{"id":185938,"date":"2025-01-23T18:18:39","date_gmt":"2025-01-23T18:18:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185938"},"modified":"2025-01-23T18:18:41","modified_gmt":"2025-01-23T18:18:41","slug":"maleic-acid-has-the-empirical-formula-cho","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/23\/maleic-acid-has-the-empirical-formula-cho\/","title":{"rendered":"Maleic acid has the empirical formula CHO"},"content":{"rendered":"\n<p>Maleic acid has the empirical formula CHO. If the molar mass of oxalic acid is 116.1 g\/mol, what is the molecular formula of maleic acid? [C=12.0g\/mol, H = 1.01 g\/mol, O = 16.0 g\/mol] a) CHO b)C_2H_2O_2 c) C_6H_12O_2 d) C_4H_4O_4 e) C_3H_6O_3<\/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<p>The given empirical formula of maleic acid is CHO, and we need to find its molecular formula. Additionally, we are told that the molar mass of oxalic acid is 116.1 g\/mol, and we are given atomic masses for carbon (C), hydrogen (H), and oxygen (O).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Calculate the molar mass of the empirical formula<\/h3>\n\n\n\n<p>The molar mass of the empirical formula CHO is calculated by adding the atomic masses of each element:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) = 12.0 g\/mol<\/li>\n\n\n\n<li>Hydrogen (H) = 1.01 g\/mol<\/li>\n\n\n\n<li>Oxygen (O) = 16.0 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>So, the molar mass of the empirical formula CHO is:<\/p>\n\n\n\n<p>[<br>12.0 \\, \\text{g\/mol} + 1.01 \\, \\text{g\/mol} + 16.0 \\, \\text{g\/mol} = 29.01 \\, \\text{g\/mol}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Determine the ratio of the molecular mass to the empirical formula mass<\/h3>\n\n\n\n<p>We are told that the molar mass of maleic acid is 116.1 g\/mol. To find the ratio between the molar mass of the molecular formula and the empirical formula mass:<\/p>\n\n\n\n<p>[<br>\\text{Ratio} = \\frac{\\text{Molar mass of maleic acid}}{\\text{Empirical formula mass}} = \\frac{116.1 \\, \\text{g\/mol}}{29.01 \\, \\text{g\/mol}} \\approx 4<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Determine the molecular formula<\/h3>\n\n\n\n<p>Since the ratio is approximately 4, this means the molecular formula of maleic acid is 4 times the empirical formula. Therefore, we multiply the empirical formula (CHO) by 4:<\/p>\n\n\n\n<p>[<br>\\text{Molecular formula} = (CHO) \\times 4 = C_4H_4O_4<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Conclusion<\/h3>\n\n\n\n<p>The molecular formula of maleic acid is <strong>C\u2084H\u2084O\u2084<\/strong>, which corresponds to option <strong>d<\/strong>.<\/p>\n\n\n\n<p>Thus, the correct answer is <strong>d) C\u2084H\u2084O\u2084<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Maleic acid has the empirical formula CHO. If the molar mass of oxalic acid is 116.1 g\/mol, what is the molecular formula of maleic acid? [C=12.0g\/mol, H = 1.01 g\/mol, O = 16.0 g\/mol] a) CHO b)C_2H_2O_2 c) C_6H_12O_2 d) C_4H_4O_4 e) C_3H_6O_3 The Correct Answer and Explanation is : The given empirical formula of [&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-185938","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185938","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=185938"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185938\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185938"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185938"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185938"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}