{"id":260507,"date":"2025-07-19T14:17:50","date_gmt":"2025-07-19T14:17:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=260507"},"modified":"2025-07-19T14:17:52","modified_gmt":"2025-07-19T14:17:52","slug":"what-is-the-mass-of-5-8-moles-of-h2s","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/19\/what-is-the-mass-of-5-8-moles-of-h2s\/","title":{"rendered":"what is the mass of 5.8 moles of H2S"},"content":{"rendered":"\n<p>what is the mass of 5.8 moles of H2S<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the mass of 5.8 moles of hydrogen sulfide (H\u2082S), the molecular weight of H\u2082S needs to be calculated. The molecular weight is the sum of the atomic weights of the atoms in the molecule. The atomic weight of hydrogen (H) is approximately 1.008 g\/mol, and the atomic weight of sulfur (S) is about 32.06 g\/mol.<\/p>\n\n\n\n<p>For H\u2082S:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>There are two hydrogen atoms, so the mass from hydrogen is 2\u00d71.008=2.016\u2009g\/mol2 \\times 1.008 = 2.016 \\, \\text{g\/mol}.<\/li>\n\n\n\n<li>The mass from sulfur is 32.06 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the molecular weight of H\u2082S is: Molecular&nbsp;weight&nbsp;of&nbsp;H\u2082S=2.016+32.06=34.076\u2009g\/mol.\\text{Molecular weight of H\u2082S} = 2.016 + 32.06 = 34.076 \\, \\text{g\/mol}.<\/p>\n\n\n\n<p>Now, to find the mass of 5.8 moles of H\u2082S, use the formula: Mass=moles\u00d7molecular&nbsp;weight.\\text{Mass} = \\text{moles} \\times \\text{molecular weight}.<\/p>\n\n\n\n<p>Substitute the given values: Mass=5.8\u2009moles\u00d734.076\u2009g\/mol=197.64\u2009g.\\text{Mass} = 5.8 \\, \\text{moles} \\times 34.076 \\, \\text{g\/mol} = 197.64 \\, \\text{g}.<\/p>\n\n\n\n<p>Thus, the mass of 5.8 moles of H\u2082S is approximately <strong>197.64 grams<\/strong>.<\/p>\n\n\n\n<p>This calculation follows from the basic principle that one mole of any substance contains Avogadro\u2019s number of molecules (approximately 6.022\u00d710236.022 \\times 10^{23} molecules), and the mass of one mole of a substance is its molecular weight in grams. This relationship allows for the conversion between moles and grams for any given substance.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>what is the mass of 5.8 moles of H2S The correct answer and explanation is: To find the mass of 5.8 moles of hydrogen sulfide (H\u2082S), the molecular weight of H\u2082S needs to be calculated. The molecular weight is the sum of the atomic weights of the atoms in the molecule. The atomic weight of [&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-260507","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260507","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=260507"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260507\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=260507"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=260507"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=260507"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}