{"id":227931,"date":"2025-06-06T15:27:55","date_gmt":"2025-06-06T15:27:55","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=227931"},"modified":"2025-06-06T15:27:57","modified_gmt":"2025-06-06T15:27:57","slug":"how-many-grams-are-in-3-moles-of-na","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/06\/how-many-grams-are-in-3-moles-of-na\/","title":{"rendered":"How many grams are in 3 moles of Na"},"content":{"rendered":"\n<p>How many grams are in 3 moles of Nal?<br>How many grams are in 3 moles of Nal?<\/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<h6 class=\"wp-block-heading\">ChatGPT said:<\/h6>\n\n\n\n<h3 class=\"wp-block-heading\">Correct Answer:<\/h3>\n\n\n\n<p><strong>There are 449.37 grams in 3 moles of NaI (Sodium Iodide).<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Explanation<\/h3>\n\n\n\n<p>To determine how many grams are in 3 moles of <strong>NaI (sodium iodide)<\/strong>, we need to use the <strong>molar mass<\/strong> of the compound and apply a simple formula from chemistry:<\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><strong>Mass (g) = Number of moles \u00d7 Molar mass (g\/mol)<\/strong><\/p>\n<\/blockquote>\n\n\n\n<h4 class=\"wp-block-heading\">Step 1: Determine the Molar Mass of NaI<\/h4>\n\n\n\n<p>NaI is a binary ionic compound made up of:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Na<\/strong> = Sodium (atomic mass \u2248 22.99 g\/mol)<\/li>\n\n\n\n<li><strong>I<\/strong> = Iodine (atomic mass \u2248 126.90 g\/mol)<\/li>\n<\/ul>\n\n\n\n<p>Add these two together:<\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><strong>Molar mass of NaI = 22.99 + 126.90 = 149.89 g\/mol<\/strong><\/p>\n<\/blockquote>\n\n\n\n<h4 class=\"wp-block-heading\">Step 2: Multiply by the Number of Moles<\/h4>\n\n\n\n<p>You are given 3 moles of NaI.<\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><strong>Mass = 3 moles \u00d7 149.89 g\/mol = 449.67 grams<\/strong><\/p>\n<\/blockquote>\n\n\n\n<p>So, <strong>3 moles of NaI = 449.67 grams<\/strong>.<\/p>\n\n\n\n<p><em>(Note: Some periodic tables may round atomic masses slightly differently, which may cause tiny variations. For instance, using 126.91 for iodine results in 149.90 g\/mol and a final value of 449.70 g. All are considered accurate within reasonable precision.)<\/em><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Importance of Moles and Molar Mass in Chemistry<\/h3>\n\n\n\n<p>Understanding the relationship between moles and grams is fundamental in chemistry because atoms and molecules are too small to count individually. The <strong>mole<\/strong> is a standard unit used to express amounts of a substance based on number (Avogadro\u2019s number, 6.022\u00d710236.022 \\times 10^{23}6.022\u00d71023) rather than weight. The <strong>molar mass<\/strong> translates this number into grams for practical use in the lab.<\/p>\n\n\n\n<p>In this case, knowing that 1 mole of NaI weighs 149.89 grams allows chemists to precisely measure out amounts needed for reactions, especially in biological or industrial settings where accurate dosing matters.<\/p>\n\n\n\n<p>So, 3 moles of NaI corresponds to <strong>449.67 grams<\/strong> of the compound.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner4-547.jpeg\" alt=\"\" class=\"wp-image-227932\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>How many grams are in 3 moles of Nal?How many grams are in 3 moles of Nal? The Correct Answer and Explanation is: ChatGPT said: Correct Answer: There are 449.37 grams in 3 moles of NaI (Sodium Iodide). Step-by-Step Explanation To determine how many grams are in 3 moles of NaI (sodium iodide), we need [&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-227931","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227931","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=227931"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227931\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=227931"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=227931"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=227931"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}