Chapter Overview
The chapter ‘Electrochemistry’ explores the relationship between electricity and chemical reactions. It introduces concepts of redox reactions, electrochemical cells (galvanic and electrolytic), and standard electrode potentials. The chapter explains the Nernst equation, electrochemical series, conductance of electrolytic solutions, and factors affecting conductivity. It also discusses electrolysis, Faraday’s laws, and the working of batteries and fuel cells. Applications in real-life industries like electroplating, purification of metals, and commercial batteries are also covered.
Important Keywords
- Electrochemistry: Study of the relationship between chemical changes and electric current.
- Redox Reaction: Reaction involving transfer of electrons between two species.
- Electrochemical Cell: Device that converts chemical energy into electrical energy.
- Galvanic Cell: Spontaneous redox cell producing electricity (e.g., Daniel cell).
- Electrolytic Cell: Uses electrical energy to drive non-spontaneous chemical reaction.
- Electrode Potential: Potential developed at electrode due to redox equilibrium.
- Standard Electrode Potential (E°): Electrode potential measured under standard conditions.
- Nernst Equation: Relates cell potential to standard potential and concentrations.
- Electrochemical Series: Arrangement of elements by their standard reduction potentials.
- Conductance: Reciprocal of resistance, used to measure ionic movement.
- Faraday’s Laws: Laws governing quantitative aspects of electrolysis.
Detailed Notes
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