{"id":167929,"date":"2024-11-16T12:07:50","date_gmt":"2024-11-16T12:07:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=167929"},"modified":"2024-11-16T12:07:52","modified_gmt":"2024-11-16T12:07:52","slug":"calculate-the-value-of-kp-at-25-%e2%88%98c-where-kc-40-a2-b-a2b","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/16\/calculate-the-value-of-kp-at-25-%e2%88%98c-where-kc-40-a2-b-a2b\/","title":{"rendered":"Calculate the value of Kp at 25 \u2218C, where Kc = 40 A2 + B &#8211;> A2B"},"content":{"rendered":"\n<p>Calculate the value of Kp at 25 \u2218C, where Kc = 40 A2 + B &#8211;> A2B<\/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 calculate the equilibrium constant ( K_p ) in terms of partial pressures from ( K_c ) (equilibrium constant in terms of concentration) for the given reaction:<\/p>\n\n\n\n<p>[<br>\\text{A}_2 + \\text{B} \\rightarrow \\text{A}_2\\text{B}<br>]<\/p>\n\n\n\n<p>The relationship between ( K_p ) and ( K_c ) is given by the following equation:<\/p>\n\n\n\n<p>[<br>K_p = K_c \\left( RT \\right)^{\\Delta n}<br>]<\/p>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>( K_p ) is the equilibrium constant in terms of partial pressures.<\/li>\n\n\n\n<li>( K_c ) is the equilibrium constant in terms of concentrations.<\/li>\n\n\n\n<li>( R ) is the gas constant, which is 0.0821 L\u00b7atm\/(mol\u00b7K).<\/li>\n\n\n\n<li>( T ) is the temperature in Kelvin.<\/li>\n\n\n\n<li>( \\Delta n ) is the change in the number of moles of gas between products and reactants.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Calculation:<\/h3>\n\n\n\n<h4 class=\"wp-block-heading\">1. Determine ( \\Delta n ):<\/h4>\n\n\n\n<p>First, we need to find the change in the number of moles of gas during the reaction. From the given reaction:<\/p>\n\n\n\n<p>[<br>\\text{A}_2 (g) + \\text{B} (g) \\rightarrow \\text{A}_2\\text{B} (g)<br>]<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Moles of gas on the left (reactants): 1 mole of ( \\text{A}_2 ) + 1 mole of ( \\text{B} ) = 2 moles of gas.<\/li>\n\n\n\n<li>Moles of gas on the right (products): 1 mole of ( \\text{A}_2\\text{B} ) = 1 mole of gas.<\/li>\n<\/ul>\n\n\n\n<p>Thus, ( \\Delta n = 1 &#8211; 2 = -1 ).<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">2. Convert temperature to Kelvin:<\/h4>\n\n\n\n<p>Given that the temperature is 25\u00b0C, we convert it to Kelvin:<\/p>\n\n\n\n<p>[<br>T = 25 + 273.15 = 298.15 \\, \\text{K}<br>]<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">3. Substitute values into the equation:<\/h4>\n\n\n\n<p>Now we can use the formula to calculate ( K_p ):<\/p>\n\n\n\n<p>[<br>K_p = K_c \\left( RT \\right)^{\\Delta n}<br>]<\/p>\n\n\n\n<p>[<br>K_p = 40 \\times (0.0821 \\times 298.15)^{-1}<br>]<\/p>\n\n\n\n<p>[<br>K_p = 40 \\times (24.47)^{-1}<br>]<\/p>\n\n\n\n<p>[<br>K_p = 40 \\times 0.0409<br>]<\/p>\n\n\n\n<p>[<br>K_p \\approx 1.636<br>]<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Answer:<\/h3>\n\n\n\n<p>The value of ( K_p ) at 25\u00b0C is approximately <strong>1.636<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The calculation follows the formula that relates ( K_p ) and ( K_c ), which accounts for the change in the number of moles of gases and the temperature. The negative value of ( \\Delta n ) indicates that there is a reduction in the number of moles of gas as the reaction progresses from reactants to products, affecting the relationship between ( K_p ) and ( K_c ). The decrease in moles of gas leads to a smaller value for ( K_p ) compared to ( K_c ).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Calculate the value of Kp at 25 \u2218C, where Kc = 40 A2 + B &#8211;> A2B The Correct Answer and Explanation is: To calculate the equilibrium constant ( K_p ) in terms of partial pressures from ( K_c ) (equilibrium constant in terms of concentration) for the given reaction: [\\text{A}_2 + \\text{B} \\rightarrow \\text{A}_2\\text{B}] [&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-167929","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167929","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=167929"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167929\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=167929"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=167929"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=167929"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}