Have you ever wondered why metals corrode over time or how a battery powers your phone? What causes a chemical reaction to produce electricity? NCERT Class 12 Chemistry Chapter 2 Notes Electrochemistry answers all these questions that deal with the relationship between electrical energy and chemical reactions. It forms the basis that is going to help students understand complex topics. In our daily lives, we often use batteries in Smartphones and electric vehicles for their charging. This phenomenon is based on Electrochemistry. Many industries depend on Electrochemistry for the refining of metals, wastewater treatment, and impurity removal.
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The NCERT Notes for Class 12 will be helpful for a quick revision of topics. These Electrochemistry Class 12 NCERT notes are designed by our subject experts, which ensures the credibility of the content provided. It contains all the important formulas of electrochemistry. The galvanic cell converts the chemical energy of the spontaneous reaction into electrical energy. Electrochemical principles are widely used in energy storage systems like lead-acid batteries in vehicles, fuel cells, lithium-ion batteries in smartphones, etc. It becomes difficult and time-consuming for students to read the NCERT books point-to-point. So, to solve this problem, we are providing these NCERT notes that cover all the topics and concepts provided in the chapter in a very clear and comprehensive way. These Electrochemistry class 12 notes are also valuable resources for various competitive exams. Also, check the NCERT Solutions for all the chapters.
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Students can download the NCERT Class 12 Chapter 2 Electrochemistry notes pdf from the icon given below to make your learning simple and effective. These cover important topics like electrochemical cells, Nernst equation, and batteries, helping in quick revision and exam preparation.
These notes cover a brief outline of topics such as electrochemical cells, the Nernst equation, the Gibbs energy of cell reaction, conductivity, Kohlrausch law and its applications, electrolysis, etc. These Class 12 Electrochemistry notes are the best resource for quick revision, also they help build a clear understanding of fundamental principles and their real-life applications, such as batteries and corrosion. Detailed notes of the chapter on electrochemistry are given below.
Conductance:
Conductance is the measure of the ease with which current flows through a conductor.
The inverse of resistance, R, is called conductance, G:
G=1/R = A/ρl = κA/l (R= ρl/A)
Where R is resistance, l is length, A is an area of cross-section, ρ (rho) is resistivity, and κ(kappa) is conductivity.
Conductivity:
The inverse of resistivity is called conductivity. The SI units of conductivity are S m-1, but quite often, κ is expressed in S cm–1.
κ = 1/ρ
The conductivity of a material in S m–1 is its conductance when it is 1 m long and its area of cross-section is 1 m2. It may be noted that 1 S cm–1.
Molar conductivity:
Molar Conductivity is described as the conducting power produced by the ions by dissolving one mole of electrolyte in a solvent.
Molar conductivity =
Conductivity and molar conductivity-
m= κ×1000/M
Equivalent conductivity-
Equivalent conductivity is defined as the conductivity power of combining ions formed by the dissolution of an electrolyte of one gram equivalent in a solution.
e= κ×1000/Ceq
We know that accurate measurement of an unknown resistance can be performed on a Wheatstone bridge.
Wheatstone bridge:
It consists of two resistors, R1 and R3, a variable resistor, R2, and the unknown resistor, R4. The Wheatstone bridge is fed by an oscillator
Unknwon resistance
Once the cell constant and the resistance of the solution in the cell are determined, the conductivity of the solution is given by the equation:
Electrolytic conductance decreases with an increase in concentration or increases with an increase in dilution.
Molar conductivity increases with dilution:
The equation of Debye-Huckel-Onsager shows the variation of molar conductivity along with concentration for strong electrolytes.
For strong electrolytes: For strong electrolytes,
Variation of molar conductivity with concentration for weak electrolytes:
Molar conductivity of weak electrolytes cannot be found for weak electrolytes because the dissociation of weak electrolytes is much lower compared to strong electrolytes.
For weak electrolytes, molar conductivity at infinite dilution can be found using Kohlrausch law.
At any concentration c, if α is the degree of dissociation, then it can be approximated by the ratio of molar conductivity
α =
At infinite dilution when ions are completely dissociated, every ion makes its unique contribution to the molar conductivity of the electrolyte, irrespective of the nature of the other ion with which it is associated.
