{"id":241909,"date":"2025-07-04T04:11:44","date_gmt":"2025-07-04T04:11:44","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=241909"},"modified":"2025-07-04T04:11:46","modified_gmt":"2025-07-04T04:11:46","slug":"how-many-chlorine-atoms-would-there-be-in-the-145-grams-of-copper-ii-chlorate-cuclo32","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/how-many-chlorine-atoms-would-there-be-in-the-145-grams-of-copper-ii-chlorate-cuclo32\/","title":{"rendered":"How many chlorine atoms would there be in the 145 grams of copper (II) chlorate Cu(ClO3)2"},"content":{"rendered":"\n

How many chlorine atoms would there be in the 145 grams of copper (II) chlorate Cu(ClO3)2? Hint: The molar mass of copper (II) chlorate is 230.45 g\/mol.<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To find how many chlorine atoms are present in 145 grams of copper (II) chlorate (Cu(ClO\u2083)\u2082), we will use the concept of moles, molar mass, and Avogadro’s number.<\/p>\n\n\n\n

Step 1: Calculate the number of moles of Cu(ClO\u2083)\u2082<\/h3>\n\n\n\n

The molar mass of copper (II) chlorate is given as 230.45 g\/mol<\/strong>. To find the number of moles of Cu(ClO\u2083)\u2082 in 145 grams, we divide the mass by the molar mass.Number of moles of Cu(ClO\u2083)\u2082=Mass of Cu(ClO\u2083)\u2082Molar mass of Cu(ClO\u2083)\u2082=145\u2009g230.45\u2009g\/mol\u22480.629\u2009mol\\text{Number of moles of Cu(ClO\u2083)\u2082} = \\frac{\\text{Mass of Cu(ClO\u2083)\u2082}}{\\text{Molar mass of Cu(ClO\u2083)\u2082}} = \\frac{145 \\, \\text{g}}{230.45 \\, \\text{g\/mol}} \\approx 0.629 \\, \\text{mol}Number of moles of Cu(ClO\u2083)\u2082=Molar mass of Cu(ClO\u2083)\u2082Mass of Cu(ClO\u2083)\u2082\u200b=230.45g\/mol145g\u200b\u22480.629mol<\/p>\n\n\n\n

Step 2: Calculate the number of chlorine atoms<\/h3>\n\n\n\n

In one formula unit of Cu(ClO\u2083)\u2082, there are 2 chlorine (Cl)<\/strong> atoms. Therefore, the total number of chlorine atoms in 0.629 moles of Cu(ClO\u2083)\u2082 is:Number of chlorine atoms=Number of moles of Cu(ClO\u2083)\u2082\u00d7Avogadro\u2019s number\u00d7Number of chlorine atoms per formula unit\\text{Number of chlorine atoms} = \\text{Number of moles of Cu(ClO\u2083)\u2082} \\times \\text{Avogadro’s number} \\times \\text{Number of chlorine atoms per formula unit}Number of chlorine atoms=Number of moles of Cu(ClO\u2083)\u2082\u00d7Avogadro\u2019s number\u00d7Number of chlorine atoms per formula unitNumber of chlorine atoms=0.629\u2009mol\u00d76.022\u00d71023\u2009atoms\/mol\u00d72\\text{Number of chlorine atoms} = 0.629 \\, \\text{mol} \\times 6.022 \\times 10^{23} \\, \\text{atoms\/mol} \\times 2Number of chlorine atoms=0.629mol\u00d76.022\u00d71023atoms\/mol\u00d72Number of chlorine atoms\u22487.57\u00d71023\u2009atoms\\text{Number of chlorine atoms} \\approx 7.57 \\times 10^{23} \\, \\text{atoms}Number of chlorine atoms\u22487.57\u00d71023atoms<\/p>\n\n\n\n

Final Answer:<\/h3>\n\n\n\n

There are approximately 7.57 \u00d7 10\u00b2\u00b3 chlorine atoms<\/strong> in 145 grams of copper (II) chlorate (Cu(ClO\u2083)\u2082).<\/p>\n\n\n\n

This approach makes use of moles to convert mass to the number of particles, which is a crucial concept in stoichiometry for understanding how many atoms or molecules are in a given mass of a substance.<\/p>\n\n\n\n

\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

How many chlorine atoms would there be in the 145 grams of copper (II) chlorate Cu(ClO3)2? Hint: The molar mass of copper (II) chlorate is 230.45 g\/mol. The Correct Answer and Explanation is: To find how many chlorine atoms are present in 145 grams of copper (II) chlorate (Cu(ClO\u2083)\u2082), we will use the concept of […]<\/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-241909","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241909","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=241909"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241909\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=241909"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=241909"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=241909"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}