Electrochemistry

This section outlines the key objectives of electrochemistry, highlighting its importance in energy conversion and chemical reactions.

Electrochemical Cells

Electrochemical cells convert chemical energy into electrical energy or vice versa, with galvanic and electrolytic cells playing key roles in energy conversion.

Daniell Cell And Its Functioning

This section introduces Daniell cells, a type of galvanic cell that converts chemical energy into electrical energy through redox reactions.

Galvanic Cells

Galvanic cells are electrochemical cells that convert chemical energy from spontaneous reactions into electrical energy.

Measurement Of Electrode Potential

This section discusses the principles and methods for measuring electrode potentials in electrochemical cells, highlighting the significance of these measurements in understanding redox reactions and calculating cell voltages.

Nernst Equation

The Nernst Equation describes the relationship between the cell potential of an electrochemical cell and the concentrations of its constituents.

Equilibrium Constant From Nernst Equation

The section discusses the principles of electrochemical cells, focusing particularly on equilibrium constants and their relationships to cell potentials.

Electrochemical Cell And Gibbs Energy Of The Reaction

This section describes the functioning of electrochemical cells, including galvanic and electrolytic cells, relationships between Gibbs energy and cell potential, and concepts of conductivity.

Conductance Of Electrolytic Solutions

This section discusses the principles of conductance and resistivity, including the definitions and relationships between electrical resistance, conductivity, and molar conductivity.

Measurement Of The Conductivity Of Ionic Solutions

This section discusses the measurement of the conductivity of ionic solutions, highlighting the significance of conductivity cells and the effect of concentration on conductivity.

Variation Of Conductivity And Molar Conductivity With Concentration

This section discusses how conductivity and molar conductivity of electrolytic solutions change with concentration.

Electrolytic Cells And Electrolysis

Electrolytic cells use electrical energy to drive non-spontaneous chemical reactions, while electrolysis involves the decomposition of compounds due to electric current.

Products Of Electrolysis

The products of electrolysis depend on the materials being electrolyzed and the type of electrodes used, influencing the electrochemical reactions that occur.

Batteries

This section discusses batteries, their types, construction, operation, and significance in converting chemical energy to electrical energy.

Primary Batteries

Primary batteries are galvanic cells that convert chemical energy into electrical energy through spontaneous redox reactions, and are designed for single-use applications.

Secondary Batteries

Secondary batteries are rechargeable electrochemical cells that can be reused multiple times, differing from primary batteries, which are non-rechargeable.

Fuel Cells

Fuel cells convert the chemical energy from fuels like hydrogen directly into electricity with high efficiency and low environmental impact.

Corrosion

Corrosion is an electrochemical process in which metals, primarily iron, are oxidized, resulting in damage to structures and objects.

Summary

This section showcases the fundamental concepts of electrochemical cells, including galvanic and electrolytic cells, along with key equations and definitions related to electrochemistry, conductivity, and electrolysis.

Exercises

This section covers a series of exercises aimed at reinforcing the fundamental concepts of electrochemistry, including calculations involving galvanic and electrolytic cells.