In the synthesis of aspirin we react salicylic acid with acetic anhydride. The balanced chemical equation is:<\/p>\n\n\n\n
2HOOCC6H4OH + C4H6O3 \u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u2122 2HOOCC6H4O2C2H3\u00c3\u201a\u00c2 + H2O
salicylic acid acetic
anhydride \u00c3\u201a\u00c2 acetyl salicylic acid water<\/p>\n\n\n\n
If we mix together\u00c3\u201a\u00c2 \u00c3\u201a\u00c2 27.9\u00c3\u201a\u00c2 grams of salicylic acid with\u00c3\u201a\u00c2 \u00c3\u201a\u00c2 14.4\u00c3\u201a\u00c2 grams of acetic anhydride in this reaction, we obtain 30.7 grams of aspirin.<\/p>\n\n\n\n
\u00c3\u201a\u00c2<\/p>\n\n\n\n
What are the theoretical yields of our experiment?\u00c3\u201a\u00c2<\/p>\n\n\n\n
The theoretical yields =\u00c3\u201a\u00c2<\/p>\n\n\n\n
\u00c3\u201a\u00c2<\/p>\n\n\n\n
What are the percentage yields of our experiment?<\/p>\n\n\n\n
the percentage yields =\u00c3\u201a\u00c2<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine the theoretical yield and percentage yield of aspirin in this experiment, we must first identify the limiting reagent and perform stoichiometric calculations based on the balanced chemical equation:<\/p>\n\n\n\n Balanced Chemical Equation:<\/strong> Moles of salicylic acid:<\/strong> Moles of acetic anhydride:<\/strong> From the balanced equation, we can see that the molar ratio between salicylic acid and acetic anhydride is 2:1. This means that for every 2 moles of salicylic acid, we need 1 mole of acetic anhydride. Let’s check which reactant is limiting.<\/p>\n\n\n\n Since salicylic acid is the limiting reactant, we use its moles to calculate the theoretical yield of aspirin. According to the balanced equation, 2 moles of salicylic acid produce 2 moles of aspirin. Therefore, the moles of aspirin produced will be equal to the moles of salicylic acid:<\/p>\n\n\n\n [ Now, convert moles of aspirin to grams:<\/p>\n\n\n\n [ Thus, the theoretical yield<\/strong> of aspirin is 36.4 grams<\/strong>.<\/p>\n\n\n\n Percentage yield is calculated using the following formula:<\/p>\n\n\n\n [ Given that the actual yield<\/strong> of aspirin is 30.7 grams, the percentage yield is:<\/p>\n\n\n\n [ The percentage yield represents the efficiency of the reaction. In this case, 84.4% of the theoretical amount of aspirin was obtained, which is a relatively high yield, indicating the reaction was fairly efficient.<\/p>\n","protected":false},"excerpt":{"rendered":" In the synthesis of aspirin we react salicylic acid with acetic anhydride. The balanced chemical equation is: 2HOOCC6H4OH + C4H6O3 \u00c3\u00a2\u00e2\u20ac \u00e2\u20ac\u2122 2HOOCC6H4O2C2H3\u00c3\u201a\u00c2 + H2Osalicylic acid aceticanhydride \u00c3\u201a\u00c2 acetyl salicylic acid water If we mix together\u00c3\u201a\u00c2 \u00c3\u201a\u00c2 27.9\u00c3\u201a\u00c2 grams of salicylic acid with\u00c3\u201a\u00c2 \u00c3\u201a\u00c2 14.4\u00c3\u201a\u00c2 grams of acetic anhydride in this reaction, we obtain 30.7 […]<\/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-182624","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182624","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=182624"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182624\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182624"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182624"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182624"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
[ 2 \\text{HOOCC}_6\\text{H}_4\\text{OH (salicylic acid)} + \\text{C}_4\\text{H}_6\\text{O}_3 (\\text{acetic anhydride}) \\rightarrow 2 \\text{HOOCC}_6\\text{H}_4\\text{O}_2\\text{C}_2\\text{H}_3 (\\text{acetylsalicylic acid}) + \\text{H}_2\\text{O} ]<\/p>\n\n\n\nStep 1: Molar Masses<\/h3>\n\n\n\n
\n
Step 2: Moles of Each Reactant<\/h3>\n\n\n\n
[
\\text{moles of salicylic acid} = \\frac{27.9 \\, \\text{g}}{138.12 \\, \\text{g\/mol}} = 0.202 \\, \\text{mol}
]<\/p>\n\n\n\n
[
\\text{moles of acetic anhydride} = \\frac{14.4 \\, \\text{g}}{102.09 \\, \\text{g\/mol}} = 0.141 \\, \\text{mol}
]<\/p>\n\n\n\nStep 3: Limiting Reactant<\/h3>\n\n\n\n
\n
[
\\frac{0.202 \\, \\text{mol}}{2} = 0.101 \\, \\text{mol of acetic anhydride}
]<\/li>\n\n\n\nStep 4: Theoretical Yield<\/h3>\n\n\n\n
\\text{moles of aspirin} = 0.202 \\, \\text{mol}
]<\/p>\n\n\n\n
\\text{mass of aspirin} = 0.202 \\, \\text{mol} \\times 180.16 \\, \\text{g\/mol} = 36.4 \\, \\text{g}
]<\/p>\n\n\n\nStep 5: Percentage Yield<\/h3>\n\n\n\n
\\text{percentage yield} = \\left( \\frac{\\text{actual yield}}{\\text{theoretical yield}} \\right) \\times 100
]<\/p>\n\n\n\n
\\text{percentage yield} = \\left( \\frac{30.7 \\, \\text{g}}{36.4 \\, \\text{g}} \\right) \\times 100 = 84.4\\%
]<\/p>\n\n\n\nConclusion<\/h3>\n\n\n\n
\n