Question

How many seconds are required to deposit 0.231 grams of tin metal from a solution that contains Sn²⁺ ions, if a current of 0.824 A is applied.

Answer 1

Electrolysis equation is:

Sn2+ + 2e- ------> Sn

1 mol of Sn requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Sn requires 192970 C

let us calculate mol of element deposited:

molar mass of Sn = 1.187*10^2 g/mol

use:

number of mol of Sn, n = mass of Sn/molar mass of Sn

= 0.231/1.187*10^2

= 1.946*10^-3 mol

total charge = mol of element deposited * charge required for 1 mol

= 1.946*10^-3*1.93*10^5

= 3.755*10^2 C

use:

time = Q/i

= 3.755*10^2/0.824

= 4.557*10^2 seconds

Answer: 4.56*10^2 seconds