Find the amount of silver liberated at the cathode if `0.5` A of current is passed through `AgNO_(3)` electrolyte for 1 hour . Atomic mass of silver = `107.9 g mol^(-1)`.

Find the amount of silver liberated at cathode if 0.500 A of current is passed through AgNO_3 electrolyte for 1 hour. Atomic weight of silver s 107.9 g mol^(-1)

(a) Electroplating unit plates 3.0g of silver on a brass plate in 3.0min. Find the current used by the unit. The electrochemical equivalent of silver is 1.12xx10^(-6)kg//C . (b) Find the amount of silver liberated at cathode if 0.05A of current is passed through AgNO_(3) electrolyte for 1hr . Atomic weight of silver is 108g//"mole" .

The amount of substance liberated when 1 ampere of current is passed for 1 second through an electrolytic solution is called ………………… .

What will be the weight of silver deposited, if 96.5 A of current is passed into aqueous solution of AgNO_(3) for 100 s?

the Amonut of Ag (atomic mass =108) deposited at the cathode when a current of 0. amp is passed through a solution of Ag CO_(3) for 1 hour is closest to

(a) Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO_(3) for 15 minutes (Given : Molar mass of Ag = 108 g mol^(-1) 1F = 96500 C mol^(-1) ) (b) Define fuel cell

A curent of 0.5 A when passed through AgNO_(3) solution for 193 s deposited 0.108 h Ag. The equivalent weight of silver is

The amount of silver deposited by passing 241. 25 C of current through silver nitrated solution is .