Electrochemistry

Electrochemistry examines the relationship between electricity and chemical reactions, particularly in converting chemical energy to electrical energy and vice versa.

Electrochemical Cells

This section introduces electrochemical cells, highlighting the differences between galvanic and electrolytic cells.

Types Of Electrochemical Cells

Electrochemical cells are classified into two main types: galvanic cells, which convert chemical energy into electrical energy, and electrolytic cells, which convert electrical energy into chemical energy.

Galvanic Cell (Voltaic Cell)

A galvanic cell converts chemical energy into electrical energy through spontaneous redox reactions.

Electrolytic Cell

An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction, playing a crucial role in various applications such as electroplating and electrolysis.

Redox Reactions And Electrode Potential

This section covers the concepts of redox reactions, electrode potential, and their significance in electrochemistry.

Redox Reactions

Redox reactions involve the transfer of electrons, where oxidation and reduction occur simultaneously, forming the foundation for electrochemical processes.

Electrode Potential

Electrode potential refers to the electric potential developed by an electrode in solution, crucial for understanding electrochemical reactions.

Standard Electrode Potential (E°)

Standard Electrode Potential (E°) measures the electrical potential of an electrode under standard conditions, with the Standard Hydrogen Electrode (SHE) as the reference.

Electrochemical Series

The electrochemical series is a list of elements organized by their standard reduction potentials, predicting the feasibility of redox reactions.

Representation Of An Electrochemical Cell

This section explains the standard notation for representing electrochemical cells, specifically galvanic cells, and highlights the function of the salt bridge.

Standard Notation For A Galvanic Cell

This section introduces the standard notation for representing a galvanic cell, including its components and function.

Salt Bridge

The salt bridge is crucial in electrochemical cells for maintaining electrical neutrality and completing the circuit.

Cell Emf And Gibbs Free Energy

This section discusses the relationship between electromotive force (EMF) in electrochemical cells and Gibbs free energy, essential for understanding energy changes in chemical reactions.

Emf (Electromotive Force)

EMF represents the potential difference between two half-cells in an electrochemical cell.

Relation Between Emf And Gibbs Free Energy

This section explores the relationship between electromotive force (EMF) and Gibbs free energy, highlighting how these concepts are interconnected in electrochemical reactions.

Nernst Equation

The Nernst Equation calculates the electrode potential of a redox reaction under non-standard conditions.

Conductance Of Electrolytic Solutions

This section discusses the concepts of conductance in electrolytic solutions, including types of conductance and the behavior of electrolytes under varying conditions.

Types Of Conductance

This section describes the different types of conductance in electrolytic solutions, including conductance, specific conductance, and molar conductance.

Variation Of Conductance

This section explains the variation in conductance of electrolytic solutions, emphasizing how strong and weak electrolytes behave differently with dilution.

Kohlrausch’s Law

Kohlrausch's Law states that the molar conductivity of an electrolyte at infinite dilution is equal to the sum of the contributions of its individual ions.

Electrolysis And Faraday’s Laws

Electrolysis involves breaking down substances using electricity, as explained by Faraday's Laws, which relate the mass of substances to the charge passed through an electrolyte.

Electrolysis

Electrolysis is a process where electrical energy is used to induce a chemical change, particularly the decomposition of substances.

Faraday’s First Law

Faraday's First Law states that the mass of a substance deposited during electrolysis is directly proportional to the charge passed.

Faraday’s Second Law

Faraday's Second Law states that the mass of a substance deposited during electrolysis is proportional to its equivalent weight and the charge passed.

Batteries And Fuel Cells

This section covers the types of batteries and fuel cells, explaining their workings, differences, and practical applications.

Primary Batteries

Primary batteries are non-rechargeable power sources that convert chemical energy into electrical energy through spontaneous redox reactions.

Secondary Batteries

This section discusses secondary batteries, their rechargeable nature, and examples.

Fuel Cells

Fuel cells convert the chemical energy of fuels directly into electricity, utilizing reactions between fuel and oxidant such as hydrogen and oxygen.

Corrosion

Corrosion is the gradual destruction of metals through chemical or electrochemical reactions with their environment, primarily affecting iron.

Definition

Corrosion is the gradual deterioration of metals due to interactions with their environment, primarily through chemical or electrochemical reactions.

Electrochemical Theory Of Corrosion

This section describes the electrochemical theory of corrosion, focusing on the oxidation of iron and factors that accelerate rusting.

Prevention Of Corrosion

Corrosion prevention involves various techniques to mitigate the gradual destruction of metals due to chemical or electrochemical reactions with their environment.

Summary

This section provides a concise overview of the key concepts discussed in the chapter on electrochemistry, focusing on the interconversion of chemical and electrical energy.