Question

Silver can be plated out of a solution containing Ag+ according to the half-reaction

Ag+(aq)+e−→Ag(s)

How much time (in minutes) does it take to plate 12 g of silver using a current of 4.4 A ?

Answer 1

40.7 minutes

Explanation

Ag⁺(aq) + e ------> Ag(s)

To deposite 1mole of Ag ,1 mole of electrons reauired

required mass of Ag = 12g

molar mass of Ag = 107.868g/mol

no of moles of Ag to be deposited = 12g/107.868g/mol = 0.11125mol

no of moles of electrons required = 0.11125mol

Faraday constant = 96485C/mol

No of coloumbs required = 0.11125mol × 96485C/mol = 10734 C

Current = 4.4A

1A = 1Coulombs per second

4.4A = 4.4Coulombs per second

Time required to deposit 12g Ag = 10734C/4.4C/s = 2439.5 s = 40.7minutes