(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.

Explanation

(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^(-)`