Question

Write down the changes that will be seen in each instance and explain the reason behind it dilute h2 s o4 was taken in an electrolytic cell and electric current was passed through it

Answer 1

Answer:

Explanation:

the electrodes must be made of an inert wire. Students should note that the electrolysis will only take place when electricity is passed through the dilute sulfuric acid solution. The electrolyte is dilute sulfuric acid (= acidified water) which, during electrolysis is split into hydrogen and oxygen gases.

Answer 2

If pure water is used in the electrolytic cell, current does not flow even on putting on the switch.

Pure water is a bad conductor of electricity. Dilute H2SO4 is acidulated water. The electrical conductivity of water increases on mixing with strong acid or base in it due to their dissociation and electrolysis of water takes place.

H2SO4 is fully dissociated in aqueous solution.

H2SO4 → (2H+) + (SO²4-)

H2O is a weak electrolyte and is only slightly dissociated.

H2O → (H+) + (OH-)

During electrolysis, the hydrogen ions migrate towards the cathode and are discharged there.

[ H+ ions gains electrons and are converted to hydrogen gas ]

(2H+) + (2e-) → H2

Cathode reaction:

2H2O (I) + 2e- → H2 (g) + 2OH+ (aq)

Anode reaction:

2H2O (I) → O2 (g) + (4H+) (aq) + 4e-

For every hydrogen ion discharged at the anode, another hydrogen ion is formed at the cathode. The net result is that the concentration of the sulphuric acid remains constant and electrolysis of water is overall reaction.

2H2O → 2H2 + O2

In this activity the volume of the hydrogen gas formed near the cathode is double that of the oxygen gas formed near the anode.