Chemistry

Problem

Electrolysis of an aqueous Cu²⁺ solution deposits 0.635 g of Cu metal onto the cathode. Assuming 100 % current efficiency, what total charge (in coulombs) passed through the cell? (Atomic mass of Cu = 63.55 g mol⁻¹) a)

9.65 \times 10^{4}\ \text{C}

3.86 \times 10^{3}\ \text{C}

1.93 \times 10^{3}\ \text{C}

9.65 \times 10^{2}\ \text{C}

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