Electric current is passed through two cells 'A' and 'B' in series. Cell 'A' contains an aqueous solution of `Ag_(2)SO_(4)` and platinum electrodes. The cell 'B' contains aqueous solution of `CuSO_(4)` and Cu electrodes. The current is passed till 1.6 g of oxygen is liberated at the anode of cell 'A'.
(i) Give equations for the reaction taking place at each electrode.
(ii) Calculate the quantities of substances deposited at the cathodes of the two cells. (Ag= 108, Cu = 63.5)

Explanation

`{{:(,(i),"In cell .A.,",2H_(2)O rarr O_(2)(g) + 4H^(+)+4e,"at anode"),(,,,Ag^(+) + e rarr Ag,"at cathode"),(,,"In cell .B.,",Cu rarr Cu^(2+) + 2e,"at anode"),(,,,Cu^(2+) + 2e rarr Cu,"at anode"),(,(ii),"Ag = 21.6 g,",Cu = 6.35 g,):}}`