To determine the limiting reactant<\/strong>, we follow these steps:<\/p>\n\n\n\n [ From the balanced equation:<\/p>\n\n\n\n Since ammonia runs out first, ammonia (NH\u2083) is the limiting reactant<\/strong>.<\/p>\n\n\n\n Here is an illustration of the reaction between ammonia (NH\u2083) and carbon dioxide (CO\u2082) to form urea ((NH\u2082)\u2082CO) and water (H\u2082O). The image visually represents the reaction process and highlights ammonia as the limiting reactant. <\/p>\n","protected":false},"excerpt":{"rendered":" Urea, (NH2)2CO is prepared by reacting ammonia with carbon dioxide. The byproduct is water. If 136 g of ammonia are reacted with 264 g of carbon dioxide, which of the reactants in the limiting reactant? The correct answer and explanation is : To determine the limiting reactant, we follow these steps: Step 1: Write the […]<\/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-198820","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198820","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=198820"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198820\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198820"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198820"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198820"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 1: Write the Balanced Chemical Equation<\/strong><\/h3>\n\n\n\n
2NH_3 + CO_2 \\rightarrow (NH_2)_2CO + H_2O
]
This equation shows that 2 moles of ammonia<\/strong> react with 1 mole of carbon dioxide<\/strong> to form 1 mole of urea<\/strong> and 1 mole of water<\/strong>.<\/p>\n\n\n\nStep 2: Convert Given Masses to Moles<\/strong><\/h3>\n\n\n\n
\n
[
\\frac{136 \\text{ g}}{17 \\text{ g\/mol}} = 8 \\text{ moles of } NH_3
]<\/li>\n\n\n\n
[
\\frac{264 \\text{ g}}{44 \\text{ g\/mol}} = 6 \\text{ moles of } CO_2
]<\/li>\n<\/ul>\n\n\n\nStep 3: Find the Limiting Reactant<\/strong><\/h3>\n\n\n\n
\n
[
\\frac{8}{2} = 4 \\text{ moles of CO}_2
]<\/li>\n\n\n\n
[
6 \\times 2 = 12 \\text{ moles of NH}_3
]<\/li>\n\n\n\nConclusion<\/strong><\/h3>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-804.png\")
<\/figure>\n\n\n\n