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 $\mathrm{C\,mol^{-1}}$, Atomic Weight of Ag = 107.9, Atomic Weight of 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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