In an electrochemical cell, Ag+ ions in AgNO3 are reduced to Ag metal at the cathode and Cu is oxidized to Cu2+ 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 C mol−1, Atomic Weight of Ag = 107.9, Atomic Weight of Cu = 63.55]

In an electrochemical cell, Ag+ ions in AgNO3 are reduced to Ag metal

1.	In an electrochemical cell, Ag+ ions in AgNO3 are reduced to Ag metal at the cathode and Cu is oxidized to Cu2+ 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 C mol−1, Atomic Weight of Ag = 107.9, Atomic Weight of Cu = 63.55]
A.	0.469 and 0.138
B.	0.235 and 0.138
C.	0.469 and 0.069
D.	0.235 and 0.069
Answer» B. 0.235 and 0.138