{"id":245380,"date":"2025-07-06T07:19:18","date_gmt":"2025-07-06T07:19:18","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=245380"},"modified":"2025-07-06T07:19:21","modified_gmt":"2025-07-06T07:19:21","slug":"calculate-the-number-of-atoms-in-each-sample-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/06\/calculate-the-number-of-atoms-in-each-sample-2\/","title":{"rendered":"Calculate the number of atoms in each sample."},"content":{"rendered":"\n<p>Calculate the number of atoms in each sample. a. 14.955 g Cr b. 39.733 g S c. 12.899 g Pt d. 97.552 g Sn<\/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 calculate the number of atoms in each sample, we use the formula:Number&nbsp;of&nbsp;atoms=Mass&nbsp;of&nbsp;sample&nbsp;(g)Molar&nbsp;mass&nbsp;(g\/mol)\u00d7Avogadro\u2019s&nbsp;number\\text{Number of atoms} = \\frac{\\text{Mass of sample (g)}}{\\text{Molar mass (g\/mol)}} \\times \\text{Avogadro&#8217;s number} Number&nbsp;of&nbsp;atoms=Molar&nbsp;mass&nbsp;(g\/mol)Mass&nbsp;of&nbsp;sample&nbsp;(g)\u200b\u00d7Avogadro\u2019s&nbsp;number<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Molar mass<\/strong> is the atomic mass of the element (in grams per mole),<\/li>\n\n\n\n<li><strong>Avogadro\u2019s number<\/strong> is 6.022\u00d71023\u2009atoms\/mol6.022 \\times 10^{23} \\, \\text{atoms\/mol}6.022\u00d71023atoms\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Let&#8217;s break it down for each sample:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">a. 14.955 g Cr (Chromium)<\/h3>\n\n\n\n<p>The atomic mass of Chromium (Cr) is 52.00 g\/mol.Number&nbsp;of&nbsp;atoms=14.955\u2009g52.00\u2009g\/mol\u00d76.022\u00d71023\u2009atoms\/mol\\text{Number of atoms} = \\frac{14.955 \\, \\text{g}}{52.00 \\, \\text{g\/mol}} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}Number&nbsp;of&nbsp;atoms=52.00g\/mol14.955g\u200b\u00d76.022\u00d71023atoms\/molNumber&nbsp;of&nbsp;atoms=14.95552.00\u00d76.022\u00d71023\\text{Number of atoms} = \\frac{14.955}{52.00} \\times 6.022 \\times 10^{23} Number&nbsp;of&nbsp;atoms=52.0014.955\u200b\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms=0.287\u00d76.022\u00d71023\\text{Number of atoms} = 0.287 \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=0.287\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms\u22481.73\u00d71023\u2009atoms\\text{Number of atoms} \\approx 1.73 \\times 10^{23} \\, \\text{atoms}Number&nbsp;of&nbsp;atoms\u22481.73\u00d71023atoms<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">b. 39.733 g S (Sulfur)<\/h3>\n\n\n\n<p>The atomic mass of Sulfur (S) is 32.06 g\/mol.Number&nbsp;of&nbsp;atoms=39.733\u2009g32.06\u2009g\/mol\u00d76.022\u00d71023\u2009atoms\/mol\\text{Number of atoms} = \\frac{39.733 \\, \\text{g}}{32.06 \\, \\text{g\/mol}} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}Number&nbsp;of&nbsp;atoms=32.06g\/mol39.733g\u200b\u00d76.022\u00d71023atoms\/molNumber&nbsp;of&nbsp;atoms=39.73332.06\u00d76.022\u00d71023\\text{Number of atoms} = \\frac{39.733}{32.06} \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=32.0639.733\u200b\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms=1.24\u00d76.022\u00d71023\\text{Number of atoms} = 1.24 \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=1.24\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms\u22487.47\u00d71023\u2009atoms\\text{Number of atoms} \\approx 7.47 \\times 