{"id":259002,"date":"2025-07-18T16:09:48","date_gmt":"2025-07-18T16:09:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=259002"},"modified":"2025-07-18T16:09:50","modified_gmt":"2025-07-18T16:09:50","slug":"the-molecular-formula-of-disulfur-dioxide-is-s2o2-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/18\/the-molecular-formula-of-disulfur-dioxide-is-s2o2-2\/","title":{"rendered":"The molecular formula of disulfur dioxide is S2O2"},"content":{"rendered":"\n<p> The molecular formula of disulfur dioxide is S2O2. What is the empirical formula of disulfur dioxide? Question 2 In Lab #7, you collected these values: mass of crucible 21.3456 g mass of crucible plus copper wire = 21.4409 g mass of crucible plus copper sulfide = 21.4649 g Calculate the moles of copper (round your answer to five decimal places) 0.00150 0.01550 0.00220 0.00110<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Question 1: Empirical Formula of Disulfur Dioxide (S\u2082O\u2082)<\/h3>\n\n\n\n<p>The molecular formula of disulfur dioxide is given as <strong>S\u2082O\u2082<\/strong>. To find the <strong>empirical formula<\/strong>, we need to reduce the subscripts in the molecular formula to their simplest whole-number ratio.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The molecular formula is <strong>S\u2082O\u2082<\/strong>, meaning there are 2 sulfur atoms and 2 oxygen atoms.<\/li>\n\n\n\n<li>To simplify the ratio, divide both the number of sulfur atoms and the number of oxygen atoms by their greatest common divisor, which is <strong>2<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>So, dividing both subscripts by 2:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>S\u2082 \u2192 S\u2081<\/strong><\/li>\n\n\n\n<li><strong>O\u2082 \u2192 O\u2081<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Thus, the <strong>empirical formula<\/strong> of disulfur dioxide is <strong>SO<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Question 2: Moles of Copper Calculation<\/h3>\n\n\n\n<p>The masses collected in the experiment are as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass of the crucible = <strong>21.3456 g<\/strong><\/li>\n\n\n\n<li>Mass of the crucible + copper wire = <strong>21.4409 g<\/strong><\/li>\n\n\n\n<li>Mass of the crucible + copper sulfide = <strong>21.4649 g<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Step 1: Calculate the mass of copper wire and copper sulfide<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Mass of copper wire = Mass of the crucible + copper wire &#8211; Mass of the crucible\n<ul class=\"wp-block-list\">\n<li><strong>21.4409 g &#8211; 21.3456 g = 0.0953 g<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>Mass of copper sulfide = Mass of the crucible + copper sulfide &#8211; Mass of the crucible\n<ul class=\"wp-block-list\">\n<li><strong>21.4649 g &#8211; 21.3456 g = 0.1193 g<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p><strong>Step 2: Calculate the mass of copper (Cu)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The difference between the mass of copper wire and the mass of copper sulfide gives the mass of sulfur that reacted with copper:\n<ul class=\"wp-block-list\">\n<li><strong>Mass of sulfur = 0.1193 g &#8211; 0.0953 g = 0.0240 g<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p>Since copper sulfide (CuS) consists of copper (Cu) and sulfur (S), we know that the mass of copper remains constant, and sulfur reacts with it to form copper sulfide.<\/p>\n\n\n\n<p><strong>Step 3: Find the moles of copper<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The molar mass of copper (Cu) is <strong>63.55 g\/mol<\/strong>.<\/li>\n\n\n\n<li>Using the mass of copper wire (which is the mass of copper before reaction):\n<ul class=\"wp-block-list\">\n<li><strong>Moles of copper = Mass of copper \/ Molar mass of copper<\/strong><\/li>\n\n\n\n<li><strong>Moles of copper = 0.0953 g \/ 63.55 g\/mol<\/strong><\/li>\n\n\n\n<li><strong>Moles of copper = 0.00150 mol<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p>Thus, the number of moles of copper is <strong>0.00150 mol<\/strong>, and the correct answer is <strong>0.00150<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For the empirical formula, the goal is to simplify the molecular formula to its lowest ratio. The ratio of sulfur to oxygen atoms is 2:2, so we divide both by 2 to get the empirical formula <strong>SO<\/strong>.<\/li>\n\n\n\n<li>In the second question, the key step was to determine the mass of copper, then convert it to moles using the molar mass of copper (63.55 g\/mol). The calculated moles of copper were <strong>0.00150 mol<\/strong>, which corresponds to the given options.<\/li>\n<\/ul>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner9-286.jpeg\" alt=\"\" class=\"wp-image-259003\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molecular formula of disulfur dioxide is S2O2. What is the empirical formula of disulfur dioxide? Question 2 In Lab #7, you collected these values: mass of crucible 21.3456 g mass of crucible plus copper wire = 21.4409 g mass of crucible plus copper sulfide = 21.4649 g Calculate the moles of copper (round your [&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-259002","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259002","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=259002"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/259002\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=259002"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=259002"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=259002"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}