{"id":14886,"date":"2023-04-18T10:00:11","date_gmt":"2023-04-18T04:30:11","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=14886"},"modified":"2023-04-19T10:25:14","modified_gmt":"2023-04-19T04:55:14","slug":"oxidation-reduction-electrolytic-cells","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/oxidation-reduction-electrolytic-cells\/","title":{"rendered":"Oxidation and Reduction in Electrolytic Cells"},"content":{"rendered":"<h2><strong>Oxidation and Reduction in Electrolytic Cells<\/strong><\/h2>\n<p>&nbsp;<\/p>\n<ul>\n<li>In an electrolytic cell, an electric current is passed through an electrolyte using electrodes.<\/li>\n<li>The electrolyte may be a molten ionic compound or an aqueous solution containing ions.<\/li>\n<li>The electrodes are usually inert conductors such as platinum or carbon. Sometimes active electrodes such as copper are used.<\/li>\n<li>During electrolysis, the electrolyte undergoes chemical changes at the electrodes. The chemical change at each electrode is actually a half-reaction of a redox reaction.<\/li>\n<li>The following table shows the oxidation and reduction in a few other electrolytic cells.<\/li>\n<\/ul>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115888\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-1.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 1\" width=\"725\" height=\"449\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-1.png 725w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-1-300x186.png 300w\" sizes=\"(max-width: 725px) 100vw, 725px\" \/><\/p>\n<ul>\n<li>In all electrolytic cells, electrons flow from the <strong>reducing agent at the anode<\/strong> to the <strong>oxidising agent at the cathode.<\/strong><\/li>\n<li>The reducing agent loses electrons and undergoes oxidation at the anode.<\/li>\n<li>On the other hand, the oxidising agent gains electrons and undergoes reduction at the cathode.<\/li>\n<\/ul>\n<p><strong>People also ask<\/strong><\/p>\n<ul>\n<li><a href=\"https:\/\/www.aplustopper.com\/electrolytic-chemical-cells\/\">Electrolytic and Chemical Cells<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/oxidation-areduction-chemical-cells\/\">Oxidation and Reduction in Chemical Cells<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/oxidation-reduction-redox-reactions\/\">What is a redox reaction?<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/changing-iron-ii-ions-iron-iii-ions-vice-versa\/\">Changing of iron(II) ions to iron(III) ions and vice versa<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/redox-reaction-displacement-metals-salt-solution\/\">Redox reaction in the displacement of metals from its salt solution<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/displacement-halogen-from-halide-solution\/\">Displacement of Halogen From Halide Solution<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/redox-reactions-transfer-electrons-distance\/\">Redox Reactions by Transfer of Electrons at a Distance<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/rusting-redox-reaction\/\">Rusting as a Redox Reaction<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/reactivity-series-metals-towards-oxygen\/\">The Reactivity Series of Metals Towards Oxygen<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/application-reactivity-series-metals-extraction-metals\/\">Application of the reactivity series of metals in the extraction of metals<\/a><\/li>\n<li><a href=\"https:\/\/www.aplustopper.com\/voltaic-cell-work\/\">How does a voltaic cell work?<\/a><\/li>\n<\/ul>\n<h2><strong>Oxidation and Reduction in Electrolytic Cells Experiment<\/strong><\/h2>\n<p><strong>Aim:<\/strong> To investigate the oxidation and reduction in electrolytic cells.<br \/>\n<strong>Materials:<\/strong> Solid lead(II) bromide, 1 mol dm<sup>-3<\/sup> potassium iodide solution, 1% starch solution, sandpaper, wooden<br \/>\n<strong>Apparatus:<\/strong> Crucible, cardboard, battery, connecting wires with crocodile clips, tripod stand, Bunsen burner, pipe-clay triangle, electrolytic cell, carbon electrodes, switch, ammeter, small test tubes, beaker, tongs.<br \/>\n<strong>Procedure:<\/strong><br \/>\n<strong>A. Electrolytic cell involving molten electrolyte<\/strong><\/p>\n<ol>\n<li>A crucible is half-filled with solid lead(II) bromide.<\/li>\n<li>The apparatus is set up as shown in Figure.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115892\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-2.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 2\" width=\"399\" height=\"263\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-2.png 399w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-2-300x198.png 300w\" sizes=\"(max-width: 399px) 100vw, 399px\" \/><\/li>\n<li>The solid lead(II) bromide is heated until it is completely melted.