Electrolytic Cells

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

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)

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 reaction

Example Creating a Copper Ring for your Beautiful Girlfriend on a random piece of metal by placing it in CuSO4 solution

Example: Cathode: spoon to be plated Anode: silver strip (however it can be an inert such as Pt) Electrolyte: 1.0M AgNO3

Electrorefining Electrolysis can be used on ores to extract the desired metal

CHLORIDE The Chloride anomaly occurs during the electrolysis of solutions containing a chloride ion.

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.

Contains a Battery and only 1 solution Comparison of Cells Voltaic Cells Spontaneous Ecell = + Cathode (SOA) + Anode (SRA) – Contains a Salt bridge Electrolytic Cells Non Spontaneous Ecell = – Cathode (SOA) – Anode (SRA) + Contains a Battery and only 1 solution