{"id":198713,"date":"2025-03-10T09:11:43","date_gmt":"2025-03-10T09:11:43","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198713"},"modified":"2025-03-10T09:11:57","modified_gmt":"2025-03-10T09:11:57","slug":"the-chemical-formula-for-barium-sulfide-is-bas-3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/the-chemical-formula-for-barium-sulfide-is-bas-3\/","title":{"rendered":"The chemical formula for barium sulfide is BaS"},"content":{"rendered":"\n

The chemical formula for barium sulfide is BaS. <\/p>\n\n\n\n

A chemist measured the amount of barium sulfide produced during an experiment. She finds that 11.7 g of barium sulfide is produced. Calculate the number of moles of barium sulfide produced.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The number of moles of barium sulfide (BaS) produced is 0.0691 moles<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

To calculate the number of moles of a substance, we use the formula:<\/p>\n\n\n\n

[
\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}
]<\/p>\n\n\n\n

Step 1: Identify Given Data<\/h4>\n\n\n\n
    \n
  • Mass of BaS produced<\/strong> = 11.7 g<\/li>\n\n\n\n
  • Molar mass of BaS<\/strong> = Sum of atomic masses of barium (Ba) and sulfur (S)<\/li>\n\n\n\n
  • Barium (Ba):<\/strong> 137.33 g\/mol<\/li>\n\n\n\n
  • Sulfur (S):<\/strong> 32.07 g\/mol<\/li>\n\n\n\n
  • Total molar mass of BaS<\/strong> = ( 137.33 + 32.07 = 169.40 ) g\/mol<\/li>\n<\/ul>\n\n\n\n

    Step 2: Calculate the Moles<\/h4>\n\n\n\n

    Using the formula:<\/p>\n\n\n\n

    [
    \\text{Moles of BaS} = \\frac{11.7 \\text{ g}}{169.40 \\text{ g\/mol}}
    ]<\/p>\n\n\n\n

    [
    = 0.0691 \\text{ moles}
    ]<\/p>\n\n\n\n

    Step 3: Interpretation<\/h4>\n\n\n\n

    This means that in the experiment, 0.0691 moles<\/strong> of BaS were formed. The mole is a fundamental unit in chemistry that helps in quantifying the amount of a substance based on Avogadro\u2019s number (6.022 \\times 10^{23}) entities per mole. This calculation is essential in stoichiometric reactions to understand the reactant-to-product relationships.<\/p>\n\n\n\n

    \"\"<\/figure>\n\n\n\n

    Here is the scientific illustration depicting the calculation of moles for barium sulfide (BaS), including a step-by-step breakdown of the process. <\/p>\n","protected":false},"excerpt":{"rendered":"

    The chemical formula for barium sulfide is BaS. A chemist measured the amount of barium sulfide produced during an experiment. She finds that 11.7 g of barium sulfide is produced. Calculate the number of moles of barium sulfide produced. The correct answer and explanation is : The number of moles of barium sulfide (BaS) produced […]<\/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-198713","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198713","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=198713"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198713\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198713"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198713"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198713"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}