Mediaspace scheduled maintenance: Aug 25, 2026 07:00 - 12:00 AM. During this time, videos will be temporarily unavailable. Check status updates.

Lecture

Chemical Equilibria and Reactivity

Description

This lecture covers the principles of chemical equilibria and reactivity, focusing on the variation of potential with pH in redox reactions, the corrosion of iron due to oxygen, protection against corrosion using different metals, titration methods, electrolysis, and Faraday's laws. It also explains the concept of electrolysis, the necessity of a higher voltage than the standard potential for non-spontaneous reactions, and the stoichiometry of products formed by an electric current.

Official source

Ontological neighbourhood

Chemistry

Physical chemistry: Electrochemistry

Related concepts (19)

Corrosion

Corrosion is a natural process that converts a refined metal into a more chemically stable oxide. It is the gradual deterioration of materials (usually a metal) by chemical or electrochemical reaction with their environment. Corrosion engineering is the field dedicated to controlling and preventing corrosion. In the most common use of the word, this means electrochemical oxidation of metal in reaction with an oxidant such as oxygen, hydrogen or hydroxide. Rusting, the formation of iron oxides, is a well-known example of electrochemical corrosion.

Faraday's laws of electrolysis

Faraday's laws of electrolysis are quantitative relationships based on the electrochemical research published by Michael Faraday in 1833. Michael Faraday reported that the mass (m) of elements deposited at an electrode is directly proportional to the charge (Q; SI units are ampere seconds or coulombs). Here, the constant of proportionality, Z, is called the electro-chemical equivalent (ECE) of the substance. Thus, the ECE can be defined as the mass of the substance deposited/liberated per unit charge.

Galvanic corrosion

Galvanic corrosion (also called bimetallic corrosion or dissimilar metal corrosion) is an electrochemical process in which one metal corrodes preferentially when it is in electrical contact with another, in the presence of an electrolyte. A similar galvanic reaction is exploited in primary cells to generate a useful electrical voltage to power portable devices. This phenomenon is named after Italian physician Luigi Galvani (1737-1798).

Corrosion inhibitor

In chemistry, a corrosion inhibitor or anti-corrosive is a chemical compound that, when added to a liquid or gas, decreases the corrosion rate of a material, typically a metal or an alloy, that comes into contact with the fluid. The effectiveness of a corrosion inhibitor depends on fluid composition, quantity of water, and flow regime. Corrosion inhibitors are common in industry, and also found in over-the-counter products, typically in spray form in combination with a lubricant and sometimes a penetrating oil.

Redox

Redox (ˈrɛdɒks , ˈriːdɒks , reduction–oxidation or oxidation–reduction) is a type of chemical reaction in which the oxidation states of substrate change. Oxidation is the loss of electrons or an increase in the oxidation state, while reduction is the gain of electrons or a decrease in the oxidation state. There are two classes of redox reactions: Electron-transfer – Only one (usually) electron flows from the atom being oxidized to the atom that is reduced. This type of redox reaction is often discussed in terms of redox couples and electrode potentials.

Related lectures (33)

Electrochemistry Fundamentals

Delves into concentration cells, solubility products, half-cell potentials, and practical electrochemistry applications, including electrolysis and corrosion prevention.

Corrosion and Protection

Explores the process of corrosion, methods of prevention, and its economic implications.

Electrochemistry: Redox Reactions and Cell Potentials

Covers redox reactions, cell potentials, and electrochemical cells in electrochemistry.

Redox Reactions: Balancing Equations and Corrosion

Covers redox equation balancing and corrosion principles.

Electrochemistry: Redox Reactions