To calculate the molar mass of Cu2O and the percentage by weight of Cu in Cu2O, let’s break it down step by step:<\/p>\n\n\n\n
Step 1: Determine the Atomic Masses<\/h3>\n\n\n\n
The atomic mass of copper (Cu) is approximately 63.55 g\/mol<\/strong>, and the atomic mass of oxygen (O) is 16.00 g\/mol<\/strong>.<\/p>\n\n\n\n In Cu2O, there are 2 copper (Cu) atoms<\/strong> and 1 oxygen (O) atom<\/strong>. The molar mass of Cu2O can be calculated by adding the atomic masses of all the elements in the formula:<\/p>\n\n\n\n So, the molar mass of Cu2O is:Molar Mass of Cu2O=127.10\u2009g\/mol+16.00\u2009g\/mol=143.10\u2009g\/mol\\text{Molar Mass of Cu2O} = 127.10 \\, \\text{g\/mol} + 16.00 \\, \\text{g\/mol} = 143.10 \\, \\text{g\/mol}Molar Mass of Cu2O=127.10g\/mol+16.00g\/mol=143.10g\/mol<\/p>\n\n\n\n Now, we calculate the percentage by weight of copper (Cu) in Cu2O. This can be done by dividing the total mass of copper in the formula by the molar mass of Cu2O and multiplying by 100.<\/p>\n\n\n\n The percentage by weight of copper in Cu2O is:%\u2009Cu=(127.10\u2009g\/mol143.10\u2009g\/mol)\u00d7100=88.8%\\% \\, \\text{Cu} = \\left( \\frac{127.10 \\, \\text{g\/mol}}{143.10 \\, \\text{g\/mol}} \\right) \\times 100 = 88.8\\%%Cu=(143.10g\/mol127.10g\/mol\u200b)\u00d7100=88.8%<\/p>\n\n\n\n This means that in every mole of Cu2O, 88.8% of the mass is due to copper.<\/p>\n\n\n\n Calculate the molar mass of Cu2O and the % by weight of Cu in Cu2O. The Correct Answer and Explanation is: To calculate the molar mass of Cu2O and the percentage by weight of Cu in Cu2O, let’s break it down step by step: Step 1: Determine the Atomic Masses The atomic mass of copper […]<\/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-258406","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/258406","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=258406"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/258406\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=258406"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=258406"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=258406"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 2: Calculate the Molar Mass of Cu2O<\/h3>\n\n\n\n
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Step 3: Calculate the Percentage by Weight of Cu in Cu2O<\/h3>\n\n\n\n
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Final Answer:<\/h3>\n\n\n\n
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