Electrolysis

We use Faraday's law of electrolysis, which is given by the formula:

m%20%3D%20%5Cfrac%7BM%20%5Ctimes%20I%20%5Ctimes%20t%7D%7Bn%20%5Ctimes%20F%7D

Where: -

m

= mass of copper deposited -

M%20%3D%2063.5%20%5C%2C%20%5Ctext%7Bgm%2Fmol%7D

= molar mass of copper -

I%20%3D%202%20%5C%2C%20%5Ctext%7BA%7D

= current -

t%20%3D%2030%20%5C%2C%20%5Ctext%7Bminutes%7D%20%3D%201800%20%5C%2C%20%5Ctext%7Bseconds%7D

n%20%3D%202

(because copper has a valency of 2 in the electrolyte) -

F%20%3D%2096500%20%5C%2C%20%5Ctext%7BC%2Fmol%7D

= Faraday's constant Substitute the values:

m%20%3D%20%5Cfrac%7B63.5%20%5Ctimes%202%20%5Ctimes%201800%7D%7B2%20%5Ctimes%2096500%7D%20%3D%20%5Cfrac%7B228600%7D%7B193000%7D%20%3D%200.2214%20%5C%2C%20%5Ctext%7Bgm%7D

Thus, the mass of copper deposited is 0.2214 gm.

Chapter Questions
1 MCQs