NEET 2026 (Phase 1) · ChemistryElectrolysisPrevious Year Question
A solution of copper sulphate is electrolysed for $10$ minutes with a current of $1.5$ amperes. The mass of copper deposited at the cathode is: (Given: Molar mass of \ce{Cu} $= 63$ g mol$^{-1}$; $1\,F = 96487$ C mol$^{-1}$)
- A.1.7018 g
- B.0.2938 g✓
- C.2.4036 g
- D.0.5876 g
Correct Answer
(B) 0.2938 g
Solution & Explanation
\textbf{Answer:} (B) 0.2938 g \textbf{Solution:} At the cathode: \ce{Cu^2+ + 2e- -> Cu} ($n = 2$). Charge passed: $Q = I t = 1.5 \times (10 \times 60) = 1.5 \times 600 = 900\ \text{C}$. Using $w = \dfrac{M \cdot Q}{n \cdot F}$, $$w = \frac{63 \times 900}{2 \times 96487} = \frac{56700}{192974} \approx 0.2938\ \text{g}.$$
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