Electrochemistry – Volatile Cell kit – MAS 4156
Kit Includes :
Glass Beaker 250ml x 2 , Copper Electrode x 1, Zinc Electrode x 1, Copper Sulphate solution 200ml, Zinc Sulphate solution 200ml , Salt bridge U-tube x 1 , Digital Voltmeter x 1, Connecting wire x 2
Galvanic Cell with an Example
Let us take an example where the two metals involved in the chemical reaction are zinc and copper. As the chemical reaction takes place, Zinc would end up losing two electrons. This will be taken up by copper to become elemental copper. Since these two metals will be placed in two separate containers and would be connected by a conducting wire, an electric current would be formed, which would transfer all electrons from one metal to another.
At the same time, the two metals shall be immersed in a salt solution, say, Zinc Sulphate and Copper Sulphate in this case. In this case, the two solutions are not mixed together directly but can be joined using a bridge or a medium. This medium shall be responsible for the transfer of ions but also make sure that the two solutions do not come to mix with each other.
Such bridge helps in completing the circuit for carrying the electric charge and also makes sure that the solutions in the containers with the metals remain neutral and do not mix with each other. As long as the salt bridge does not interfere with the redox reaction, under which oxidization and reduction are taking place, it does not matter which salt bridge is being used in the chemical reaction.
Some Important Terms
Some of the important terms brought into use in a galvanic cells are listed below:
- Phase boundaries: It refers to the two metals which act as cathode and anode.
- Salt bridge: The connecting bridge or medium that allows a redox reaction to take place.
- Oxidation and reduction: The chemical processes that allow the electric current to form and flow through a galvanic cell.
Video procedure for experiment.