{"id":239312,"date":"2025-07-02T19:43:58","date_gmt":"2025-07-02T19:43:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=239312"},"modified":"2025-07-02T19:44:00","modified_gmt":"2025-07-02T19:44:00","slug":"indicate-how-the-concentration-of-each-species-in-the-chemical-equation-will-change-to-reestablish-equilibrium-after-changing-the-concentration-of-the-reactant-or-product","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/02\/indicate-how-the-concentration-of-each-species-in-the-chemical-equation-will-change-to-reestablish-equilibrium-after-changing-the-concentration-of-the-reactant-or-product\/","title":{"rendered":"Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after changing the concentration of the reactant or product"},"content":{"rendered":"\n

Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after changing the concentration of the reactant or product: An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. C2H4(g) + Cl2(g) \u00e2\u2021\u0152 2C2H4Cl(g) After the concentration of C2H4 is increased: After the concentration of C2H4Cl2 is increased: Answer Book Uncorrected<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

Of course. Here is the correctly filled-out table and a detailed explanation.<\/p>\n\n\n\n

Correct Answer<\/h3>\n\n\n\n

Chemical Equation:<\/strong> C\u2082H\u2084(g) + Cl\u2082(g) \u21cc 2C\u2082H\u2084Cl\u2082(g)<\/p>\n\n\n\n

Condition<\/td>C\u2082H\u2084<\/td>Cl\u2082<\/td>2C\u2082H\u2084Cl\u2082<\/td><\/tr>
after the concentration of C\u2082H\u2084 is increased<\/strong><\/td>\u2191<\/td>\u2193<\/td>\u2191<\/td><\/tr>
after the concentration of C\u2082H\u2084Cl\u2082 is increased<\/strong><\/td>\u2191<\/td>\u2191<\/td>\u2191<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n

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

This problem is governed by Le Ch\u00e2telier’s Principle<\/strong>, which states that if a change (or “stress”) is applied to a system at equilibrium, the system will adjust itself to counteract the change and re-establish a new equilibrium. The stresses here are changes in the concentration of a reactant and a product.<\/p>\n\n\n\n

Scenario 1: After the concentration of C\u2082H\u2084 is increased<\/strong><\/p>\n\n\n\n

    \n
  1. The Stress:<\/strong>\u00a0The concentration of the reactant C\u2082H\u2084 is increased. This disrupts the existing equilibrium.<\/li>\n\n\n\n
  2. The Shift:<\/strong>\u00a0According to Le Ch\u00e2telier’s Principle, the system will try to reduce the concentration of the added C\u2082H\u2084. It can do this by favoring the forward reaction, which consumes the reactants. Therefore, the equilibrium will\u00a0shift to the right<\/strong>, towards the product side.<\/li>\n\n\n\n
  3. The Result:<\/strong>\n
      \n
    • C\u2082H\u2084:<\/strong>\u00a0The system consumes C\u2082H\u2084 to shift right. However, the shift does not consume all of the C\u2082H\u2084 that was initially added. As a result, the new equilibrium concentration of C\u2082H\u2084 will be\u00a0higher<\/strong>\u00a0than it was in the original equilibrium. (\u2191)<\/li>\n\n\n\n
    • Cl\u2082:<\/strong>\u00a0As the equilibrium shifts to the right, the other reactant, Cl\u2082, is also consumed. Its concentration will\u00a0decrease<\/strong>. (\u2193)<\/li>\n\n\n\n
    • C\u2082H\u2084Cl\u2082:<\/strong>\u00a0The forward reaction produces C\u2082H\u2084Cl\u2082. Therefore, its concentration will\u00a0increase<\/strong>. (\u2191)<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

      Scenario 2: After the concentration of C\u2082H\u2084Cl\u2082 is increased<\/strong><\/p>\n\n\n\n

        \n
      1. The Stress:<\/strong>\u00a0The concentration of the product, C\u2082H\u2084Cl\u2082, is increased.<\/li>\n\n\n\n
      2. The Shift:<\/strong>\u00a0To counteract this stress, the system will favor the reaction that consumes the added product. This is the reverse reaction. Therefore, the equilibrium will\u00a0shift to the left<\/strong>, towards the reactant side.<\/li>\n\n\n\n
      3. The Result:<\/strong>\n
          \n
        • C\u2082H\u2084Cl\u2082:<\/strong>\u00a0The system consumes the product to shift left. However, just as in the first scenario, the shift does not consume all of the added C\u2082H\u2084Cl\u2082. The new equilibrium concentration of C\u2082H\u2084Cl\u2082 will be\u00a0higher<\/strong>\u00a0than its original concentration. (\u2191)<\/li>\n\n\n\n
        • C\u2082H\u2084:<\/strong>\u00a0As the equilibrium shifts to the left, the reactant C\u2082H\u2084 is produced. Its concentration will\u00a0increase<\/strong>. (\u2191)<\/li>\n\n\n\n
        • Cl\u2082:<\/strong>\u00a0The other reactant, Cl\u2082, is also produced during the shift to the left. Its concentration will also\u00a0increase<\/strong>. (\u2191)<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
          \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

          Indicate how the concentration of each species in the chemical equation will change to reestablish equilibrium after changing the concentration of the reactant or product: An up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration. C2H4(g) + […]<\/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-239312","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239312","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=239312"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239312\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=239312"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=239312"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=239312"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}