Question

A current of 4.69 A is passed through a Sn(NO3)2 solution for 1.20 hours. How much tin is plated out of the solution?

Answer 1

Sn(NO3)2   ---- > Sn²⁺ + 2NO3^-

Sn²⁺ + 2e-   ----- > Sn

C = A * sec

C = 4.69 A * 4320 sec = 20260.8 C

96500 C charge is carried by 1 mole of electron so

20260.8 C charge will be carried out by 0.210 mole of electron

From the balanced equation we can say that

2 mole of electrons produces 1 mole of Sn so

0.210 mole of electorns will be produced by 0.105 mole of Sn

1 mole of Sn = 118.71 g

0.105 mole of Sn = 12.46 g

Therefore, 12.46 g of Sn will be plated out.