Question

How many columns of electricity required to oxidise one mole of Al to Al3+

Answer 1

3 Faradays.

The trick lies in knowing exactly how many electrons are involved in ionisation for such radicals.

Answer 2

${\huge{\underline{\red{Question:-}}}}$

How many faradays of electricity are involved in each ofthe case

(a) 0.25 mole Al3+ is converted to Al.

${\huge{\underline{\red{Solution:-}}}}$

The reaction of conversion of Al³⁺ into Al is given as:

Al³⁺ + 3e⁻ → Al

According to the above reaction, 3 Faraday of electricity is used to convert 1 mole of Al³⁺ into Al.

⇒ Electricity required for 0.25 moles = 0.25 × 3

⇒ Electricity required = 0.75

So, 0.75 Faraday of electricity is involved when 0.25 mole Al³⁺ is converted to Al.