Question

How many faradays of charge is required to deposit 0.5mole of Copper by electrolysis of CuSO4?

Answer 1

Explanation:

The correct option is Bwe can calculate the mole of copper get deposited by 0.5 Faraday 0.5 faraday × 1 mole of copper/2 faraday on solving this equation ...

Answer 2

1 faraday of charge is the ideal answer.

Given:

• Copper = 0.5mole.

Faradays Law :

• The significance of the emf caused in a circuit is proportional to the rate of alternate of the magnetic flux that cuts throughout the circuit.

Explanation:

• 1 CuSo₄ = Cu²⁺ + So₄²⁻ , +2e⁻ and cathode Cu(s).
• 0.5 CuSo₄, then +1e⁻ to deposit Cu⁺² ion as Cu(s).
• 1 faraday of charge is needed to deposit 0.5mole of Copper with the aid of using electrolysis of CuSO4.
• Amount of rate with the aid of using 0.5 moles of copper=96485.3321 C mol⁻¹.

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