Question

The amount of electricity required to produce one mole of copper from copper sulphate solution will be

• A. 1 Faraday
• B. 2.33 Faraday
• C. 2 Faraday
• D. 1.33 Faraday

Hint:

Charge required \(=\) \(nF\), where \(n\) is number of electrons involved in electrode reaction.

Answer 1

The Correct Option is C

Step 1: Write electrode reduction reaction.
In CuSO\(_4\) solution, copper is deposited as:
\[ Cu^{2+} + 2e^- \rightarrow Cu(s) \]
Step 2: Determine electrons needed.
To produce 1 mole of copper, we need 2 moles of electrons.
Step 3: Relation between charge and moles of electrons.
1 Faraday = charge required to supply 1 mole of electrons.
Thus 2 moles electrons need 2 Faraday.
Final Answer:
\[ \boxed{2 \text{ Faraday}} \]