$0.592 \ g$ of copper is deposited in $60 \ minutes$ by passing $0.5 \ amperes$ current through a solution of copper$(II)$ sulphate. The electrochemical equivalent of copper$(II)$ (in $g \ C^{-1}$) is $\left(F=96500 \ C \ mol^{-1}\right)$
- A$3.3 \times 10^{-3}$
- B$3.3 \times 10^{-4}$
- C$6.6 \times 10^{-3}$
- D$6.6 \times 10^{-4}$
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