How many seconds will it take to plate 6.46 g of silver metal from a solution of Ag+ using a current of 18.4 amps in an electrolyte cell?

Question

1 A = 1 C/s

and

F = 96,485 C/mol

Answer 1

Convert 6.46 g Ag to mols:

6.46 g Ag x 1 mol / 108 g = 0.0598 mols Ag

Find moles of electrons:

Ag⁺ + 1e- ==> Ag(s)

0.0598 mols Ag = 0.0598 mols electrons

Find number of coulombs:

0.0598 mols e- x 96,485 C /mol = 5771 C

Find number of seconds:

5771 C x 1 sec / 18.4 C = 314 sec