{"id":194991,"date":"2025-02-25T10:47:28","date_gmt":"2025-02-25T10:47:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194991"},"modified":"2025-02-25T10:47:54","modified_gmt":"2025-02-25T10:47:54","slug":"what-is-the-mass-of-a-sulfur-hexafluoride-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/25\/what-is-the-mass-of-a-sulfur-hexafluoride-molecule\/","title":{"rendered":"What is the mass of a sulfur hexafluoride molecule"},"content":{"rendered":"\n<p>What is the mass of a sulfur hexafluoride molecule  <\/p>\n\n\n\n<p>___grams<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>The mass of a single sulfur hexafluoride (SF\u2086) molecule is <strong>146.06 atomic mass units (amu)<\/strong>. To convert this into grams, we use Avogadro\u2019s number ( (6.022 \\times 10^{23}) ), which tells us how many molecules are in one mole:<\/p>\n\n\n\n<p>[<br>\\frac{146.06 \\text{ g\/mol}}{6.022 \\times 10^{23} \\text{ molecules\/mol}}<br>]<\/p>\n\n\n\n<p>[<br>= 2.43 \\times 10^{-22} \\text{ grams per molecule}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Molecular Weight Calculation<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur (S) has an atomic mass of <strong>32.06 amu<\/strong>.<\/li>\n\n\n\n<li>Fluorine (F) has an atomic mass of <strong>18.998 amu<\/strong>.<\/li>\n\n\n\n<li>Since there are <strong>six fluorine atoms<\/strong>, their total mass is:<br>[<br>6 \\times 18.998 = 113.99 \\text{ amu}<br>]<\/li>\n\n\n\n<li>Adding the mass of sulfur:<br>[<br>32.06 + 113.99 = 146.06 \\text{ amu}<br>]<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Conversion to Grams<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The molecular weight of SF\u2086 is <strong>146.06 g\/mol<\/strong>, meaning <strong>one mole<\/strong> (i.e., ( 6.022 \\times 10^{23} ) molecules) weighs <strong>146.06 grams<\/strong>.<\/li>\n\n\n\n<li>To find the mass of a single molecule, we divide by Avogadro\u2019s number:<br>[<br>\\frac{146.06}{6.022 \\times 10^{23}} = 2.43 \\times 10^{-22} \\text{ g}<br>]<\/li>\n<\/ul>\n\n\n\n<p>Thus, the mass of one sulfur hexafluoride molecule is <strong>(2.43 \\times 10^{-22}) grams<\/strong>.<\/p>\n\n\n\n<p>Now, I will generate an image representing the molecular structure of sulfur hexafluoride.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1501.png\" alt=\"\" class=\"wp-image-194992\"\/><\/figure>\n\n\n\n<p>Here is the 3D molecular structure of sulfur hexafluoride (SF\u2086). It shows the sulfur atom at the center with six fluorine atoms symmetrically arranged in an octahedral geometry. Let me know if you need any modifications!<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the mass of a sulfur hexafluoride molecule ___grams The Correct Answer and Explanation is : The mass of a single sulfur hexafluoride (SF\u2086) molecule is 146.06 atomic mass units (amu). To convert this into grams, we use Avogadro\u2019s number ( (6.022 \\times 10^{23}) ), which tells us how many molecules are in one [&hellip;]<\/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-194991","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194991","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=194991"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194991\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194991"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194991"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194991"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}