Question

0.592 g of copper is deposited in 60 minutes by passing 0.5 amperes current through a solution of copper (II) sulphate. The electro chemical equivalent of copper (II) in g/C is:

• A. $3.3 \times 10^{-3}$
• B. $3.3 \times 10^{-4}$
• C. $6.6 \times 10^{-3}$
• D. $6.6 \times 10^{-4}$

Hint:

The electrochemical equivalent is calculated by dividing the mass of the substance deposited by the total charge passed through the solution.

Answer 1

The Correct Option is B

The total charge passed is $Q = I \times t = 0.5 \, \text{A} \times 3600 \, \text{s} = 1800 \, \text{C}$. The electrochemical equivalent $k$ is given by $k = \frac{\text{mass deposited}}{\text{charge passed}} = \frac{0.592}{1800} \approx 3.3 \times 10^{-4} \, \text{g/C}$.