{"id":250202,"date":"2025-07-10T08:16:14","date_gmt":"2025-07-10T08:16:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=250202"},"modified":"2025-07-10T08:16:16","modified_gmt":"2025-07-10T08:16:16","slug":"what-is-the-molar-mass-of-lead-ii-iodide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/10\/what-is-the-molar-mass-of-lead-ii-iodide\/","title":{"rendered":"What is the molar mass of lead (II) iodide"},"content":{"rendered":"\n<p>What is the molar mass of lead (II) iodide? 334 g 461 g 668.2 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-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct answer is 461 g.<\/p>\n\n\n\n<p>To calculate the molar mass of lead (II) iodide (PbI\u2082), follow these steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Identify the atomic masses<\/strong>: The atomic mass of lead (Pb) is approximately 207.2 g\/mol, and the atomic mass of iodine (I) is about 126.9 g\/mol.<\/li>\n\n\n\n<li><strong>Determine the number of atoms in the formula<\/strong>: In PbI\u2082, there is one lead atom and two iodine atoms.<\/li>\n\n\n\n<li><strong>Calculate the total mass<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The contribution of lead (Pb) is 1 \u00d7 207.2 g\/mol = 207.2 g\/mol.<\/li>\n\n\n\n<li>The contribution of iodine (I) is 2 \u00d7 126.9 g\/mol = 253.8 g\/mol.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Add the individual contributions<\/strong>: The total molar mass is: 207.2\u2009g\/mol+253.8\u2009g\/mol=461\u2009g\/mol.207.2 \\, \\text{g\/mol} + 253.8 \\, \\text{g\/mol} = 461 \\, \\text{g\/mol}.<\/li>\n<\/ol>\n\n\n\n<p>Thus, the molar mass of lead (II) iodide is 461 g\/mol.<\/p>\n\n\n\n<p>Understanding molar mass is important because it allows for conversions between the mass of a substance and the number of moles. A mole is defined as 6.022 \u00d7 10\u00b2\u00b3 particles, and the molar mass represents the mass of one mole of a substance. The molar mass is often used in stoichiometry to calculate how much of each reactant or product is involved in a chemical reaction.<\/p>\n\n\n\n<p>In this case, knowing the molar mass of PbI\u2082 is useful for determining how much lead (II) iodide is needed to prepare a certain number of moles or for calculating the mass of the compound produced in a reaction.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the molar mass of lead (II) iodide? 334 g 461 g 668.2 g The correct answer and explanation is: The correct answer is 461 g. To calculate the molar mass of lead (II) iodide (PbI\u2082), follow these steps: Thus, the molar mass of lead (II) iodide is 461 g\/mol. Understanding molar mass 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-250202","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/250202","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=250202"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/250202\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=250202"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=250202"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=250202"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}