{"id":199334,"date":"2025-03-11T15:21:48","date_gmt":"2025-03-11T15:21:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199334"},"modified":"2025-03-11T15:21:51","modified_gmt":"2025-03-11T15:21:51","slug":"the-empirical-formula-for-copper-sulfide-is-cus-cu2s-cu2s2-cus2-the-percent-compositon-of-copper-sulfide-is-50-copper-and-50sulfur-54-copper-and-46-sulfur-80-copper-and-20-sulfur-20-copper-and-80-sulf","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/11\/the-empirical-formula-for-copper-sulfide-is-cus-cu2s-cu2s2-cus2-the-percent-compositon-of-copper-sulfide-is-50-copper-and-50sulfur-54-copper-and-46-sulfur-80-copper-and-20-sulfur-20-copper-and-80-sulf\/","title":{"rendered":"The empirical formula for copper sulfide is CuS Cu2S Cu2S2 CuS2 the percent compositon of copper sulfide is 50% copper and 50%sulfur 54% copper and 46% sulfur 80% copper and 20% sulfur 20% copper and 80% sulfur"},"content":{"rendered":"\n

The empirical formula for copper sulfide is CuS Cu2S Cu2S2 CuS2 the percent compositon of copper sulfide is 50% copper and 50%sulfur 54% copper and 46% sulfur 80% copper and 20% sulfur 20% copper and 80% sulfur<\/p>\n\n\n\n

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

The correct empirical formula for copper sulfide depends on the experimental determination of its composition. However, the most common forms of copper sulfide are CuS<\/strong> and Cu\u2082S<\/strong>.<\/p>\n\n\n\n

The correct answer for the percent composition of copper sulfide<\/strong> is:
Cu\u2082S (Copper(I) sulfide) with 80% Copper and 20% Sulfur.<\/strong><\/p>\n\n\n\n

\n\n\n\n

Explanation<\/strong><\/h3>\n\n\n\n

The empirical formula represents the simplest whole-number ratio of atoms in a compound. Copper sulfide exists in different forms, but we will analyze the percent composition of Cu\u2082S<\/strong>.<\/p>\n\n\n\n

Step 1: Determine the Molar Mass of Cu\u2082S<\/strong><\/h4>\n\n\n\n
    \n
  • Copper (Cu) atomic mass = 63.55 g\/mol<\/strong><\/li>\n\n\n\n
  • Sulfur (S) atomic mass = 32.07 g\/mol<\/strong><\/li>\n\n\n\n
  • Cu\u2082S contains 2 copper atoms<\/strong> and 1 sulfur atom<\/strong>:<\/li>\n<\/ul>\n\n\n\n

    [
    \\text{Molar mass of Cu\u2082S} = (2 \\times 63.55) + (1 \\times 32.07)
    ]<\/p>\n\n\n\n

    [
    = 127.10 + 32.07 = 159.17 \\text{ g\/mol}
    ]<\/p>\n\n\n\n

    Step 2: Calculate Percent Composition<\/strong><\/h4>\n\n\n\n
      \n
    • % Copper<\/strong> =
      [
      \\left( \\frac{127.10}{159.17} \\right) \\times 100 = 79.9\\% \\approx 80\\%
      ]<\/li>\n\n\n\n
    • % Sulfur<\/strong> =
      [
      \\left( \\frac{32.07}{159.17} \\right) \\times 100 = 20.1\\% \\approx 20\\%
      ]<\/li>\n<\/ul>\n\n\n\n

      Thus, the percent composition of Cu\u2082S is approximately 80% copper and 20% sulfur<\/strong>, making it the correct answer.<\/p>\n\n\n\n

      \n\n\n\n

      Why Other Options Are Incorrect?<\/strong><\/h3>\n\n\n\n
        \n
      • CuS (Copper(II) sulfide) has 54% Cu and 46% S<\/strong>, so it is incorrect.<\/li>\n\n\n\n
      • CuS\u2082 and Cu\u2082S\u2082 are not standard empirical formulas<\/strong> and do not match the given choices.<\/li>\n<\/ul>\n\n\n\n

        Thus, the correct empirical formula<\/strong> is Cu\u2082S<\/strong> with 80% Copper and 20% Sulfur<\/strong>.<\/p>\n\n\n\n

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

        Here is the scientific diagram illustrating the composition of Copper(I) Sulfide (Cu\u2082S), showing the molecular representation, atomic masses, and percentage composition. <\/p>\n","protected":false},"excerpt":{"rendered":"

        The empirical formula for copper sulfide is CuS Cu2S Cu2S2 CuS2 the percent compositon of copper sulfide is 50% copper and 50%sulfur 54% copper and 46% sulfur 80% copper and 20% sulfur 20% copper and 80% sulfur The correct answer and explanation is : The correct empirical formula for copper sulfide depends on the experimental […]<\/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-199334","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199334","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=199334"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199334\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199334"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199334"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199334"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}