{"id":219414,"date":"2025-05-26T05:51:50","date_gmt":"2025-05-26T05:51:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=219414"},"modified":"2025-05-26T05:51:53","modified_gmt":"2025-05-26T05:51:53","slug":"write-balanced-half-reactions-for-the-following-redox-reaction","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/26\/write-balanced-half-reactions-for-the-following-redox-reaction\/","title":{"rendered":"Write balanced half-reactions for the following redox reaction"},"content":{"rendered":"\n

Write balanced half-reactions for the following redox reaction:<\/p>\n\n\n\n

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

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

Balanced Half-Reactions:<\/strong><\/h3>\n\n\n\n

Reduction half-reaction:<\/strong>
Cl2(g)+2e\u2212\u21922Cl\u2212(aq)\\text{Cl}_2(g) + 2e^- \\rightarrow 2\\text{Cl}^-(aq)<\/p>\n\n\n\n

Oxidation half-reaction:<\/strong>
2NO2(g)+2H2O(l)\u21922NO3\u2212(aq)+4H+(aq)+2e\u22122\\text{NO}_2(g) + 2\\text{H}_2O(l) \\rightarrow 2\\text{NO}_3^-(aq) + 4\\text{H}^+(aq) + 2e^-<\/p>\n\n\n\n

\n\n\n\n

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

Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species. In any redox reaction, one species loses electrons (oxidation), while another gains electrons (reduction). To analyze the given redox reaction: Cl2(g)+2NO2(g)+2H2O(l)\u21922Cl\u2212(aq)+2NO3\u2212(aq)+4H+(aq)\\text{Cl}_2(g) + 2\\text{NO}_2(g) + 2\\text{H}_2O(l) \\rightarrow 2\\text{Cl}^-(aq) + 2\\text{NO}_3^-(aq) + 4\\text{H}^+(aq)<\/p>\n\n\n\n

we must identify which species are oxidized and which are reduced.<\/p>\n\n\n\n

\n\n\n\n

Step 1: Assign oxidation states.<\/strong><\/p>\n\n\n\n

    \n
  • In Cl2\\text{Cl}_2, chlorine is in its elemental form: oxidation state = 0.<\/li>\n\n\n\n
  • In Cl\u2212\\text{Cl}^-, oxidation state = -1.<\/li>\n\n\n\n
  • Chlorine goes from 0 to -1: gain of electrons \u2192 reduction<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Hence, the reduction half-reaction<\/strong> is: Cl2(g)+2e\u2212\u21922Cl\u2212(aq)\\text{Cl}_2(g) + 2e^- \\rightarrow 2\\text{Cl}^-(aq)<\/p>\n\n\n\n

      \n
    • In NO2\\text{NO}_2, nitrogen has an oxidation state of +4.<\/li>\n\n\n\n
    • In NO3\u2212\\text{NO}_3^-, nitrogen has an oxidation state of +5.<\/li>\n\n\n\n
    • Nitrogen goes from +4 to +5: loss of electrons \u2192 oxidation<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      So the oxidation half-reaction<\/strong> is: 2NO2(g)+2H2O(l)\u21922NO3\u2212(aq)+4H+(aq)+2e\u22122\\text{NO}_2(g) + 2\\text{H}_2O(l) \\rightarrow 2\\text{NO}_3^-(aq) + 4\\text{H}^+(aq) + 2e^-<\/p>\n\n\n\n

      \n\n\n\n

      Step 2: Balance mass and charge.<\/strong><\/p>\n\n\n\n

      Each half-reaction is balanced for atoms and charges. The electrons cancel when the two reactions are added together: Cl2+2e\u2212\u21922Cl\u22122NO2+2H2O\u21922NO3\u2212+4H++2e\u2212\\text{Cl}_2 + 2e^- \\rightarrow 2\\text{Cl}^- \\\\ 2\\text{NO}_2 + 2\\text{H}_2O \\rightarrow 2\\text{NO}_3^- + 4\\text{H}^+ + 2e^-<\/p>\n\n\n\n

      Combining both yields the balanced redox equation.<\/p>\n\n\n\n

      This systematic breakdown helps in understanding the flow of electrons and balancing redox equations correctly.<\/p>\n\n\n\n

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

      Write balanced half-reactions for the following redox reaction: The Correct Answer and Explanation is: Balanced Half-Reactions: Reduction half-reaction:Cl2(g)+2e\u2212\u21922Cl\u2212(aq)\\text{Cl}_2(g) + 2e^- \\rightarrow 2\\text{Cl}^-(aq) Oxidation half-reaction:2NO2(g)+2H2O(l)\u21922NO3\u2212(aq)+4H+(aq)+2e\u22122\\text{NO}_2(g) + 2\\text{H}_2O(l) \\rightarrow 2\\text{NO}_3^-(aq) + 4\\text{H}^+(aq) + 2e^- Explanation Redox (reduction-oxidation) reactions involve the transfer of electrons between chemical species. In any redox reaction, one species loses electrons (oxidation), while another […]<\/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-219414","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219414","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=219414"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219414\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=219414"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=219414"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=219414"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}