Applications of Kohlrausch's Law -
α =
solubility= κ×1000
Electrochemical cells are devices that convert chemical energy into electrical energy or vice versa through redox reactions. Students can also refer to NCERT Solutions for Class 12 Chapter 2 Electrochemistry to practise and solve questions from these topics effectively.
Converts the chemical energy of a spontaneous reaction into electrical energy.
Two half cells -
Cu+2 +2e-→Cu(s) (reduction half cell)
Zn(s)→Zn2++2e- (oxidation half cell)
Overall cell reaction-
Zn(s)+ Cu+2(aq)→ Zn2+(aq)+Cu(s)
The Potential difference between two electrodes of a Galvanic Cell is called cell potential.
Emf Of Cell is the potential difference between the anode and the cathode when no current is drawn through the cell.
Ecell= Eright-Eleft
Feasibility of a reaction-
Ecell= Eright-Eleft
Reduction Half-
Oxidation Half-
For the above reaction, the reaction is feasible if
Ecell=EAg+/Ag -ECu+2/Cu is positive.
-It is denoted by Pt(s)│H2(g)│H+(aq)
For reaction-
Mn+aq+ne-→Ms
E(Mn+│M) =EoM-RT/nF ln[{M(s)}/{Mn+(aq)}]
E(Mn+│M)=EoM-2.303RT/nFlog[{M(s)}/{Mn+(aq)}]
E(Mn+│M)=EoM-2.303×8.314×298n×96500 log[{M(s)}/{Mn+(aq)}]
E(Mn+│M) =EoM-0.059nlog[{M(s)}/{Mn+(aq)}]
Here [M(s)] is taken as zero
E(Mn+│M) =EoM-0.059nlog[1/{Mn+(aq)}]
E=E0-0.059nlog[1/{Mn+(aq)}] at 25⁰C
Equilibrium Constant from Nernst Equation:
For a chemical reaction-
aA+bB→cC+dD
Ecell = E0cell - (RT/nF) ln(Q)
This is the Nernst equation at 298 K, where:
-
-
-
-
-
Using the Nernst Equation, the concentration of the unknown species can be found.
At equilibrium, the Nernst equation takes the form of –
E⁰cell=2.303 (RT/nF)log(K)
Electrochemical Cell and Gibbs Energy of the Reaction:
∆rG=-nFEcell
This equation can help to predict the feasibility of the reaction.
Electrolysis- The process in which chemical changes take place due to the passage of current.
There are two Faraday’s Laws Of Electrolysis, Faraday’s first law of electrolysis says that the quantity of substance deposited at the electrode is in direct proportion to the amount the electricity passed through the solution.
where w is the gram of substance deposited on passing Q coulombs of electricity if a current of 1 ampere is passed for t seconds.
Faraday’s second law of electrolysis- It says that when an equal amount of electricity is passed through different solutions lined up in series, the mass of the substance deposited at the electrodes is in direct proportion to the equivalent weight. Students can also download these NCERT Class 12 Chapter 2 Electrochemistry notes pdf to study offline anytime and anywhere.
Weight of Cu deposited = Weight of Ag deposited
= Eq. wt. of Cu = Eq. wt. of Ag
Reactions occurring at the electrode are-
Anode
Zn→Zn+2+2e-
Cathode
2NH4+(aq) + 2MnO2+2e-→Zn+2 + 2MnOOH+2NH3
Overall-
Zn+2NH4+ (aq) + 2MnO2 + Zn+2 + 2MnOOH+2NH3
-Found in electrical circuits.
-Reactions occurring at the electrodes are-
Anode-
ZnHg+2OH-→ZnOs+H2O+2e-
Cathode-
HgO(s)+ H2O+2e-→Hgl+2OH-
Overall-
ZnHg+ HgO(s)→ ZnO(s)+2OH-
-Battery used in automobiles.
