{"id":262059,"date":"2025-07-20T11:22:31","date_gmt":"2025-07-20T11:22:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=262059"},"modified":"2025-07-20T11:22:33","modified_gmt":"2025-07-20T11:22:33","slug":"how-many-atoms-are-in-55-3-g-of-potassium-bromite-kbro2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/20\/how-many-atoms-are-in-55-3-g-of-potassium-bromite-kbro2\/","title":{"rendered":"How many atoms are in 55.3 g of potassium bromite (KBrO2)"},"content":{"rendered":"\n<p>How many atoms are in 55.3 g of potassium bromite (KBrO2)?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find how many atoms are in 55.3 g of potassium bromite (KBrO2), the following steps are involved:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the molar mass of KBrO2<\/h3>\n\n\n\n<p>The molar mass is the sum of the atomic masses of all elements in one mole of the compound.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Potassium (K) has an atomic mass of approximately 39.1 g\/mol.<\/li>\n\n\n\n<li>Bromine (Br) has an atomic mass of approximately 79.9 g\/mol.<\/li>\n\n\n\n<li>Oxygen (O) has an atomic mass of approximately 16.0 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Now, calculate the molar mass of KBrO2: Molar&nbsp;mass&nbsp;of&nbsp;KBrO2=39.1\u2009g\/mol&nbsp;(K)+79.9\u2009g\/mol&nbsp;(Br)+2\u00d716.0\u2009g\/mol&nbsp;(O)=39.1+79.9+32.0=151.0\u2009g\/mol\\text{Molar mass of KBrO2} = 39.1 \\, \\text{g\/mol (K)} + 79.9 \\, \\text{g\/mol (Br)} + 2 \\times 16.0 \\, \\text{g\/mol (O)} = 39.1 + 79.9 + 32.0 = 151.0 \\, \\text{g\/mol}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the number of moles in 55.3 g of KBrO2<\/h3>\n\n\n\n<p>The number of moles is calculated by dividing the mass of the substance by its molar mass: Number&nbsp;of&nbsp;moles=55.3\u2009g151.0\u2009g\/mol=0.366\u2009mol\\text{Number of moles} = \\frac{55.3 \\, \\text{g}}{151.0 \\, \\text{g\/mol}} = 0.366 \\, \\text{mol}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculate the total number of formula units in 0.366 moles<\/h3>\n\n\n\n<p>Avogadro&#8217;s number tells us that one mole of any substance contains 6.022\u00d710236.022 \\times 10^{23} formula units (atoms, molecules, or ions). For KBrO2, we have: Number&nbsp;of&nbsp;formula&nbsp;units=0.366\u2009mol\u00d76.022\u00d71023\u2009units\/mol=2.2\u00d71023\u2009formula&nbsp;units\\text{Number of formula units} = 0.366 \\, \\text{mol} \\times 6.022 \\times 10^{23} \\, \\text{units\/mol} = 2.2 \\times 10^{23} \\, \\text{formula units}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Calculate the number of atoms<\/h3>\n\n\n\n<p>Each formula unit of KBrO2 contains:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>1 potassium (K) atom<\/li>\n\n\n\n<li>1 bromine (Br) atom<\/li>\n\n\n\n<li>2 oxygen (O) atoms<\/li>\n<\/ul>\n\n\n\n<p>So, the total number of atoms in each formula unit is: Total&nbsp;atoms&nbsp;per&nbsp;formula&nbsp;unit=1+1+2=4\u2009atoms\\text{Total atoms per formula unit} = 1 + 1 + 2 = 4 \\, \\text{atoms}<\/p>\n\n\n\n<p>Now, calculate the total number of atoms: Total&nbsp;number&nbsp;of&nbsp;atoms=2.2\u00d71023\u2009formula&nbsp;units\u00d74\u2009atoms=8.8\u00d71023\u2009atoms\\text{Total number of atoms} = 2.2 \\times 10^{23} \\, \\text{formula units} \\times 4 \\, \\text{atoms} = 8.8 \\times 10^{23} \\, \\text{atoms}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The total number of atoms in 55.3 g of potassium bromite (KBrO2) is approximately 8.8\u00d710238.8 \\times 10^{23} atoms.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>How many atoms are in 55.3 g of potassium bromite (KBrO2)? The correct answer and explanation is: To find how many atoms are in 55.3 g of potassium bromite (KBrO2), the following steps are involved: Step 1: Determine the molar mass of KBrO2 The molar mass is the sum of the atomic masses of all [&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-262059","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/262059","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=262059"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/262059\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=262059"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=262059"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=262059"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}