A current of 1.50 A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The weight of silver deposited was 1.50 g. How long did the current flow ? [Molar mass of `Ag = 108 g mol^(-1)`?, 1 F = `96500 C mol^(-1)`]

Explanation

Quantity of charge required to deposit 108 g Ag = 96500 C
Quantity of charge required to deposit 1.5 g Ag `=(96500)/108 xx 1.5 = 1340.28 C`
Time taken `=Q/l = (1340.28)/1.50 = 893.5s`