{"id":185094,"date":"2025-01-22T06:09:48","date_gmt":"2025-01-22T06:09:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185094"},"modified":"2025-01-22T06:09:50","modified_gmt":"2025-01-22T06:09:50","slug":"the-standard-reaction-free-energy-ag-194","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/the-standard-reaction-free-energy-ag-194\/","title":{"rendered":"The Standard Reaction Free Energy AG\u00b0 = -194"},"content":{"rendered":"\n<p>The Standard Reaction Free Energy AG\u00b0 = -194. KJ For This Reaction: SnO2(S) + 2 CO(G)\u2014Sn(S) + 200 (9) Use This Information To Complete The Table Below. Round Each Of Your Answers To The Nearest KJ Reaction AG 2Sn(S) + 4CO2(G) 25n0, (S) + 4CO(G) OkJ KJ Sn(S) + 200,(3) \u2014 Sn0,-) + 200(3) Sn0,6) +<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>\ue203To determine the standard Gibbs free energy changes (\u0394G\u00b0) for the given reactions, we can utilize the provided \u0394G\u00b0 value of -194 kJ for the reaction:\ue204<\/p>\n\n\n\n<p>\ue203SnO\u2082(s) + 2 CO(g) \u2192 Sn(s) + 2 CO\u2082(g)\ue204<\/p>\n\n\n\n<p><strong>1. Reaction: 2 Sn(s) + 4 CO\u2082(g) \u2192 2 SnO\u2082(s) + 4 CO(g)<\/strong><\/p>\n\n\n\n<p>\ue203This reaction is the reverse of the original reaction, but with all coefficients multiplied by 2.\ue204 \ue203Reversing a reaction changes the sign of \u0394G\u00b0, and multiplying the coefficients by a factor scales \u0394G\u00b0 by the same factor.\ue204 \ue203Therefore:\ue204<\/p>\n\n\n\n<p>\ue203\u0394G\u00b0 = 2 \u00d7 (+194 kJ) = +388 kJ\ue204<\/p>\n\n\n\n<p><strong>2. Reaction: Sn(s) + 2 CO\u2082(g) \u2192 SnO\u2082(s) + 2 CO(g)<\/strong><\/p>\n\n\n\n<p>\ue203This reaction is the reverse of the original reaction without any coefficient changes.\ue204 \ue203Reversing the reaction changes the sign of \u0394G\u00b0:\ue204<\/p>\n\n\n\n<p>\ue203\u0394G\u00b0 = +194 kJ\ue204<\/p>\n\n\n\n<p><strong>3. Reaction: SnO\u2082(s) + 2 CO\u2082(g) \u2192 Sn(s) + 2 CO(g)<\/strong><\/p>\n\n\n\n<p>\ue203This reaction is not directly related to the original reaction.\ue204 \ue203To determine its \u0394G\u00b0, we need to consider the following steps:\ue204<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\ue203The original reaction: SnO\u2082(s) + 2 CO(g) \u2192 Sn(s) + 2 CO\u2082(g) with \u0394G\u00b0 = -194 kJ.\ue204<\/li>\n\n\n\n<li>\ue203Reversing this reaction: Sn(s) + 2 CO\u2082(g) \u2192 SnO\u2082(s) + 2 CO(g) with \u0394G\u00b0 = +194 kJ.\ue204<\/li>\n<\/ul>\n\n\n\n<p>\ue203Therefore, the \u0394G\u00b0 for SnO\u2082(s) + 2 CO\u2082(g) \u2192 Sn(s) + 2 CO(g) is -194 kJ.\ue204<\/p>\n\n\n\n<p><strong>Summary:<\/strong><\/p>\n\n\n\n<p>\ue203| Reaction | \u0394G\u00b0 (kJ) | |&#8212;|&#8212;| | 2 Sn(s) + 4 CO\u2082(g) \u2192 2 SnO\u2082(s) + 4 CO(g) | +388 | | Sn(s) + 2 CO\u2082(g) \u2192 SnO\u2082(s) + 2 CO(g) | +194 | | SnO\u2082(s) + 2 CO\u2082(g) \u2192 Sn(s) + 2 CO(g) | -194 |\ue204<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>\ue203The Gibbs free energy change (\u0394G\u00b0) indicates the spontaneity of a reaction under standard conditions.\ue204 \ue203A negative \u0394G\u00b0 signifies a spontaneous reaction, while a positive \u0394G\u00b0 indicates non-spontaneity.\ue204 \ue203When a reaction is reversed, the sign of \u0394G\u00b0 changes because the direction of spontaneity is inverted.\ue204 \ue203Additionally, scaling the stoichiometric coefficients of a reaction by a factor scales \u0394G\u00b0 by the same factor, as \u0394G\u00b0 is an extensive property proportional to the amount of reactants and products involved.\ue204 \ue203These principles allow us to calculate the \u0394G\u00b0 values for related reactions based on known \u0394G\u00b0 values.\ue204<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The Standard Reaction Free Energy AG\u00b0 = -194. KJ For This Reaction: SnO2(S) + 2 CO(G)\u2014Sn(S) + 200 (9) Use This Information To Complete The Table Below. Round Each Of Your Answers To The Nearest KJ Reaction AG 2Sn(S) + 4CO2(G) 25n0, (S) + 4CO(G) OkJ KJ Sn(S) + 200,(3) \u2014 Sn0,-) + 200(3) Sn0,6) [&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-185094","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185094","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=185094"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185094\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185094"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185094"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185094"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}