{"id":90812,"date":"2025-06-01T10:38:07","date_gmt":"2025-06-01T10:38:07","guid":{"rendered":"https:\/\/exam.pscnotes.com\/mcq\/?p=90812"},"modified":"2025-06-01T10:38:07","modified_gmt":"2025-06-01T10:38:07","slug":"consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s","status":"publish","type":"post","link":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/","title":{"rendered":"Consider the following redox reaction:\n2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)"},"content":{"rendered":"

Consider the following redox reaction:
\n2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s) + SO2 (g)
\nIdentify the species among the following acting as oxidant and reductant, respectively:<\/p>\n

[amp_mcq option1=”Cu(I) and S of Cu2S” option2=”Cu and S of SO2″ option3=”Cu and O of SO2″ option4=”Cu(I) and O of SO2″ correct=”option1″]<\/p>\n

\n
\n
This question was previously asked in<\/div>\n
UPSC CAPF – 2023<\/div>\n<\/div>\n
Download PDF<\/a>Attempt Online<\/a><\/div>\n<\/div>\n
\nIn the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows:
\nIn Cu\u2082O, Cu is +1, O is -2.
\nIn Cu\u2082S, Cu is +1, S is -2.
\nIn Cu, Cu is 0.
\nIn SO\u2082, S is +4, O is -2.
\nCu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1).
\nS changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it.
\nThus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant.
\n<\/section>\n
\nAn oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.
\n<\/section>\n
\nThis is a self-reduction reaction where the same element (Copper) is present in both reactants and is reduced, while another element (Sulfur) is oxidized. Specifically, Copper from both Cu\u2082O and Cu\u2082S is reduced. The sulfur from Cu\u2082S is oxidized. Therefore, Cu(I) collectively from the reactants acts as the oxidant, and S in Cu\u2082S acts as the reductant.
\n<\/section>\n","protected":false},"excerpt":{"rendered":"

Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s) + SO2 (g) Identify the species among the following acting as oxidant and reductant, respectively: [amp_mcq option1=”Cu(I) and S of Cu2S” option2=”Cu and S of SO2″ option3=”Cu and O of SO2″ option4=”Cu(I) and O of SO2″ correct=”option1″] This question was previously asked … <\/p>\n

