{"id":189774,"date":"2025-02-10T08:34:01","date_gmt":"2025-02-10T08:34:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=189774"},"modified":"2025-02-10T08:34:03","modified_gmt":"2025-02-10T08:34:03","slug":"if-you-started-with-0-0364-mol-of-copperii-chloride-and-ended-with-2-26-g-of-isolated-copper","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/10\/if-you-started-with-0-0364-mol-of-copperii-chloride-and-ended-with-2-26-g-of-isolated-copper\/","title":{"rendered":"If you started with 0.0364 mol of copper(II) chloride and ended with 2.26 g of isolated copper"},"content":{"rendered":"\n<p>If you started with 0.0364 mol of copper(II) chloride and ended with 2.26 g of isolated copper, what is your percent yield? The molar mass of copper(II) chloride is 134.45 g\/mol and the molar mass of copper is 63.55 g\/mol.<\/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>To calculate the percent yield, we first need to determine the theoretical yield and then use the formula for percent yield:<\/p>\n\n\n\n<p>[<br>\\text{Percent Yield} = \\left( \\frac{\\text{Actual Yield}}{\\text{Theoretical Yield}} \\right) \\times 100<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Calculate the Theoretical Yield<\/h3>\n\n\n\n<p>The reaction we&#8217;re working with involves the reduction of copper(II) chloride (CuCl\u2082) to copper (Cu). The balanced equation for this reaction is:<\/p>\n\n\n\n<p>[<br>\\text{CuCl}_2 \\to \\text{Cu} + \\text{Cl}_2<br>]<\/p>\n\n\n\n<p>From the balanced equation, 1 mole of CuCl\u2082 produces 1 mole of Cu.<\/p>\n\n\n\n<p>We know:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The starting amount of CuCl\u2082 is 0.0364 mol.<\/li>\n\n\n\n<li>The molar mass of copper (Cu) is 63.55 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Since the mole ratio between CuCl\u2082 and Cu is 1:1, 0.0364 mol of CuCl\u2082 will theoretically yield 0.0364 mol of Cu. To convert moles of copper to grams, use the molar mass of copper:<\/p>\n\n\n\n<p>[<br>\\text{Theoretical Yield of Cu} = 0.0364 \\, \\text{mol} \\times 63.55 \\, \\text{g\/mol} = 2.31 \\, \\text{g}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate Percent Yield<\/h3>\n\n\n\n<p>The actual yield of copper is given as 2.26 g. Now, we can calculate the percent yield:<\/p>\n\n\n\n<p>[<br>\\text{Percent Yield} = \\left( \\frac{2.26 \\, \\text{g}}{2.31 \\, \\text{g}} \\right) \\times 100 = 97.8\\%<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The percent yield is a measure of the efficiency of a chemical reaction. It compares the actual amount of product obtained from the reaction (in this case, copper) to the theoretical amount predicted by stoichiometric calculations. The closer the actual yield is to the theoretical yield, the more efficient the reaction is. A percent yield of 97.8% means that nearly all of the copper(II) chloride reacted to produce copper, with very little loss or side reactions. This is a high yield, indicating a successful and efficient reaction.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>If you started with 0.0364 mol of copper(II) chloride and ended with 2.26 g of isolated copper, what is your percent yield? The molar mass of copper(II) chloride is 134.45 g\/mol and the molar mass of copper is 63.55 g\/mol. The Correct Answer and Explanation is : To calculate the percent yield, we first need [&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-189774","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189774","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=189774"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/189774\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=189774"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=189774"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=189774"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}