[" 3) A current of "1.50A" was passed through an elec- "],[" trolytic cell containing "AgNO" ,solution with inert "],[" electrodes.The mass of silver deposited in cath- "],[" ode was "1.50g" .How long did the current flow? "],[" (Atomic mass of "Ag=108u,IF=96500C" ).( "" मिछि। "]

A current of 1.50A was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The mass of silver deposited to cathode was 1.50g. How long did the current flow? (atomic mass of Ag = 108u, 1F = 96500C).

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 1.50g . How long did the current flow ? (Molar mass of Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1) ).

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 1.50g . How long did the current flow ? (Molar mass of Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1) ).

A current of 1.50 was passed through on electrolyte solution containing AgNO_3 solution with inert electrodes. The weight of Ag deposited was 1.50g . How long did the current flow?

(a) Current of 1.5 ampere was passed through an electrolyte containing AgNO_(3) solution with inert electrodes. The weight of silver deposited was 1.5 g. How long did the current flow ? (b) Write the reactions taking place at anode and at cathode in the above cell. (c ) Give the reactions taking place at the two electrodes if they are made up of silver.

How much time is required for 1.5 g Ag to deposit when 1.50 A current is passed through an electrolytic cell containing AgNO_(3) solution with inert electrodes?