-Reactions taking place at electrodes-
Anode-
Pbs+SO42-(aq)→PbSO4(s)+ 2e-
Cathode-
PbO2(s)+SO42-(aq)+ 4H+ (aq)+ 2e-→PbSO4+2H2O
Overall-
Pb+ PbO2+2H2SO4(aq)→ 2PbSO4+ 2H2O
2. Nickel-cadmium storage cell-
-Has a longer life than the lead storage battery.
-Reactions occurring at electrodes-
Anode-
Cd+2OH-→CdO + H2O+2e-
Cathode−
2Ni(OH)3 + 2e-→2Ni(OH)2+2OH-(aq)
Overall-
Cd+2Ni(OH)3→CdO+2Ni(OH)2(s) + H2O(l)
Fuel Cells-
Anode-
2[H2+2OH-(aq)→2H2O+2e-]
Cathode-
O2+2H2O + 4e-→4OH-(aq)
Overall-
2H2(g)+ O2→2H2O
-Deterioration of metal over time due to its reaction with air and water.
-Except gold, platinum, and palladium all other metals undergo corrosion.
Rusting of iron-
At anode-
[Fe→Fe2+(aq) + 2e-]×2
At cathode-
4H+ + O2 + 4e-→2H2O
Overall reaction-
2Fe + 4H+ + O2→2Fe+2(aq)+ 2H2O
Prevention of corrosion-
Given below previous years NCERT Chapter 2 Electrochemistry questions and answers to help you understand important concepts and exam trends. Practising these will improve your accuracy.
Question 1. Give reason: In the experimental determination of electrolytic conductance, Direct Current (DC) is not used.
Answer:
Direct Current (DC) is not used in the experimental determination of electrolytic conductance because it causes electrolysis and polarization at the electrodes.
Explanation:
1. Electrolysis occurs with DC:
Because DC causes continuous movement of ions in one direction, this leads to chemical changes at the electrodes, i.e., electrolysis, which interferes with accurate conductance measurement.
2. Polarization of electrodes:
3. AC prevents these issues:
DC is avoided because it causes electrolysis and electrode polarization, which interfere with the correct determination of electrolytic conductance. AC is used instead for accurate results.
Question 2. Define the following: Fuel cell
Answer:
A fuel cell is an electrochemical device that converts the chemical energy of a fuel, typically hydrogen, and an oxidizing agent, usually oxygen, directly into electricity through electrochemical reactions.
Unlike batteries, fuel cells can continuously generate electricity as long as they have a supply of fuel and oxidant. They are known for their efficiency and clean operation, producing only electricity, water, and heat when hydrogen is used as the fuel. Fuel cells are used in various applications, including transportation and stationary power generation.
Question 3. The electrical resistance of a column of 0.05 M NaOH solution of area
Answer:
We are given:
- Concentration of NaOH solution:
- Area of cross-section:
- Length of solution column:
- Resistance:
We are to calculate:
1. Resistivity (
2. Conductivity (
3. Molar conductivity (
1. Resistivity (
Resistivity is given by:
Substitute values:
2. Conductivity (
3. Molar conductivity (
Hence, the answer is resistivity is 100 ohm cm, conductivity is 0.01 Scm-1, and molar conductivity is (200 Scm2 mol-1).
Besides NCERT Class 12 Chemistry Chapter 2 Notes Electrochemistry students can follow the links given below for NCERT notes for each chapter of class 12:
NCERT exemplar solutions for each subject are given below:
NCERT solutions for every subject are given below:
Frequently Asked Questions (FAQs)
Class 12 NCERT Chemistry Chapter 2 Electrochemistry covers topics such as the concepts of electrolytes, electrolysis, and the relationship between electricity and chemical reactions, including Faraday's laws of electrolysis.
Electrochemistry is crucial because it helps us understand how chemical energy can be converted into electrical energy and vice versa. This principle is fundamental in batteries, fuel cells, and electrolysis processes, which have practical applications in various industries and technologies.
To effectively study Chapter 2, you can create concise notes from the textbook, solve numerical problems, and review diagrams related to electrochemical cells.
Faraday laws of electrolysis consist of two main laws, the first law states that the mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. The second law states that the mass of any element altered is proportional to its equivalent weight.
Electroplating is the process of depositing a thin layer of a metal, such as gold or silver, onto the surface of another metal using an electrochemical cell.
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