Electrochemistry
Class 12 Chemistry · Chemistry Part I · Chapter 2
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History
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Summary
Electrochemistry studies the relationship between chemical energy and electrical energy. In a galvanic (voltaic) cell a spontaneous redox reaction produces electricity; oxidation occurs at the anode and reduction at the cathode. Each electrode has a standard electrode potential, measured against the standard hydrogen electrode (assigned zero), and the standard cell potential is \(E^{\circ}_{cell}=E^{\circ}_{cathode}-E^{\circ}_{anode}\). The Nernst equation gives the potential under non-standard conditions, \(E=E^{\circ}-\dfrac{RT}{nF}\ln Q\), and at equilibrium relates to the equilibrium constant and to free energy through \(\Delta G^{\circ}=-nFE^{\circ}_{cell}\). Ionic conduction is described by conductivity and molar conductivity \(\Lambda_m\), which increases on dilution; for strong electrolytes it follows Debye-Huckel-Onsager behaviour and Kohlrausch's law of independent migration of ions lets us find limiting molar conductivities. Electrolysis uses electrical energy to drive non-spontaneous reactions, with the amounts deposited governed by Faraday's laws. Practical cells include the dry cell, mercury cell, lead storage battery, nickel-cadmium cell and fuel cells, while corrosion of iron is an electrochemical process that can be prevented by coating or sacrificial protection.
Galvanic cells and electrode potentialsStandard hydrogen electrode and EMF seriesNernst equation and equilibriumConductivity and molar conductivityKohlrausch's law and electrolysisBatteries, fuel cells and corrosion
Key terms
Galvanic cell
A device that converts the chemical energy of a spontaneous redox reaction into electrical energy.
Standard electrode potential
The potential of an electrode relative to the standard hydrogen electrode under standard conditions.
Nernst equation
Relates electrode or cell potential to concentration, \(E=E^{\circ}-\dfrac{RT}{nF}\ln Q\).
Molar conductivity
Conductance of all ions from one mole of electrolyte, \(\Lambda_m\), which rises on dilution.
Kohlrausch's law
Limiting molar conductivity is the sum of independent contributions of the cation and anion.
Faraday's laws
The mass of substance deposited at an electrode is proportional to the charge passed.
Extra questions & answers
Try one from this chapter
In a galvanic cell, oxidation occurs at the: