{"id":194803,"date":"2025-02-25T06:50:47","date_gmt":"2025-02-25T06:50:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194803"},"modified":"2025-02-25T06:50:49","modified_gmt":"2025-02-25T06:50:49","slug":"calculate-the-molar-mass-of-al2co33","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/25\/calculate-the-molar-mass-of-al2co33\/","title":{"rendered":"calculate the molar mass of Al2(CO3)3"},"content":{"rendered":"\n<p>calculate the molar mass of Al2(CO3)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 molar mass of a compound is calculated by adding together the atomic masses of each element present in the formula, multiplied by the number of atoms of that element in the formula. For ( \\text{Al}_2(\\text{CO}_3)_3 ), aluminum sulfate, we can calculate the molar mass as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Aluminum (( \\text{Al} )): The atomic mass of aluminum is approximately 26.98 g\/mol. There are 2 atoms of aluminum in the formula:<br>[<br>2 \\times 26.98 \\, \\text{g\/mol} = 53.96 \\, \\text{g\/mol}<br>]<\/li>\n\n\n\n<li>Carbon (( \\text{C} )): The atomic mass of carbon is about 12.01 g\/mol. There are 3 carbonate groups (( \\text{CO}_3 )), each containing 1 carbon atom:<br>[<br>3 \\times 12.01 \\, \\text{g\/mol} = 36.03 \\, \\text{g\/mol}<br>]<\/li>\n\n\n\n<li>Oxygen (( \\text{O} )): The atomic mass of oxygen is approximately 16.00 g\/mol. Each carbonate group contains 3 oxygen atoms, and there are 3 carbonate groups:<br>[<br>3 \\times 3 \\times 16.00 \\, \\text{g\/mol} = 144.00 \\, \\text{g\/mol}<br>]<\/li>\n<\/ul>\n\n\n\n<p>Adding these together, the total molar mass of ( \\text{Al}_2(\\text{CO}_3)_3 ) is:<br>[<br>53.96 \\, \\text{g\/mol} + 36.03 \\, \\text{g\/mol} + 144.00 \\, \\text{g\/mol} = 233.99 \\, \\text{g\/mol}<br>]<\/p>\n\n\n\n<p>This calculation shows how the molar mass of a compound is directly linked to its molecular formula, providing insights into its chemical properties. Each element&#8217;s atomic mass contributes to the overall mass of the compound, highlighting the importance of understanding chemical formulas when studying substances&#8217; molecular characteristics. This is crucial for applications in chemistry ranging from stoichiometric calculations in reactions to the preparation of solutions with precise concentrations.<\/p>\n\n\n\n<p>Now, I will generate an image that visually represents the molecule Al2(CO3)3.<\/p>\n\n\n\n<p>Here is an illustration representing the molecular structure of ( \\text{Al}_2(\\text{CO}_3)_3 ) (aluminum carbonate). Each atom type is color-coded for clarity: aluminum is in silver, carbon in black, and oxygen in red. This visual aids in understanding how the atoms are arranged and bonded in this compound.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1441.png\" alt=\"\" class=\"wp-image-194804\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>calculate the molar mass of Al2(CO3)3 The Correct Answer and Explanation is : The molar mass of a compound is calculated by adding together the atomic masses of each element present in the formula, multiplied by the number of atoms of that element in the formula. For ( \\text{Al}_2(\\text{CO}_3)_3 ), aluminum sulfate, we can calculate [&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-194803","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194803","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=194803"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194803\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194803"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194803"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194803"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}