Electrolytic Cells REVERSE spontaneous reactions through the input of electricity A non spontaneous reaction that is forced to occur with the input of energy Electrolysis of Water in acidic solution ID: 538048
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Electrolytic CellsSlide2
Electrolytic Cells
REVERSE spontaneous reactions through the input of
electricity
A non spontaneous reaction that is forced to occur with the input
of energy Slide3
Electrolysis of Water
in acidic solution Slide4
Electroplating
Commercial uses of electrolysis is electroplating
A relatively inexpensive metal (steel or copper) can be coated with a layer of more expensive metal (silver or gold)Slide5
The metal to be coated is the cathode, while ions of the metal that will be deposited onto the cathode are present in the electrolyte
The minimal voltage will allow the reaction to proceed, however a higher voltage will increase the speed of the reactionSlide6
Example
Creating a Copper Ring for your Beautiful Girlfriend on a random piece of metal by placing it in CuSO
4
solutionSlide7
Example:
Cathode: spoon to be plated
Anode: silver strip (however it can be an inert such as Pt)
Electrolyte: 1.0M AgNO3Slide8
Electrorefining
Electrolysis can be used on ores to extract the desired metalSlide9Slide10
CHLORIDE
The Chloride anomaly occurs during the electrolysis of solutions containing a chloride ion.Slide11
Because the strongest reducing agent is at the anode, water would be expected to react, producing O2(g)
Instead, chloride ions react and chlorine gas (Cl2) is produced at the anode. Slide12
Comparison of Cells