{"id":194380,"date":"2025-02-24T05:16:42","date_gmt":"2025-02-24T05:16:42","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194380"},"modified":"2025-02-24T05:16:46","modified_gmt":"2025-02-24T05:16:46","slug":"the-empirical-formula-for-a-compound-is-ch2o","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/24\/the-empirical-formula-for-a-compound-is-ch2o\/","title":{"rendered":"The empirical formula for a compound is CH2O"},"content":{"rendered":"\n

The empirical formula for a compound is CH2O. The compound has a molar mass of 90.1 g\/mol. Determine the molecular formula for the compound.<\/p>\n\n\n\n

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

Solution: Determining the Molecular Formula<\/strong><\/h3>\n\n\n\n

Step 1: Determine the Empirical Formula Mass<\/strong><\/h4>\n\n\n\n

The empirical formula of the compound is CH\u2082O<\/strong>. To find its empirical formula mass, we sum the atomic masses of its constituent elements:<\/p>\n\n\n\n

    \n
  • Carbon (C): 12.01 g\/mol<\/strong><\/li>\n\n\n\n
  • Hydrogen (H): 2 \u00d7 1.008 g\/mol<\/strong> = 2.016 g\/mol<\/strong><\/li>\n\n\n\n
  • Oxygen (O): 16.00 g\/mol<\/strong><\/li>\n<\/ul>\n\n\n\n

    Empirical formula mass = 12.01 + 2.016 + 16.00 = 30.03 g\/mol<\/strong><\/p>\n\n\n\n

    Step 2: Find the Molecular Formula Factor<\/strong><\/h4>\n\n\n\n

    To determine the molecular formula, we use the given molar mass of the compound (90.1 g\/mol<\/strong>) and divide it by the empirical formula mass:<\/p>\n\n\n\n

    [
    \\frac{\\text{Molar Mass}}{\\text{Empirical Formula Mass}} = \\frac{90.1}{30.03} \\approx 3
    ]<\/p>\n\n\n\n

    This means that the molecular formula is 3 times<\/strong> the empirical formula.<\/p>\n\n\n\n

    Step 3: Determine the Molecular Formula<\/strong><\/h4>\n\n\n\n

    Now, we multiply each subscript in CH\u2082O<\/strong> by 3<\/strong>:<\/p>\n\n\n\n

      \n
    • Carbon: C \u00d7 3 = C\u2083<\/strong><\/li>\n\n\n\n
    • Hydrogen: H\u2082 \u00d7 3 = H\u2086<\/strong><\/li>\n\n\n\n
    • Oxygen: O \u00d7 3 = O\u2083<\/strong><\/li>\n<\/ul>\n\n\n\n

      Thus, the molecular formula<\/strong> of the compound is C\u2083H\u2086O\u2083<\/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. However, the molecular formula provides the actual number of atoms in a molecule. The molecular formula is a multiple of the empirical formula. In this case, the empirical formula CH\u2082O<\/strong> has a mass of 30.03 g\/mol<\/strong>, and the given molecular mass is 90.1 g\/mol<\/strong>. Since 90.1 \/ 30.03 \u2248 3<\/strong>, we scale up the empirical formula by a factor of 3<\/strong>, leading to the molecular formula C\u2083H\u2086O\u2083<\/strong>. This formula corresponds to molecules like glyceraldehyde or lactic acid, which are biologically significant compounds.<\/p>\n\n\n\n

      Now, let’s generate an image representing this molecular structure.<\/p>\n\n\n\n

      Here is a 3D molecular model of C\u2083H\u2086O\u2083<\/strong>, illustrating the atomic arrangement with Carbon (black), Hydrogen (white), and Oxygen (red). The structure represents a common molecular form like lactic acid. Let me know if you need any modifications or explanations!<\/p>\n\n\n\n

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

      The empirical formula for a compound is CH2O. The compound has a molar mass of 90.1 g\/mol. Determine the molecular formula for the compound. The Correct Answer and Explanation is : Solution: Determining the Molecular Formula Step 1: Determine the Empirical Formula Mass The empirical formula of the compound is CH\u2082O. To find its empirical […]<\/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-194380","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194380","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=194380"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194380\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194380"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194380"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194380"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}