A solution of \(Ag_2SO_4\) is electrolyzed for 15 minutes with a current of 5 amperes. What is the mass of the silver deposited?
[Atomic mass of Ag = 108 g/mol]
Answer & explanation
Correct answer: option 3
The correct answer is Option (3) → 5.04 g
Silver is deposited at the cathode by \( \ce{Ag^{+}} \) + e− → Ag, so 1 mol of electrons (1 F = 96500 C) deposits 1 mol of Ag (108 g).
Charge passed, Q = I × t = 5 A × (15 × 60) s = 4500 C
Mass of Ag = (108 g × 4500 C) / 96500 C = 5.036 g ≈ 5.04 g
Note: NTA picked this question from an NCERT (2026-27) example and changed the figures. Do not ignore NCERT while practising numericals.
NCERT (2026-27 edition):
Electrolytic Cells and Electrolysis – “… A solution of CuSO4 is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode?”