{"id":257572,"date":"2025-07-17T14:33:27","date_gmt":"2025-07-17T14:33:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=257572"},"modified":"2025-07-17T14:33:29","modified_gmt":"2025-07-17T14:33:29","slug":"for-this-question-you-must-do-all-of-your-calculations-and-your-answer-with-proper-sig-figs","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/17\/for-this-question-you-must-do-all-of-your-calculations-and-your-answer-with-proper-sig-figs\/","title":{"rendered":"For this question, you must do all of your calculations and your answer with proper sig figs."},"content":{"rendered":"\n<p>For this question, you must do all of your calculations and your answer with proper sig figs. During an experiment, you use 1.68 g of copper to start your reaction. After you carry through all the different steps, you recover 1.90 g of copper. What is the percent error of the recovered copper? Enter your answer with the correct number of significant figures and the correct sign (but do not enter units).<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate the percent error, we use the formula:Percent&nbsp;Error=\u2223Experimental&nbsp;Value\u2212Accepted&nbsp;Value\u2223\u2223Accepted&nbsp;Value\u2223\u00d7100\\text{Percent Error} = \\frac{\\left| \\text{Experimental Value} &#8211; \\text{Accepted Value} \\right|}{\\left| \\text{Accepted Value} \\right|} \\times 100Percent&nbsp;Error=\u2223Accepted&nbsp;Value\u2223\u2223Experimental&nbsp;Value\u2212Accepted&nbsp;Value\u2223\u200b\u00d7100<\/p>\n\n\n\n<p>In this case:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>experimental value<\/strong> is the mass of copper recovered, which is <strong>1.90 g<\/strong>.<\/li>\n\n\n\n<li>The <strong>accepted value<\/strong> is the initial amount of copper used, which is <strong>1.68 g<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Now, let&#8217;s plug these values into the formula:Percent&nbsp;Error=\u22231.90\u22121.68\u2223\u22231.68\u2223\u00d7100\\text{Percent Error} = \\frac{\\left| 1.90 &#8211; 1.68 \\right|}{\\left| 1.68 \\right|} \\times 100Percent&nbsp;Error=\u22231.68\u2223\u22231.90\u22121.68\u2223\u200b\u00d7100Percent&nbsp;Error=0.221.68\u00d7100\\text{Percent Error} = \\frac{0.22}{1.68} \\times 100Percent&nbsp;Error=1.680.22\u200b\u00d7100Percent&nbsp;Error=0.13095\u00d7100=13.1\\text{Percent Error} = 0.13095 \\times 100 = 13.1Percent&nbsp;Error=0.13095\u00d7100=13.1<\/p>\n\n\n\n<p>So, the <strong>percent error<\/strong> is <strong>13.1%<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Significant Figures<\/strong>: In the problem, both values (1.68 g and 1.90 g) have <strong>3 significant figures<\/strong>. When performing arithmetic with measured quantities, the result should be expressed with the correct number of significant figures. Here, the difference (0.22) has 2 significant figures, so the final answer should be rounded to <strong>3 significant figures<\/strong> to match the precision of the given data.<\/li>\n\n\n\n<li><strong>Absolute Error<\/strong>: The absolute difference between the experimental and accepted values is 0.22 g. This is the discrepancy between the amount of copper used and the amount recovered.<\/li>\n\n\n\n<li><strong>Result<\/strong>: The final percent error is reported as <strong>13.1%<\/strong>, rounded to 3 significant figures.<\/li>\n<\/ol>\n\n\n\n<p>This calculation shows the discrepancy between the expected and actual recovery of copper, indicating that the recovered amount was slightly higher than initially used, but the error is not excessively large.<\/p>\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-banner6-793.jpeg\" alt=\"\" class=\"wp-image-257573\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>For this question, you must do all of your calculations and your answer with proper sig figs. During an experiment, you use 1.68 g of copper to start your reaction. After you carry through all the different steps, you recover 1.90 g of copper. What is the percent error of the recovered copper? Enter 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-257572","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257572","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=257572"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257572\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=257572"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=257572"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=257572"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}