{"id":231433,"date":"2025-06-11T06:15:36","date_gmt":"2025-06-11T06:15:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=231433"},"modified":"2025-06-11T06:15:38","modified_gmt":"2025-06-11T06:15:38","slug":"c6h8-o2-a-co2-h2o-how-many-moles-of-o2-are-needed-to-form-60-moles-of-co2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/11\/c6h8-o2-a-co2-h2o-how-many-moles-of-o2-are-needed-to-form-60-moles-of-co2\/","title":{"rendered":"C6H8 + O2 ——\u00e0 CO2 + H2O How many moles of O2 are needed to form 60 moles of CO2"},"content":{"rendered":"\n

C6H8 + O2 ——\u00e0 CO2 + H2O How many moles of O2 are needed to form 60 moles of CO2<\/p>\n\n\n\n

Correct Answer: 80 moles of O2<\/strong><\/p>\n\n\n\n

To determine the number of moles of a reactant required to produce a specific amount of product, one must first ensure the chemical equation is balanced. A balanced equation adheres to the Law of Conservation of Mass, stating that atoms are neither created nor destroyed in a chemical reaction.<\/p>\n\n\n\n

The initial, unbalanced equation is:
C6H8 + O2 \u2192 CO2 + H2O<\/p>\n\n\n\n

Step 1: Balance the Chemical Equation<\/strong>
The first step is to balance the atoms on both sides of the reaction.<\/p>\n\n\n\n

    \n
  1. Balance Carbon (C):<\/strong>\u00a0There are 6 carbon atoms on the reactant side (in C6H8). To balance this, a coefficient of 6 is placed before CO2 on the product side.
    C6H8 + O2 \u2192 6CO2 + H2O<\/li>\n\n\n\n
  2. Balance Hydrogen (H):<\/strong>\u00a0There are 8 hydrogen atoms on the reactant side. To balance this, a coefficient of 4 is placed before H2O on the product side (4 x 2 = 8 H atoms).
    C6H8 + O2 \u2192 6CO2 + 4H2O<\/li>\n\n\n\n
  3. Balance Oxygen (O):<\/strong>\u00a0Now, count the oxygen atoms on the product side. There are (6 x 2) = 12 oxygen atoms in 6CO2 and (4 x 1) = 4 oxygen atoms in 4H2O, for a total of 16 oxygen atoms. To balance this, a coefficient of 8 is placed before O2 on the reactant side (8 x 2 = 16 O atoms).<\/li>\n<\/ol>\n\n\n\n

    The final, balanced equation is:
    C6H8 + 8O2 \u2192 6CO2 + 4H2O<\/strong><\/p>\n\n\n\n

    Step 2: Use the Molar Ratio<\/strong>
    This balanced equation provides the stoichiometric or molar ratio between the reactants and products. It shows that for every 8 moles of oxygen (O2) that react, 6 moles of carbon dioxide (CO2) are produced. This ratio is constant for this reaction:<\/p>\n\n\n\n

    8 moles O2 : 6 moles CO2<\/strong><\/p>\n\n\n\n

    Step 3: Calculate the Required Moles<\/strong>
    The problem requires finding the moles of O2 needed to form 60 moles of CO2. Using the molar ratio as a conversion factor, the calculation is set up to cancel the units of “moles CO2” and find “moles O2.”<\/p>\n\n\n\n

    Moles of O2 = (60 moles CO2) \u00d7 (8 moles O2 \/ 6 moles CO2)<\/p>\n\n\n\n

    Moles of O2 = (60 \u00d7 8) \/ 6
    Moles of O2 = 480 \/ 6
    Moles of O2 = 80<\/p>\n\n\n\n

    Therefore, 80 moles of O2 are needed to form 60 moles of CO2.<\/p>\n\n\n\n

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

    C6H8 + O2 ——\u00e0 CO2 + H2O How many moles of O2 are needed to form 60 moles of CO2 Correct Answer: 80 moles of O2 To determine the number of moles of a reactant required to produce a specific amount of product, one must first ensure the chemical equation is balanced. A balanced equation […]<\/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-231433","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231433","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=231433"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231433\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231433"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231433"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231433"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}