How many ffardays of electricity are required to produce 13 gram of aluminium from aluminium chloride solution ?
(Give : Molar mass of Al = 27.0 gram `mol^(-1)`)

Explanation

Equation
`AlCl_(3)to Al^(3+)+3Cl^(-)`
`Al^(3+)3e^(-)to Al_((S))`
1 mole of Al requires passage of 3 mole of electrons and charge on 3 mole of electrons is 3 faraday
Moles of Al produced `=("Mass of Al")/("Molar mass of Al")`
`=(13)/(27)=0.48` moles
`because` 3 F of electricity produces 1 mole of Al.
`therefore` No. of faradays of electricity rquired to produce 0.48 mole of Al
`= 0.48xx3`
= 1.44 faraday.