{"id":13595,"date":"2022-11-18T16:00:41","date_gmt":"2022-11-18T10:30:41","guid":{"rendered":"https:\/\/www.aplustopper.com\/?p=13595"},"modified":"2022-11-19T16:28:32","modified_gmt":"2022-11-19T10:58:32","slug":"electrochemical-series-mean","status":"publish","type":"post","link":"https:\/\/www.aplustopper.com\/electrochemical-series-mean\/","title":{"rendered":"What does electrochemical series mean?"},"content":{"rendered":"
The Electrochemical Series:<\/strong><\/p>\n Constructing the electrochemical series based on the potential difference between two metals<\/strong><\/p>\n Constructing the electrochemical series based on the ability of a metal to displace another metal from its salt solution<\/strong><\/p>\n People also ask<\/strong><\/p>\n The electrochemical series can be used to<\/p>\n (a) determine the terminals of a voltaic cell<\/strong><\/p>\n (b) compare the standard cell voltages of voltaic cells<\/strong><\/p>\n (c) predict the ability of a metal to displace another metal from its salt solution<\/strong><\/p>\n The importance<\/strong> of electrochemical industries in our daily life is as follows:<\/p>\n The pollution<\/strong> caused by the industrial processes involving electrochemical industries is as follows:<\/p>\n Chemical wastes from electrochemical industries may be poisonous and can endanger our health. Therefore, these wastes must be treated and disposed of in a safe and orderly manner.<\/p>\n Aim:<\/strong> To construct the electrochemical series based on the potential difference between two metals. Results: Discussion:<\/strong><\/p>\n Conclusion:<\/strong> Aim:<\/strong> To construct the electrochemical series based on the ability of a metal to displace another metal from its salt solution. Results: Conclusion:<\/strong> Aim:<\/strong> To confirm the predictions of the metal displacement reaction. Results: Discussion:<\/strong><\/p>\n Conclusion:<\/strong> <\/p>\n","protected":false},"excerpt":{"rendered":" What does electrochemical series mean? The Electrochemical Series: The electrochemical series is an arrangement of metals based on the tendency of each metal atom to donate electrons. The greater the tendency to donate electrons, the more electropositive is the metal and the higher it is in the electrochemical series. The electrochemical series can be constructed […]<\/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":[5040,5041,5043,5044,5042,5039],"yoast_head":"\n\n
\n(a) the potential difference between two metals.
\n(b) the ability of a metal to displace another metal from its salt solution.<\/li>\n<\/ul>\n\n
\nThe greater the voltage produced by the cell, the further the two metals are in the electrochemical series.<\/li>\n\n
\n\u2022 Part of the zinc plate dissolves.
\n\u2022 A brown solid forms on the surface of the remaining part of the zinc plate.
\n\u2022 The blue colour of the copper(II) sulphate solution becomes colourless.
\nThe brown solid is copper metal. The solution turns colourless because zinc displaces copper from the copper(II) sulphate solution. Therefore, zinc is above copper in the electrochemical series.
\nThis reaction is called the metal displacement reaction<\/strong>. The equation for the reaction is
\nZn(s) + CuSO4<\/sub>(aq) \u2192\u00a0ZnSO4<\/sub>(aq) + Cu(s)<\/li>\n\n
Importance of Electrochemical Series<\/strong><\/h2>\n
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Importance of Electrochemical Industries<\/strong><\/h2>\n
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Electrochemical Series\u00a0<\/strong>Experiment 1<\/h2>\n
\nProblem statement:<\/strong> How can the electrochemical series be constructed based on the potential difference between two metals?
\nHypothesis:<\/strong> The further apart the pair of metals in the electrochemical series, the greater is their potential difference.
\nVariables:<\/strong>
\n(a) Manipulated variable: Pairs of metals
\n(b) Responding variable: Potential difference
\n(c) Controlled variables: Type of electrolyte, concentration of electrolyte, copper electrode
\nOperational definition:<\/strong> The reading of the voltmeter is the potential difference between two metals.
\nMaterials:<\/strong> 0.1 mol dm-3<\/sup> copper(II) sulphate solution, copper strip, lead strip, iron nail, zinc strip, magnesium ribbon, aluminium strip and sandpaper.
\nApparatus:<\/strong> Voltmeter, 250 cm3<\/sup> beaker and connecting wires with crocodile clips.
