$A$ solution of copper sulphate is electrolysed for $10 \text{ minutes}$ with a current of $1.5 \text{ amperes}$. The mass of copper deposited at the cathode is:
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)
(Given: Molar mass of $Cu = 63 \text{ g mol}^{-1}$; $1F = 96487 \text{ C mol}^{-1}$)
- A$(1)$ $0.2938 \text{ g}$
- B$(2)$ $0.5876 \text{ g}$
- C$(3)$ $2.4036 \text{ g}$
- D$(4)$ $1.7018 \text{ g}$
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