{"id":197908,"date":"2025-03-07T19:20:40","date_gmt":"2025-03-07T19:20:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=197908"},"modified":"2025-03-07T19:20:43","modified_gmt":"2025-03-07T19:20:43","slug":"the-density-of-germanium-ge-is-5-323-g-ml-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/07\/the-density-of-germanium-ge-is-5-323-g-ml-2\/","title":{"rendered":"The density of germanium (Ge) is 5.323 g\/mL"},"content":{"rendered":"\n<p>The density of germanium (Ge) is 5.323 g\/mL. Enter the volume value in units of mL to the nearest 0.01 mL and include the unit. Enter mass value in units of grams to the nearest 0.001 g and include the unit. The volume of 145.1 g of Ge to the nearest 0.01 mL is Number Units. The mass of 15.4 mL of Ge to the nearest 0.001 g is Number Units.<\/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<p>To calculate both the volume and mass of Germanium (Ge) given its density, we can use the formula for density:<\/p>\n\n\n\n<p>[<br>\\text{Density} = \\frac{\\text{Mass}}{\\text{Volume}}<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Density of Germanium (Ge) = 5.323 g\/mL<\/li>\n\n\n\n<li>Mass is in grams (g)<\/li>\n\n\n\n<li>Volume is in milliliters (mL)<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">1. Volume Calculation for 145.1 g of Ge:<\/h3>\n\n\n\n<p>The formula can be rearranged to calculate the volume:<\/p>\n\n\n\n<p>[<br>\\text{Volume} = \\frac{\\text{Mass}}{\\text{Density}}<br>]<\/p>\n\n\n\n<p>Substituting the given values:<\/p>\n\n\n\n<p>[<br>\\text{Volume} = \\frac{145.1 \\, \\text{g}}{5.323 \\, \\text{g\/mL}} \\approx 27.3 \\, \\text{mL}<br>]<\/p>\n\n\n\n<p>So, the volume of 145.1 g of Ge is approximately <strong>27.30 mL<\/strong> (rounded to the nearest 0.01 mL).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">2. Mass Calculation for 15.4 mL of Ge:<\/h3>\n\n\n\n<p>Now, we use the same density formula to calculate the mass for a given volume. We rearrange the density formula to solve for mass:<\/p>\n\n\n\n<p>[<br>\\text{Mass} = \\text{Density} \\times \\text{Volume}<br>]<\/p>\n\n\n\n<p>Substituting the given values:<\/p>\n\n\n\n<p>[<br>\\text{Mass} = 5.323 \\, \\text{g\/mL} \\times 15.4 \\, \\text{mL} \\approx 82.0 \\, \\text{g}<br>]<\/p>\n\n\n\n<p>So, the mass of 15.4 mL of Ge is approximately <strong>82.000 g<\/strong> (rounded to the nearest 0.001 g).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Summary of Results:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The volume of 145.1 g of Ge is <strong>27.30 mL<\/strong>.<\/li>\n\n\n\n<li>The mass of 15.4 mL of Ge is <strong>82.000 g<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Density is a physical property that represents how much mass is contained in a given volume. In this case, the density of Germanium is provided as 5.323 g\/mL. Using the formula for density, we can easily calculate either the mass or volume when one is known.<\/p>\n\n\n\n<p>The first part of the question asks for the volume of a known mass (145.1 g). By dividing the mass by the density, we calculate the volume. The second part asks for the mass of a known volume (15.4 mL). By multiplying the volume by the density, we calculate the mass.<\/p>\n\n\n\n<p>Both of these calculations follow basic principles of density, and the results have been rounded according to the required significant figures.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The density of germanium (Ge) is 5.323 g\/mL. Enter the volume value in units of mL to the nearest 0.01 mL and include the unit. Enter mass value in units of grams to the nearest 0.001 g and include the unit. The volume of 145.1 g of Ge to the nearest 0.01 mL is Number [&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-197908","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/197908","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=197908"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/197908\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=197908"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=197908"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=197908"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}