{"id":183781,"date":"2025-01-17T05:54:24","date_gmt":"2025-01-17T05:54:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183781"},"modified":"2025-01-17T05:54:26","modified_gmt":"2025-01-17T05:54:26","slug":"what-is-the-heat-of-combustion-of-ethane-c2h6-in-kilojoules-per-mole-of-ethane","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/17\/what-is-the-heat-of-combustion-of-ethane-c2h6-in-kilojoules-per-mole-of-ethane\/","title":{"rendered":"What is the heat of combustion of ethane, C2H6, in kilojoules per mole of ethane"},"content":{"rendered":"\n

What is the heat of combustion of ethane, C2H6, in kilojoules per mole of ethane?<\/p>\n\n\n\n

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

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

The heat of combustion of ethane (C2H6C_2H_6) is \u22121560\u2009kJ\/mol-1560 \\, \\text{kJ\/mol}. This value represents the energy released when one mole of ethane undergoes complete combustion in the presence of excess oxygen, forming carbon dioxide (CO2CO_2) and water (H2OH_2O).<\/p>\n\n\n\n

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

1. Combustion Reaction of Ethane<\/strong><\/h4>\n\n\n\n

The balanced chemical equation for the combustion of ethane is: C2H6+72O2\u21922CO2+3H2OC_2H_6 + \\frac{7}{2} O_2 \\rightarrow 2 CO_2 + 3 H_2O<\/p>\n\n\n\n

In this reaction:<\/p>\n\n\n\n

    \n
  • Ethane reacts with oxygen.<\/li>\n\n\n\n
  • Carbon is oxidized to CO2CO_2, and hydrogen is oxidized to H2OH_2O.<\/li>\n<\/ul>\n\n\n\n

    2. Heat of Combustion Definition<\/strong><\/h4>\n\n\n\n

    The heat of combustion is the energy released when one mole of a substance is completely burned in oxygen. It is always a negative value (exothermic process) because energy is released.<\/p>\n\n\n\n

    3. Bond Energies and Enthalpy Changes<\/strong><\/h4>\n\n\n\n

    The heat of combustion can be calculated from bond enthalpies:<\/p>\n\n\n\n

      \n
    • Energy is required to break the bonds in C2H6C_2H_6 and O2O_2.<\/li>\n\n\n\n
    • Energy is released when new bonds are formed in CO2CO_2 and H2OH_2O.<\/li>\n<\/ul>\n\n\n\n

      Net energy change = Energy released – Energy absorbed.<\/p>\n\n\n\n

      From bond enthalpy tables, the experimentally determined value for ethane\u2019s combustion is \u22121560\u2009kJ\/mol-1560 \\, \\text{kJ\/mol}.<\/p>\n\n\n\n

      4. Energy Significance<\/strong><\/h4>\n\n\n\n

      This value is significant for understanding:<\/p>\n\n\n\n

        \n
      • Fuel efficiency<\/strong>: Ethane is a high-energy fuel used in industrial applications.<\/li>\n\n\n\n
      • Environmental impact<\/strong>: Combustion releases CO2CO_2, contributing to the greenhouse effect.<\/li>\n<\/ul>\n\n\n\n

        5. Practical Application<\/strong><\/h4>\n\n\n\n

        Knowing the heat of combustion is crucial for designing combustion systems, calculating energy outputs, and evaluating fuel alternatives.<\/p>\n","protected":false},"excerpt":{"rendered":"

        What is the heat of combustion of ethane, C2H6, in kilojoules per mole of ethane? The Correct Answer and Explanation is : The heat of combustion of ethane (C2H6C_2H_6) is \u22121560\u2009kJ\/mol-1560 \\, \\text{kJ\/mol}. This value represents the energy released when one mole of ethane undergoes complete combustion in the presence of excess oxygen, forming carbon […]<\/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-183781","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183781","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=183781"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183781\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183781"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183781"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183781"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}