Which weighs more, 5.00 g or 0.0225 mol of acetaminophen 1C8H9NO 22?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine which weighs more between 5.00 grams and 0.0225 moles of acetaminophen (C\u2088H\u2089NO\u2082), we first need to calculate the mass of 0.0225 moles of acetaminophen. To do this, we need to know the molar mass of acetaminophen.<\/p>\n\n\n\n The molecular formula of acetaminophen is C\u2088H\u2089NO\u2082. To find the molar mass, we sum up the atomic masses of each element in the molecule:<\/p>\n\n\n\n So, the molar mass of acetaminophen is:<\/p>\n\n\n\n [ Now, to find the mass of 0.0225 moles of acetaminophen, we use the formula:<\/p>\n\n\n\n [ Substituting the values:<\/p>\n\n\n\n [ We are comparing:<\/p>\n\n\n\n Clearly, 5.00 g weighs more than 3.4 g.<\/p>\n\n\n\n Therefore, 5.00 g<\/strong> weighs more than 0.0225 moles of acetaminophen<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" Which weighs more, 5.00 g or 0.0225 mol of acetaminophen 1C8H9NO 22? The Correct Answer and Explanation is : To determine which weighs more between 5.00 grams and 0.0225 moles of acetaminophen (C\u2088H\u2089NO\u2082), we first need to calculate the mass of 0.0225 moles of acetaminophen. To do this, we need to know the molar mass […]<\/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-188622","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188622","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=188622"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188622\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=188622"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=188622"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=188622"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Calculate the Molar Mass of Acetaminophen<\/h3>\n\n\n\n
\n
(8 \\times 12.01) + (9 \\times 1.008) + (1 \\times 14.01) + (2 \\times 16.00)
]
[
= 96.08 + 9.072 + 14.01 + 32.00 = 151.16 \\, \\text{g\/mol}
]<\/p>\n\n\n\nStep 2: Calculate the Mass of 0.0225 Moles of Acetaminophen<\/h3>\n\n\n\n
\\text{Mass} = \\text{Moles} \\times \\text{Molar Mass}
]<\/p>\n\n\n\n
\\text{Mass} = 0.0225 \\, \\text{mol} \\times 151.16 \\, \\text{g\/mol} = 3.4 \\, \\text{g}
]<\/p>\n\n\n\nStep 3: Compare the Two Quantities<\/h3>\n\n\n\n
\n
Conclusion<\/h3>\n\n\n\n