Electrochemistry Class 12 Handwritten Notes
Electrochemistry is the branch of chemistry that deals with the relationship between electrical energy and chemical changes. It involves redox (oxidation-reduction) reactions where electrons are transferred. This chapter covers:
- Electrochemical cells: Devices that convert chemical energy into electrical energy (e.g., galvanic/voltaic cells) and vice versa (e.g., electrolytic cells).
- Galvanic cells: Use spontaneous redox reactions to produce electricity.
- Electrode potential: Measured as standard electrode potential under standard conditions.
- Nernst equation: Used to calculate electrode potential under non-standard conditions.
- Electrolysis: The process of driving non-spontaneous reactions using electricity.
- Conductance: The ability of a solution to conduct electricity, dependent on ion concentration.
- Kohlrausch’s law: Helps in calculating the limiting molar conductivity of electrolytes
Electrochemistry Class 12 Handwritten Notes pdf
Electrochemistry Formulas Class 12 – Complete List with Equations & Short Notes
Electrochemistry Class 12 Handwritten Notes
1. Electrode Potential (E)
- Standard Electrode Potential:
E0= standard electrode potential at 25°C, 1 atm, 1 M
2. Nernst Equation
For a general reaction:
aA + bB → cC + dD
- n: number of electrons transferred
- Use natural log (ln) with 2.303 RT/nF if needed
- Derivation of Nernst equation
3. Gibbs Free Energy and Cell Potential
- ΔG: Gibbs free energy
- F: Faraday’s constant (96,500 C/mol)
- n: number of electrons
4. Kohlrausch’s Law (Limiting Molar Conductivity)
5. Conductance and Resistance
- G: Conductance (S or ℧)
- R: Resistance (Ω)
- ρ: Resistivity
- l: length of conductor
- A: cross-sectional area
6. Relation ship between Cell constant ,conductance and conductivity
7. Conductivity
8. Molar Conductivity
- κ: conductivity (S/cm)
- C: concentration (mol/L)
9.Faraday’s Laws of Electrolysis
melc.: mass deposited
Z: electrochemical equivalent
I: current (A)
t: time (s)
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