{"id":249786,"date":"2025-07-09T21:15:27","date_gmt":"2025-07-09T21:15:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249786"},"modified":"2025-07-09T21:15:30","modified_gmt":"2025-07-09T21:15:30","slug":"the-reaction-below-has-a-kp-value-of-145","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/the-reaction-below-has-a-kp-value-of-145\/","title":{"rendered":"The reaction below has a Kp value of 145.\u00a0"},"content":{"rendered":"\n
\"\"<\/figure>\n\n\n\n

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

The correct answer is 2.12 x 10\u2076.<\/p>\n\n\n\n

To find the value of the equilibrium constant in terms of concentration (Kc) from the given equilibrium constant in terms of partial pressure (Kp), we utilize the following standard formula which connects the two constants:<\/p>\n\n\n\n

Kp = Kc(RT)^\u0394n<\/p>\n\n\n\n

Let’s break down each part of this equation and determine the values needed for the calculation.<\/p>\n\n\n\n

    \n
  1. Identify Known Values<\/strong>:\n
      \n
    • Kp = 145 (given)<\/li>\n\n\n\n
    • T = 25\u00b0C. For gas law calculations, temperature must be in Kelvin. T(K) = T(\u00b0C) + 273.15. So, T = 25 + 273.15 = 298.15 K.<\/li>\n\n\n\n
    • R is the ideal gas constant. The appropriate value to use here is 0.08206 L\u00b7atm\/(mol\u00b7K).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Calculate the Change in Moles of Gas (\u0394n)<\/strong>:
      The term \u0394n represents the change in the number of moles of gas from the reactant side to the product side of the reaction. It is calculated as:
      \u0394n = (total moles of gaseous products) \u2013 (total moles of gaseous reactants)Let’s examine the balanced chemical equation:
      C\u2083H\u2088(g) + 5 O\u2082(g) \u21cc 3 CO\u2082(g) + 4 H\u2082O(l)It is very important to only count the moles of substances in the gaseous state (g). In this reaction, the water (H\u2082O) is a liquid (l), so it is not included in the calculation for \u0394n.
      • Moles of gaseous products = moles of CO\u2082(g) = 3 mol<\/li>
      • Moles of gaseous reactants = moles of C\u2083H\u2088(g) + moles of O\u2082(g) = 1 mol + 5 mol = 6 mol<\/li><\/ul>Now, we can calculate \u0394n:
        \u0394n = 3 \u2013 6 = -3<\/li>\n\n\n\n
      • Solve for Kc<\/strong>:
        We need to rearrange the original formula to solve for Kc:
        Kc = Kp \/ (RT)^\u0394nNow, we can substitute all the known values into this rearranged equation:
        Kc = 145 \/ ( (0.08206) * (298.15) )\u207b\u00b3
        Kc = 145 \/ (24.466)\u207b\u00b3Calculating the value inside the parenthesis raised to the power of -3:
        (24.466)\u207b\u00b3 \u2248 6.82 x 10\u207b\u2075Finally, divide Kp by this value to find Kc:
        Kc = 145 \/ (6.82 x 10\u207b\u2075)
        Kc \u2248 2,125,000When expressed in scientific notation and rounded to three significant figures, the result is:
        Kc \u2248 2.12 x 10\u2076<\/li>\n<\/ol>\n\n\n\n

        This value corresponds to the third answer choice.<\/p>\n\n\n\n

        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        The Correct Answer and Explanation is: The correct answer is 2.12 x 10\u2076. To find the value of the equilibrium constant in terms of concentration (Kc) from the given equilibrium constant in terms of partial pressure (Kp), we utilize the following standard formula which connects the two constants: Kp = Kc(RT)^\u0394n Let’s break down each […]<\/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-249786","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249786","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=249786"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249786\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249786"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249786"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249786"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}