The correct answer is d. all of the above<\/strong>.<\/p>\n\n\n\n Here\u2019s a breakdown of each choice:<\/p>\n\n\n\n Since all three choices describe 1 mole of diborane in different ways (volume, mass, and number of molecules), the correct answer is d. all of the above<\/strong>.<\/p>\n\n\n\n Which of the following represents 1 mole of diborane gas, B2H6?a. 22.4 L diborane gas at STPb. 27.68 g diborane gasc. 6.02 \u00d7 1023 diborane gas moleculesd. all of the abovee. none of the above The correct answer and explanation is : The correct answer is d. all of the above. Here\u2019s a breakdown of […]<\/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-206229","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206229","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=206229"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/206229\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=206229"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=206229"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=206229"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}\n
At Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 L. This is a direct application of the Ideal Gas Law (PV = nRT), where 1 mole of gas at 0\u00b0C (273.15 K) and 1 atm pressure has a volume of 22.4 L. Since diborane gas is treated as an ideal gas under these conditions, it follows this rule, so 1 mole of diborane gas will occupy 22.4 L at STP.<\/li>\n\n\n\n
To find the molar mass of diborane (B2H6), we need to sum the atomic masses of boron (B) and hydrogen (H). Boron has an atomic mass of approximately 10.81 g\/mol, and hydrogen has an atomic mass of 1.008 g\/mol. The molar mass of diborane is:
[
\\text{Molar mass of B2H6} = 2(10.81) + 6(1.008) = 21.62 + 6.048 = 27.668 \\, \\text{g\/mol}
]
Thus, 1 mole of diborane weighs approximately 27.68 grams.<\/li>\n\n\n\n
This is the definition of 1 mole of any substance according to Avogadro\u2019s number. 1 mole of any substance contains 6.02 \u00d7 10\u00b2\u00b3 particles (atoms, molecules, etc.), so 1 mole of diborane will contain 6.02 \u00d7 10\u00b2\u00b3 molecules of B2H6.<\/li>\n<\/ol>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-1551.png\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"