The formula for copper(II) phosphate is Cu\u2083(PO\u2084)\u2082. In this compound, copper exists in a +2 oxidation state, and phosphate is the anion with the formula PO\u2084\u00b3\u207b. The structure shows that there are 3 copper ions (Cu\u00b2\u207a) and 2 phosphate ions (PO\u2084\u00b3\u207b) per formula unit.<\/p>\n\n\n\n
To determine how many phosphorus (P) atoms are present in 3.70 mol of copper(II) phosphate (Cu\u2083(PO\u2084)\u2082), follow these steps:<\/p>\n\n\n\n
Step 1: Understanding the formula<\/h3>\n\n\n\n
In the formula Cu\u2083(PO\u2084)\u2082, there are 2 phosphate ions (PO\u2084) per formula unit<\/strong>. Each phosphate ion contains 1 phosphorus (P) atom<\/strong>. Therefore, for every formula unit of Cu\u2083(PO\u2084)\u2082, there are 2 phosphorus atoms.<\/p>\n\n\n\n Since there are 2 phosphorus atoms in 1 formula unit of Cu\u2083(PO\u2084)\u2082, there are also 2 phosphorus atoms in 1 mole of Cu\u2083(PO\u2084)\u2082.<\/p>\n\n\n\n Avogadro\u2019s number tells us that 1 mole of a substance contains 6.022 \u00d7 10\u00b2\u00b3<\/strong> entities (atoms, molecules, etc.). Therefore, 1 mole of Cu\u2083(PO\u2084)\u2082 contains 2 \u00d7 6.022 \u00d7 10\u00b2\u00b3<\/strong> phosphorus atoms.<\/p>\n\n\n\n The total number of phosphorus atoms in 3.70 mol of Cu\u2083(PO\u2084)\u2082 is:3.70\u2009mol\u00d7(2\u00d76.022\u00d71023\u2009atoms\/mol)=4.45\u00d71024\u2009P atoms3.70 \\, \\text{mol} \\times \\left(2 \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol}\\right) = 4.45 \\times 10^{24} \\, \\text{P atoms}3.70mol\u00d7(2\u00d76.022\u00d71023atoms\/mol)=4.45\u00d71024P atoms<\/p>\n\n\n\n Thus, the number of phosphorus atoms in 3.70 mol of copper(II) phosphate is 4.45 \u00d7 10\u00b2\u2074<\/strong> phosphorus atoms.<\/p>\n\n\n\n The number of phosphorus atoms in 3.70 mol of copper(II) phosphate is 4.45 \u00d7 10\u00b2\u2074<\/strong> P atoms.<\/p>\n\n\n\n What is the formula for copper(II) phosphate? Capitalization and punctuation count. Formula: Cu3(PO4)2. How many atoms of phosphorus are in 3.70 mol of copper(II) phosphate? Number of P atoms: 229.4. The Correct Answer and Explanation is: The formula for copper(II) phosphate is Cu\u2083(PO\u2084)\u2082. In this compound, copper exists in a +2 oxidation state, and phosphate […]<\/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-248405","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248405","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=248405"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/248405\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=248405"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=248405"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=248405"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 2: Find the number of phosphorus atoms per mole of copper(II) phosphate<\/h3>\n\n\n\n
Step 3: Use Avogadro\u2019s number to calculate the number of atoms<\/h3>\n\n\n\n
Step 4: Calculate the number of phosphorus atoms in 3.70 mol of copper(II) phosphate<\/h3>\n\n\n\n
Final Answer:<\/h3>\n\n\n\n
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