{"id":196754,"date":"2025-03-05T19:47:12","date_gmt":"2025-03-05T19:47:12","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196754"},"modified":"2025-03-05T19:47:56","modified_gmt":"2025-03-05T19:47:56","slug":"given-the-following-equation-2-c4h10-13-o2-8-co2-10-h2o","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/05\/given-the-following-equation-2-c4h10-13-o2-8-co2-10-h2o\/","title":{"rendered":"Given the following equation: 2 C4H10 + 13 O2 &#8212;> 8 CO2 + 10 H2O"},"content":{"rendered":"\n<p>Given the following equation: 2 C4H10 + 13 O2 &#8212;> 8 CO2 + 10 H2O, show what the following molar ratios should be. <\/p>\n\n\n\n<p>a. C4H10 \/ O2 <\/p>\n\n\n\n<p>b. O2 \/ CO2<\/p>\n\n\n\n<p> c. O2 \/ H2O <\/p>\n\n\n\n<p>d. C4H10 \/ CO2<\/p>\n\n\n\n<p> e. C4H10 \/ H2O 2.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-281.png\" alt=\"\" class=\"wp-image-196755\"\/><\/figure>\n\n\n\n<p>The balanced chemical equation for the combustion of butane (C\u2084H\u2081\u2080) is:\ue206<\/p>\n\n\n\n<p>2 C\u2084H\u2081\u2080 + 13 O\u2082 \u27f6 8 CO\u2082 + 10 H\u2082O\ue206<\/p>\n\n\n\n<p>This equation indicates that 2 moles of butane react with 13 moles of oxygen to produce 8 moles of carbon dioxide and 10 moles of water. The molar ratios between the reactants and products can be determined directly from the coefficients in the balanced equation:\ue206<\/p>\n\n\n\n<p>a. <strong>C\u2084H\u2081\u2080 \/ O\u2082<\/strong>: The ratio of moles of butane to moles of oxygen is 2:13.\ue206<\/p>\n\n\n\n<p>b. <strong>O\u2082 \/ CO\u2082<\/strong>: The ratio of moles of oxygen to moles of carbon dioxide is 13:8.\ue206<\/p>\n\n\n\n<p>c. <strong>O\u2082 \/ H\u2082O<\/strong>: The ratio of moles of oxygen to moles of water is 13:10.\ue206<\/p>\n\n\n\n<p>d. <strong>C\u2084H\u2081\u2080 \/ CO\u2082<\/strong>: The ratio of moles of butane to moles of carbon dioxide is 2:8, which simplifies to 1:4.\ue206<\/p>\n\n\n\n<p>e. <strong>C\u2084H\u2081\u2080 \/ H\u2082O<\/strong>: The ratio of moles of butane to moles of water is 2:10, which simplifies to 1:5.\ue206<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>In a balanced chemical equation, the coefficients represent the stoichiometric relationships between reactants and products, indicating the exact proportions in which substances react and are produced. These coefficients are essential for understanding the quantitative aspects of chemical reactions, allowing chemists to predict the amounts of reactants needed and products formed.\ue206<\/p>\n\n\n\n<p>For the combustion of butane, the balanced equation shows that 2 moles of C\u2084H\u2081\u2080 react with 13 moles of O\u2082 to yield 8 moles of CO\u2082 and 10 moles of H\u2082O. From this, we can derive the following molar ratios:\ue206<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>C\u2084H\u2081\u2080 \/ O\u2082<\/strong>: The coefficient of C\u2084H\u2081\u2080 is 2, and for O\u2082, it is 13. Therefore, the molar ratio is 2:13.\ue206<\/li>\n\n\n\n<li><strong>O\u2082 \/ CO\u2082<\/strong>: The coefficient of O\u2082 is 13, and for CO\u2082, it is 8, giving a molar ratio of 13:8.\ue206<\/li>\n\n\n\n<li><strong>O\u2082 \/ H\u2082O<\/strong>: The coefficient of O\u2082 is 13, and for H\u2082O, it is 10, resulting in a molar ratio of 13:10.\ue206<\/li>\n\n\n\n<li><strong>C\u2084H\u2081\u2080 \/ CO\u2082<\/strong>: The coefficient of C\u2084H\u2081\u2080 is 2, and for CO\u2082, it is 8. Simplifying the ratio 2:8 gives 1:4.\ue206<\/li>\n\n\n\n<li><strong>C\u2084H\u2081\u2080 \/ H\u2082O<\/strong>: The coefficient of C\u2084H\u2081\u2080 is 2, and for H\u2082O, it is 10. Simplifying the ratio 2:10 gives 1:5.\ue206<\/li>\n<\/ul>\n\n\n\n<p>Understanding these molar ratios is crucial in stoichiometric calculations, which involve determining the quantities of reactants and products in chemical reactions. For instance, if a chemist knows the amount of butane available, they can use these ratios to calculate the exact amount of oxygen required for complete combustion, as well as the amounts of carbon dioxide and water that will be produced.\ue206<\/p>\n\n\n\n<p>These ratios also have practical implications in industrial processes where butane is used as a fuel. Ensuring the correct proportions of butane and oxygen can optimize combustion efficiency, reduce waste, and minimize the production of unwanted byproducts. Moreover, understanding the amounts of carbon dioxide and water produced is essential for environmental considerations, such as assessing greenhouse gas emissions and designing appropriate mitigation strategies.\ue206<\/p>\n\n\n\n<p>In summary, the molar ratios derived from the balanced chemical equation provide a foundational understanding of the quantitative relationships in the combustion of butane, enabling precise calculations and informed decisions in both laboratory and industrial settings.\ue206<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Given the following equation: 2 C4H10 + 13 O2 &#8212;> 8 CO2 + 10 H2O, show what the following molar ratios should be. a. C4H10 \/ O2 b. O2 \/ CO2 c. O2 \/ H2O d. C4H10 \/ CO2 e. C4H10 \/ H2O 2. The correct answer and explanation is : The balanced chemical equation [&hellip;]<\/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-196754","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196754","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=196754"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196754\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196754"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196754"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196754"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}