What is meant by the following terms?

i) Electrolysis
ii) Electrolytes
iii) Cations
iv. Anions

Distinguish between

i) Electrolytes and non – electrolytes
ii) Strong and weak electrolytes
iii) Caution and anions

Which of the following substances are electrolytes and which are non – electrolytes? Explain your answer. Copper (II) Chloride, Sugar, ether, Zinc sulphate.

Explain the following briefly

i) Ionic theory of electrolysis
ii) Migration of ions

Write down example of half reaction of half reaction occurring at

a) Anode
b) Cathode

Distinguish between REDUCTION from OXIDATION

Aluminum oxide, zinc bromide, paraffin wax, sodium, hydrogen chloride, silver chloride, Iodine and lead.

From the above list, choose substances.

a) Which conduct electricity.

i. When solid
ii. When molten, but not when solid,
iii. When in aqueous solution

b) Which do not readily conduct electricity under any conditions.

Briefly describe strength and concetration of an electrolyte.

a) What in electrolytic cell

b) Draw example of electrolytic cell.

Mention factor for discharging ions during electrolysis.

Briefly explain how the following affect discharging.

i. Concentration
ii. Nature of the electrode

State faradays laws of Electrolysis.

A steady of 4A was passed through an aqueous solution of copper (II) sulphate for 30 minutes. Calculate the mass of copper deposited at cathode in

How much quantity will be produced when ten hours were used to deposit by 20A.

An electric steady current of 2A was passed through fused aluminum oxide. Calculate the time taken to deposit 25g of Aluminum metal.

Calculate

i. The mass of the product at the cathode
ii. The volume of the product (at r.t.p) at the anode when a current of 8 amps passes for 80 minutes through the solution of copper (II) sulphate using platinum electrodes. (1 faraday = 96000 coulomb;
molar gas volume = 24dm³ at r.t.p)

Two voltammeter containing copper (II) Sulphate and silver nitrate solution were connected in series. It was found that 0.449g of copper and 1.542g of silver were deposited at the cathode. Show that the results agree with the faradays second law of electrolysis.

A current of 1.5 A was passed through silver nitrate and copper (II) Sulphate solutions connected in series for 10 minutes. If 0.35g of silver was deposited in the first all, calculate the mass of copper deposited for equivalent time.

During the electrolysis of a copper salt, 0.21g of copper was deposited in five minutes. If a current of 2A was passing through the solution, calculate the electrochemical equivalent of copper.

Outline four areas where the knowledge of electrolysis is applied.