1 / 24

Application of Electrolytic Cells Lesson 11

Application of Electrolytic Cells Lesson 11. Electrolysis describes what happens in an electrolytic cell and means to use electricity to make chemicals . Many elements are made by electrolysis Pb Al Zn Na K Li H 2 Cl 2 F 2 I 2 O 2 Pb 2+ + 2e - → Pb (s)

lew
Télécharger la présentation

Application of Electrolytic Cells Lesson 11

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Application of Electrolytic Cells Lesson 11

  2. Electrolysis describes what happens in an electrolytic cell and means to use electricity to make chemicals. Many elements are made by electrolysis Pb Al Zn Na K Li H2 Cl2 F2 I2 O2 Pb2+ + 2e- → Pb(s) 2Cl-→ Cl2(g) + 2e- This is sometimes called electrowinning- the element is won from its ion

  3. Making Aluminum by Electrolysis Alcan (70,000 employees in 55 countries) Kitimat B.C. 2.7 MT 7 % world production

  4. Aluminum

  5. Aluminum Production by Electrolysis Name of the Ore imported from (Guinea and Brazil) Bauxite Al2O3.3H2O Heating drives off the water Al2O3.3H2O + Heat → Al2O3 +3H2O Melting point of Bauxite is 2045 0C This istoohot! Cryolite is added Lowers the melting point to 1000 0C

  6. Reduction of water You cannot reduce Aluminum in water! It must be molten!

  7. Liquid Al floats to the top and is removed DC Power - + Oxygen gas C C - Reduction Cathode Al3+ + 3e-→ Al(s) + Oxidation Anode O2-→ 1/2O2(g) + 2e- Al3+ O2- Al2O3(l) Cation Cathode Reduction Anion Anode Oxidation

  8. Electroplating Auplatinga Cu penny Electroplatingis the process of reducing a metalon to the surface of another Electrolyte: Must contain the ion of the metal that plates Cathode: The metalto be covered with a new metal Anode:Metal to be plated on top the other metal DC Power - + e- - Reduction Cathode Au+ + e-→ Au(s) Au + Oxidation Anode Au(s) → Au+ + 1e- Au+ CN- Cu Cu

  9. +ve -ve stainless steel or Au AuCN

  10. Au plated

  11. Copper Ring Gold Plated

  12. Tanya’s Ring Gold Plated

  13. Electroplating Agplatinga Loonie DC Power - + e- - Reduction Cathode Ag+ + e-→ Ag(s) Ag + Oxidation Anode Ag(s) → Ag+ + 1e- Ag+ NO3- $1 $1

  14. Electrorefinning Lead Trail, B.C. Teck 16 mines in BC Major World Producer of Zn, Cu, Pb, and Coal

  15. Lead Refinery-Trail

  16. The Electrorefinning of Lead Electrorefining is the process of purifying a metalby electrolysis. The electrolyte must contain Pb Impuremetal is oxidizedat theanodeand pure metal is reduced at the cathode. This is the same as electroplating. DC Power - + Cathode: Pure Pb Anode:Impure Pb - Reduction Cathode Pb2+ + 2e-→ Pb(s) Pb2+ NO3-

  17. The impurities in Pb are: Au Ag Zn

  18. At the Anode Au does not oxidize The voltage is controlled so that: Ag does not oxidize Pb oxidizes Zn oxidizes

  19. At the Cathode The voltage is controlled so that: Pb2+ reduces Zn2+ does not reduce

  20. The Electrorefinning of Lead Electrorefining is the process of purifying a metalby electrolysis. The electrolyte must contain Pb Impuremetal is oxidizedat theanodeand pure metal is reduced at the cathode. This is the same as electroplating. DC Power - + Cathode: Pure Pb Anode:Impure Pb - Reduction Cathode Pb2+ + 2e-→ Pb(s) + Oxidation Anode Zn(s) → Zn2+ + 2e- Pb(s) → Pb2+ + 2e- Pb2+ NO3- Zn2+ Au Ag Solid Au and Cu are released from the anode and fall to the bottom

  21. Video of the thermite reaction used to make Iron The Thermite reaction is very exothermic and produces white hot molten iron. Fe2O3 + 2Al(s)→ Al2O3(s) + 2Fe(l) + energy

More Related