1. Video Tutorial on Electrolysis,Electroplating and Standard ElectrodePotential. Prepared by Lawrence Kok http://lawrencekok.blogspot.com

2. Video on Standard Electrode Potential and Voltaic CellGalvanizing Iron with ZincExcellent Silver crystal formationElectrolysis of waterElectrolysis of waterElectrolysis of KI 3. Factors Affecting the Products of Electrolysis (Standard Electrode Potential) Electrolysis of aqueous NaCIAnode (+ve) Cathode (-ve)Which anion will be Oxidised at Anode ? Which cation will be Reduced at Cathode ? 4. Factors Affecting the Products of Electrolysis (Standard Electrode Potential)Electrolysis of aqueous NaCI Anode (+ve) Cathode (-ve) O2 formedH2 formed Which anion will be Oxidised at Anode ? Which cation will be Reduced at Cathode ?OH- ion will be oxidised to O2 gas H+ ion will be reduced to H2 gas 5. Factors Affecting the Products of Electrolysis (Standard Electrode Potential) Electrolysis of aqueous Potassium Iodide (KI)Cathode (-ve) Anode (+ve)Which anion will be Oxidised at Anode?Which cation will be Reduced at Cathode ? 6. Factors Affecting the Products of Electrolysis (Standard Electrode Potential)Electrolysis of aqueous Potassium Iodide (KI) Cathode (-ve) Anode (+ve)I2 formedH2 formed Which anion will be Oxidised at Anode?Which cation will be Reduced at Cathode ? I - ion will be oxidised to I2 gas H+ ion will be reduced to H2 gas 7. Factors Affecting the Products of Electrolysis (Standard Electrode Potential) Electrolysis of aqueous Potassium Sulphate (KI)Cathode (-ve)Anode (+ve)Which anion will be Oxidised at Anode? Which cation will be Reduced at Cathode? 8. Factors Affecting the Products of Electrolysis (Standard Electrode Potential)Electrolysis of aqueous Potassium Sulphate (KI) Cathode (-ve)Anode (+ve)O2 formedH2 formed Which anion will be Oxidised at Anode? Which cation will be Reduced at Cathode? OH - ion will be oxidised to O2 gasH+ ion will be reduced to H2 gasConclusion: Cation to Cathode Gain electron (Reduction) More (+ve) E red will be preferred Anion to Anode Lose electron (Oxidation) More (+ve) E oxi will be preferred 9. Factors Affecting the Products of Electrolysis (Concentration) DILUTED Copper (II) ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE?Concentrated Copper (II) ChlorideWhich anion will be Oxidised at ANODE? Which cation will be Reduced at CATHODE? 10. Factors Affecting the Products of Electrolysis ( Concentration) DILUTED Copper (II) ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE?Concentrated Copper (II) ChlorideWhich anion will be Oxidised at ANODE? Which cation will be Reduced at CATHODE? 11. Factors Affecting the Products of Electrolysis ( Concentration) DILUTED Copper (II) ChlorideOxygen at Anode Copper at CathodeWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE?Concentrated Copper (II) ChlorideChlorine at AnodeCopper at CathodeWhich anion will be Oxidised at ANODE? Which cation will be Reduced at CATHODE? 12. Factors Affecting the Products of Electrolysis ( Concentration)DILUTED Sodium ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Concentrated Sodium ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? 13. Factors Affecting the Products of Electrolysis ( Concentration)DILUTED Sodium ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Concentrated Sodium ChlorideWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? 14. Factors Affecting the Products of Electrolysis ( Concentration)DILUTED Copper (II) ChlorideOxygen at Anode Copper at CathodeWhich anion will be Oxidised at ANODE? Which cation will be Reduced at CATHODE? Concentrated Copper (II) ChlorideChlorine at Anode Copper at CathodeWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? 15. Factors Affecting the Products of Electrolysis ( Type of Electrodes) Copper (II) Chloride with CARBON ELECTRODEWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Copper (II) Chloride with COPPER ELECTRODE Which anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? 16. Factors Affecting the Products of Electrolysis ( Type of Electrodes) Copper (II) Chloride with CARBON ELECTRODEWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Copper (II) Chloride with COPPER ELECTRODE Which anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? 17. Factors Affecting the Products of Electrolysis ( Type of Electrodes) Copper (II) Chloride with CARBON ELECTRODEOxygen at Anode Copper at CathodeWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Copper (II) Chloride with COPPER ELECTRODECopper at Cathode Copper dissolve at Anode Which anion will be Oxidised at ANODE? Which cation will be Reduced at CATHODE? 