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 1.50A 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 1.5 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?

A current of 2 ampere was passed through solution of CuSO_4 and AgNO_3 in series. 0.635 g of copper was deposited .Then the weight of silver deposited will be:

A current of 2 ampere was passed through solutions of CuSO_4 and AgNO_3 in series. 0.635 g of copper was deposited. Then the weight of silver deposited will be-