A current o f1.5 A is passed through a silver voltameter for 35 minutes .The mass of silver deposited during electrolysis is 3.528 g Calculate the electrochmical equivalent of silver.

State and explain Faraday 's laws of electrolysis. A current of 6 amperes is passed through a solution of Ag NO_3 for 20 minutes. 8 gm of silver is deposited. Find out the electrochemical equivalent of silver.

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.

A currect of 0.2 A is passed throgh a silver voltameter for 3 hours and 20 minutes. Find the mass of silver liberated ECE of hydrogen =0.0000105 gC^(-1) ,chemical equivalent of hydrogen =1 and ECE and that for silver =108

State and explain Faraday 's laws of electrolysis. When a current of 6 ampere strength is passed through AgNO_3 solution for 10 minutes, 4 gms of silver is deposited. Find out the electrochemical equivalent of silver.

A current of 0.5 amperes was passed through a solution of silver nitrate for six min. Find the mass of silver deposited. (Atomic mass of Ag = 108 )

State and explain Faraday's laws of electrolysis. When a current of 24A strength is passed through AgNO_(3) solution for 10 min 16 grams of silver is deposited . Find out the electrochemical equivalent of silver.

One ampere current flows for one minute through a silver voltameter. It deposits 0.067 g of silver on the cathode. Calculate (i) the electrochemical equivalent of copper. (ii) how much charge will flow to deposited 108 g of silver ? (iii) how much charge is carried by a silver ion ? ( Avagadro's number, N =6.024xx10^(23) ).