What is the mass of 2.31 x 1023 formula units of SrF2?<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The correct answer is: 48.19 grams<\/strong><\/p>\n\n\n\n To find the mass of 2.31 \u00d7 10\u00b2\u00b3 formula units of SrF\u2082 (strontium fluoride), follow these steps:<\/p>\n\n\n\n SrF\u2082 consists of one strontium (Sr) atom and two fluorine (F) atoms.<\/p>\n\n\n\n The molar mass of SrF\u2082 is calculated by adding the mass of one Sr atom and two F atoms:<\/p>\n\n\n\n [ Use Avogadro’s number (6.022 \u00d7 10\u00b2\u00b3 formula units\/mol) to convert from formula units to moles. This step is important because molar mass relates grams to moles.<\/p>\n\n\n\n [ Now, multiply the number of moles by the molar mass to get the mass in grams:<\/p>\n\n\n\n [ The key to solving this problem is converting the given number of formula units into moles using Avogadro\u2019s number, which provides the connection between the number of particles and the amount of substance in moles. From there, using the molar mass of SrF\u2082, we can calculate the mass. The molar mass represents the mass of one mole of SrF\u2082 formula units, and since the number of formula units given is a fraction of a mole, we scale the mass accordingly.<\/p>\n\n\n\n In summary, 2.31 \u00d7 10\u00b2\u00b3 formula units of SrF\u2082 corresponds to approximately 48.19 grams<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":" What is the mass of 2.31 x 1023 formula units of SrF2? The Correct Answer and Explanation is : The correct answer is: 48.19 grams To find the mass of 2.31 \u00d7 10\u00b2\u00b3 formula units of SrF\u2082 (strontium fluoride), follow these steps: Step 1: Calculate the molar mass of SrF\u2082. SrF\u2082 consists of one strontium […]<\/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-150186","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/150186","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=150186"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/150186\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=150186"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=150186"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=150186"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Calculate the molar mass of SrF\u2082.<\/h3>\n\n\n\n
\n
Molar\\ mass\\ of\\ SrF_2 = (87.62\\ g\/mol) + 2 \\times (18.998\\ g\/mol) = 125.616\\ g\/mol
]<\/p>\n\n\n\nStep 2: Convert the number of formula units to moles.<\/h3>\n\n\n\n
\\frac{2.31 \\times 10^{23}\\ formula\\ units}{6.022 \\times 10^{23}\\ formula\\ units\/mol} = 0.3837\\ mol
]<\/p>\n\n\n\nStep 3: Calculate the mass of SrF\u2082.<\/h3>\n\n\n\n
mass\\ of\\ SrF_2 = 0.3837\\ mol \\times 125.616\\ g\/mol = 48.19\\ g
]<\/p>\n\n\n\nExplanation:<\/h3>\n\n\n\n