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Home » Chemistry Homework Help » Organic Chemistsry » Electrolytic Cells
Electrolytic Cells
So far we have been discussing the process of conversion of chemical energy into electrical energy by means of electrochemical cell. In the reverse process the passage of electricity through the electrolytes in their molten or dissolved state can cause chemical change under suitable conditions. For example, the passage of electricity through the acidified water results in the formation of hydrogen the acidified water results is the formation of hydrogen and oxygen gases. The purpose of chemical decomposition of the electrolyte by the passage of electricity through its molten or dissolved state is called electrolysis.

Electrolytic cell: the device in which the process of electrolysis is carried out is called electrolytic cell. It consists of:

(i) Electrolytic tank, which is made of some non-conducting material like glass, wood or Bakelite.

(ii) Electrolyte in its dissolved state or molten state.

(iii) Source of electricity; and electrochemical cell or battery.

(iv) Two metallic rods, suspended in the electrolyte and connected to the battery through conducting wires. These rods are called electrodes. The electrode connected to the negative terminal of the battery is called cathode while the other one which is connected to the positive terminal is called anode. The apparatus used to constitute electrolytic cell.

The process of electrolysis can be explained on the basis of the theory of ionization. When an electrolyte is dissolved in water, it splits up into charged particles called ions. The positively charged ions are called cations while the negatively charged ions are called anions. The ions are free to move about in aqueous solution. When electric current is passed through the solution, the ions respond to the applied potential difference and their movement is directed towards the oppositely charged electrodes. The cations move upwards the negatively charged electrode while anions move towards the positively charged electrode. The formation of products of the respective electrodes is due to oxidization (loss of electrons) at the anode and reduction (gain of electrons) at the cathode. For example, when electricity is passed through the molten sodium chloride (NaCl), sodium is deposited at the cathode while Cl2 gas is liberated at the anode. The process can be represented as:
                
                    NaCl(l) Na+ + Cl-
 
Anode:               Cl- ½ Cl2 + e- (oxidization)

Cathode: Na+ + e- Na            (reduction)


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