You visited us 1 times! Enjoying our articles? Unlock Full Access!

Redox Reactions and Couple

Give reasons:...

Question

Give reasons:
On the basis of $E^{o}$ values, $O_{2}$ gas should be liberated at anode but it is $C l_{2}$ gas which is liberated in the electrolysis of aqueous NaCl.

Open in App

Solution

It is due to the phenomenon of over-voltage. Experimentally, it is observed that the actual voltage required for electrolysis is greater than that calculated from standard potentials. This addition voltage required is called over-voltage. It is required because the rate of transfer of electrons at the interface of electrode and solutions for both half reactions is slow. The over-voltage required for formation of oxygen is much larger than that required for the formation of chlorine. Hence, chlorine gas which is liberated in the electrolysis of aqueous NaCl.

Suggest Corrections

Similar questions

S n^{2 +}

H^{+}

H_{2} (g)

E_{S n^{2 +} / S n}^{\circ}

E^{\circ}

O_{2}

C l_{2}

C H_{3} C O O H

S n^{2 +}

H^{+}

H_{2} (g)

E_{S n^{2 +} / S n}^{\circ}

E^{\circ}

O_{2}

C l_{2}

C H_{3} C O O H

N a O H, 4 g

O_{2}

H_{2}

N a O H, 2.8 l i t r e

H_{2} O

11.2

H_{2}

O_{2}

Join BYJU'S Learning Program