A silver cup is plated with silver by passing 9650 coulombs of charge.The amount of Ag deposited is

A silver cup is plated with silver by passing 965 C of electricity. The amount of Ag deposited is

When a metal is electroplated with silver (Ag)

One litre of 0.5 M KCl is electrolysed by passing 9650 coulombs of electricity. The pH of resulting solution is

In an electroplating experiment, mg of silver is deposited when 4 A of current flows for 2 min. The amount of silver (in g) deposited by 6 A of current for 40 s will be

If 965 coulombs of electricity is passed through a metal cup dipped in silver(l) salt solution, in order to plate it with silver. Then the amount of silver deposited on its surface is (Given : the molar mass of Ag = 108 g mol^(-1), 1F = 96500 coulombs)

A current of 3 amperes was passed through silver nitrate solution for 125 seconds. The amount of silver deposited at cathode was 0.42 g. Calculate the equivalent mass of silver.

An electric current of 0.4 A is passed through a silver voltameter fro half an hour.Find the amount of silver deposited on the cathode. ECE of silver = 1.12 xx 10^(-4) kg C^(-1)

When 9.65 coulomb of electricity is passed through a solution of silver nitrate (Atomic mass of Ag = 108 g mol^(-1) , the amount of silver deposited is :

The electrochemical equivalent of silver is 0.0011191 g. When an electric current of 0.5 ampere is passed through an aquesus silver nitrate solution of 200 sec, the amount fo silver deposited is:

An electrolytic cell contains a solution of Ag_(2)SO_(4) and have platinum electrodes. A current is passed until 1.6gm of O_(2) has been liberated at anode. The amount of silver deposited at cathode would be