Question

The number of Faradays required to deposit 1g equivalent of aluminum from a solution of all is

Answer 1

According to Faraday's law, 3 mole of Faraday is required to deposit 1g equivalent of aluminum from a solution.

Faraday's law is used in electrochemical studies.

Faraday is defined as the no. Of moles of electron passed due to passing of 1 Faraday charge per gm.

1Faraday can be calculated as:

1.63*10^-19*6.023*10^23=96500 coulomb

Faraday is a dimensionless quantity.

Hence, For Al3+ Ion 3 Faraday charge will be deposited.