{"id":253658,"date":"2025-07-12T06:26:26","date_gmt":"2025-07-12T06:26:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=253658"},"modified":"2025-07-12T06:26:28","modified_gmt":"2025-07-12T06:26:28","slug":"how-many-moles-of-butane-c4h10-are-found-in-392-3-grams-of-c4h10-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/12\/how-many-moles-of-butane-c4h10-are-found-in-392-3-grams-of-c4h10-2\/","title":{"rendered":"How many moles of butane, C4H10, are found in 392.3 grams of C4H10"},"content":{"rendered":"\n

How many moles of butane, C4H10, are found in 392.3 grams of C4H10?<\/p>\n\n\n\n

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

To calculate the number of moles of butane (C4H10) in 392.3 grams, we follow these steps:<\/p>\n\n\n\n

    \n
  1. Determine the molar mass of butane (C4H10):<\/strong>
    The molar mass is calculated by adding the atomic masses of all the elements in the formula C4H10.
    • Carbon (C) has an atomic mass of approximately 12.01 grams per mole.<\/li>
    • Hydrogen (H) has an atomic mass of approximately 1.008 grams per mole.<\/li><\/ul>The molar mass of butane is: 4\u00d712.01\u2009g\/mol+10\u00d71.008\u2009g\/mol=48.04\u2009g\/mol+10.08\u2009g\/mol=58.12\u2009g\/mol4 \\times 12.01 \\, \\text{g\/mol} + 10 \\times 1.008 \\, \\text{g\/mol} = 48.04 \\, \\text{g\/mol} + 10.08 \\, \\text{g\/mol} = 58.12 \\, \\text{g\/mol}<\/li>\n\n\n\n
    • Use the formula for moles:<\/strong>
      The formula to calculate the number of moles (n) from mass (m) is: n=mMn = \\frac{m}{M} where:\n
        \n
      • nn is the number of moles,<\/li>\n\n\n\n
      • mm is the mass of the substance (392.3 grams), and<\/li>\n\n\n\n
      • MM is the molar mass (58.12 g\/mol).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Calculate the number of moles:<\/strong>
        Now we can substitute the values into the formula: n=392.3\u2009g58.12\u2009g\/mol\u22486.74\u2009moln = \\frac{392.3 \\, \\text{g}}{58.12 \\, \\text{g\/mol}} \\approx 6.74 \\, \\text{mol}<\/li>\n<\/ol>\n\n\n\n

        So, the number of moles of butane in 392.3 grams is approximately 6.74 moles<\/strong>.<\/p>\n\n\n\n

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

        Moles are a fundamental concept in chemistry used to count the number of particles in a substance, whether atoms, molecules, or ions. The molar mass tells you how much one mole of a substance weighs in grams. By dividing the mass of a substance by its molar mass, we determine how many moles are in that mass. This is a key conversion factor in stoichiometry, enabling chemists to quantify reactants and products in chemical reactions. The calculation involves basic knowledge of atomic weights and the molar concept, providing a way to work with microscopic particles on a macroscopic scale.<\/p>\n","protected":false},"excerpt":{"rendered":"

        How many moles of butane, C4H10, are found in 392.3 grams of C4H10? The correct answer and explanation is: To calculate the number of moles of butane (C4H10) in 392.3 grams, we follow these steps: So, the number of moles of butane in 392.3 grams is approximately 6.74 moles. Explanation: Moles are a fundamental concept […]<\/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-253658","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253658","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=253658"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253658\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=253658"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=253658"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=253658"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}