A current of 0.15 A passed through a salt solution for 150 minute depositing 0.783 g of the metal . If atomic mass of the metal is 112, then find valency of the metal.

When a current of 0.15 ampere is passsed through a solution of a salt of a metal for 150 minutes, 0.783 gm of the metal is deposited . Find the valency of the metal.(At. Wt. of metal = 112)

24125 coulomb electricity when passed through an electrolyte deposits 2.25 gm of the metal. If atomic mass of the metal is 27, find oxidation number of the metal ion.

Define electrochemical equivalent and chemical equivalent. How are they related with each other ? A current of 5 amperes is passed through an electrolyte for 15 minutes when 3 gms of the metal was deposited. Calculate the electrochemical equivalent of the metal.

State and explain Faraday's law of electrolysis. When a current of 1.5 amperes strength is passed through a solution of a salt of a metal ( atomic mass = 112 ) for 15 min , 0.783 g of the metal is deposited. Find out the valency of the metal.

A current of 9.65 ampere folwing for 10 minute depostits 3.0 g of a metal. The equivalent weight of the metal is :

A current of 0.5 A flowing for 30 min deposits 0.2964g of a metal at the cathode. Calculate the equivalent mass of the metal.