{"id":192335,"date":"2025-02-17T13:47:45","date_gmt":"2025-02-17T13:47:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=192335"},"modified":"2025-02-17T13:47:47","modified_gmt":"2025-02-17T13:47:47","slug":"complete-the-table-below-for-calculating-the-molar-mass-of-the-ionic-compound-chromiumii-chloride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/17\/complete-the-table-below-for-calculating-the-molar-mass-of-the-ionic-compound-chromiumii-chloride\/","title":{"rendered":"Complete the table below for calculating the molar mass of the ionic compound chromium(II) chloride"},"content":{"rendered":"\n<p>Complete the table below for calculating the molar mass of the ionic compound chromium(II) chloride. Cation Anion Formula Cr2+ CI Molar mass of ion g\/mol g\/mol X X Number of ions mol mol Molar mass chromium(II) chloride = || Mass of ion in one mole of chromium(II) chloride g\/mol g 6<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>I have displayed the table for you with the correct values. Here&#8217;s the explanation:<\/p>\n\n\n\n<p>To calculate the molar mass of chromium(II) chloride (Cr2Cl2), we need to consider both the cation (Cr\u00b2\u207a) and the anion (Cl\u207b). Chromium (Cr) has a molar mass of approximately 52.00 g\/mol, and chlorine (Cl) has a molar mass of about 35.45 g\/mol.<\/p>\n\n\n\n<p>In the formula Cr\u2082Cl\u2082:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The cation, Cr\u00b2\u207a, appears twice (since we have Cr2+), so we multiply its molar mass by 2.<\/li>\n\n\n\n<li>The anion, Cl\u207b, also appears twice, so we multiply its molar mass by 2 as well.<\/li>\n<\/ul>\n\n\n\n<p>Molar mass of Cr2+ = 52.00 g\/mol \u00d7 2 = 104.00 g\/mol<br>Molar mass of Cl- = 35.45 g\/mol \u00d7 2 = 70.90 g\/mol<\/p>\n\n\n\n<p>When we add these values together, we get the molar mass of chromium(II) chloride:<br>104.00 g\/mol + 70.90 g\/mol = 174.90 g\/mol.<\/p>\n\n\n\n<p>So, the molar mass of chromium(II) chloride is approximately 174.9 g\/mol, and this is the mass of one mole of the compound.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Complete the table below for calculating the molar mass of the ionic compound chromium(II) chloride. Cation Anion Formula Cr2+ CI Molar mass of ion g\/mol g\/mol X X Number of ions mol mol Molar mass chromium(II) chloride = || Mass of ion in one mole of chromium(II) chloride g\/mol g 6 The Correct Answer and [&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-192335","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192335","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=192335"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192335\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192335"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192335"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192335"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}