An electrolytic cell is made of an aqueous solution of CuSO4. If a current of 3.44 A is used in the cell?

Molar mass of Cu = 63.55 g/mol
No. of moles of Cu = (10.0 g) / (63.55 g/mol) = 10.0/63.55 mol

Cu²⁺(aq) + 2e⁻ → Cu
OR: Mole ratio e⁻ : Cu = 2 : 1
No. of moles of e⁻ passed = (10.0/63.55 mol) × 2 = 20.0/63.55 mol

1 mole of e⁻ carries 96500 C of charges.
Amount of charges, Q = (20.0/63.55 mol) × (96500 C/mol) = 30370 C

Time taken = (30370 A s) / (3.44 A) = 8828 s = (8828/60) = 147.1 min

CuSO4 → Cu{2+} + SO4{2-} [balanced as written]
Cu{2+} + 2 e{-} → Cu

(10.0 g Cu) / (63.5463 g Cu/mol) x (2 mol e{-} / 1 mol Cu) x (9.64853399 × 10^4 C/mol e{-}) / (3.44 A) =
8828 seconds