Detailed SolutionConsider the following redox reaction:
\n2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)<\/span><\/a><\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1085],"tags":[1105,1096,1239],"class_list":["post-90812","post","type-post","status-publish","format-standard","hentry","category-upsc-capf","tag-1105","tag-chemistry","tag-inorganic-chemistry","no-featured-image-padding"],"yoast_head":"\nConsider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)<\/title>\n<meta name=\"description\" content=\"In the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows: In Cu\u2082O, Cu is +1, O is -2. In Cu\u2082S, Cu is +1, S is -2. In Cu, Cu is 0. In SO\u2082, S is +4, O is -2. Cu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1). S changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it. Thus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant. An oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.\" \/>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)\" \/>\n<meta property=\"og:description\" content=\"In the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows: In Cu\u2082O, Cu is +1, O is -2. In Cu\u2082S, Cu is +1, S is -2. In Cu, Cu is 0. In SO\u2082, S is +4, O is -2. Cu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1). S changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it. Thus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant. An oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.\" \/>\n<meta property=\"og:url\" content=\"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/\" \/>\n<meta property=\"og:site_name\" content=\"MCQ and Quiz for Exams\" \/>\n<meta property=\"article:published_time\" content=\"2025-06-01T10:38:07+00:00\" \/>\n<meta name=\"author\" content=\"rawan239\" \/>\n<meta name=\"twitter:card\" content=\"summary_large_image\" \/>\n<meta name=\"twitter:label1\" content=\"Written by\" \/>\n\t<meta name=\"twitter:data1\" content=\"rawan239\" \/>\n\t<meta name=\"twitter:label2\" content=\"Est. reading time\" \/>\n\t<meta name=\"twitter:data2\" content=\"2 minutes\" \/>\n<!-- \/ Yoast SEO Premium plugin. -->","yoast_head_json":{"title":"Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)","description":"In the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows: In Cu\u2082O, Cu is +1, O is -2. In Cu\u2082S, Cu is +1, S is -2. In Cu, Cu is 0. In SO\u2082, S is +4, O is -2. Cu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1). S changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it. Thus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant. An oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.","robots":{"index":"index","follow":"follow","max-snippet":"max-snippet:-1","max-image-preview":"max-image-preview:large","max-video-preview":"max-video-preview:-1"},"canonical":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/","og_locale":"en_US","og_type":"article","og_title":"Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)","og_description":"In the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows: In Cu\u2082O, Cu is +1, O is -2. In Cu\u2082S, Cu is +1, S is -2. In Cu, Cu is 0. In SO\u2082, S is +4, O is -2. Cu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1). S changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it. Thus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant. An oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.","og_url":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/","og_site_name":"MCQ and Quiz for Exams","article_published_time":"2025-06-01T10:38:07+00:00","author":"rawan239","twitter_card":"summary_large_image","twitter_misc":{"Written by":"rawan239","Est. reading time":"2 minutes"},"schema":{"@context":"https:\/\/schema.org","@graph":[{"@type":"WebPage","@id":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/","url":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/","name":"Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)","isPartOf":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#website"},"datePublished":"2025-06-01T10:38:07+00:00","dateModified":"2025-06-01T10:38:07+00:00","author":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209"},"description":"In the reaction 2Cu\u2082O (s) + Cu\u2082S (s) \u2192 6Cu (s) + SO\u2082 (g), the oxidation states are as follows: In Cu\u2082O, Cu is +1, O is -2. In Cu\u2082S, Cu is +1, S is -2. In Cu, Cu is 0. In SO\u2082, S is +4, O is -2. Cu changes from +1 to 0, so it is reduced. The species causing reduction (oxidant) contains Cu(+1). Both Cu\u2082O and Cu\u2082S contain Cu(+1). S changes from -2 (in Cu\u2082S) to +4 (in SO\u2082), so it is oxidized. The species causing oxidation (reductant) is Cu\u2082S, specifically the S atom within it. Thus, Cu(I) acts as the oxidant and S of Cu\u2082S acts as the reductant. An oxidant (oxidizing agent) is a substance that accepts electrons and is itself reduced. A reductant (reducing agent) is a substance that donates electrons and is itself oxidized. In this reaction, Cu(I) gains electrons to become Cu(0), hence Cu(I) is the oxidant. S(-2) loses electrons to become S(+4), hence S(-2) is the reductant.","breadcrumb":{"@id":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/#breadcrumb"},"inLanguage":"en-US","potentialAction":[{"@type":"ReadAction","target":["https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/"]}]},{"@type":"BreadcrumbList","@id":"https:\/\/exam.pscnotes.com\/mcq\/consider-the-following-redox-reaction2cu2o-s-cu2s-s-6cu-s\/#breadcrumb","itemListElement":[{"@type":"ListItem","position":1,"name":"Home","item":"https:\/\/exam.pscnotes.com\/mcq\/"},{"@type":"ListItem","position":2,"name":"UPSC CAPF","item":"https:\/\/exam.pscnotes.com\/mcq\/category\/upsc-capf\/"},{"@type":"ListItem","position":3,"name":"Consider the following redox reaction: 2Cu2O (s) + Cu2S (s) \u2014\u2014 6Cu (s)"}]},{"@type":"WebSite","@id":"https:\/\/exam.pscnotes.com\/mcq\/#website","url":"https:\/\/exam.pscnotes.com\/mcq\/","name":"MCQ and Quiz for Exams","description":"","potentialAction":[{"@type":"SearchAction","target":{"@type":"EntryPoint","urlTemplate":"https:\/\/exam.pscnotes.com\/mcq\/?s={search_term_string}"},"query-input":"required name=search_term_string"}],"inLanguage":"en-US"},{"@type":"Person","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/5807dafeb27d2ec82344d6cbd6c3d209","name":"rawan239","image":{"@type":"ImageObject","inLanguage":"en-US","@id":"https:\/\/exam.pscnotes.com\/mcq\/#\/schema\/person\/image\/","url":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","contentUrl":"https:\/\/secure.gravatar.com\/avatar\/761a7274f9cce048fa5b921221e7934820d74514df93ef195a9d22af0c1c9001?s=96&d=mm&r=g","caption":"rawan239"},"sameAs":["https:\/\/exam.pscnotes.com"],"url":"https:\/\/exam.pscnotes.com\/mcq\/author\/rawan239\/"}]}},"amp_enabled":true,"_links":{"self":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90812","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/comments?post=90812"}],"version-history":[{"count":0,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/posts\/90812\/revisions"}],"wp:attachment":[{"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/media?parent=90812"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/categories?post=90812"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/exam.pscnotes.com\/mcq\/wp-json\/wp\/v2\/tags?post=90812"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}