18. Factors Affecting the Products of Electrolysis ( Type of Electrodes) Silver Nitrate with CARBON ELECTRODEWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE?Silver Nitrate with SILVER ELECTRODEWhich cation will be Reduced at CATHODE? Which anion will be Oxidised at ANODE? 19. Factors Affecting the Products of Electrolysis ( Type of Electrodes) Silver Nitrate with CARBON ELECTRODEWhich anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE?Silver Nitrate with SILVER ELECTRODEWhich cation will be Reduced at CATHODE? Which anion will be Oxidised at ANODE? 20. Factors Affecting the Products of Electrolysis ( Type of Electrodes)Silver Nitrate with CARBON ELECTRODEOxygen at AnodeSilver at Cathode Which anion will be Oxidised at ANODE?Which cation will be Reduced at CATHODE? Silver Nitrate with SILVER ELECTRODESilver at Cathode Silver dissolve at AnodeWhich cation will be Reduced at CATHODE?Which anion will be Oxidised at ANODE? 21. Electroplating Process to coat surface of metal with a thin layer of metal of choice (silver, gold, copper) Object to be plated is on the CATHODE Anode is electroplating metal of choice Electrolyte solution contains metal of choice 22. Electroplating Process to coat surface of metal with a thin layer of metal of choice (silver, gold, copper) Object to be plated is on the CATHODE Anode is electroplating metal of choice Electrolyte solution contains metal of choiceConclusion : Rate of Cu2+/Ag+ ions formation at ANODE = Rate of Cu/Ag metal deposition at CATHODE Concentration of electrolyte remains constant Anode (+ve) Electrode dissolves Mass decreases Cathode (-ve) Electrode deposited Mass increases 23. Faradays 1st Law of Electrolysis Amount of substance produced during electrolysis is directly proportional to amount of charge Amt, mass formed Charge, QFaradays 2nd Law of Electrolysis Amount of different substance produced by same amount of electricity is inverselyproportional to the charge on its ionsNotes on Law of Electrolysis Quantity of electric current, charge, Q is measured in Coulomb One Coulomb is quantity of charge transferred by a current of 1 Ampere in 1 second Quantity Charge, Q = Current (A) X Time (s) Current (I) = Charge flow per unit time, I = Q/t 1 Faraday = Faraday constant = Charge on 1 mole of electrons = 96500C/mol Charge on 1 electron = 1.60 x 10 -19C Charge on 1 mole electron = 1 mole electron x Charge on 1 electron = ( 6.02 x 10 23 x 1.60 x 10 -19 C = 96500C Charge on 1 mole of electron = 96500C/mol = 1 Faraday = Faraday Constant 1 Faraday = Quantity of electricity, 96500C supplied to produce 1 mole electron for rxn 1 mole of electron has a total charge of 96500C Amount of product form depends on 1) Current 2) Time 3) Charge on ion 24. Ex 1 : Electrolysis of Copper (II) Sulphate using current 0.15A for 5hrs. Calculate amt of copper formedEx 2 : Electrolysis of Copper /Silver salt solution using Faradays 2nd LawCalculate the mass of copper and silver formed when 3 Faraday is used 25. Ex 1 : Electrolysis of Copper (II) Sulphate using current 0.15A for 5hrs. Calculate amt of copper formedAnsEx 2 : Electrolysis of Copper /Silver salt solution using Faradays 2nd LawCalculate the mass of copper and silver formed when 3 Faraday is used Ans Faradays 2nd Law 3 Faraday = 3 mol of Ag = 1.5 mol Cu = (3 x 108)g= ( 1.5 x 63.5)g = 324g= 95.25g 26. Ex 3 : Electrolysis of Copper /Silver/ Sulphuric acid using Faradays 2nd LawCalculate the mass of Copper , Vol of H2 and O2 formed at stp if 0.32g Ag is formed 27. Ex 3 : Electrolysis of Copper /Silver/ Sulphuric acid using Faradays 2nd LawCalculate the mass of Copper , Vol of H2 and O2 formed at stp if 0.32g Ag is formed AnsMoles Ag = 0.32/108 = 2.96 x 10 -3 mol 28. Ex 4 : Find the mass of Cu produced at cathode by a current (I) = 3.00A, Time = 2hrsEx 5 : Electrolysis of Cr2(SO4)3 yield 0.86g of Chromium after passing current for 12.5mins Find the amt of current usedEx 6: Calculate time /hrs needed to produce 25.0g of chromium from Cr2(SO4)3 with a current of 1.1A 29. Ex 4 : Find the mass of Cu produced at cathode by a current (I) = 3.00A, Time = 2hrsAnsEx 5 : Electrolysis of Cr2(SO4)3 yield 0.86g of Chromium after passing current for 12.5mins Find the amt of current used AnsEx 6: Calculate time /hrs needed to produce 25.0g of chromium from Cr2(SO4)3 with a current of 1.1A Ans 30. AcknowledgementsThanks to source of pictures and video used in this presentationThanks to Creative Commons for excellent contribution on licenseshttp://creativecommons.org/licenses/Prepared by Lawrence KokCheck out more video tutorials from my site and hope you enjoy this tutorialhttp://lawrencekok.blogspot.com