Problem:<\/strong> Solution:<\/strong> Number of atoms = (number of moles) \u00d7 (Avogadro\u2019s number) Rounded to correct significant figures (2 significant figures, since 5.8 has 2), the answer is:<\/p>\n\n\n\n 3.5\u00d710243.5 \\times 10^{24}3.5\u00d71024 atoms of neon<\/strong><\/p>\n\n\n\n Textbook-Style Explanation (around 300 words):<\/strong><\/p>\n\n\n\n In chemistry, the concept of the mole is essential for relating the macroscopic amounts of substances to the number of particles involved. The mole serves as a bridge between the atomic scale and laboratory-scale quantities. One mole of any pure substance contains exactly 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 representative particles. This constant is known as Avogadro’s number and applies universally to atoms, molecules, ions, or other entities depending on the context.<\/p>\n\n\n\n To determine the number of atoms present in a given sample of neon gas, first identify the number of moles provided. In this case, the sample contains 5.8 moles of neon. Since neon is a monatomic gas (its formula is simply Ne), each mole directly corresponds to the same number of neon atoms as given by Avogadro’s number.<\/p>\n\n\n\n The calculation proceeds by multiplying the number of moles by Avogadro\u2019s constant: Number of atoms=moles of Ne\u00d76.022\u00d71023\u2009atoms\/mol.\\text{Number of atoms} = \\text{moles of Ne} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}.Number of atoms=moles of Ne\u00d76.022\u00d71023atoms\/mol.<\/p>\n\n\n\n Substituting the values: 5.8\u2009mol\u00d76.022\u00d71023\u2009atoms\/mol=3.49276\u00d71024\u2009atoms.5.8 \\, \\text{mol} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol} = 3.49276 \\times 10^{24} \\, \\text{atoms}.5.8mol\u00d76.022\u00d71023atoms\/mol=3.49276\u00d71024atoms.<\/p>\n\n\n\n When reporting the final answer, consider significant figures. The given data (5.8 moles) has two significant figures, so the result is rounded accordingly to 3.5\u00d710243.5 \\times 10^{24}3.5\u00d71024 atoms.<\/p>\n\n\n\n This result indicates that in 5.8 moles of neon gas, there are approximately 3.5\u00d710243.5 \\times 10^{24}3.5\u00d71024 individual neon atoms. This enormous number reflects the extremely small size of individual atoms and illustrates why the mole is such a practical unit in chemistry.<\/p>\n\n\n\n How many atoms of neon are in 5.8 moles of neon gas The Correct Answer and Explanation is: Problem:How many atoms of neon are in 5.8 moles of neon gas? Solution:To calculate the number of atoms, use Avogadro\u2019s number, which states that 1 mole of any substance contains 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 representative particles (in this […]<\/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-231774","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231774","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=231774"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231774\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231774"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231774"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231774"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
How many atoms of neon are in 5.8 moles of neon gas?<\/p>\n\n\n\n
To calculate the number of atoms, use Avogadro\u2019s number, which states that 1 mole of any substance contains 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 representative particles (in this case, atoms).<\/p>\n\n\n\n
Number of atoms = 5.8\u2009mol\u00d76.022\u00d71023\u2009atoms\/mol5.8 \\, \\text{mol} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}5.8mol\u00d76.022\u00d71023atoms\/mol
Number of atoms = 34.9276\u00d7102334.9276 \\times 10^{23}34.9276\u00d71023
Number of atoms = 3.49276\u00d710243.49276 \\times 10^{24}3.49276\u00d71024 atoms<\/p>\n\n\n\n
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