Journal of Thermodynamics & Catalysis
Open Access

Evolution of the Oxidation Reaction and its Stability

Javad Samimi^{* *}Correspondence: Javad Samimi, Department of Chemistry, University of Shiraz, Shiraz, Iran, Email:

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Description

Chemical reactions are the essence of transformations that occur in our universe, playing a vital role in various natural and synthetic processes. Among these reactions, oxidation stands as a fundamental concept, driving numerous chemical transformations. Oxidation reactions involve the loss of electrons or an increase in oxidation state, often accompanied by the addition of oxygen or other electronegative elements. Understanding the principles underlying oxidation reactions is crucial in fields ranging from biology to industrial chemistry. Oxidation is a chemical process in which a substance loses electrons, leading to an increase in its oxidation state. This process commonly involves the transfer of electrons from one substance to another. A substance that undergoes oxidation is referred to as the reducing agent, as it facilitates the reduction of another substance by donating electrons. The component of oxidation, reduction, involves the gain of electrons and a decrease in oxidation state. Combustion reactions are perhaps the most familiar type of oxidation reactions. Typically involving oxygen as the oxidizing agent, these reactions produce heat and light as energy is released. For instance, the burning of hydrocarbons such as methane in the presence of oxygen leads to the formation of carbon dioxide and water, releasing energy in the process. Here, one substance loses electrons while another gains electrons. Common examples include the rusting of iron, where iron undergoes oxidation by reacting with oxygen and moisture to form iron oxide. Biological systems heavily rely on oxidation reactions to generate energy. Cellular respiration, for instance, involves a series of oxidation reactions where glucose is oxidized to produce AdenosineTri-Phosphate (ATP), the cell's primary energy currency. Electrochemical reactions involve the transfer of electrons through an external circuit. Electrolysis of water is a prime example where water molecules undergo oxidation at the anode to produce oxygen gas and hydrogen ions. Catalysts can accelerate oxidation reactions by providing an alternative pathway with lower activation energy. Enzymes in biological systems act as catalysts for various oxidation reactions, enhancing reaction rates without being consumed in the process. Higher temperatures often facilitate faster oxidation reactions by increasing the kinetic energy of particles, leading to more collisions and successful reactions. Pressure, particularly in gaseous systems, can also affect reaction rates. The concentration of reactants can significantly impact the rate of oxidation reactions. Higher concentrations generally lead to increased reaction rates due to more frequent collisions between reactant molecules. Understanding oxidation reactions is crucial in preventing oxidation in metals. Protective coatings, such as painting or galvanization, create barriers to prevent oxidation of metal surfaces. Combustion of fossil fuels and biological oxidation processes are essential for energy production. These processes generate power used in various industries and for electricity generation. Oxidation reactions play a vital role in food preservation, flavor development, and browning reactions. Antioxidants are often added to prevent undesirable oxidation in food products. Oxidation reactions are common and have farreaching implications in various fields, from chemistry to biology, industry, and everyday life.