{"id":267967,"date":"2025-07-23T18:13:31","date_gmt":"2025-07-23T18:13:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267967"},"modified":"2025-07-23T18:13:33","modified_gmt":"2025-07-23T18:13:33","slug":"calculate-the-molar-mass-of-molecular-iodine-i2-79-9-g-mol-only-atomic-masses-and-not-molar-masses-can-be-calculated-for-elements-159-8-g-mol-126-9-g-mol-253-8-g-mol","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/calculate-the-molar-mass-of-molecular-iodine-i2-79-9-g-mol-only-atomic-masses-and-not-molar-masses-can-be-calculated-for-elements-159-8-g-mol-126-9-g-mol-253-8-g-mol\/","title":{"rendered":"Calculate the molar mass of molecular iodine, I2: 79.9 g\/mol Only atomic masses, and not molar masses, can be calculated for elements. 159.8 g\/mol 126.9 g\/mol 253.8 g\/mol"},"content":{"rendered":"\n<p>Calculate the molar mass of molecular iodine, I2: 79.9 g\/mol Only atomic masses, and not molar masses, can be calculated for elements. 159.8 g\/mol 126.9 g\/mol 253.8 g\/mol<\/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>The molar mass of molecular iodine (I\u2082) is calculated by adding the molar masses of two iodine (I) atoms.<\/p>\n\n\n\n<p>The atomic mass of iodine (I) is approximately <strong>126.9 g\/mol<\/strong>. Since iodine exists as a diatomic molecule (I\u2082) in its natural form, we need to multiply the atomic mass of iodine by 2 to find the molar mass of I\u2082.<\/p>\n\n\n\n<p><strong>Molar mass of I\u2082 = 126.9 g\/mol \u00d7 2 = 253.8 g\/mol<\/strong><\/p>\n\n\n\n<p>This means that 1 mole of molecular iodine weighs <strong>253.8 grams<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Atomic mass vs. Molar mass<\/strong>: The atomic mass of an element is the mass of a single atom, typically measured in atomic mass units (amu or g\/mol). The molar mass is the mass of one mole of molecules or atoms of a substance, expressed in grams per mole (g\/mol). For elements, the atomic mass and the molar mass are numerically equal, but the molar mass applies to a collection of atoms (1 mole).<\/li>\n\n\n\n<li><strong>Iodine in nature<\/strong>: Iodine is a halogen element and is typically found in nature as a diatomic molecule (I\u2082). This is why we multiply the atomic mass of iodine by 2.<\/li>\n\n\n\n<li><strong>Why 253.8 g\/mol?<\/strong> The molar mass of iodine (I) is 126.9 g\/mol, and when we have two iodine atoms in I\u2082, we multiply this value by 2. Hence, the molar mass of I\u2082 is <strong>253.8 g\/mol<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the correct molar mass of molecular iodine (I\u2082) is <strong>253.8 g\/mol<\/strong>.<\/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-banner6-1730.jpeg\" alt=\"\" class=\"wp-image-267971\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the molar mass of molecular iodine, I2: 79.9 g\/mol Only atomic masses, and not molar masses, can be calculated for elements. 159.8 g\/mol 126.9 g\/mol 253.8 g\/mol The Correct Answer and Explanation is: The molar mass of molecular iodine (I\u2082) is calculated by adding the molar masses of two iodine (I) atoms. The atomic [&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-267967","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267967","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=267967"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267967\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267967"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267967"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267967"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}