Question

Amount of electricity required to reduce 0.5 mole of Al3+ ions to Al atoms is​

Answer 1

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

How many faradays of electricity are involved in each ofthe case

(a) 0.5 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 0.5 moles = 0.5 × 3

⇒ Electricity required = 0.15

So, 0.15 Faraday of electricity is involved when 0.5 mole Al³⁺ is converted to Al.

Answer 2

Answer:

Electricity required = 0.15

Explanation:

Electricity is the glide of electrons. All remember is made of atoms, and an atom has a center, referred to as a nucleus. The nucleus carries undoubtedly charged debris referred to as protons and uncharged debris referred to as neutrons. The nucleus of an atom is surrounded with the aid of using negatively charged debris referred to as electrons.

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

Al³⁺ + 3e⁻ → Al

According to the above response, three Faraday of power is used to transform 1 mole of Al³⁺ into Al.

⇒ Electricity required for 0.five moles = 0.five × three=

=⇒ Electricity required = 0.15

So, 0.15 Faraday of power is concerned while 0. five mole Al³⁺ is transformed to Al.

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