} = \\text{moles of meso-1,2-dibromo-1,2-diphenylethane} \\times \\text{molar mass of meso-1,2-dibromo-1,2-diphenylethane}
]
[
\\text{theoretical yield} = 0.010 \\, \\text{mol} \\times 340 \\, \\text{g\/mol} = 3.40 \\, \\text{g}
]<\/p>\n\n\n\nStep 3: Calculate the percentage yield<\/h3>\n\n\n\n
[
\\text{percentage yield} = \\left( \\frac{\\text{actual yield}}{\\text{theoretical yield}} \\right) \\times 100
]
[
\\text{percentage yield} = \\left( \\frac{2.55 \\, \\text{g}}{3.40 \\, \\text{g}} \\right) \\times 100 = 75.0\\%
]<\/p>\n\n\n\nConclusion:<\/h3>\n\n\n\n