{"id":266283,"date":"2025-07-22T19:22:24","date_gmt":"2025-07-22T19:22:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=266283"},"modified":"2025-07-22T19:22:27","modified_gmt":"2025-07-22T19:22:27","slug":"how-many-moles-of-sodium-atoms-are-in-5-g-of-sodium-carbonate","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/22\/how-many-moles-of-sodium-atoms-are-in-5-g-of-sodium-carbonate\/","title":{"rendered":"How many moles of sodium atoms are in 5 g of sodium carbonate"},"content":{"rendered":"\n<p>How many moles of sodium atoms are in 5 g of sodium carbonate?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the number of moles of sodium atoms in 5 g of sodium carbonate (Na\u2082CO\u2083), we need to follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Calculate the molar mass of sodium carbonate (Na\u2082CO\u2083)<\/h3>\n\n\n\n<p>The molar mass of Na\u2082CO\u2083 can be calculated by adding the atomic masses of all the atoms in the compound. The atomic masses of sodium (Na), carbon (C), and oxygen (O) are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na) = 22.99 g\/mol<\/li>\n\n\n\n<li>Carbon (C) = 12.01 g\/mol<\/li>\n\n\n\n<li>Oxygen (O) = 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>For Na\u2082CO\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na) contributes: 2 \u00d7 22.99 = 45.98 g\/mol<\/li>\n\n\n\n<li>Carbon (C) contributes: 1 \u00d7 12.01 = 12.01 g\/mol<\/li>\n\n\n\n<li>Oxygen (O) contributes: 3 \u00d7 16.00 = 48.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Therefore, the molar mass of Na\u2082CO\u2083 is: 45.98+12.01+48.00=105.99\u2009g\/mol45.98 + 12.01 + 48.00 = 105.99 \\, \\text{g\/mol}45.98+12.01+48.00=105.99g\/mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Convert the mass of sodium carbonate to moles<\/h3>\n\n\n\n<p>Now, we can convert the given mass of Na\u2082CO\u2083 (5 g) to moles using the molar mass: moles&nbsp;of&nbsp;Na\u2082CO\u2083=mass&nbsp;of&nbsp;Na\u2082CO\u2083molar&nbsp;mass&nbsp;of&nbsp;Na\u2082CO\u2083=5\u2009g105.99\u2009g\/mol\u22480.0471\u2009mol\\text{moles of Na\u2082CO\u2083} = \\frac{\\text{mass of Na\u2082CO\u2083}}{\\text{molar mass of Na\u2082CO\u2083}} = \\frac{5 \\, \\text{g}}{105.99 \\, \\text{g\/mol}} \\approx 0.0471 \\, \\text{mol}moles&nbsp;of&nbsp;Na\u2082CO\u2083=molar&nbsp;mass&nbsp;of&nbsp;Na\u2082CO\u2083mass&nbsp;of&nbsp;Na\u2082CO\u2083\u200b=105.99g\/mol5g\u200b\u22480.0471mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Determine the number of moles of sodium atoms<\/h3>\n\n\n\n<p>In one mole of sodium carbonate (Na\u2082CO\u2083), there are 2 moles of sodium (Na) atoms because the chemical formula has two sodium atoms per formula unit of Na\u2082CO\u2083. So, to find the moles of sodium atoms, we multiply the moles of Na\u2082CO\u2083 by 2: moles&nbsp;of&nbsp;Na=2\u00d70.0471\u2009mol=0.0942\u2009mol\\text{moles of Na} = 2 \\times 0.0471 \\, \\text{mol} = 0.0942 \\, \\text{mol}moles&nbsp;of&nbsp;Na=2\u00d70.0471mol=0.0942mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>There are approximately <strong>0.0942 moles<\/strong> of sodium atoms in 5 g of sodium carbonate.<\/p>\n\n\n\n<p>This calculation is based on the molar mass of Na\u2082CO\u2083 and the stoichiometric relationship between sodium and sodium carbonate.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1573.jpeg\" alt=\"\" class=\"wp-image-266286\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>How many moles of sodium atoms are in 5 g of sodium carbonate? The Correct Answer and Explanation is: To find the number of moles of sodium atoms in 5 g of sodium carbonate (Na\u2082CO\u2083), we need to follow these steps: Step 1: Calculate the molar mass of sodium carbonate (Na\u2082CO\u2083) The molar mass 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-266283","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266283","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=266283"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/266283\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=266283"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=266283"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=266283"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}