{"id":189904,"date":"2025-02-11T03:50:06","date_gmt":"2025-02-11T03:50:06","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189904"},"modified":"2025-02-11T03:50:09","modified_gmt":"2025-02-11T03:50:09","slug":"the-chemical-formula-for-barium-sulfide-is-bas","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/11\/the-chemical-formula-for-barium-sulfide-is-bas\/","title":{"rendered":"The Chemical Formula For Barium Sulfide Is Bas"},"content":{"rendered":"\n

The Chemical Formula For Barium Sulfide Is Bas. A Chemist Determined By Measurements That 0.085 Moles Of Barium Sulfide Participate In A Chemical Reaction. Calculate The Mass Of Barium Sulfide That Participates Be Sure Your Answer Has The Correct Number Of Significant Digits. D. ?<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

To calculate the mass of barium sulfide (BaS) that participates in a chemical reaction, we need to follow the steps of converting moles into grams. The formula for this conversion is:<\/p>\n\n\n\n

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

Step-by-Step Calculation<\/h3>\n\n\n\n
    \n
  1. Find the Molar Mass of Barium Sulfide (BaS):<\/strong>
    The molar mass of a compound is the sum of the molar masses of its individual elements. From the periodic table:<\/li>\n<\/ol>\n\n\n\n
      \n
    • The atomic mass of barium (Ba) is approximately 137.33 g\/mol.<\/li>\n\n\n\n
    • The atomic mass of sulfur (S) is approximately 32.07 g\/mol. So, the molar mass of BaS is: [
      137.33 \\, \\text{g\/mol (Ba)} + 32.07 \\, \\text{g\/mol (S)} = 169.4 \\, \\text{g\/mol}
      ]<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Use the Given Moles of Barium Sulfide:<\/strong>
        The problem states that 0.085 moles of BaS participate in the reaction.<\/li>\n\n\n\n
      2. Calculate the Mass:<\/strong>
        Now that we know the molar mass of BaS (169.4 g\/mol) and the moles of BaS (0.085 moles), we can calculate the mass: [
        \\text{Mass} = 0.085 \\, \\text{moles} \\times 169.4 \\, \\text{g\/mol} = 14.39 \\, \\text{grams}
        ]<\/li>\n<\/ol>\n\n\n\n

        Final Answer:<\/h3>\n\n\n\n

        The mass of barium sulfide (BaS) that participates in the reaction is 14.39 grams<\/strong>.<\/p>\n\n\n\n

        Significant Figures:<\/h3>\n\n\n\n
          \n
        • The given data (0.085 moles) has 2 significant digits.<\/li>\n\n\n\n
        • The molar mass of BaS is given with 4 significant digits, so the final answer should be rounded to 2 significant digits to match the least precise value (0.085 moles).<\/li>\n<\/ul>\n\n\n\n

          Thus, the final mass is 14 grams<\/strong> (rounded to two significant digits).<\/p>\n\n\n\n

          Now, I will generate an image to visualize the chemical reaction and calculations.<\/p>\n\n\n\n

          Here is the illustration that shows the process of converting moles of Barium Sulfide (BaS) into mass. It includes the calculation steps and labels for clarity.<\/p>\n\n\n\n

          Let me know if you need any further explanations!<\/p>\n\n\n\n

          \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

          The Chemical Formula For Barium Sulfide Is Bas. A Chemist Determined By Measurements That 0.085 Moles Of Barium Sulfide Participate In A Chemical Reaction. Calculate The Mass Of Barium Sulfide That Participates Be Sure Your Answer Has The Correct Number Of Significant Digits. D. ? The Correct Answer and Explanation is : To calculate the […]<\/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-189904","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189904","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=189904"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189904\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189904"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189904"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189904"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}