10^{23} \\, \\text{atoms}Number&nbsp;of&nbsp;atoms\u22487.47\u00d71023atoms<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">c. 12.899 g Pt (Platinum)<\/h3>\n\n\n\n<p>The atomic mass of Platinum (Pt) is 195.08 g\/mol.Number&nbsp;of&nbsp;atoms=12.899\u2009g195.08\u2009g\/mol\u00d76.022\u00d71023\u2009atoms\/mol\\text{Number of atoms} = \\frac{12.899 \\, \\text{g}}{195.08 \\, \\text{g\/mol}} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}Number&nbsp;of&nbsp;atoms=195.08g\/mol12.899g\u200b\u00d76.022\u00d71023atoms\/molNumber&nbsp;of&nbsp;atoms=12.899195.08\u00d76.022\u00d71023\\text{Number of atoms} = \\frac{12.899}{195.08} \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=195.0812.899\u200b\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms=0.0662\u00d76.022\u00d71023\\text{Number of atoms} = 0.0662 \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=0.0662\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms\u22483.98\u00d71022\u2009atoms\\text{Number of atoms} \\approx 3.98 \\times 10^{22} \\, \\text{atoms}Number&nbsp;of&nbsp;atoms\u22483.98\u00d71022atoms<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">d. 97.552 g Sn (Tin)<\/h3>\n\n\n\n<p>The atomic mass of Tin (Sn) is 118.71 g\/mol.Number&nbsp;of&nbsp;atoms=97.552\u2009g118.71\u2009g\/mol\u00d76.022\u00d71023\u2009atoms\/mol\\text{Number of atoms} = \\frac{97.552 \\, \\text{g}}{118.71 \\, \\text{g\/mol}} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}Number&nbsp;of&nbsp;atoms=118.71g\/mol97.552g\u200b\u00d76.022\u00d71023atoms\/molNumber&nbsp;of&nbsp;atoms=97.552118.71\u00d76.022\u00d71023\\text{Number of atoms} = \\frac{97.552}{118.71} \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=118.7197.552\u200b\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms=0.823\u00d76.022\u00d71023\\text{Number of atoms} = 0.823 \\times 6.022 \\times 10^{23}Number&nbsp;of&nbsp;atoms=0.823\u00d76.022\u00d71023Number&nbsp;of&nbsp;atoms\u22484.96\u00d71023\u2009atoms\\text{Number of atoms} \\approx 4.96 \\times 10^{23} \\, \\text{atoms}Number&nbsp;of&nbsp;atoms\u22484.96\u00d71023atoms<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Summary of Results:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>a) 14.955 g Cr: 1.73\u00d710231.73 \\times 10^{23}1.73\u00d71023 atoms<\/li>\n\n\n\n<li>b) 39.733 g S: 7.47\u00d710237.47 \\times 10^{23}7.47\u00d71023 atoms<\/li>\n\n\n\n<li>c) 12.899 g Pt: 3.98\u00d710223.98 \\times 10^{22}3.98\u00d71022 atoms<\/li>\n\n\n\n<li>d) 97.552 g Sn: 4.96\u00d710234.96 \\times 10^{23}4.96\u00d71023 atoms<\/li>\n<\/ul>\n\n\n\n<p>This calculation is based on the molar masses and the relationship between mass, moles, and atoms using Avogadro&#8217;s constant.<\/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-banner5-642.jpeg\" alt=\"\" class=\"wp-image-245381\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the number of atoms in each sample. a. 14.955 g Cr b. 39.733 g S c. 12.899 g Pt d. 97.552 g Sn The Correct Answer and Explanation is: To calculate the number of atoms in each sample, we use the formula:Number&nbsp;of&nbsp;atoms=Mass&nbsp;of&nbsp;sample&nbsp;(g)Molar&nbsp;mass&nbsp;(g\/mol)\u00d7Avogadro\u2019s&nbsp;number\\text{Number of atoms} = \\frac{\\text{Mass of sample (g)}}{\\text{Molar mass (g\/mol)}} \\times \\text{Avogadro&#8217;s number} [&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 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