1 / 16

Electrolytic Cells and Applications in Electroplating

Learn about electrolytic cells, their components, and how they are used in processes like electrolysis of salts and electroplating. Explore the differences and similarities with voltaic cells.

courtneyweldon
Download Presentation

Electrolytic Cells and Applications in Electroplating

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. Electrolytic Cells Aim: Write half reactions for electrolysis of a salt and electroplating

  2. What is an Electrolytic Cell? Electrolytic Cell:A cell where a battery forces a redox reaction to occur (non-spontaneous reaction). Opposite of a voltaic cell. Uses: 1) To obtain group 1 and group 2 metals. Electrolysis of salts, "Salt splitting". 2) Electroplating: plating a metal on top of another (Ex. Gold plated jewelry)

  3. Parts of an Electrolytic Cell Electrolytic cells have only one cell. Electrolytic cells are powered by a battery or power source. Converts 
electrical to chemical energy. Anode- still the site of oxidation. Assigned as the POSITIVE electrode. Cathode- still the site of reduction. 
Assigned as the NEGATIVE electrode.

  4. Electrolysis of a Salt Molten salt breaks up into ions 
in solution NaCl(l) → ________________ Na+ is attracted to negative cathode and is reduced _______________________ Cl1- is attracted to the positive anode and is oxidized ________________________

  5. Example: Electrolysis of a Salt Write the oxidation and reduction 1/2 reaction for the following cell: ox 1/2: red 1/2: MgF2 (l)

  6. Electroplating The metallic ions in solution 
with positive charge attract to the negative cathode and reduce onto 
it (plating). ______________________ The metal anode is oxidized to produce more positive metal ions in solution to continue the process. ______________________ - + *Negative ions do not play a 
part in the electroplating

  7. Example: Write the oxidation and reduction half reactions for the plating of the Al glasses from by the Au ox 1/2: red 1/2: + - AuNO3

  8. Similarities Between Voltaic and 
Electrolytic Cells 1) Both use redox reactions 2) The anode is the site of oxidation 3) The cathode is the site of reduction 4) The electrons flow through the wire 
from anode to cathode

  9. Differences Between Voltaic and 
Electrolytic Cells Voltaic Electrolytic Non-spontaneous reaction - forced through use of a battery Anode is positive Cathode is negative One Cell Spontaneous redox reaction Anode isnegative Cathode is positive Two Half Cells

  10. Electrolysis of a Salt a) MgCl2  ox 1/2:  red 1/2: MgCl2 (l) KBr (l) a) KBr2  ox 1/2:  red 1/2:

  11. Electrolysis of a Salt c) CaO  ox 1/2:  red 1/2: CaO (l)

  12. Electroplating a)  ox 1/2:  red 1/2: Zn  ZnCl2 (aq)  b)  ox 1/2:  red 1/2: Mn  Mn(NO­3)4 (aq) 

  13. Voltaic Cells

  14. Voltaic Cells

  15. Voltaic Cells

More Related