<\/li>\n<li>The switch is turned on to allow electricity to pass through the molten lead(II) bromide for about 20 minutes. Any changes are observed.<\/li>\n<li>After 20 minutes, the switch is turned off and both electrodes are taken out from the electrolyte. The molten electrolyte is carefully poured into a beaker using tongs. The product left at the bottom of the crucible is observed.<\/li>\n<\/ol>\n<p><strong>B. Electrolytic cell involving aqueous electrolyte<\/strong><\/p>\n<ol>\n<li>An electrolytic cell is half-filled with 0.5 mol dm<sup>-3<\/sup> potassium iodide solution.<\/li>\n<li>The apparatus is set up as shown in Figure.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115893\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-3.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 3\" width=\"410\" height=\"232\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-3.png 410w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-3-300x170.png 300w\" sizes=\"(max-width: 410px) 100vw, 410px\" \/><\/li>\n<li>The switch is turned on to allow electricity to pass through the electrolyte for 15 minutes. Any changes at the anode and cathode are observed.<\/li>\n<li>The product at the anode is tested with 1 % starch solution while the gas collected at the cathode is tested with a lighted wooden splinter.<\/li>\n<\/ol>\n<p><strong>Results:<\/strong><br \/>\n<strong>A. Electrolytic cell involving molten electrolyte<br \/>\n<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"74\"><strong>Electrode<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"369\"><strong>Observation<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"148\"><strong>Inference<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"74\">Anode<\/td>\n<td style=\"text-align: center;\" width=\"369\">A brown gas with a pungent and choking smell is released.<\/td>\n<td style=\"text-align: center;\" width=\"148\">Bromine gas is released.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"74\">Cathode<\/td>\n<td style=\"text-align: center;\" width=\"369\">A shiny grey globule is found at the bottom of the crucible.<\/td>\n<td style=\"text-align: center;\" width=\"148\">Lead is produced.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong> B. Electrolytic cell involving aqueous electrolyte<br \/>\n<\/strong><\/p>\n<table border=\"2\">\n<tbody>\n<tr>\n<td style=\"text-align: center;\" width=\"69\"><strong>Electrode<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"368\"><strong>Observation<\/strong><\/td>\n<td style=\"text-align: center;\" width=\"151\"><strong>Inference<\/strong><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"69\">Anode<\/td>\n<td style=\"text-align: center;\" width=\"368\">The solution in the test tube turns from colourless to brown.<br \/>\nIt gives a dark blue colouration when tested with starch solution.<\/td>\n<td style=\"text-align: center;\" width=\"151\">Iodine is produced.<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center;\" width=\"69\">Cathode<\/td>\n<td style=\"text-align: center;\" width=\"368\">Gas bubbles are released. A colourless gas which burns with a &#8216;pop&#8217; sound is produced.<\/td>\n<td style=\"text-align: center;\" width=\"151\">Hydrogen gas is produced.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p><strong>Discussion:<\/strong><\/p>\n<ol>\n<li>In the electrolysis of molten lead(II) bromide:<br \/>\n(a) Molten lead(II) bromide contains lead(II) ions, Pb<sup>2+<\/sup> and bromide ions, Br<sup>&#8211;<\/sup>.<br \/>\n(b) Pb<sup>2+<\/sup> ions move to the cathode while Br<sup>&#8211;<\/sup> ions move to the anode.<br \/>\n(c) At the <strong>anode,<\/strong> Br<sup>&#8211;<\/sup> ions act as the reducing agent, losing electrons to become bromine molecules. Thus, Br<sup>&#8211;<\/sup> ions undergo <strong>oxidation.<br \/>\n<\/strong><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115895\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-4.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 4\" width=\"405\" height=\"82\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-4.png 405w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-4-300x61.png 300w\" sizes=\"(max-width: 405px) 100vw, 405px\" \/><br \/>\nAt the <strong>cathode,<\/strong> Pb<sup>2+<\/sup> ions act as the oxidising agent, accepting electrons to become metallic lead. Thus, Pb<sup>2+<\/sup> ions undergo <strong>reduction.<br \/>\n<\/strong><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115896\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-5.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 5\" width=\"386\" height=\"87\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-5.png 386w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-5-300x68.png 300w\" sizes=\"(max-width: 386px) 100vw, 386px\" \/><br \/>\n(d) Hence, electrons are transferred from Br<sup>&#8211;<\/sup> ions, the reducing agent, at the anode to Pb<sup>2+<\/sup> ions, the oxidising agent, at the cathode.