When a steady current of 2A was passed through two electrolytic cells A and B containing electrolytes ZnSO_{4} and CuSO_{4} connected in series,2\; g of Cu were deposited at the cathode of cell B. How long did the current flow ? What mass of Zn was deposited at cathode of cell A ?
[Atomic mass :Cu=63.5gmol^{-1},\; Zn=65gmol^{-1};\; 1F=96500\; C\; mol^{-1}]

 

 
 
 
 
 

Answers (1)
S safeer

Given- 

current = 2A

Cu deposited = 2 g

Cu=63.5gmol^{-1},\; Zn=65gmol^{-1};\; 1F=96500\; C\; mol^{-1}

m=ZxIxt

2 = 63.5 x 2 x t/2x96500

t = 3039.4 s

m1/m2 = eq wt 1/eq wt 2

2 / m2 = (63.5/2) / (65/2)

Hence, m2 = 2.05 g

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