{"id":261376,"date":"2025-07-20T05:56:01","date_gmt":"2025-07-20T05:56:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=261376"},"modified":"2025-07-20T05:56:04","modified_gmt":"2025-07-20T05:56:04","slug":"consider-the-initial-rate-data-at-a-certain-temperature-in-the-table-for-the-reaction-described-by-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/20\/consider-the-initial-rate-data-at-a-certain-temperature-in-the-table-for-the-reaction-described-by-2\/","title":{"rendered":"Consider the initial-rate data at a certain temperature in the table for the reaction described by"},"content":{"rendered":"\n<p>Consider the initial-rate data at a certain temperature in the table for the reaction described by: [NO2]o (M) 0.650 1.10 1.76 <a href=\"M\">O3<\/a> 0.800 0.800 1.40 Initial rate (Ms) 3.25 x 10^4 5.50 x 10^4 15.40 x 10^4 2 NO2(g) + O3(g) -> N2O5(g) + O2(g) Determine the value and units of the rate constant, k. Units: 4.9 x 10^4 M^-1 s^-1<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/image-578.png\" alt=\"\" class=\"wp-image-261377\"\/><\/figure>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>\u2083 (m) by comparing Experiments 2 and 3. We use the fact that n = 1:<\/p>\n\n\n\n<p>(Rate\u2083 \/ Rate\u2082) = (k[NO\u2082]\u2083\u00b9[O\u2083]\u2083\u1d50) \/ (k[NO\u2082]\u2082\u00b9[O\u2083]\u2082\u1d50)<br>(15.40 x 10\u2074) \/ (5.50 x 10\u2074) = (k(1.76)\u00b9(1.40)\u1d50) \/ (k(1.10)\u00b9(0.800)\u1d50)<br>2.80 = (1.60) * (1.75)\u1d50<br>2.80 \/ 1.60 = (1.75)\u1d50<br>1.75 = (1.75)\u1d50<br>Therefore, m = 1. The reaction is first order in O\u2083.<\/p>\n\n\n\n<p>The complete rate law is Rate = k[NO\u2082][O\u2083]. The overall reaction order is 1 + 1 = 2.<\/p>\n\n\n\n<p>Now, we can calculate the rate constant, k, by rearranging the rate law and using data from any experiment. Using data from Experiment 1:<\/p>\n\n\n\n<p>k = Rate \/ ([NO\u2082][O\u2083])<br>k = (3.25 x 10\u2074 M\/s) \/ (0.650 M * 0.800 M)<br>k = (3.25 x 10\u2074 M\/s) \/ (0.520 M\u00b2)<br>k = 62,500 M\u207b\u00b9\u00b7s\u207b\u00b9 = 6.25 x 10\u2074 M\u207b\u00b9\u00b7s\u207b\u00b9<\/p>\n\n\n\n<p>The units for k are derived from the rate law: Units of k = (M\/s) \/ (M * M) = M\u207b\u00b9\u00b7s\u207b\u00b9.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1139.jpeg\" alt=\"\" class=\"wp-image-261378\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Consider the initial-rate data at a certain temperature in the table for the reaction described by: [NO2]o (M) 0.650 1.10 1.76 O3 0.800 0.800 1.40 Initial rate (Ms) 3.25 x 10^4 5.50 x 10^4 15.40 x 10^4 2 NO2(g) + O3(g) -> N2O5(g) + O2(g) Determine the value and units of the rate constant, k. [&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-261376","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261376","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=261376"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261376\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261376"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261376"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261376"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}