Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AC Be sure your answer has the correct number of significant digits.<\/p>\n\n\n\n
2Zn (s) +N\u2082 (g)+4H2O (1)\u21922Zn2+ (aq) +N\u2082H\u2084(aq)+4OH (aq)<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To calculate the standard reaction free energy (( \\Delta G^\\circ )) for the reaction:<\/p>\n\n\n\n [ We use the relationship:<\/p>\n\n\n\n [ This calculation determines the standard Gibbs free energy change for the reaction under standard conditions. The negative sign in the equation ( \\Delta G^\\circ = -n F E^\\circ_{\\text{cell}} ) reflects the relationship between spontaneity and cell potential. Since the cell potential (( E^\\circ_{\\text{cell}} )) is negative, the reaction is non-spontaneous under standard conditions (( \\Delta G^\\circ > 0 )).<\/p>\n\n\n\n Proper use of significant figures ensures that the final result reflects the precision of the given data. Both ( E^\\circ ) values are given to 2 decimal places, so the result for ( \\Delta G^\\circ ) is reported with 5 significant figures, consistent with the constants used.<\/p>\n","protected":false},"excerpt":{"rendered":" Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AC Be sure your answer has the correct number of significant digits. 2Zn (s) +N\u2082 (g)+4H2O (1)\u21922Zn2+ (aq) +N\u2082H\u2084(aq)+4OH (aq) The Correct Answer and Explanation is : To calculate the standard reaction free energy (( \\Delta G^\\circ )) for 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-185092","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185092","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=185092"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185092\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185092"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185092"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185092"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
2\\text{Zn (s)} + \\text{N}_2 \\text{(g)} + 4\\text{H}_2\\text{O (l)} \\rightarrow 2\\text{Zn}^{2+} \\text{(aq)} + \\text{N}_2\\text{H}_4 \\text{(aq)} + 4\\text{OH}^- \\text{(aq)}
]<\/p>\n\n\n\n
\\Delta G^\\circ = -n F E^\\circ_{\\text{cell}}
]<\/p>\n\n\n\nSteps:<\/h3>\n\n\n\n
\n
\n
\n
[
E^\\circ_{\\text{cell}} = E^\\circ_{\\text{reduction}} + E^\\circ_{\\text{oxidation}} = -1.16 \\, \\text{V} + 0.76 \\, \\text{V} = -0.40 \\, \\text{V}.
]<\/li>\n\n\n\n
The oxidation of 2 moles of Zn produces 4 moles of electrons, so ( n = 4 ).<\/li>\n\n\n\n
[
\\Delta G^\\circ = -n F E^\\circ_{\\text{cell}} = -(4)(96485 \\, \\text{C\/mol})(-0.40 \\, \\text{V})
]
[
\\Delta G^\\circ = +154,376 \\, \\text{J\/mol} = +154.38 \\, \\text{kJ\/mol}.
]<\/li>\n<\/ol>\n\n\n\nExplanation:<\/h3>\n\n\n\n