Question

The number of Faradays needed to reduce \(4\,g\) equivalents of \(Cu^{2+}\) to Cu metal will be

• A. 1
• B. 2
• C. \(\dfrac{1}{2}\)
• D. 4

Hint:

1 Faraday \(\Rightarrow\) 1 gram equivalent deposited. Therefore, for \(n\) gram equivalents, charge needed = \(n\) Faradays.

Answer 1

The Correct Option is D

Step 1: Faraday’s law of electrolysis.
1 Faraday of charge deposits 1 gram equivalent of any substance.
Step 2: Given quantity.
We need to reduce \(4\) gram equivalents of \(Cu^{2+}\).
Step 3: Required Faradays.
Since \(1\) Faraday deposits \(1\) gram equivalent,
\[ \text{Faradays required} = 4 \] Final Answer: \[ \boxed{4} \]