{"id":166429,"date":"2024-11-13T17:14:35","date_gmt":"2024-11-13T17:14:35","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=166429"},"modified":"2024-11-13T17:14:37","modified_gmt":"2024-11-13T17:14:37","slug":"the-value-of-%ce%b4h-for-the-reaction-below-is-186-kj","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/13\/the-value-of-%ce%b4h-for-the-reaction-below-is-186-kj\/","title":{"rendered":"The value of \u03b4h\u00b0 for the reaction below is -186 kj."},"content":{"rendered":"\n<p>the value of \u03b4h\u00b0 for the reaction below is -186 kj. h 2 (g) cl 2 (g) \u2192 2hcl (g) the value of \u03b4h\u00b0 f for hcl (g) is <strong><em>__<\/em><\/strong> kj\/mol.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To find the value of ( \\Delta H_f^\\circ ) (standard enthalpy of formation) for HCl(g), we can use the relationship between the enthalpy change of a reaction and the standard enthalpies of formation of the reactants and products.<\/p>\n\n\n\n<p>The given reaction is:<\/p>\n\n\n\n<p>[<br>H_2(g) + Cl_2(g) \\rightarrow 2HCl(g)<br>]<\/p>\n\n\n\n<p>The standard enthalpy change of the reaction, ( \\Delta H^\\circ ), is -186 kJ. The standard enthalpy of formation, ( \\Delta H_f^\\circ ), is the enthalpy change when one mole of a compound is formed from its elements in their standard states. For elements like hydrogen and chlorine in their gaseous forms (( H_2(g) ) and ( Cl_2(g) )), the standard enthalpy of formation is zero, since they are in their most stable forms.<\/p>\n\n\n\n<p>To find the ( \\Delta H_f^\\circ ) for HCl(g), we use the following equation for the reaction:<\/p>\n\n\n\n<p>[<br>\\Delta H^\\circ = \\sum \\Delta H_f^\\circ (\\text{products}) &#8211; \\sum \\Delta H_f^\\circ (\\text{reactants})<br>]<\/p>\n\n\n\n<p>For the given reaction:<\/p>\n\n\n\n<p>[<br>\\Delta H^\\circ = [2 \\times \\Delta H_f^\\circ (\\text{HCl(g)})] &#8211; [\\Delta H_f^\\circ (H_2(g)) + \\Delta H_f^\\circ (Cl_2(g))]<br>]<\/p>\n\n\n\n<p>Since the standard enthalpy of formation of ( H_2(g) ) and ( Cl_2(g) ) is zero:<\/p>\n\n\n\n<p>[<br>\\Delta H^\\circ = 2 \\times \\Delta H_f^\\circ (\\text{HCl(g)})<br>]<\/p>\n\n\n\n<p>Substituting the known value for ( \\Delta H^\\circ ):<\/p>\n\n\n\n<p>[<br>-186 \\, \\text{kJ} = 2 \\times \\Delta H_f^\\circ (\\text{HCl(g)})<br>]<\/p>\n\n\n\n<p>Solving for ( \\Delta H_f^\\circ (\\text{HCl(g)}) ):<\/p>\n\n\n\n<p>[<br>\\Delta H_f^\\circ (\\text{HCl(g)}) = \\frac{-186}{2} = -93 \\, \\text{kJ\/mol}<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The value of ( \\Delta H_f^\\circ ) for HCl(g) is <strong>-93 kJ\/mol<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The enthalpy of formation ( \\Delta H_f^\\circ ) refers to the heat change that occurs when one mole of a substance is formed from its constituent elements in their standard states.<\/li>\n\n\n\n<li>In this case, the elements hydrogen (H(_2)) and chlorine (Cl(_2)) are in their standard forms, so their ( \\Delta H_f^\\circ ) values are zero.<\/li>\n\n\n\n<li>The standard enthalpy change of the reaction ( \\Delta H^\\circ ) is given as -186 kJ, which is the heat released when hydrogen and chlorine gases react to form HCl gas.<\/li>\n\n\n\n<li>By using the enthalpy equation for reactions and knowing that the standard enthalpies of formation for H(_2(g)) and Cl(_2(g)) are zero, we can calculate the enthalpy of formation for HCl(g) as -93 kJ\/mol.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>the value of \u03b4h\u00b0 for the reaction below is -186 kj. h 2 (g) cl 2 (g) \u2192 2hcl (g) the value of \u03b4h\u00b0 f for hcl (g) is __ kj\/mol. The Correct Answer and Explanation is: To find the value of ( \\Delta H_f^\\circ ) (standard enthalpy of formation) for HCl(g), we can use [&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-166429","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166429","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=166429"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/166429\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=166429"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=166429"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=166429"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}