{"id":195497,"date":"2025-02-28T10:13:11","date_gmt":"2025-02-28T10:13:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=195497"},"modified":"2025-02-28T10:13:14","modified_gmt":"2025-02-28T10:13:14","slug":"how-many-moles-are-there-in-24-grams-of-fef","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/28\/how-many-moles-are-there-in-24-grams-of-fef\/","title":{"rendered":"How many moles are there in 24 grams of FeF"},"content":{"rendered":"\n<p>a) How many moles are there in 24 grams of FeF?<br>b) How many molecules are there in 450 grams of Na\u2082SO\u2084?<br>c) How many moles are there in 2.3 x 10 atoms of Silver (Ag)?<br>d) How many grams are there in 7.4 x 10&#8243; moles of AgNO,?<\/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>Let&#8217;s address each of your questions step by step:<\/p>\n\n\n\n<p><strong>a) How many moles are there in 24 grams of FeF?<\/strong><\/p>\n\n\n\n<p>It seems there might be a typographical error in your query, as &#8220;FeF&#8221; is not a common chemical formula. Perhaps you intended to refer to iron(III) fluoride, which has the chemical formula FeF\u2083. Assuming this is the case, we can calculate the number of moles in 24 grams of FeF\u2083.<\/p>\n\n\n\n<p>First, determine the molar mass of FeF\u2083 by summing the atomic masses of its constituent elements:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Iron (Fe): 55.845 g\/mol<\/li>\n\n\n\n<li>Fluorine (F): 18.998 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Since there are three fluorine atoms in the compound:<\/p>\n\n\n\n<p>Molar mass of FeF\u2083 = 55.845 g\/mol + 3 \u00d7 18.998 g\/mol = 112.839 g\/mol<\/p>\n\n\n\n<p>Next, use the formula:<\/p>\n\n\n\n<p>Number of moles = Mass (g) \/ Molar mass (g\/mol)<\/p>\n\n\n\n<p>For 24 grams of FeF\u2083:<\/p>\n\n\n\n<p>Number of moles = 24 g \/ 112.839 g\/mol \u2248 0.213 moles<\/p>\n\n\n\n<p><strong>b) How many molecules are there in 450 grams of Na\u2082SO\u2084?<\/strong><\/p>\n\n\n\n<p>To find the number of molecules, we first calculate the number of moles and then use Avogadro&#8217;s number to convert moles to molecules.<\/p>\n\n\n\n<p>The molar mass of sodium sulfate (Na\u2082SO\u2084) is calculated as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na): 22.989769 g\/mol \u00d7 2 = 45.979538 g\/mol<\/li>\n\n\n\n<li>Sulfur (S): 32.065 g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 15.999 g\/mol \u00d7 4 = 63.996 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Total molar mass of Na\u2082SO\u2084 = 45.979538 g\/mol + 32.065 g\/mol + 63.996 g\/mol = 142.040538 g\/mol<\/p>\n\n\n\n<p>Number of moles = 450 g \/ 142.040538 g\/mol \u2248 3.168 moles<\/p>\n\n\n\n<p>Using Avogadro&#8217;s number (6.022 \u00d7 10\u00b2\u00b3 molecules\/mol):<\/p>\n\n\n\n<p>Number of molecules = 3.168 moles \u00d7 6.022 \u00d7 10\u00b2\u00b3 molecules\/mol \u2248 1.91 \u00d7 10\u00b2\u2074 molecules<\/p>\n\n\n\n<p><strong>c) How many moles are there in 2.3 \u00d7 10\u00b9\u2070 atoms of Silver (Ag)?<\/strong><\/p>\n\n\n\n<p>To convert atoms to moles, divide the number of atoms by Avogadro&#8217;s number:<\/p>\n\n\n\n<p>Number of moles = Number of atoms \/ Avogadro&#8217;s number<\/p>\n\n\n\n<p>Number of moles = 2.3 \u00d7 10\u00b9\u2070 atoms \/ 6.022 \u00d7 10\u00b2\u00b3 atoms\/mol \u2248 3.82 \u00d7 10\u207b\u00b9\u2074 moles<\/p>\n\n\n\n<p><strong>d) How many grams are there in 7.4 \u00d7 10\u00b9\u2070 moles of AgNO\u2083?<\/strong><\/p>\n\n\n\n<p>First, calculate the molar mass of silver nitrate (AgNO\u2083):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Silver (Ag): 107.8682 g\/mol<\/li>\n\n\n\n<li>Nitrogen (N): 14.0067 g\/mol<\/li>\n\n\n\n<li>Oxygen (O): 15.999 g\/mol \u00d7 3 = 47.997 g\/mol<\/li>\n<\/ul>\n\n\n\n<p>Total molar mass of AgNO\u2083 = 107.8682 g\/mol + 14.0067 g\/mol + 47.997 g\/mol = 169.8719 g\/mol<\/p>\n\n\n\n<p>To find the mass corresponding to 7.4 \u00d7 10\u00b9\u2070 moles:<\/p>\n\n\n\n<p>Mass (g) = Number of moles \u00d7 Molar mass (g\/mol)<\/p>\n\n\n\n<p>Mass = 7.4 \u00d7 10\u00b9\u2070 moles \u00d7 169.8719 g\/mol \u2248 1.26 \u00d7 10\u00b9\u00b3 grams<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>In chemistry, the mole is a fundamental unit used to quantify the amount of a substance. One mole corresponds to Avogadro&#8217;s number (6.022 \u00d7 10\u00b2\u00b3) of entities, whether they are atoms, molecules, ions, or other particles. This large number provides a bridge between the atomic scale and the macroscopic scale we observe.<\/p>\n\n\n\n<p>The molar mass of a compound is the mass of one mole of that substance, expressed in grams per mole (g\/mol). It is calculated by summing the atomic masses of all atoms present in the molecular formula. For instance, the molar mass of FeF\u2083 is derived from adding the atomic mass of one iron atom and three fluorine atoms.<\/p>\n\n\n\n<p>To determine the number of moles from a given mass, divide the mass by the molar mass. Conversely, to find the mass from a given number of moles, multiply the number of moles by the molar mass. When converting between the number of particles (atoms or molecules) and moles, Avogadro&#8217;s number serves as the conversion factor.<\/p>\n\n\n\n<p>These calculations are essential in stoichiometry, allowing chemists to predict the outcomes of chemical reactions, determine reactant quantities, and analyze compounds&#8217; compositions. Accurate molar mass determination and mole calculations are foundational skills in chemistry, enabling precise formulation and understanding of chemical processes.<\/p>\n\n\n\n<p>Understanding these concepts ensures accurate measurements and predictions in chemical experiments and industrial applications, highlighting the importance of the mole as a central unit in chemical quantification.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>a) How many moles are there in 24 grams of FeF?b) How many molecules are there in 450 grams of Na\u2082SO\u2084?c) How many moles are there in 2.3 x 10 atoms of Silver (Ag)?d) How many grams are there in 7.4 x 10&#8243; moles of AgNO,? The Correct Answer and Explanation is : Let&#8217;s address [&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-195497","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195497","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=195497"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195497\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=195497"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=195497"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=195497"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}