Electrochemistry
Electrochemical systems use electrodes and an ion-conducting electrolyte to convert chemical and electrical energy.
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Electrochemistry, Electrolytes and Ohm's Law
Electrochemical systems use electrodes and an ion-conducting electrolyte to convert chemical and electrical energy.
Open article →Resistance, Conductivity and Molar Conductivity
Resistance depends on cell geometry; conductivity characterises the solution; molar and equivalent conductivity scale it to amount.
Open article →Measuring Conductivity, Dilution and Kohlrausch's Law
An AC bridge and KCl calibration measure conductivity; dilution and ionic contributions explain limiting molar conductivity.
Open article →Galvanic, Electrolytic and Daniell Cells
Galvanic cells produce current from a spontaneous reaction; electrolytic cells consume current; the Daniell cell shows separated half-reactions.
Open article →Cell EMF and the Standard Hydrogen Electrode
Cell potential is electrical energy per charge; SHE gives the reference for electrode potentials.
Open article →Cell Thermodynamics, Equilibrium and Nernst Equation
Electron transfer links cell potential to Gibbs energy, equilibrium constant and non-standard composition.
Open article →Electrolysis and Faraday's Laws
An electrolytic cell drives a non-spontaneous reaction; deposited mass follows charge and electrochemical equivalent.
Open article →Primary, Lead-Acid and Lithium-Ion Batteries
Dry and button cells are primary; lead storage and lithium-ion systems are rechargeable.
Open article →Fuel Cells, Corrosion and Protection
A fuel cell continuously converts supplied reactants to electricity; wet iron forms tiny galvanic regions that cause corrosion.
Open article →Electrochemical Series and Applications
The electrochemical series ranks reduction tendency and supports cell prediction, batteries, sensors and electrolysis.
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