Faraday's law of electrolysis states that the amount of substance produced in an electrolysis reaction is proportional to the quantity of charge passed through the electrolyte.
Electrolysis: An overview of what electrolysis is, and how it works, including the different types of electrolytes, half-cell reactions, and electrolytic cells.
Faraday's Law: A detailed explanation of Faraday's Law, including a derivation of its equation, and its relationship to the amount of electric charge and the molar mass of the substance being electrolyzed.
Electrochemical Cells: A description of electrochemical cells, including the differences between galvanic or voltaic cells and electrolytic cells, and how they are represented in schematic diagrams.
Electrolytic Reactions: An introduction to the concept of electrolytic reactions, which are chemical reactions that occur as a result of the movement of electrons, protons, or ions in an electrolytic cell.
Electrolyte Solutions: The properties of electrolyte solutions, including their electrical conductivity, pH, and ionization, and how these properties are related to Faraday's Law.
Stoichiometry of Electrolysis: An introduction to the stoichiometry of electrolysis, including the Faraday constant, which is a conversion factor used to relate the amount of electric charge passed through a cell to the molar mass of the substance being electrolyzed.
Electrolysis Applications: An overview of some important applications of electrolysis, including the production of metals, extraction of nonmetals, electroplating, and the electrolysis of water.
Factors Affecting Electrolysis: An explanation of the various factors that can affect the rate and efficiency of electrolysis, such as the concentration of the electrolyte, temperature, and current density.
Faraday's Law in Industry: Examples of how Faraday's Law is used in various industrial applications to monitor and control electrochemical processes, such as the production of aluminum, copper, and zinc.
Electrolysis Theory: An in-depth examination of some of the theoretical concepts related to faraday's law, such as Nernst equation, Le Chatelier's principle, and Butler-Volmer equation, and how they are applied in real-world electrochemical cells.
First law of electrolysis: Also known as Faraday's law of electrolysis, states that the amount of chemical change caused by an electric current is directly proportional to the amount of electricity that passes through it. This law applies to both electrolytic and electrochemical reactions.
Second law of electrolysis: Also known as Faraday's law of induction, states that an electric current is induced in a conductor when it is subjected to a changing magnetic field. This law is the basis for the operation of transformers and electrical generators, and it is essential in understanding the behavior of electromechanical systems.
Third law of electrolysis: Essentially states that the equivalent weight of any given element or radical is proportional to its valence or its combining power. Faraday's third law is useful in calculating the values of Faraday's first and second laws, as well as in specifying the amount of chemical change that will occur during an electrochemical reaction.