In an electrochemical cell, $\mathrm{Ag}^{+}$ ions in $\mathrm{AgNO}_{3}$ are reduced to Ag metal at the cathode and Cu is oxidized to $\mathrm{Cu}^{2+}$ at the anode. A current of 0.7 A is passed through the cell for 10 min . The mass (in grams) of silver deposited and copper dissolved, respectively, are: [Faraday Constant $=96,485 \mathrm{C} \mathrm{mol}^{-1}$, Atomic Weight of $\mathrm{Ag}=107.9$, Atomic Weight of $\mathrm{Cu}=63.55$ ]
(a)0.235 and 0.138
(b)0.469 and 0.069
(c)0.469 and 0.138
(d)0.235 and 0.069
Answer
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