\nProcedure:<\/strong><\/p>\n\n
\n<\/li>\n
\n<\/strong><\/p>\n\n\n
\n Pair of metals<\/strong><\/td>\n Potential difference (V)<\/strong><\/td>\n Negative terminal of the cell<\/strong><\/td>\n<\/tr>\n \n Magnesium and copper<\/td>\n 2.7<\/td>\n Magnesium<\/td>\n<\/tr>\n \n Aluminium and copper<\/td>\n 2.0<\/td>\n Aluminium<\/td>\n<\/tr>\n \n Zinc and copper<\/td>\n 1.1<\/td>\n Zinc<\/td>\n<\/tr>\n \n Iron and copper<\/td>\n 0.8<\/td>\n Iron<\/td>\n<\/tr>\n \n Lead and copper<\/td>\n 0.5<\/td>\n Lead<\/td>\n<\/tr>\n \n Copper and copper<\/td>\n 0.0<\/td>\n –<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n \n
\n<\/li>\n
\nThe descending order of the electropositivity of the metals in the electrochemical series is magnesium, aluminium, zinc, iron, lead, copper. The hypothesis is accepted.<\/p>\nElectrochemical Series\u00a0<\/strong>Experiment 2<\/h2>\n
\nProblem statement:<\/strong> How can the electrochemical series be constructed based on the ability of a metal to displace
\nanother metal from its salt solution?
\nHypothesis:<\/strong> A metal which is situated at a higher position in the electrochemical series is able to displace a metal below it in the series from its salt solution.
\nVariables:<\/strong>
\n(a) Manipulated variables: Pairs of metal and salt solution used
\n(b) Responding variable : Precipitation of metal or change in colour of solution
\n(c) Controlled variable : Concentration of salt solution
\nOperational definition:<\/strong> Metal displacement reaction occurs when there is a deposition of metal or change in colour of solution.
\nMaterials:<\/strong> 1 mol dm-3<\/sup> copper(II) nitrate solution, 1 mol dm-3<\/sup> lead(II) nitrate solution, 1 mol dm-3<\/sup> iron(II) nitrate solution, 1 mol dm-3<\/sup> zinc nitrate solution, 1 mol dm-3<\/sup> magnesium nitrate solution, copper strip, lead strip, iron nail, zinc strip, magnesium ribbon and sandpaper.
\nApparatus:<\/strong> Test tubes and test tube rack.
\nProcedure:<\/strong><\/p>\n\n
\n<\/strong>
\nDiscussion:<\/strong><\/p>\n\n
\n<\/li>\n
\nThe descending order of electropositivity of the metals in the electrochemical series is magnesium, zinc, iron, lead, copper. The hypothesis is accepted.<\/p>\nElectrochemical Series\u00a0<\/strong>Experiment 3<\/h2>\n
\nProblem statement: <\/strong>How to confirm the predictions of the metal displacement reaction?
\nHypothesis:<\/strong> If a metal can displace another metal from its salt solution, then there is a change of colour in the solution or a precipitation of metal.
\nVariables:<\/strong>
\n(a) Manipulated variables: Pairs of metal and salt solution used
\n(b) Responding variable: Precipitation of metal or change in colour of solution
\n(c) Controlled variable: Concentration of salt solution
\nMaterials:<\/strong> 0.1 mol dm-3<\/sup> silver nitrate solution, 0.1 mol dm-3<\/sup> potassium nitrate solution, 0.1 mol dm-3<\/sup> tin(II) nitrate solution, copper strip, magnesium ribbon, iron nail and sandpaper.
\nApparatus:<\/strong> Test tubes and test tube rack.
\nProcedure:<\/strong><\/p>\n\n
\n<\/li>\n
\n<\/strong><\/p>\n\n\n
\n Test tube<\/strong><\/td>\n Prediction<\/strong><\/td>\n Observation<\/strong><\/td>\n<\/tr>\n \n X<\/td>\n Copper is above silver in the electrochemical series. Thus, copper will displace silver from silver nitrate solution.<\/td>\n The copper strip dissolves. A shiny grey solid is deposited. The colourless solution turns blue.<\/td>\n<\/tr>\n \n Y<\/td>\n Magnesium is below potassium in the electrochemical series. Thus, magnesium will not displace potassium from potassium nitrate solution.<\/td>\n No visible change.<\/td>\n<\/tr>\n \n Z<\/td>\n Iron is above tin in the electrochemical series. Thus, iron will displace tin from tin(II) nitrate solution.<\/td>\n The iron nail dissolves. A shiny grey solid is deposited. The colourless solution turns light green.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n \n
\nThe shiny grey solid is silver metal. The colourless solution turns blue because copper(II) ions have been released into the solution. The equation for the reaction is
\nCu(s) + 2AgNO3<\/sub>(aq) \u2192\u00a0Cu(NO3<\/sub>)2<\/sub>(aq) + 2Ag(s)
\nThe prediction is correct. The metal displacement reaction occurs.<\/li>\n
\nThe prediction is correct. The metal displacement reaction does not occur.<\/li>\n
\nThe shiny grey solid is tin metal. The colourless solution turns light green because iron(II) ions have been released into the solution. The equation for the reaction is
\nFe(s) + Sn(NO3<\/sub>)2<\/sub>(aq) \u2192\u00a0Fe(NO3<\/sub>)2<\/sub>(aq) + Sn(s)
\nThe prediction is correct. The metal displacement reaction occurs.<\/li>\n<\/ol>\n
\nThe ability of a metal to displace another metal from its salt solution can be predicted using the electrochemical series. The prediction can be confirmed through an experiment. The hypothesis is accepted.<\/p>\n