Applications of Electrolysis

Electrolysis is a very important and useful phenomenon. The phenomenon of electrolysis has wide range of applications. It is used in large number of industrial manufacturing processes.

Let us discuss some of the many applications of electrolysis

Determination of equivalent masses of elements:

  • According to second law of electrolysis when the same quantity of electronic current is passed through solutions of salts of two different cells, the amounts of the metals deposited on the cathodes of the two cells are proportional to their equivalent masses of the respective metals.

  • If the amounts of the metals deposited on the cathodes be WA and WB respectively, then 
    \frac{W_A}{W_B} =\frac{Equivalent\ Mass\ of\ A}{Equivalent\ Mass\ of\ B}

  • Knowing the equivalent mass of one metal, the equivalent mass of the other metal can be calculated from the above relationship.

  • The equivalent masses of those non-metals which are evolved at anodes can also be determined by this method.

Electrometallurgy:

Electrometallurgy is the process of extraction of metal from ore by electrolysis.

The metals like sodium, potassium, magnesium, calcium aluminum, etc., are obtained by electrolytes of fused electrolytes.

Fused electrolyte 

Metal isolated

NaCl + CaCl2 + KF   

Na

CaCl2 + CaF2

Ca

Al2O3 + cryolite

Al

MgCi2 (35%) + NaCl (50%) + CaCl2 (15%)

Mg

NaOH   

Na

KCl + CaCl2 

K

Manufacture of non-metals:

Non-metals like hydrogen, fluorine, chlorine are obtained by electrolysis.

Electro-refining of metals:

This is the process of refining the metal. i.e. removing impurity from metal by the use of electrolysis method.

The metals like copper, silver, gold, aluminum, tin, etc., are refined by electrolysis.

Manufacture of compounds:

Compounds like NaOH, KOH, Na2CO3 KCIO3, white lead, KMnO4, etc., are manufactured by electrolysis.

Electroplating:

The process of coating an inferior metal with a superior metal by electrolysis is known as electroplating.

The aims of electroplating are:

  • To prevent the inferior metal from corrosion.

  • To make it more attractive in appearance.

The object to be electroplated is made the cathode and block of the metal to be deposited is made the anode in an electrolytic bath containing a solution of a salt of the anodic metal. On passing electric current in the cell, the metal of the anode dissolves out and is deposited on the cathode-article in the form of a thin film. The following are the requirements for fine coating:

  • The surface of the article should be free from greasy matter and its oxide layer. The surface is cleaned with chromic acid or detergents.

  • The surface of the article should be rough so that the metal deposited sticks permanently.

  • The concentration of the electrolyte should be so adjusted as to get smooth coating.

  • Current density must be the same throughout.

Refer to the following video for electroplating

For electroplating

Anode

Cathode

Electrolyte

With copper

With silver

With nickel

With gold

With zinc

With thin

Cu

Ag

Ni

Au

Zn

Sn

Object

Object

Object

Object

Iron objects

Iron objects

CuSo4 + dilute H2So4

KAg(CN)2

Nickel ammonium sulphate

KAu(CN)2

ZnSO4

SnSO4

Thickness of coated layer

 Let the dimensions of metal sheet to be coated be (a cm × b cm).

Thickness of coated layer = c cm

Volume of coated layer = (a × b × c) cm3

Mass of the deposited substance = Volume × density =   (a × b × c) × d g

\Rightarrow(a × b × c) × d = (I×t×E)/96500

Using above relation we may calculate the thickness of coated layer.

Note:    

Sometimes radius of atom of deposited metal is given instead of density, e.g.,

Radius of silver atom           = 10-8 cm

Atomic mass of Ag             = 108

Mass of single silver atom    = 108/(6.023× 1023 ) g

Volume of single atom         = 4/3× πR = 4/3×3.14×(10-8)3 cm3

Density of Ag  =  (Mass of single atom )/(Volume of single atom) 

= (108/6.023 × 1023)/(4/3×3.14×10-8 )3 

Current efficiency

Sometimes the ammeter shows false current due to mechanical fault. In this case,

% Current efficiency =  (Actual current)/(Ammeter current)×100 

Question 1:

Which of the following elements is not obtained by electrolysis?

a. Hydrogen

b. Fluorine

c. Copper

d. Chlorine

Question 2: 

Which of the following metals is not refined by electrolysis?

a. Gold

b. Silver

c. Copper

d. Iron

Question 3: 

The process of coating an inferior metal with a superior metal  is known as

a. electroplating 

b. electrolysis

c. electrorefining

d. electrophoresis

Question 4:  

Which of the following compounds is not manufactured by electrolysis.?

ICompounds like NaOH, KOH, Na2CO3 KCIO3, white lead, KMnO4, etc., are 

a. NaOH

b.KOH

c.Na2CO3

d. HCl

Q.1 Q.2 Q.3 Q.4
c d a d

Related Resources:- 

To know more about the study material of engineering and medical exams, please fill up the form given below: 

Name
Email Id
Mobile

Exam
Target Year

Related Resources
Concentration Cells

Concentration Cells The cells in which EMF arises...

Molar Conductivity

Electrolytic Conductance The conductance is the...

Commercial Production of Chemicals

Commercial Production of Chemicals As we discussed...

Arrhenius Theory of Electrolytic Dissociation

Arrhenius Theory of Electrolytic dissociation In...

Nernst Equation

Electrode and Cell Potentials EMF of A Galvanic...

Electrode Potential

Electrode Potential What is electrode potential?...

Electrochemical Series

Electrochemical Series By measuring the potentials...

Faradays Laws of Electrolysis

Faraday’s Laws of Electrolysis The...

Daniell Cell

Daniell Cell It is designed to make use of the...

Solved Examples On Electrochemistry

Solved Examples on Electrochemistry Example 1....

Electrolysis and Electrolytic Cell

Electrolysis and Electrochemical Cells...

KOHLRAUSCH S LAW

Kohlrausch’s law Kohlrausch’s law...

Batteries

Batteries Any cell or Battery (more than one cells...