Question

A solution of CuSO₄ is electrolyzed using a current of 1.5 amperes for 10 minutes. What mass of Cu is deposited at the cathode? (At. mass of Cu = 63.7)

• A. 0.395 g
• B. 0.150 g
• C. 0.637 g
• D. 0.297 g

Hint:

Remember to use the formula for electrolysis calculations, which involves current, time, and the molar mass of the substance being deposited.

Answer 1

The Correct Option is D

Step 1: Formula for the mass of Cu deposited.
The formula to calculate the mass deposited during electrolysis is given by: \[ \text{Mass} = \frac{I \times t \times M}{n \times F} \] Where: - \( I \) is the current (1.5 A), - \( t \) is the time (10 minutes = 600 seconds), - \( M \) is the molar mass of Cu (63.7 g/mol), - \( n \) is the number of electrons involved in the deposition (for Cu, \( n = 2 \)), - \( F \) is Faraday’s constant (96,500 C/mol).

Step 2: Calculation.
Substituting the given values into the formula: \[ \text{Mass} = \frac{1.5 \times 600 \times 63.7}{2 \times 96,500} = 0.297 \, \text{g} \]
Step 3: Conclusion.
The mass of Cu deposited is 0.297 g. Hence, the correct answer is (D) 0.297 g.