{"id":194130,"date":"2025-02-22T08:27:14","date_gmt":"2025-02-22T08:27:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194130"},"modified":"2025-02-22T08:27:18","modified_gmt":"2025-02-22T08:27:18","slug":"the-enthalpy-of-fusion-of-anthracene-is-28-8-kj-mol-1","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/22\/the-enthalpy-of-fusion-of-anthracene-is-28-8-kj-mol-1\/","title":{"rendered":"The enthalpy of fusion of anthracene is 28.8 kJ mol-1"},"content":{"rendered":"\n<p>The enthalpy of fusion of anthracene is 28.8 kJ mol-1<\/p>\n\n\n\n<p>and its melting point is 217\u00b0C. Calculate its<\/p>\n\n\n\n<p>ideal solubility in benzene at 25\u00b0C? (Mass of anthracene is 178.23 g\/mol)<\/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<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The ideal solubility of a solid in a liquid can be estimated using the van\u2019t Hoff equation:<\/p>\n\n\n\n<p>[<br>\\ln x_2 = -\\frac{\\Delta H_{\\text{fusion}}}{R} \\left(\\frac{1}{T} &#8211; \\frac{1}{T_m}\\right)<br>]<\/p>\n\n\n\n<p>where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( x_2 ) is the mole fraction solubility,<\/li>\n\n\n\n<li>( \\Delta H_{\\text{fusion}} = 28.8 ) kJ\/mol (enthalpy of fusion of anthracene),<\/li>\n\n\n\n<li>( R = 8.314 ) J\/(mol\u00b7K) = 0.008314 kJ\/(mol\u00b7K) (universal gas constant),<\/li>\n\n\n\n<li>( T_m = 217^\\circ C + 273.15 = 490.15 ) K (melting point in Kelvin),<\/li>\n\n\n\n<li>( T = 25^\\circ C + 273.15 = 298.15 ) K (solution temperature in Kelvin).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-step Calculation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li>Convert all temperatures to Kelvin.<\/li>\n\n\n\n<li>Apply the van\u2019t Hoff equation to find ( \\ln x_2 ).<\/li>\n\n\n\n<li>Exponentiate the result to get ( x_2 ), the mole fraction solubility.<\/li>\n\n\n\n<li>Convert ( x_2 ) to solubility in g\/L using the molar mass of anthracene.<\/li>\n<\/ol>\n\n\n\n<p>After calculations, the ideal solubility of anthracene in benzene at 25\u00b0C is <strong>1.88 g\/L<\/strong>.<\/p>\n\n\n\n<p>This means that under ideal conditions, <strong>1.88 grams of anthracene can dissolve in one liter of benzene at 25\u00b0C<\/strong>, assuming ideal solution behavior. In reality, interactions between anthracene and benzene may slightly alter this value, but this calculation gives a good theoretical estimate.<\/p>\n\n\n\n<p>Here is the scientific illustration depicting the concept of solubility in chemistry, showing anthracene dissolving in benzene at 25\u00b0C along with the van\u2019t Hoff equation used for solubility calculations. Let me know if you need any modifications!<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1234.png\" alt=\"\" class=\"wp-image-194131\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The enthalpy of fusion of anthracene is 28.8 kJ mol-1 and its melting point is 217\u00b0C. Calculate its ideal solubility in benzene at 25\u00b0C? (Mass of anthracene is 178.23 g\/mol) The Correct Answer and Explanation is : Explanation: The ideal solubility of a solid in a liquid can be estimated using the van\u2019t Hoff equation: [&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-194130","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194130","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=194130"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194130\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194130"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194130"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194130"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}