{"id":243136,"date":"2025-07-04T12:36:14","date_gmt":"2025-07-04T12:36:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=243136"},"modified":"2025-07-04T12:36:16","modified_gmt":"2025-07-04T12:36:16","slug":"the-chemical-formula-of-one-of-the-nitrogen-oxides-is-n2o5","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/the-chemical-formula-of-one-of-the-nitrogen-oxides-is-n2o5\/","title":{"rendered":"The chemical formula of one of the nitrogen oxides is N2O5"},"content":{"rendered":"\n<p>The chemical formula of one of the nitrogen oxides is N2O5. What mass of nitrogen would be found in 54 g of N2O5? Select one: 33 g 46 g 14 g 7g 28 g<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the mass of nitrogen in 54 g of N2O5, we need to follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Find the molar mass of N2O5<\/h3>\n\n\n\n<p>The molar mass of N2O5 is calculated by adding the atomic masses of nitrogen (N) and oxygen (O) in the formula.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Atomic mass of nitrogen (N) = 14.01 g\/mol<\/li>\n\n\n\n<li>Atomic mass of oxygen (O) = 16.00 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>The molar mass of N2O5 is:Molar&nbsp;mass&nbsp;of&nbsp;N2O5=2\u00d714.01\u2009g\/mol&nbsp;(N)+5\u00d716.00\u2009g\/mol&nbsp;(O)=28.02\u2009g\/mol+80.00\u2009g\/mol=108.02\u2009g\/mol\\text{Molar mass of N2O5} = 2 \\times 14.01 \\, \\text{g\/mol (N)} + 5 \\times 16.00 \\, \\text{g\/mol (O)} = 28.02 \\, \\text{g\/mol} + 80.00 \\, \\text{g\/mol} = 108.02 \\, \\text{g\/mol}Molar&nbsp;mass&nbsp;of&nbsp;N2O5=2\u00d714.01g\/mol&nbsp;(N)+5\u00d716.00g\/mol&nbsp;(O)=28.02g\/mol+80.00g\/mol=108.02g\/mol<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the mass of nitrogen in N2O5<\/h3>\n\n\n\n<p>The formula N2O5 contains 2 nitrogen atoms. The mass of nitrogen in one mole of N2O5 is:Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;N2O5=2\u00d714.01\u2009g=28.02\u2009g\\text{Mass of nitrogen in N2O5} = 2 \\times 14.01 \\, \\text{g} = 28.02 \\, \\text{g}Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;N2O5=2\u00d714.01g=28.02g<\/p>\n\n\n\n<p>So, in 108.02 g of N2O5, there is 28.02 g of nitrogen.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Use the ratio to find the mass of nitrogen in 54 g of N2O5<\/h3>\n\n\n\n<p>Now, we use a proportion to find the mass of nitrogen in 54 g of N2O5:Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;54&nbsp;g&nbsp;of&nbsp;N2O5Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;108.02&nbsp;g&nbsp;of&nbsp;N2O5=54\u2009g108.02\u2009g\\frac{\\text{Mass of nitrogen in 54 g of N2O5}}{\\text{Mass of nitrogen in 108.02 g of N2O5}} = \\frac{54 \\, \\text{g}}{108.02 \\, \\text{g}} Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;108.02&nbsp;g&nbsp;of&nbsp;N2O5Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;54&nbsp;g&nbsp;of&nbsp;N2O5\u200b=108.02g54g\u200bMass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;54&nbsp;g&nbsp;of&nbsp;N2O5=54\u2009g108.02\u2009g\u00d728.02\u2009g=14.01\u2009g\\text{Mass of nitrogen in 54 g of N2O5} = \\frac{54 \\, \\text{g}}{108.02 \\, \\text{g}} \\times 28.02 \\, \\text{g} = 14.01 \\, \\text{g}Mass&nbsp;of&nbsp;nitrogen&nbsp;in&nbsp;54&nbsp;g&nbsp;of&nbsp;N2O5=108.02g54g\u200b\u00d728.02g=14.01g<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<p>The mass of nitrogen in 54 g of N2O5 is 14 g. Therefore, the correct answer is <strong>14 g<\/strong>.<\/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-banner5-302.jpeg\" alt=\"\" class=\"wp-image-243138\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The chemical formula of one of the nitrogen oxides is N2O5. What mass of nitrogen would be found in 54 g of N2O5? Select one: 33 g 46 g 14 g 7g 28 g The Correct Answer and Explanation is: To determine the mass of nitrogen in 54 g of N2O5, we need to follow [&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-243136","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243136","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=243136"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243136\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243136"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243136"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243136"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}