{"id":233335,"date":"2025-06-13T04:45:13","date_gmt":"2025-06-13T04:45:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=233335"},"modified":"2025-06-13T04:45:15","modified_gmt":"2025-06-13T04:45:15","slug":"to-work-out-the-theoretical-yield-of-the-preparation-of-dibenzalacetone-it-is-useful-to-first-have-a-reaction-equation-complete-with-molar-ratios","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/13\/to-work-out-the-theoretical-yield-of-the-preparation-of-dibenzalacetone-it-is-useful-to-first-have-a-reaction-equation-complete-with-molar-ratios\/","title":{"rendered":"To work out the theoretical yield of the preparation of dibenzalacetone, it is useful to first have a reaction equation complete with molar ratios."},"content":{"rendered":"\n

To work out the theoretical yield of the preparation of dibenzalacetone, it is useful to first have a reaction equation complete with molar ratios. Using the following equation, what is the correct stoichiometric ratio of acetone:benzaladehyde to yield dibenzalacetone? +\\ Acetone Benzaldehyde Dibenzalacetone 2:1 1:2 1:1<\/p>\n\n\n\n

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

Correct Answer:<\/strong> 1:2 (Acetone : Benzaldehyde)<\/strong><\/p>\n\n\n\n

\n\n\n\n

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

To calculate the theoretical yield of dibenzalacetone, we must first understand the balanced chemical equation and the stoichiometric ratio between the reactants. The reaction used in the preparation of dibenzalacetone is a classic example of an aldol condensation<\/strong> reaction. In this synthesis, acetone (CH\u2083COCH\u2083)<\/strong> reacts with benzaldehyde (C\u2086H\u2085CHO)<\/strong> in the presence of a base (commonly NaOH) to produce dibenzalacetone (C\u2081\u2087H\u2081\u2084O)<\/strong> and water as a by-product.<\/p>\n\n\n\n

The balanced reaction is: CH3COCH3+2\u2009C6H5CHO\u2192C17H14O+H2O\\text{CH}_3\\text{COCH}_3 + 2 \\, \\text{C}_6\\text{H}_5\\text{CHO} \\rightarrow \\text{C}_{17}\\text{H}_{14}\\text{O} + \\text{H}_2\\text{O}CH3\u200bCOCH3\u200b+2C6\u200bH5\u200bCHO\u2192C17\u200bH14\u200bO+H2\u200bO<\/p>\n\n\n\n

In this reaction:<\/p>\n\n\n\n

    \n
  • 1 mole of acetone<\/strong> reacts with 2 moles of benzaldehyde<\/strong>.<\/li>\n\n\n\n
  • This occurs because acetone contains two \u03b1-hydrogens<\/strong>, one on each side of the carbonyl group, allowing it to undergo two aldol condensations \u2014 one with each molecule of benzaldehyde.<\/li>\n\n\n\n
  • The final product, dibenzalacetone<\/strong>, has two benzylidene groups<\/strong> (\u2013CH=CH\u2013C\u2086H\u2085) attached to the central carbonyl carbon of acetone.<\/li>\n<\/ul>\n\n\n\n

    This stoichiometric ratio is critical for determining the limiting reagent<\/strong> and calculating the theoretical yield<\/strong> of the product. If benzaldehyde is present in excess, then acetone will be the limiting reagent. Conversely, if the ratio is inverted, benzaldehyde becomes the limiting reagent.<\/p>\n\n\n\n

    Understanding and using the correct molar ratio \u2014 1 mole of acetone to 2 moles of benzaldehyde (1:2)<\/strong> \u2014 ensures that the reaction can proceed completely and form one mole of dibenzalacetone per mole of acetone.<\/p>\n\n\n\n

    Therefore, the correct stoichiometric ratio for this reaction is:<\/p>\n\n\n\n

    \n

    \u2705 1:2 (Acetone : Benzaldehyde)<\/strong><\/p>\n\n\n\n

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

    To work out the theoretical yield of the preparation of dibenzalacetone, it is useful to first have a reaction equation complete with molar ratios. Using the following equation, what is the correct stoichiometric ratio of acetone:benzaladehyde to yield dibenzalacetone? +\\ Acetone Benzaldehyde Dibenzalacetone 2:1 1:2 1:1 The Correct Answer and Explanation is: Correct Answer: 1:2 […]<\/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-233335","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233335","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=233335"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233335\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233335"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233335"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233335"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}