<br \/>\n(e) The overall equation is as follows.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115897\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-6.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 6\" width=\"359\" height=\"28\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-6.png 359w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-6-300x23.png 300w\" sizes=\"(max-width: 359px) 100vw, 359px\" \/><\/li>\n<li>In the electrolysis of potassium iodide solution:<br \/>\n(a) Potassium iodide solution contains hydrogen ions, H<sup>+<\/sup>, potassium ions, K<sup>+<\/sup>, hydroxide ions, OH<sup>&#8211;<\/sup> and iodide ions, I<sup>&#8211;<\/sup>.<br \/>\n(b) H<sup>+<\/sup> ions and K<sup>+<\/sup> ions move to the cathode while OH<sup>&#8211;<\/sup> ions and I<sup>&#8211;<\/sup> ions move to the anode.<br \/>\n(c) At the <strong>anode,<\/strong>\u00a0I<sup>&#8211;<\/sup> ions are selectively discharged because of their high concentration in the electrolyte. I<sup>&#8211;<\/sup>\u00a0ions act as the reducing agent, losing electrons to become iodine molecules. In other words, I ions undergo <strong>oxidation.<br \/>\n<\/strong><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115928\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-7.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 7\" width=\"403\" height=\"84\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-7.png 403w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-7-300x63.png 300w\" sizes=\"(max-width: 403px) 100vw, 403px\" \/><br \/>\n(d) At the <strong>cathode,<\/strong> H<sup>+<\/sup> ions are selectively discharged because their position in the electrochemical series is lower than K<sup>+\u00a0<\/sup>ions. H<sup>+<\/sup> ions act as the oxidising agent, gaining electrons to become hydrogen molecules. In other words, H<sup>+<\/sup> ions undergo <strong>reduction.<br \/>\n<\/strong><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115961\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-8.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 8\" width=\"415\" height=\"89\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-8.png 415w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-8-300x64.png 300w\" sizes=\"(max-width: 415px) 100vw, 415px\" \/><br \/>\n(e) The overall equation is as follows.<br \/>\n<img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-115996\" src=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-9.png\" alt=\"Oxidation and Reduction in Electrolytic Cells 9\" width=\"390\" height=\"29\" srcset=\"https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-9.png 390w, https:\/\/www.aplustopper.com\/wp-content\/uploads\/2017\/06\/Oxidation-and-Reduction-in-Electrolytic-Cells-9-300x22.png 300w\" sizes=\"(max-width: 390px) 100vw, 390px\" \/><\/li>\n<\/ol>\n<p><strong>Conclusion:<\/strong><br \/>\nIn an electrolytic cell, oxidation occurs at the anode (positive electrode) while reduction occurs at the cathode (negative electrode).<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Oxidation and Reduction in Electrolytic Cells &nbsp; In an electrolytic cell, an electric current is passed through an electrolyte using electrodes. The electrolyte may be a molten ionic compound or an aqueous solution containing ions. The electrodes are usually inert conductors such as platinum or carbon. Sometimes active electrodes such as copper are used. During [&hellip;]<\/p>\n","protected":false},"author":3,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_genesis_hide_title":false,"_genesis_hide_breadcrumbs":false,"_genesis_hide_singular_image":false,"_genesis_hide_footer_widgets":false,"_genesis_custom_body_class":"","_genesis_custom_post_class":"","_genesis_layout":"","footnotes":""},"categories":[84],"tags":[5907,5913,5903,5912,5914,5904,5905,5906],"yoast_head":"<!-- This site is optimized with the Yoast SEO Premium plugin v17.8 (Yoast SEO v17.8) - https:\/\/yoast.com\/wordpress\/plugins\/seo\/ -->\n<title>Oxidation and Reduction in Electrolytic Cells - A Plus Topper<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/www.aplustopper.com\/oxidation-reduction-electrolytic-cells\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Oxidation and Reduction in Electrolytic Cells\" \/>\n<meta property=\"og:description\" content=\"Oxidation and Reduction in Electrolytic Cells &nbsp; In an electrolytic cell, an electric current is passed through an electrolyte using electrodes. 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The electrolyte may be a molten ionic compound or an aqueous solution containing ions. The electrodes are usually inert conductors such as platinum or carbon. Sometimes active electrodes such as copper are used. 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