If 5 mg of Zn(s) is electrochemically deposited in the Daniell cell, how much charge should be passed through the cell assuming that there are not any parasitic reactions in the electrolysis.
Answer: 14.8C
Ans :
Number of mol of Zn = mass / molar mass
= ( 5x 10-3 g) / ( 65.38 g/mol) = 7.65 x 10-5 mol
Each mol of Zinc requires twice the number of mol of electrons
so number of mol of electrons = 2 x 7.65 x 10-5 mol = 1.53 x 10-4 mol
Each mol of electrons require 96485 C of charge
So 1.53 x 10-4 mol electrons will require :
= 1.53 x 10-4 x 96485
= 14.8 C
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