a. Balancing the equation:<\/h3>\n\n\n\n
The unbalanced reaction is:
[ \\text{Fe}_2\\text{O}_3 + \\text{CO} \\rightarrow \\text{Fe} + \\text{CO}_2 ]<\/p>\n\n\n\n
To balance this equation, follow these steps:<\/p>\n\n\n\n
- \n
- Balance Iron (Fe):<\/strong>
On the left side, we have (\\text{Fe}_2\\text{O}_3), which contains 2 iron atoms. On the right side, iron is represented as (\\text{Fe}). To balance the iron atoms, we place a coefficient of 2 in front of (\\text{Fe}):
[ \\text{Fe}_2\\text{O}_3 + \\text{CO} \\rightarrow 2\\text{Fe} + \\text{CO}_2 ]<\/li>\n\n\n\n- Balance Oxygen (O):<\/strong>
On the left side, (\\text{Fe}_2\\text{O}_3) has 3 oxygen atoms, and on the right side, (\\text{CO}_2) has 2 oxygen atoms. To balance the oxygen, we place a coefficient of 3 in front of (\\text{CO}_2):
[ \\text{Fe}_2\\text{O}_3 + \\text{CO} \\rightarrow 2\\text{Fe} + 3\\text{CO}_2 ]<\/li>\n\n\n\n- Balance Carbon (C):<\/strong>
On the left side, we have (\\text{CO}), which has 1 carbon atom. On the right side, we now have 3 carbon atoms because of the 3 (\\text{CO}_2) molecules. To balance the carbon, place a coefficient of 3 in front of (\\text{CO}):
[ \\text{Fe}_2\\text{O}_3 + 3\\text{CO} \\rightarrow 2\\text{Fe} + 3\\text{CO}_2 ]<\/li>\n\n\n\n- Final Balanced Equation:<\/strong>
[ \\text{Fe}_2\\text{O}_3 + 3\\text{CO} \\rightarrow 2\\text{Fe} + 3\\text{CO}_2 ]<\/li>\n<\/ol>\n\n\n\nb. Possible Ratios:<\/h3>\n\n\n\n
From the balanced equation:<\/p>\n\n\n\n
[ \\text{Fe}_2\\text{O}_3 + 3\\text{CO} \\rightarrow 2\\text{Fe} + 3\\text{CO}_2 ]<\/p>\n\n\n\n
We can write the ratios of the reactants and products based on their coefficients:<\/p>\n\n\n\n
- \n
- Fe\u2082O\u2083 to CO<\/strong>: The ratio of (\\text{Fe}_2\\text{O}_3) to (\\text{CO}) is 1:3. For every 1 molecule of (\\text{Fe}_2\\text{O}_3), 3 molecules of (\\text{CO}) are required.<\/li>\n\n\n\n
- Fe\u2082O\u2083 to Fe<\/strong>: The ratio of (\\text{Fe}_2\\text{O}_3) to (\\text{Fe}) is 1:2. For every 1 molecule of (\\text{Fe}_2\\text{O}_3), 2 atoms of Fe are produced.<\/li>\n\n\n\n
- CO to CO\u2082<\/strong>: The ratio of (\\text{CO}) to (\\text{CO}_2) is 3:3, which simplifies to 1:1. For every 1 molecule of CO, 1 molecule of CO\u2082 is produced.<\/li>\n<\/ul>\n\n\n\n
Explanation:<\/h4>\n\n\n\n
The balanced equation demonstrates the stoichiometric relationship between reactants and products in a chemical reaction. The coefficients indicate the ratio in which substances combine and react. These ratios are crucial for understanding the amounts of each substance required or produced during a chemical reaction. Stoichiometry allows for the calculation of the necessary reactants or expected products in any given chemical process. In this case, understanding that for every 1 mole of Fe\u2082O\u2083, 3 moles of CO are required to produce 2 moles of Fe and 3 moles of CO\u2082 can help in practical applications, like industrial production of iron using carbon monoxide.<\/p>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-505.png\")
<\/figure>\n\n\n\nHere is the diagram illustrating the balanced chemical equation for the reaction:<\/p>\n\n\n\n
[ \\text{Fe}_2\\text{O}_3 + 3\\text{CO} \\rightarrow 2\\text{Fe} + 3\\text{CO}_2 ]<\/p>\n","protected":false},"excerpt":{"rendered":"
Fe2O3 + CO \u2192 Fe + CO2 a. Balance the equation b. Write all possible ratios The correct answer and explanation is : a. Balancing the equation: The unbalanced reaction is:[ \\text{Fe}_2\\text{O}_3 + \\text{CO} \\rightarrow \\text{Fe} + \\text{CO}_2 ] To balance this equation, follow these steps: b. Possible Ratios: From the balanced equation: [ \\text{Fe}_2\\text{O}_3 […]<\/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-197545","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/197545","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=197545"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/197545\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=197545"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=197545"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=197545"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- Fe\u2082O\u2083 to Fe<\/strong>: The ratio of (\\text{Fe}_2\\text{O}_3) to (\\text{Fe}) is 1:2. For every 1 molecule of (\\text{Fe}_2\\text{O}_3), 2 atoms of Fe are produced.<\/li>\n\n\n\n
- Balance Oxygen (O):<\/strong>