{"id":262396,"date":"2025-07-20T15:10:28","date_gmt":"2025-07-20T15:10:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=262396"},"modified":"2025-07-20T15:10:30","modified_gmt":"2025-07-20T15:10:30","slug":"if-0-25-grams-of-sodium-borohydride-are-used-for-this-reaction","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/20\/if-0-25-grams-of-sodium-borohydride-are-used-for-this-reaction\/","title":{"rendered":"If 0.25 grams of sodium borohydride are used for this reaction"},"content":{"rendered":"\n<p>If 0.25 grams of sodium borohydride are used for this reaction, how many moles of sodium borohydride were added?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To calculate how many moles of sodium borohydride (NaBH\u2084) were added, we will use the formula: Moles=MassMolar&nbsp;Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Identify the mass of sodium borohydride<\/h3>\n\n\n\n<p>From the question, the mass of sodium borohydride is given as 0.25 grams.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Calculate the molar mass of sodium borohydride<\/h3>\n\n\n\n<p>Sodium borohydride (NaBH\u2084) consists of:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium (Na) with an atomic mass of approximately 23.0 g\/mol,<\/li>\n\n\n\n<li>Boron (B) with an atomic mass of approximately 10.8 g\/mol,<\/li>\n\n\n\n<li>Hydrogen (H) with an atomic mass of approximately 1.008 g\/mol, and<\/li>\n\n\n\n<li>Four hydrogen atoms from the borohydride part, each with a mass of 1.008 g\/mol.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the molar mass of NaBH\u2084 is: Molar&nbsp;Mass&nbsp;of&nbsp;NaBH\u2084=23.0+10.8+(4\u00d71.008)=23.0+10.8+4.032=37.832&nbsp;g\/mol\\text{Molar Mass of NaBH\u2084} = 23.0 + 10.8 + (4 \\times 1.008) = 23.0 + 10.8 + 4.032 = 37.832 \\text{ g\/mol}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Calculate the moles of sodium borohydride<\/h3>\n\n\n\n<p>Now that we know the mass and the molar mass, we can calculate the number of moles: Moles&nbsp;of&nbsp;NaBH\u2084=0.25&nbsp;grams37.832&nbsp;g\/mol\u22480.00661&nbsp;moles\\text{Moles of NaBH\u2084} = \\frac{0.25 \\text{ grams}}{37.832 \\text{ g\/mol}} \\approx 0.00661 \\text{ moles}<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The number of moles of sodium borohydride added is approximately 0.00661 moles.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Moles are a measure of the amount of substance, and the relationship between mass and moles allows chemists to quantify how much of a substance is present. To convert mass into moles, we need to know the molar mass of the substance. By dividing the mass of sodium borohydride by its molar mass, we get the number of moles that were used in the reaction.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>If 0.25 grams of sodium borohydride are used for this reaction, how many moles of sodium borohydride were added? The correct answer and explanation is: To calculate how many moles of sodium borohydride (NaBH\u2084) were added, we will use the formula: Moles=MassMolar&nbsp;Mass\\text{Moles} = \\frac{\\text{Mass}}{\\text{Molar Mass}} Step 1: Identify the mass of sodium borohydride From the [&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-262396","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/262396","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=262396"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/262396\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=262396"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=262396"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=262396"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}