{"id":193378,"date":"2025-02-19T10:59:20","date_gmt":"2025-02-19T10:59:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=193378"},"modified":"2025-02-19T10:59:22","modified_gmt":"2025-02-19T10:59:22","slug":"diborane-b2h6-molar-mass-27-69-g-mol-can-be-made-from-sodium-borohydride-nabh-molar-mass-37-85-g-mol-by-reacting-it-with-iodine-in-the-following-reaction-2nabh4-s12-b2he-g-2-nal-s-h2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/19\/diborane-b2h6-molar-mass-27-69-g-mol-can-be-made-from-sodium-borohydride-nabh-molar-mass-37-85-g-mol-by-reacting-it-with-iodine-in-the-following-reaction-2nabh4-s12-b2he-g-2-nal-s-h2\/","title":{"rendered":"Diborane (B2H6, molar mass 27.69 g\/mol) can be made from sodium borohydride (NaBH, molar mass 37.85 g\/mol) by reacting it with iodine in the following reaction: 2NaBH4 (s)+12 B2He (g)+ 2 Nal (s)+ H2 (9) If 1.203 g NaBH4 is combined with excess l2 and 0.295 g B2Hs is isolated"},"content":{"rendered":"\n

Diborane (B2H6, molar mass 27.69 g\/mol) can be made from sodium borohydride (NaBH, molar mass 37.85 g\/mol) by reacting it with iodine in the following reaction: 2NaBH4 (s)+12 B2He (g)+ 2 Nal (s)+ H2 (9) If 1.203 g NaBH4 is combined with excess l2 and 0.295 g B2Hs is isolated, what is the percent yield of B2H6?<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The percent yield of B2H6 (diborane) is approximately 67.04%.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

The reaction provided involves the conversion of sodium borohydride (NaBH4) into diborane (B2H6) through a reaction with iodine (I2). To calculate the percent yield, we follow these steps:<\/p>\n\n\n\n

    \n
  1. Convert mass of NaBH4 to moles<\/strong>:
    The molar mass of NaBH4 is 37.85 g\/mol. Given that 1.203 grams of NaBH4 is used, we calculate the moles of NaBH4: [
    \\text{moles of NaBH4} = \\frac{1.203 \\, \\text{g}}{37.85 \\, \\text{g\/mol}} \\approx 0.0318 \\, \\text{mol}
    ]<\/li>\n\n\n\n
  2. Determine moles of B2H6 produced<\/strong>:
    According to the balanced chemical equation, 2 moles of NaBH4 produce 1 mole of B2H6. Thus, the moles of B2H6 produced theoretically can be calculated as: [
    \\text{moles of B2H6 (theoretical)} = \\frac{0.0318 \\, \\text{mol NaBH4}}{2} = 0.0159 \\, \\text{mol B2H6}
    ]<\/li>\n\n\n\n
  3. Convert mass of B2H6 obtained to moles<\/strong>:
    The molar mass of B2H6 is 27.69 g\/mol. With 0.295 grams of B2H6 isolated, we convert this to moles: [
    \\text{moles of B2H6 (obtained)} = \\frac{0.295 \\, \\text{g}}{27.69 \\, \\text{g\/mol}} \\approx 0.0106 \\, \\text{mol B2H6}
    ]<\/li>\n\n\n\n
  4. Calculate percent yield<\/strong>:
    The percent yield is the ratio of the actual yield (moles obtained) to the theoretical yield (moles predicted) multiplied by 100: [
    \\text{percent yield} = \\left( \\frac{0.0106 \\, \\text{mol B2H6}}{0.0159 \\, \\text{mol B2H6}} \\right) \\times 100 \\approx 67.04\\%
    ]<\/li>\n<\/ol>\n\n\n\n

    This means that 67.04% of the theoretical B2H6 was produced in the reaction.<\/p>\n\n\n\n

    I will now generate an image of the chemical equation for the reaction.<\/p>\n\n\n\n

    Here is an image of the chemical equation for the reaction you asked about. Let me know if you need further clarification!<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    Diborane (B2H6, molar mass 27.69 g\/mol) can be made from sodium borohydride (NaBH, molar mass 37.85 g\/mol) by reacting it with iodine in the following reaction: 2NaBH4 (s)+12 B2He (g)+ 2 Nal (s)+ H2 (9) If 1.203 g NaBH4 is combined with excess l2 and 0.295 g B2Hs is isolated, what is the percent yield […]<\/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-193378","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193378","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=193378"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193378\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=193378"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=193378"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=193378"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}