CBSE Class 12 Chemistry Electrochemistry Notes Set E

Download CBSE Class 12 Chemistry Electrochemistry Notes Set E in PDF format. All Revision notes for Class 12 Chemistry have been designed as per the latest syllabus and updated chapters given in your textbook for Chemistry in Class 12. Our teachers have designed these concept notes for the benefit of Class 12 students. You should use these chapter wise notes for revision on daily basis. These study notes can also be used for learning each chapter and its important and difficult topics or revision just before your exams to help you get better scores in upcoming examinations, You can also use Printable notes for Class 12 Chemistry for faster revision of difficult topics and get higher rank. After reading these notes also refer to MCQ questions for Class 12 Chemistry given on studiestoday

Revision Notes for Class 12 Chemistry Unit 03 Electrochemistry

Class 12 Chemistry students should refer to the following concepts and notes for Unit 03 Electrochemistry in Class 12. These exam notes for Class 12 Chemistry will be very useful for upcoming class tests and examinations and help you to score good marks

Unit 03 Electrochemistry Notes Class 12 Chemistry

 

ELECTROCHEMISTRY CONCEPTS 

Electrochemistry may be defined as the branch of chemistry which deals with the quantitative study of interrelation ship between chemical energy and electrical energy and inter-conversion of one form into another.relationships between electrical energy taking place in redox reactions. 

A cell is of two types:- 

I. Galvanic Cell 

II. Electrolytic cell. 

In Galvanic cell the chemical energy of a spontaneous redox reaction is converted into electrical work. 

In Electrolytic cell electrical energy is used to carry out a non-spontaneous redox reaction. 

The Standard Electrode Potential for any electrode dipped in an appropriate solution is defined with respect to standard electrode potential of hydrogen electrode taken as zero. The standard potential of the cell can be obtained by taking the difference of the standard potentials of cathode and anode. 

E0cell = E0cathode-E0anode 

The standard potential of the cells are related of standard Gibbs energy.

ΔrG=-nFE0cell 

The standard potential of the cells is related to equilibrium constant. 

ΔrG= -RTink 

Concentration dependence of the potentials of the electrodes and the cells are given by Nernst equation.
aA+bB ne--→ cC + dD 

Nernst equation can be written as 

Ecell = E0 cell-RT/nF ln[C]c[D]d/[A]a[B]b 

The conductivity, K of an electrolytic solution depends on the concentration of the electrolyte, nature of solvent and temperature.
Molar Conductivity, Δm, is defined by K/C where C is the concentration in Mol L-1 ΔM= k*1000/m  

the unit of molar conductivity is Ω -1 cm2 mol-1. Conductivity decrease but molar conductivity increases with decrease in concentration. It increases slowly with decrease in concentration for strong electrolyte while the increase is very dilute solutions. 

Kohlrausch law of independent migration of ions. The law states that limiting conductivity of an electrolyte can be represented as the sum of the individual contribution to the anion and cation of the electrolyte. 

Faraday’s laws of Electrolysis 

I. The amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the quantity of electricity passed through the electrolyte. 

II. The amount of different substances liberated by the same quantity of electricity passing through the electrolytic solution is proportional to their chemical equivalent weights. 

Batteries and full cells are very useful forms of galvanic cells There are mainly two types of batteries. Corrosion of metals is an electrochemical phenomenon In corrosion metal is oxidized by loss of electrons to oxygen and  ormation of oxides.

Anode (Oxidation): 2Fe(s) →2Fe2+ + 4e- 

Cathode (Reduction): O2(g) + 4H+(aq) + 4e-→2H2

Atmospheric Oxidation: 2Fe2+(aq) + 2H2O(l) + 1/2O2(g)→Fe2O3(s) + 4H+(aq) 

QUESTION CARRING 1 MARK 

1. What is the effect of temperature on molar conductivity? 

Ans. Molar conductivity of an electrolyte increases with increase in temperature. 

2. Why is it not possible to measure single electrode potential? 

Ans. (It is not possible to measure single electrode potential because the half cell containing single electrode cannot exist independently, as charge cannot flow on its own in a single electrode.) 

3. Name the factor on which emf of a cell depends:- 

Ans. Emf of a cell depends on following factora. Nature of reactants. 

b. Concentration of solution in two half cells. 

c. Temperature 

d. Pressure of gas. 

4. What are the units of molar conductivity? 
( cm2 ohm-1 mol-1 or Scm2mol-1
 
5. Write Nernst equation – 
For the general cell reaction 
aA+bB→cC+dD 
Ans. Ecell = E0cell-RTln[C]c[[D]d/nF [A]a[B]b 
 
6. What is the EMF of the cell when the cell reaction attains equilibrium? 
Ans. Zero 
 
7. What is the electrolyte used in a dry cell? 
Ans. A paste of NH4Cl, MnO2 and C 
 
8. How is cell constant calculated from conductance values? 
Ans. Cell constant= specific conductance/ observed conductance. 
 
9. What flows in the internal circuit of a galvanic cell. 
Ans. Ions 
 
10. Define electrochemical series. 
Ans. The arrangement of various electrodes in the decreasing or increasing order of their standard reduction potentials is called electrochemical series. 

QUESTIONS CARRYING TWO MARKS 
 
1. How can you increase the reduction potential of an electrode.? 
For the reaction 
Mn+(aq) + ne-- → M (s) 
Ans. Nernst equation is: 
E0M n+ /M= EM n+ / M - 2.303RTlog 1/nF [Mn+
EM n+/M can be increased by 
 
a. increase in concentration of Mn+ ions in solution 
b. by increasing the temperature. 
 
 

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CBSE Class 12 Chemistry Unit 03 Electrochemistry Notes

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Notes for Chemistry CBSE Class 12 Unit 03 Electrochemistry

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Unit 03 Electrochemistry Notes for Chemistry CBSE Class 12

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Unit 03 Electrochemistry CBSE Class 12 Chemistry Notes

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Notes for CBSE Chemistry Class 12 Unit 03 Electrochemistry

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