{"id":47065,"date":"2025-07-02T10:05:31","date_gmt":"2025-07-02T10:05:31","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=47065"},"modified":"2025-07-02T10:05:32","modified_gmt":"2025-07-02T10:05:32","slug":"what-is-the-number-density-of-lead-in-1-cm3","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/what-is-the-number-density-of-lead-in-1-cm3\/","title":{"rendered":"What is the number density of lead in 1\/cm^3"},"content":{"rendered":"\n<p>What is the number density of lead in 1\/cm^3?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the number density of lead (Pb) in units of 1\/cm\u00b3, we need to know the mass density of lead and its atomic mass. Here\u2019s how we can go through the calculation:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the mass density of lead<\/h3>\n\n\n\n<p>The mass density of lead (\u03c1) is given as approximately <strong>11.34 g\/cm\u00b3<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Find the molar mass of lead<\/h3>\n\n\n\n<p>The molar mass of lead (Pb) is <strong>207.2 g\/mol<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Convert mass density to molar density<\/h3>\n\n\n\n<p>To find the number of moles per cubic centimeter, we divide the mass density by the molar mass:Molar&nbsp;density=Mass&nbsp;densityMolar&nbsp;mass=11.34\u2009g\/cm3207.2\u2009g\/mol\u22480.0548\u2009mol\/cm3\\text{Molar density} = \\frac{\\text{Mass density}}{\\text{Molar mass}} = \\frac{11.34 \\, \\text{g\/cm}^3}{207.2 \\, \\text{g\/mol}} \\approx 0.0548 \\, \\text{mol\/cm}^3Molar&nbsp;density=Molar&nbsp;massMass&nbsp;density\u200b=207.2g\/mol11.34g\/cm3\u200b\u22480.0548mol\/cm3<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Convert moles to number of atoms<\/h3>\n\n\n\n<p>Now, we convert moles to the number of atoms. This requires Avogadro\u2019s number, which is 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023 atoms\/mol.Number&nbsp;density=Molar&nbsp;density\u00d7Avogadro\u2019s&nbsp;number\\text{Number density} = \\text{Molar density} \\times \\text{Avogadro&#8217;s number}Number&nbsp;density=Molar&nbsp;density\u00d7Avogadro\u2019s&nbsp;numberNumber&nbsp;density=0.0548\u2009mol\/cm3\u00d76.022\u00d71023\u2009atoms\/mol\\text{Number density} = 0.0548 \\, \\text{mol\/cm}^3 \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}Number&nbsp;density=0.0548mol\/cm3\u00d76.022\u00d71023atoms\/molNumber&nbsp;density\u22483.30\u00d71022\u2009atoms\/cm3\\text{Number density} \\approx 3.30 \\times 10^{22} \\, \\text{atoms\/cm}^3Number&nbsp;density\u22483.30\u00d71022atoms\/cm3<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<p>The number density of lead in 1\/cm\u00b3 is approximately <strong>3.30 \u00d7 10\u00b2\u00b2 atoms\/cm\u00b3<\/strong>. This means that in every cubic centimeter of lead, there are roughly 3.30 \u00d7 10\u00b2\u00b2 lead atoms.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-213.jpeg\" alt=\"\" class=\"wp-image-47069\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-213.jpeg 1024w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-213-300x300.jpeg 300w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-213-150x150.jpeg 150w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-213-768x768.jpeg 768w\" sizes=\"auto, (max-width: 1024px) 100vw, 1024px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the number density of lead in 1\/cm^3? The Correct Answer and Explanation is: To calculate the number density of lead (Pb) in units of 1\/cm\u00b3, we need to know the mass density of lead and its atomic mass. Here\u2019s how we can go through the calculation: Step 1: Determine the mass density of [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-47065","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/47065","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=47065"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/47065\/revisions"}],"predecessor-version":[{"id":47070,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/47065\/revisions\/47070"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=47065"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=47065"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=47065"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}