{"id":146377,"date":"2024-09-30T19:25:31","date_gmt":"2024-09-30T19:25:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=146377"},"modified":"2024-09-30T19:25:33","modified_gmt":"2024-09-30T19:25:33","slug":"construct-the-expression-for-kc-for-the-following-reaction-4hclaq-o2g-2h2o0-2cl2g","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/09\/30\/construct-the-expression-for-kc-for-the-following-reaction-4hclaq-o2g-2h2o0-2cl2g\/","title":{"rendered":"Construct the expression for Kc for the following reaction 4HCl(aq) + O2(g) = 2H2O(0) + 2Cl2(g )"},"content":{"rendered":"\n

Construct the expression for Kc for the following reaction 4HCl(aq) + O2(g) = 2H2O(0) + 2Cl2(g )<\/p>\n\n\n\n

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

To construct the equilibrium constant expression ( K_c ) for the reaction:<\/p>\n\n\n\n

[ 4 \\text{HCl} (aq) + \\text{O}_2 (g) \\rightleftharpoons 2 \\text{H}_2\\text{O} (l) + 2 \\text{Cl}_2 (g) ]<\/p>\n\n\n\n

we follow the guidelines for writing the equilibrium constant expression based on the stoichiometry of the balanced chemical equation.<\/p>\n\n\n\n

Expression for ( K_c )<\/h3>\n\n\n\n

The equilibrium constant ( K_c ) is defined as the ratio of the concentration of products to the concentration of reactants, each raised to the power of their respective coefficients in the balanced equation.<\/p>\n\n\n\n

For the reaction given:<\/p>\n\n\n\n

[
K_c = \\frac{[\\text{H}_2\\text{O}]^2 [\\text{Cl}_2]^2}{[\\text{HCl}]^4 [\\text{O}_2]}
]<\/p>\n\n\n\n

Explanation<\/h3>\n\n\n\n
    \n
  1. Understanding ( K_c )<\/strong>: The equilibrium constant ( K_c ) quantifies the ratio of the concentration of products to reactants at equilibrium. It indicates how far a reaction proceeds toward products under specific conditions.<\/li>\n\n\n\n
  2. Coefficients and Concentrations<\/strong>: Each term in the expression corresponds to a species involved in the reaction. The concentrations of gaseous and aqueous species are included, while the concentrations of solids and liquids are omitted from the expression. In this reaction, (\\text{H}_2\\text{O}) is a liquid, so it is not included in the ( K_c ) expression. The concentrations are expressed in terms of molarity (moles per liter).<\/li>\n\n\n\n
  3. Applying Stoichiometry<\/strong>: The coefficients in the balanced equation are crucial. For example, since there are 2 moles of (\\text{H}_2\\text{O}) produced, its concentration is squared. Similarly, the concentration of (\\text{Cl}_2) is squared, and the concentrations of (\\text{HCl}) and (\\text{O}_2) are raised to the fourth and first power, respectively, based on their coefficients.<\/li>\n\n\n\n
  4. Equilibrium Considerations<\/strong>: At equilibrium, the concentrations of reactants and products remain constant, and this expression allows chemists to calculate the ratio of these concentrations, predicting the position of equilibrium for various conditions.<\/li>\n<\/ol>\n\n\n\n

    In summary, the expression for ( K_c ) provides insights into the dynamics of the reaction and the favorability of product formation under equilibrium conditions.<\/p>\n","protected":false},"excerpt":{"rendered":"

    Construct the expression for Kc for the following reaction 4HCl(aq) + O2(g) = 2H2O(0) + 2Cl2(g ) The Correct Answer and Explanation is : To construct the equilibrium constant expression ( K_c ) for the reaction: [ 4 \\text{HCl} (aq) + \\text{O}_2 (g) \\rightleftharpoons 2 \\text{H}_2\\text{O} (l) + 2 \\text{Cl}_2 (g) ] we follow the […]<\/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-146377","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/146377","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=146377"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/146377\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=146377"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=146377"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=146377"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}