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How Many Faradays of Electricity Are Required to Produce 13 Gram of Aluminium from Aluminium Chloride Solution? - Chemistry

How many faradays of electricity are required to produce 13 gram of aluminium from aluminium chloride solution? (Given: Molar mass of Al = 27.0-gram mol–1)

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Solution

AlCl3  Al+3 + 3Cl-

Al+3 + 3e-  Al

1 mole of Al requires passage of 3 moles of electrons. The charge on 3 moles of e- is 3 Faraday.

Moles of Al produced = `"mass of Al"/"molar mass of Al"`

= `13/27`

= 0.48 moles

As 3F of electricity produces 1 mole of Al

∴ No. of faradays of electricity required to produce 0.48 mole of Al

= 0.48 x 3

= 1.44 Faraday

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