Question

Q.02 How many faradays of electricity are involved in each ofthe case
(a) 0.25 mole Al3+ is converted to Al.​

Answer 1

Given:

No of moles of Al³⁺ = 0.25

To Find:

The amount of electricity required to convert the given Al³⁺ into Al.

Calculation:

- 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 Faraday

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

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.