Question

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.

Answer 1

I = 0.15 amperes 

t = 150 mins 

= t = 150 x 60sec 

= t = 9000sec 

Q = It 

= Q = 0.15 x 9000 coulombs 

= Q = 1350 coulombs 

Hence, 135 coulombs of electricity deposit is equal to 0.783g of metal.

96500 coulombs of electricity \(\frac{0.783\times96500}{1350}\) = 55.97 gm of metal 

Hence equivalent mass of the metal is 55.97

Answer 2

I = 0.15 amperes t = 150 mins = t = 150 x 60sec = t = 9000sec Q = It = Q = 0.15 x 9000 coulombs = Q = 1350 coulombs Hence, 135 coulombs of electricity deposit is equal to 0.783g of metal. 96500 coulombs of electricity 0.783×9650013500.783×965001350 = 55.97 gm of metal Hence equivalent mass of the metal is 55.97