What is the mass in grams of 6.21x 10^22 formula units of silver chloride? The molar mass of silver chloride is 143.3 grams\/mole.<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n To determine the mass in grams of (6.21 \\times 10^{22}) formula units of silver chloride (AgCl), we use the relationship between formula units, Avogadro\u2019s number, and molar mass.<\/p>\n\n\n\n Avogadro\u2019s number is: The number of moles of AgCl is calculated as:<\/p>\n\n\n\n [ [ [ Now, we multiply the number of moles by the molar mass of AgCl:<\/p>\n\n\n\n [ [ [ The mass of (6.21 \\times 10^{22}) formula units of silver chloride is 14.8 grams<\/strong>.<\/p>\n\n\n\n This problem involves basic stoichiometric principles. We first converted the given formula units into moles using Avogadro\u2019s number. Then, using the molar mass of silver chloride, we found the corresponding mass. Understanding these conversions is crucial in chemistry, as they allow for calculations involving substances at the atomic and molecular level.<\/p>\n","protected":false},"excerpt":{"rendered":" What is the mass in grams of 6.21x 10^22 formula units of silver chloride? The molar mass of silver chloride is 143.3 grams\/mole. The correct answer and explanation is : To determine the mass in grams of (6.21 \\times 10^{22}) formula units of silver chloride (AgCl), we use the relationship between formula units, Avogadro\u2019s number, […]<\/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-201901","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201901","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=201901"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201901\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201901"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201901"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201901"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Use Avogadro\u2019s Number<\/strong><\/h3>\n\n\n\n
[
6.022 \\times 10^{23} \\text{ formula units per mole}
]
This means that one mole of AgCl contains (6.022 \\times 10^{23}) formula units.<\/p>\n\n\n\nStep 2: Determine the Number of Moles<\/strong><\/h3>\n\n\n\n
\\text{Moles of AgCl} = \\frac{\\text{Formula Units of AgCl}}{\\text{Avogadro’s Number}}
]<\/p>\n\n\n\n
= \\frac{6.21 \\times 10^{22}}{6.022 \\times 10^{23}}
]<\/p>\n\n\n\n
= 0.1032 \\text{ moles}
]<\/p>\n\n\n\nStep 3: Convert to Mass<\/strong><\/h3>\n\n\n\n
\\text{Mass} = \\text{Moles} \\times \\text{Molar Mass}
]<\/p>\n\n\n\n
= 0.1032 \\times 143.3
]<\/p>\n\n\n\n
= 14.8 \\text{ grams}
]<\/p>\n\n\n\nFinal Answer:<\/strong><\/h3>\n\n\n\n
Explanation:<\/strong><\/h3>\n\n\n\n