A solution of a salt of a metal was electrolysed for ` 150 ` minutes with a current of ` 0 . 15` amperes. The weight fo metal deposted was `0. 783 g`. The equivalent weight to the metal is .

A solution of a salt of metal was electrolysed for 150 minutes with a current of 0.15 amperes. The mass of the metal deposited at the cathode is 0.783g. Calculate the equivalent mass of the metal.

A solution of a salt of metal was electrolysed for 15 minutes with a current of 0.15 amperes. The mass of the metal deposited at the cathode is 0.783 g. Calculate the equivalent mass of the metal.

The solution of a salt of a metal of atomic mass 112 was electrolysed for 15 minutes with a current of 1.5 ampere. The mass of the metal deposited was 0.788 g. Find 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 :