`10^(5)` coloumb charge liberated 1 gm silver (Ag). If now charge is doubled then the amount of liberated Ag will be :

A certain charge liberates 0.8 gm of O_(2) . The same charge will liberate how many gm of silver

Charge required to liberated 11.5 g sodium is .

(A) 1 faraday = 96,500 coulomb. It is a charge of 1 mole electrons. (R) 1 faraday charge liberates one gram equivalent of substance at an electrode.

On passing 96500 coulomb of charge through a solution CuSO_(4) the amount of copper liberated is

When the electrolytis of silver sulphate was carried out by Pt electrodes. 1-6 g oxygen was liberated at the anode, the amount of silver deposited at cathode will be

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolyte cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly proportionation to the amount of charge passed through it. The mass of substance liberated at electrode is calculate using the following realation : m=(itE)/(96500) Here, E represent the equivalent mass and 96500 C is called the faraday constant. Faraday (96500 C) is the charge of 1 mole electron i.e., 6.023 xx 10^(23) electrons, it is used to liberate on gram equivalent of the substance. The passage of current liberates H_2 at cathode and Cl_2 at anode. The solution is