Electrochemistry

Equivalent Conductance (^eq.)

It is defined as the conductance of that volume of solution which has one equivalent dissolved in it.

V = Volume of solution which has one equivalent in it.

N normality (Number of equivalents per liter or 1000cc)

Molar Conductivity (^m)

It is defined as the conductance of 1 cm³of volume of electrolyte which has one mole dissolved in it.

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	Introduction
	Conductors - Metallic and Electrolytic
	Types of Electrolytes
	Factors Influencing Electrolytic Conduction
	Basic Concepts
	Specific Conductance
	Equivalent Conductance
	Relation between Equivalent Conductivity and Specific Conductivity
	Variation of Molar Conductivity With Concentration
	Kohlrausch's Law
	Applications of Kohlrausch's Law
	Calculation of Degree of Dissociation - Degree of Dissociation [a]
	Calculation Of Dissociation Constant K
	Quantitative Aspect of Electrolysis
	Faraday's Laws Of Electrolysis
	Galvanic Cells (Voltaic Cell)
	Construction and Working of an Electrochemical Cell
	Electrode Potential
	Metal Electrodes
	Standard Electrode Potential
	Measurement of Electrode Potential
	Determination of Single Electrode Potential
	Cell Potential or EMF of a Cell
	Characteristics of Electrochemical Series
	Application of Electrochemical Series [ECS]
	Problems
	Standard Reduction Potentials at 298 K
	Calculation of Cell Potential
	Nernst Equation
	Nernst Equation for EMF of a Cell
	Equilibrium Constant From Nernst Equation
	Gibb's Free Energy and Cell Potential (EMF)
	Predicting Products of Electrolysis from Electrode Potential
	Cells - Primary, Secondary and Fuel Cells
	Primary Cells
	Mercury Cell
	Secondary Cell
	Fuel Cell
	Corrosion
	Manufacture of Caustic Soda (NaOH)
	Manufacture of Sodium Metal
	Manufacture of Aluminium
	Manufacture of Chlorine
	Summary
	Conclusion
Animations
	Motion of Free Electrons in a Wire
	Electrolytes
	To Verify Ohm's Law Experimentally

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