{"id":168642,"date":"2024-11-17T19:50:43","date_gmt":"2024-11-17T19:50:43","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=168642"},"modified":"2024-11-17T19:50:45","modified_gmt":"2024-11-17T19:50:45","slug":"79-2-g-of-c14h30-is-cracked-to-produce-40-0-g-of-c7h16-17-6-g-of-c3h8-and-22-4-g-of-c2h4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/17\/79-2-g-of-c14h30-is-cracked-to-produce-40-0-g-of-c7h16-17-6-g-of-c3h8-and-22-4-g-of-c2h4\/","title":{"rendered":"79.2 g of C14H30 is cracked to produce 40.0 g of C7H16, 17.6 g of C3H8, and 22.4 g of C2H4."},"content":{"rendered":"\n

79.2 g of C14H30 is cracked to produce 40.0 g of C7H16, 17.6 g of C3H8, and 22.4 g of C2H4. Options: a) The molar mass of C14H30 is 210 g\/mol. b) The cracking process is an example of a combustion reaction. c) The molar mass of C7H16 is 100 g\/mol. d) The molar mass of C3H8 is 44 g\/mol.<\/p>\n\n\n\n

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

The correct answer is d) The molar mass of C3H8 is 44 g\/mol.<\/strong><\/p>\n\n\n\n

Here\u2019s an explanation for each option:<\/p>\n\n\n\n

    \n
  1. Option a: The molar mass of C14H30 is 210 g\/mol.<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • To determine the molar mass of C14H30, we add up the atomic masses of carbon and hydrogen.\n
        \n
      • Carbon (C) has an atomic mass of 12 g\/mol, and hydrogen (H) has an atomic mass of 1 g\/mol.<\/li>\n\n\n\n
      • So, the molar mass of C14H30 is:
        [
        (14 \\times 12) + (30 \\times 1) = 168 + 30 = 198 \\text{ g\/mol}.
        ]<\/li>\n\n\n\n
      • Since 198 g\/mol is not equal to 210 g\/mol, this option is incorrect.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
          \n
        1. Option b: The cracking process is an example of a combustion reaction.<\/strong><\/li>\n<\/ol>\n\n\n\n
            \n
          • Combustion reactions typically involve the burning of a substance with oxygen, producing carbon dioxide and water.<\/li>\n\n\n\n
          • Cracking, however, is a process where large hydrocarbons like C14H30 are broken down into smaller molecules (like C7H16, C3H8, and C2H4) and does not require oxygen. This makes cracking a type of decomposition reaction, not combustion. Therefore, this option is incorrect.<\/li>\n<\/ul>\n\n\n\n
              \n
            1. Option c: The molar mass of C7H16 is 100 g\/mol.<\/strong><\/li>\n<\/ol>\n\n\n\n
                \n
              • We can calculate the molar mass of C7H16:
                [
                (7 \\times 12) + (16 \\times 1) = 84 + 16 = 100 \\text{ g\/mol}.
                ]<\/li>\n\n\n\n
              • This is correct, but it does not relate to the other calculations in this particular question, so it\u2019s not the answer we\u2019re looking for.<\/li>\n<\/ul>\n\n\n\n
                  \n
                1. Option d: The molar mass of C3H8 is 44 g\/mol.<\/strong><\/li>\n<\/ol>\n\n\n\n
                    \n
                  • We calculate the molar mass of C3H8:
                    [
                    (3 \\times 12) + (8 \\times 1) = 36 + 8 = 44 \\text{ g\/mol}.
                    ]<\/li>\n\n\n\n
                  • This is correct, and since the molar mass of C3H8 is directly given in the question as part of the options, this is the correct answer.<\/li>\n<\/ul>\n\n\n\n

                    Thus, option d<\/strong> is the correct choice.<\/p>\n","protected":false},"excerpt":{"rendered":"

                    79.2 g of C14H30 is cracked to produce 40.0 g of C7H16, 17.6 g of C3H8, and 22.4 g of C2H4. Options: a) The molar mass of C14H30 is 210 g\/mol. b) The cracking process is an example of a combustion reaction. c) The molar mass of C7H16 is 100 g\/mol. d) The molar mass […]<\/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-168642","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168642","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=168642"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168642\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=168642"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=168642"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=168642"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}