{"id":238279,"date":"2025-06-18T03:56:23","date_gmt":"2025-06-18T03:56:23","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=238279"},"modified":"2025-06-18T03:56:25","modified_gmt":"2025-06-18T03:56:25","slug":"calculate-the-mass-of-2-50x104-molecules-of-nitrogen-gas","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/18\/calculate-the-mass-of-2-50x104-molecules-of-nitrogen-gas\/","title":{"rendered":"Calculate the mass of\u00a02.50\u00d7104\u00a0molecules of nitrogen gas."},"content":{"rendered":"\n<pre id=\"preorder-ask-header-text\" class=\"wp-block-preformatted\"><br><br><\/pre>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/image-684.png\" alt=\"\" class=\"wp-image-238280\"\/><\/figure>\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>The correct answer to the problem is <strong>1.16 \u00d7 10\u207b\u00b9\u2078 g<\/strong>.<\/p>\n\n\n\n<p>To determine the mass of 2.50 \u00d7 10\u2074 molecules of nitrogen gas, we use the molar mass of nitrogen gas and Avogadro&#8217;s number. The molar mass of nitrogen gas (N\u2082) is approximately 28.02 g\/mol, and Avogadro&#8217;s number is 6.022 \u00d7 10\u00b2\u00b3 molecules per mole.<\/p>\n\n\n\n<p>First, we convert the number of molecules into moles using the relationship:<\/p>\n\n\n\n<p>Number&nbsp;of&nbsp;moles=Number&nbsp;of&nbsp;moleculesAvogadro\u2019s&nbsp;number\\text{Number of moles} = \\frac{\\text{Number of molecules}}{\\text{Avogadro&#8217;s number}}<\/p>\n\n\n\n<p>Number&nbsp;of&nbsp;moles=2.50\u00d71046.022\u00d71023\\text{Number of moles} = \\frac{2.50 \u00d7 10\u2074}{6.022 \u00d7 10\u00b2\u00b3}<\/p>\n\n\n\n<p>Number&nbsp;of&nbsp;moles\u22484.15\u00d710\u221220&nbsp;mol\\text{Number of moles} \u2248 4.15 \u00d7 10\u207b\u00b2\u2070 \\text{ mol}<\/p>\n\n\n\n<p>Next, we use the molar mass of nitrogen gas to find the mass:<\/p>\n\n\n\n<p>Mass=Number&nbsp;of&nbsp;moles\u00d7Molar&nbsp;mass\\text{Mass} = \\text{Number of moles} \u00d7 \\text{Molar mass}<\/p>\n\n\n\n<p>Mass=(4.15\u00d710\u221220)\u00d7(28.02)\\text{Mass} = (4.15 \u00d7 10\u207b\u00b2\u2070) \u00d7 (28.02)<\/p>\n\n\n\n<p>Mass\u22481.16\u00d710\u221218&nbsp;g\\text{Mass} \u2248 1.16 \u00d7 10\u207b\u00b9\u2078 \\text{ g}<\/p>\n\n\n\n<p>Thus, the correct answer is <strong>1.16 \u00d7 10\u207b\u00b9\u2078 g<\/strong>.<\/p>\n\n\n\n<p>This problem demonstrates the relationship between the number of molecules, moles, and mass in chemistry. It highlights the importance of Avogadro\u2019s number in converting between molecular quantities and macroscopic masses. Understanding these conversions is essential for stoichiometry in chemical reactions, where precise amounts of reactants and products must be calculated. The concept also has applications in determining molecular weights, calculating reaction yields, and analyzing the composition of materials at the atomic level. By systematically breaking down the problem, we see how fundamental constants like Avogadro\u2019s number and molar mass enable us to work efficiently with microscopic quantities and apply them to practical chemistry calculations.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner5-698.jpeg\" alt=\"\" class=\"wp-image-238281\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The Correct Answer and Explanation is: The correct answer to the problem is 1.16 \u00d7 10\u207b\u00b9\u2078 g. To determine the mass of 2.50 \u00d7 10\u2074 molecules of nitrogen gas, we use the molar mass of nitrogen gas and Avogadro&#8217;s number. The molar mass of nitrogen gas (N\u2082) is approximately 28.02 g\/mol, and Avogadro&#8217;s number is [&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-238279","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238279","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=238279"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238279\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=238279"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=238279"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=238279"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}