What volume of chlorine gas measured at StP will be liberated by a current of 2.5 A flowing for a period of 1.8 hours through an

Question

Katen [24]

2 years ago

8

What volume of chlorine gas measured at StP will be liberated by a current of 2.5 A flowing for a period of 1.8 hours through an

aqueous solution of AGCL

Chemistry

1 answer:

Oliga [24] · Answer 1 · 2023-06-21T10:37:12+03:00

The volume of chlorine gas measured at STP will be liberated by a current of 2.5 A flowing for a period of 1.8 hours through an aqueous solution of AgCl is 1.88 litre.

<h3>What is Faraday's law ?</h3>

According to Faraday's Law , During Electrolysis , The amount of substance liberated at the cathode or anode is directly proportional to the electricity that is passed through the cell.

The reaction taking place at anode is:

2Cl → Cl₂ +2e −

The total charge is calculated as

Q=I×t= 2.5×1.8×60×60 coulomb

Q = 16200 coulomb

The amount of chlorine liberated by passing 16200 coulomb of electric charge

= 16200/(2*96500)

= 0.084 mole

Volume of Cl₂ at STP is

1 mole at STP has 22.4 L of Gas

0.084 mole of Cl₂ at STP will be equal to 22.4 *0.084 = 1.88 litre of Cl₂

To know more about Faraday's Law

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