{"id":94,"date":"2024-10-24T20:57:48","date_gmt":"2024-10-25T00:57:48","guid":{"rendered":"https:\/\/sites.temple.edu\/chemdemo\/?p=94"},"modified":"2024-10-25T16:22:01","modified_gmt":"2024-10-25T20:22:01","slug":"electroplating-pennies","status":"publish","type":"post","link":"https:\/\/sites.temple.edu\/chemdemo\/2024\/10\/24\/electroplating-pennies\/","title":{"rendered":"Electroplating Pennies"},"content":{"rendered":"\n<h2 class=\"wp-block-heading\">Plating of Nickel onto Copper<\/h2>\n\n\n\n<h2 class=\"wp-block-heading\">Source<\/h2>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Reference:<\/strong> A Demo A Day: Vol 2, Bilash et al., page 262.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\">Materials Needed<\/h2>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Power supply and cords with alligator clips (one end)<\/li>\n\n\n\n<li>NiCl\u2082\u00b76H\u2082O (65 g)<\/li>\n\n\n\n<li>0.1 M HCl<\/li>\n\n\n\n<li>Copper (Cu) foil<\/li>\n\n\n\n<li>Beaker<\/li>\n\n\n\n<li>Steel wool<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\">Procedure<\/h2>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Prepare Nickel Solution:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Dissolve 65 g of NiCl\u2082\u00b76H\u2082O in 500 mL of 0.1 M HCl.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Prepare Copper Electrodes:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Clean the Cu foil (or penny) with steel wool.<\/li>\n\n\n\n<li>Attach leads to the Cu electrodes.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electrolysis Setup:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Immerse the Cu electrodes in the nickel solution.<\/li>\n\n\n\n<li>Note that there is no reaction without current.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Initiate Current:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Turn on the power supply to about 6 volts.<\/li>\n\n\n\n<li>Observe the plating process.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\">Chemical Reactions<\/h2>\n\n\n\n<h3 class=\"wp-block-heading\">Table 1: Oxidation and Reduction of Copper and Nickel<\/h3>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th>Reaction Type<\/th><th>Equation<\/th><th>Standard Electrode Potential (V)<\/th><\/tr><\/thead><tbody><tr><td>Oxidation of Copper<\/td><td>Cu(s) \u2192 Cu\u00b2\u207a(aq) + 2e\u207b<\/td><td>E\u00b0ox = -0.34<\/td><\/tr><tr><td>Reduction of Nickel<\/td><td>Ni\u00b2\u207a(aq) + 2e\u207b \u2192 Ni(s)<\/td><td>E\u00b0red = -0.25<\/td><\/tr><tr><td>Overall Reaction<\/td><td>Cu(s) + Ni\u00b2\u207a(aq) \u2192 Cu\u00b2\u207a(aq) + Ni(s)<\/td><td>E\u00b0tot = -0.59<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h3 class=\"wp-block-heading\">Table 2: Reduction of Silver and Copper<\/h3>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th>Reaction Type<\/th><th>Equation<\/th><th>Standard Electrode Potential (V)<\/th><\/tr><\/thead><tbody><tr><td>Reduction of Silver<\/td><td>2Ag\u207a(aq) + 2e\u207b \u2192 2Ag(s)<\/td><td>E\u00b0red = 0.80<\/td><\/tr><tr><td>Reduction of Copper<\/td><td>Cu\u00b2\u207a + 2e\u207b \u2192 Cu(s)<\/td><td>E\u00b0red = -0.34<\/td><\/tr><tr><td>Overall Reaction (with Nickel)<\/td><td>Cu(s) + Ni\u00b2\u207a(aq) \u2192 Cu\u00b2\u207a(aq) + Ni(s)<\/td><td>E\u00b0tot = 0.46<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<h3 class=\"wp-block-heading\">Table 3: Reduction of Lead and Zinc<\/h3>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th>Reaction Type<\/th><th>Equation<\/th><th>Standard Electrode Potential (V)<\/th><\/tr><\/thead><tbody><tr><td>Reduction of Lead<\/td><td>Pb\u00b2\u207a(aq) + 2e\u207b \u2192 Pb(s)<\/td><td>E\u00b0red = -0.13<\/td><\/tr><tr><td>Reduction of Zinc<\/td><td>Zn(s) \u2192 Zn\u00b2\u207a + 2e\u207b<\/td><td>E\u00b0red = 0.76<\/td><\/tr><tr><td>Overall Reaction (with Nickel)<\/td><td>Cu(s) + Ni\u00b2\u207a(aq) \u2192 Cu\u00b2\u207a(aq) + Ni(s)<\/td><td>E\u00b0tot = 0.63<\/td><\/tr><\/tbody><\/table><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Plating of Nickel onto Copper Source Materials Needed Procedure Chemical Reactions Table 1: Oxidation and Reduction of Copper and Nickel Reaction Type Equation Standard Electrode&#8230;<\/p>\n<div class=\"more-link-wrapper\"><a class=\"more-link\" href=\"https:\/\/sites.temple.edu\/chemdemo\/2024\/10\/24\/electroplating-pennies\/\">Continue Reading<span class=\"screen-reader-text\">Electroplating Pennies<\/span><\/a><\/div>\n","protected":false},"author":36673,"featured_media":0,"comment_status":"open","ping_status":"","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[2],"tags":[],"class_list":["post-94","post","type-post","status-publish","format-standard","hentry","category-demonstrations","entry"],"_links":{"self":[{"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/posts\/94","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/users\/36673"}],"replies":[{"embeddable":true,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/comments?post=94"}],"version-history":[{"count":1,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/posts\/94\/revisions"}],"predecessor-version":[{"id":95,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/posts\/94\/revisions\/95"}],"wp:attachment":[{"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/media?parent=94"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/categories?post=94"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/sites.temple.edu\/chemdemo\/wp-json\/wp\/v2\/tags?post=94"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}