510 marks

Electrochemistry and Redox reactions

This chapter deals with redox reactions, electrochemical cells, and their applications.

31 Topics

45h prep

3.3% subject weight

31 Topics

Electronic concepts of oxidation and reduction

2m1/10

📌 Key FormulaOxidation: loss of electrons, Reduction: gain of electrons.

Redox reactions

2m1/10

📌 Key FormulaSimultaneous oxidation and reduction.

Oxidation number

2m2/10

📌 Key FormulaRules for assigning oxidation numbers.

Rules for assigning oxidation number

2m2/10

📌 Key FormulaSet of rules.

Balancing of redox reactions

2m3/10

📌 Key FormulaIon-electron method (half-reaction method), oxidation number method.

Electrolytic and metallic conduction

2m1/10

📌 Key FormulaConduction in electrolytes vs metals.

Conductance in electrolytic solutions

2m2/10

📌 Key FormulaSpecific and molar conductance.

Molar conductivities and their variation with concentration

2m2/10

📌 Key FormulaΛ_m = κ/c, Λ_m increases with dilution.

Kohlrausch’s law and its applications

2m3/10

📌 Key FormulaΛ_m° = λ_c° + λ_a°, used to find Λ° for weak electrolytes, degree of dissociation.

Electrochemical cells

2m1/10

📌 Key FormulaGalvanic cells produce electricity, electrolytic cells use electricity.

Electrolytic and Galvanic cells

2m1/10

📌 Key FormulaDifferences.

Different types of electrodes

2m2/10

📌 Key FormulaStandard hydrogen electrode, calomel electrode, etc.

Electrode potentials including standard electrode potential

2m2/10

📌 Key FormulaE° values, electrochemical series.

Half - cell and cell reactions

2m2/10

📌 Key FormulaWriting cell notation and reactions.

emf of a Galvanic cell and its measurement

2m2/10

📌 Key FormulaE_cell = E_cathode - E_anode

Nernst equation and its applications

2m3/10

📌 Key FormulaE = E° - (RT/nF) ln Q

Relationship between cell potential and Gibbs' energy change

2m2/10

📌 Key FormulaΔG = -nFE

Dry cell and lead accumulator

2m1/10

📌 Key FormulaPrimary and secondary batteries.

Fuel cells

2m1/10

📌 Key FormulaConvert chemical energy to electrical energy, e.g., H₂-O₂ cell.

The first law of thermodynamics- Concept of work

2m2/10

📌 Key FormulaΔU = q + w (sign convention)

Hess’s law of constant heat summation

2m3/10

📌 Key FormulaΔH_reaction = Σ ΔH_products - Σ ΔH_reactants

The second law of thermodynamics

2m1/10

📌 Key FormulaSpontaneous processes, entropy increase.

Heat internal energy and enthalpy

2m2/10

📌 Key FormulaH = U + PV, ΔH = q_p

Entropy

2m2/10

📌 Key FormulaMeasure of disorder, ΔS = q_rev/T

Free energy

2m2/10

📌 Key FormulaG = H - TS, ΔG = ΔH - TΔS

Criterion of spontaneity

2m1/10

📌 Key FormulaΔG < 0 for spontaneous process.

Fusion

2m1/10

📌 Key FormulaMelting, enthalpy of fusion.

Vapourization

2m1/10

📌 Key FormulaVaporization, enthalpy of vaporization.

Heat of reaction

2m2/10

📌 Key FormulaEnthalpy change for reaction.

Pressure-volume work

2m2/10

📌 Key Formulaw = -PΔV (for constant pressure)

Work and heat

2m1/10

📌 Key FormulaForms of energy transfer.

510 marks

Electrochemistry and Redox reactions

This chapter deals with redox reactions, electrochemical cells, and their applications.

31 Topics

45h prep

3.3% subject weight

31 Topics

Electronic concepts of oxidation and reduction

2m1/10

📌 Key FormulaOxidation: loss of electrons, Reduction: gain of electrons.

Redox reactions

2m1/10

📌 Key FormulaSimultaneous oxidation and reduction.

Oxidation number

2m2/10

📌 Key FormulaRules for assigning oxidation numbers.

Rules for assigning oxidation number

2m2/10

📌 Key FormulaSet of rules.

Balancing of redox reactions

2m3/10

📌 Key FormulaIon-electron method (half-reaction method), oxidation number method.

Electrolytic and metallic conduction

2m1/10

📌 Key FormulaConduction in electrolytes vs metals.

Conductance in electrolytic solutions

2m2/10

📌 Key FormulaSpecific and molar conductance.

Molar conductivities and their variation with concentration

2m2/10

📌 Key FormulaΛ_m = κ/c, Λ_m increases with dilution.

Kohlrausch’s law and its applications

2m3/10

📌 Key FormulaΛ_m° = λ_c° + λ_a°, used to find Λ° for weak electrolytes, degree of dissociation.

Electrochemical cells

2m1/10

📌 Key FormulaGalvanic cells produce electricity, electrolytic cells use electricity.

Electrolytic and Galvanic cells

2m1/10

📌 Key FormulaDifferences.

Different types of electrodes

2m2/10

📌 Key FormulaStandard hydrogen electrode, calomel electrode, etc.

Electrode potentials including standard electrode potential

2m2/10

📌 Key FormulaE° values, electrochemical series.

Half - cell and cell reactions

2m2/10

📌 Key FormulaWriting cell notation and reactions.

emf of a Galvanic cell and its measurement

2m2/10

📌 Key FormulaE_cell = E_cathode - E_anode

Nernst equation and its applications

2m3/10

📌 Key FormulaE = E° - (RT/nF) ln Q

Relationship between cell potential and Gibbs' energy change

2m2/10

📌 Key FormulaΔG = -nFE

Dry cell and lead accumulator

2m1/10

📌 Key FormulaPrimary and secondary batteries.

Fuel cells

2m1/10

📌 Key FormulaConvert chemical energy to electrical energy, e.g., H₂-O₂ cell.

The first law of thermodynamics- Concept of work

2m2/10

📌 Key FormulaΔU = q + w (sign convention)

Hess’s law of constant heat summation

2m3/10

📌 Key FormulaΔH_reaction = Σ ΔH_products - Σ ΔH_reactants

The second law of thermodynamics

2m1/10

📌 Key FormulaSpontaneous processes, entropy increase.

Heat internal energy and enthalpy

2m2/10

📌 Key FormulaH = U + PV, ΔH = q_p

Entropy

2m2/10

📌 Key FormulaMeasure of disorder, ΔS = q_rev/T

Free energy

2m2/10

📌 Key FormulaG = H - TS, ΔG = ΔH - TΔS

Criterion of spontaneity

2m1/10

📌 Key FormulaΔG < 0 for spontaneous process.

Fusion

2m1/10

📌 Key FormulaMelting, enthalpy of fusion.

Vapourization

2m1/10

📌 Key FormulaVaporization, enthalpy of vaporization.

Heat of reaction

2m2/10

📌 Key FormulaEnthalpy change for reaction.

Pressure-volume work

2m2/10

📌 Key Formulaw = -PΔV (for constant pressure)

Work and heat

2m1/10

📌 Key FormulaForms of energy transfer.