(a) A current of 1.50 amp was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of Ag deposited was 1.50 g. How long did the current flow ? (b) Write the reactions taking place at the anode and cathode in the above cell. (c) Give reactions taking place at the two electrodes if these are made up of Ag.

(a) A current of 1.50 amp was passed through an electrolytic cell cont

1.	(a) A current of 1.50 amp was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of Ag deposited was 1.50 g. How long did the current flow ? (b) Write the reactions taking place at the anode and cathode in the above cell. (c) Give reactions taking place at the two electrodes if these are made up of Ag.
Answer» Solution :(a) `I = 1.50 A, m = 1.50 g` ATOMIC MASS of Ag = 108 Eq. of mass of Ag = 108 108 g silver is deposited by = 96500 C 1.5 g silver is deposited by `=96500/108 xx 1.5 = 1340.28` C Quantity of electricity Q = `l xx t` or `t = Q/l` SUBSTITUTING the values, we get `t = (1340.28)/1.5 = 893.52 s` (b) At cathode: `Ag^(+) + e^(-) to Ag(s)` At anode: `2H_(2)O to 4H^(+) + O_(2) + 4e^(-)` ( c) At anode: `Ag^(+) + e^(-) to Ag(s)` At anode: `Ag to Ag^(+) + e^(-)`