electrolysis of molten lead bromide is considered to be a reaction in which oxidation and reduction go side by i.e.,a redox reaction.

Open in App

Solution

When electricity is passed through molten lead bromide, it decomposes to Pb²⁺ ions and Br^- ions. The Pb²⁺ ions move towards cathode and gain two electrons to from lead atoms. So, Pb²⁺ ions are reduced. Side by side, the Br^- ions move towards anode and loose electrons to from bromine gas. Thus, bromide ions are oxidized. Hence, electrolysis of lead bromide is a redox reaction.

$P b B r_{2} (l) \to P b (l) + B r_{2} (g) A t c a t h o d e : P b^{2 +} + 2 e \to P b (l) A t a n o d e : 2 B r^{-} \to B r_{2} (g) + 2 e$

Suggest Corrections

Similar questions

(a) State observation at the anode when aqueous copper sulphate solution is electrolysed using copper electrodes.

(b) During electrolysis of molten lead bromide, graphite anode is preferred to other electrodes. Give reason.

Give reasons for the following :

(a) Electrolysis of molten lead bromide is considered to be a reaction in which oxidation and reduction go side, i.e., a redox reaction.

(b) The blue colour of aqueous copper sulphate fades when it is electrolysed using platinum electrodes.

(d) Aluminium is extracted from its oxide by electrolytic reduction and not by conventional reducing agents.

(e) The ratio hydrogen and oxygen formed at the cathode and anode is 2: 1 by volume.

(f) In the electrolysis of acidified water, dilute sulphuric acid is preferred to dilute nitric acid for acidification.

(g) Ammonia is unionised in the gaseous state but in the aqueous solution, it is a weak electrolyte.

(h) A graphite anode is preferred to other inert electrodes during electrolysis of fused lead bromide.

(i) For electroplating with silver, silver nitrate is not used as the electrolyte.

(j) Carbon tetrachloride is a liquid but does not conduct an electrolyte.

(k) Potassium is not extracted by electrolysis of its aqueous salt solution.

Join BYJU'S Learning Program