1 ampere current is passing through an electrolytic cell in which molten Nacl is electrolised, if time taken is 965 sec, then find out weight of metal & volume of gas at anode at stp
Answers
Answer:
0.23g of Na deposited at cathode and 0.224 litres Cl2 gas released at anode
Given:
The magnitude of the current passing through the NaCl solution = 1A
The duration through which the current flows: 965s
To find:
The weight of the metal and the volume of the gas produced at the anode.
Solution:
The weight of the metal produced is 0.23 g and the volume of the gas produced at the anode is 0.112L.
According to Faraday's law of electrolysis, the mass of the substance deposited is proportional to its equivalent mass.
The reaction in the given electrolysis is:
At cathode: Na⁺ (aq) + e⁻ → Na (s)
At anode: Cl⁻ (aq) → 1/2 Cl₂ (g) + e⁻
1 F of electrons is required to produce 1 equivalent (23g) of Na. We know that 1 F electrons have 96500C of charge.
The charge Q being provided in the given question = i.t
or Q = 1 X 965
= 965C
= 0.01 F
Using the unitary method,
0.01 F of electrons will produce 0.23g of sodium metal.
Similarly at the anode, 1 F produces half a molecule of chlorine gas.
So 1 mole Cl₂ is produced by 2F.
From 0.01 F, only 1 X 0.01 / 2 moles of Cl₂ (g) is produced
= 0.005 moles
= 0.005 X 22.4 L
= 0.112 L