A current of 0.5 ampere when passed through `AgNO_(3)` solution for 193 sec. deposited 0.108 g of Ag. Find the equivalent weight of Ag.

A current 0.5 ampere when passed through AgNO_(3) solution for 193 sec. Deposited 0.108 g of Ag. Find the equivalent weight of Ag.

A current 0.5 ampere when passed through AgNO_(3) solution for 193 sec. Deposited 0.108 g of Ag. Find the equivalent weight of Ag.

A current of 0.5 ampere when passed through AgNO_(3) solution for 193 seconds deposited 0.108 g. of silver. The equivalent weight of Ag is

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

A current of 4 amper is passed through AgNO_3 solution for 30 min, which deposits 7 gm of silver. Find the current efficiency. (Ag = 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.

Assertion (A): A current of 96.5 amperes is passed into aquesous AgNO_(3) solution for 100 seconds. The weight of silver deposited is 10.8g (At.wt. of Ag=108). Reason (R): The mass of a substance deposited during the electrolysis of an electrolyte is inveresly propotional to the quantity passing through the electrolyte.

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 )