{"id":164715,"date":"2024-11-10T12:44:26","date_gmt":"2024-11-10T12:44:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=164715"},"modified":"2024-11-10T12:44:28","modified_gmt":"2024-11-10T12:44:28","slug":"what-is-the-molar-mass-of-boron-b","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/10\/what-is-the-molar-mass-of-boron-b\/","title":{"rendered":"What is the molar mass of boron (B)"},"content":{"rendered":"\n<p>What is the molar mass of boron (B)?<br>A. 5 g\/mol<br>B. 10.81 g<br>O C. 10.81 g\/mol<br>D. 5 g<\/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>The correct answer is <strong>C. 10.81 g\/mol<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The molar mass of an element refers to the mass of one mole of its atoms, and it is typically expressed in grams per mole (g\/mol). To determine the molar mass of boron (B), we need to refer to its atomic mass, which is listed on the periodic table.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Boron has an atomic number of <strong>5<\/strong>, meaning it has 5 protons in its nucleus.<\/li>\n\n\n\n<li>The atomic mass of boron is <strong>approximately 10.81 u<\/strong> (atomic mass units), which is the weighted average of the masses of all naturally occurring isotopes of boron. This value is rounded to <strong>10.81 g\/mol<\/strong> for practical use in calculations involving moles.<\/li>\n<\/ul>\n\n\n\n<p>Since atomic mass is measured in unified atomic mass units (u), and 1 u is equivalent to 1 g\/mol, the atomic mass of boron is directly equal to its molar mass of <strong>10.81 g\/mol<\/strong>. Therefore, option <strong>C<\/strong> is the correct answer.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Why the other options are incorrect:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>A. 5 g\/mol<\/strong>: This is incorrect because the molar mass of boron is much greater than 5 g\/mol. The atomic number (5) does not equate to the molar mass.<\/li>\n\n\n\n<li><strong>B. 10.81 g<\/strong>: This option incorrectly omits the &#8220;per mole&#8221; aspect. The molar mass must be expressed in units of grams per mole (g\/mol), not just grams.<\/li>\n\n\n\n<li><strong>D. 5 g<\/strong>: This is not a correct choice because the value 5 g does not correspond to the molar mass of boron. It only matches the atomic number.<\/li>\n<\/ul>\n\n\n\n<p>Thus, <strong>C. 10.81 g\/mol<\/strong> correctly represents the molar mass of boron, reflecting its atomic mass and providing the correct conversion between atomic mass units and grams per mole.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the molar mass of boron (B)?A. 5 g\/molB. 10.81 gO C. 10.81 g\/molD. 5 g The Correct Answer and Explanation is : The correct answer is C. 10.81 g\/mol. Explanation: The molar mass of an element refers to the mass of one mole of its atoms, and it is typically expressed in grams [&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-164715","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164715","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=164715"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164715\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=164715"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=164715"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=164715"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}