{"id":206553,"date":"2025-04-01T11:34:59","date_gmt":"2025-04-01T11:34:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=206553"},"modified":"2025-04-01T11:35:02","modified_gmt":"2025-04-01T11:35:02","slug":"perform-the-following","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/01\/perform-the-following\/","title":{"rendered":"Perform the following"},"content":{"rendered":"\n<p>Perform the following:<\/p>\n\n\n\n<p>a. Write the formula for copper (II) phosphate.<br>b. Calculate the molecular weight for copper (II) phosphate.<br>c. Calculate the number of moles of copper (II) phosphate in 129.4 g of copper (II) phosphate.<br>d. Calculate the total number of atoms of phosphorus in 129.4 g of copper (II) phosphate.<\/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<h3 class=\"wp-block-heading\">a. Formula for Copper (II) Phosphate:<\/h3>\n\n\n\n<p>Copper (II) phosphate is composed of copper in the +2 oxidation state (Cu\u00b2\u207a) and phosphate ions (PO\u2084\u00b3\u207b). To balance the charges, we need to have two phosphate ions for each copper ion:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The formula for the phosphate ion is PO\u2084\u00b3\u207b.<\/li>\n\n\n\n<li>Copper (II) has a charge of +2, so to balance the -6 charge from two phosphate ions, we need one copper (II) ion.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the formula for copper (II) phosphate is:<br><strong>Cu\u2083(PO\u2084)\u2082<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">b. Calculating the Molecular Weight of Copper (II) Phosphate:<\/h3>\n\n\n\n<p>To calculate the molecular weight of Cu\u2083(PO\u2084)\u2082, we sum the atomic masses of all the atoms in the formula:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Copper (Cu): The atomic mass of copper is approximately 63.55 g\/mol.<\/li>\n\n\n\n<li>Phosphorus (P): The atomic mass of phosphorus is approximately 30.97 g\/mol.<\/li>\n\n\n\n<li>Oxygen (O): The atomic mass of oxygen is approximately 16.00 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Now, calculating the molecular weight:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For copper: There are 3 copper atoms, so ( 3 \\times 63.55 = 190.65 \\, \\text{g\/mol} ).<\/li>\n\n\n\n<li>For phosphorus: There are 2 phosphorus atoms, so ( 2 \\times 30.97 = 61.94 \\, \\text{g\/mol} ).<\/li>\n\n\n\n<li>For oxygen: There are 8 oxygen atoms (4 per phosphate ion and 2 phosphate ions), so ( 8 \\times 16.00 = 128.00 \\, \\text{g\/mol} ).<\/li>\n<\/ul>\n\n\n\n<p>The molecular weight of Cu\u2083(PO\u2084)\u2082 is:<br>[ 190.65 + 61.94 + 128.00 = 380.59 \\, \\text{g\/mol} ].<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">c. Calculating the Number of Moles of Copper (II) Phosphate in 129.4 g:<\/h3>\n\n\n\n<p>To find the number of moles of copper (II) phosphate in 129.4 g, we use the formula:<\/p>\n\n\n\n<p>[<br>\\text{moles} = \\frac{\\text{mass}}{\\text{molar mass}}<br>]<\/p>\n\n\n\n<p>Substitute the given values:<br>[<br>\\text{moles} = \\frac{129.4 \\, \\text{g}}{380.59 \\, \\text{g\/mol}} \\approx 0.340 \\, \\text{moles}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">d. Calculating the Total Number of Atoms of Phosphorus:<\/h3>\n\n\n\n<p>Each molecule of copper (II) phosphate, Cu\u2083(PO\u2084)\u2082, contains 2 phosphorus (P) atoms. Therefore, for 0.340 moles of Cu\u2083(PO\u2084)\u2082, the number of moles of phosphorus atoms is:<\/p>\n\n\n\n<p>[<br>\\text{moles of phosphorus} = 0.340 \\, \\text{moles} \\times 2 \\, \\text{atoms of phosphorus per formula unit} = 0.680 \\, \\text{moles of phosphorus}<br>]<\/p>\n\n\n\n<p>To find the total number of atoms of phosphorus, multiply the moles of phosphorus by Avogadro&#8217;s number (( 6.022 \\times 10^{23} ) atoms\/mol):<\/p>\n\n\n\n<p>[<br>\\text{atoms of phosphorus} = 0.680 \\, \\text{moles} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol} \\approx 4.09 \\times 10^{23} \\, \\text{atoms}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Results:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>a. The formula for copper (II) phosphate is <strong>Cu\u2083(PO\u2084)\u2082<\/strong>.<\/li>\n\n\n\n<li>b. The molecular weight of copper (II) phosphate is <strong>380.59 g\/mol<\/strong>.<\/li>\n\n\n\n<li>c. The number of moles of copper (II) phosphate in 129.4 g is approximately <strong>0.340 moles<\/strong>.<\/li>\n\n\n\n<li>d. The total number of atoms of phosphorus in 129.4 g of copper (II) phosphate is approximately <strong>4.09 \u00d7 10\u00b2\u00b3 atoms<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>These calculations provide an understanding of how to convert between grams, moles, and atoms for chemical compounds, particularly with ionic compounds like copper (II) phosphate.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full is-resized\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/04\/image-10.png\" alt=\"\" class=\"wp-image-206558\" style=\"aspect-ratio:1;width:1200px;height:auto\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Perform the following: a. Write the formula for copper (II) phosphate.b. Calculate the molecular weight for copper (II) phosphate.c. Calculate the number of moles of copper (II) phosphate in 129.4 g of copper (II) phosphate.d. Calculate the total number of atoms of phosphorus in 129.4 g of copper (II) phosphate. The correct answer and explanation [&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-206553","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206553","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=206553"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206553\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206553"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206553"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206553"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}