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