Where do redox reactions find applications?

Answer

A redox reaction is a chemical reaction in which a reduction and an oxidation occur (hence the name red–ox : reductionaloxidation). The element/molecule that undergoes a reduction gains electrons from the element/molecule that is oxidizing. A simple example of this is the formation of hydrogen fluoride (HF) from hydrogen gas (H₂) and fluorine gas (F₂). The oxidation reaction consists of converting H₂ in two H⁺ ions and two free electrons. The reduction reaction, on the other hand, consists of taking up two free electrons by the F₂ molecule for the formation of 2 F^– ions.

Redox reactions can proceed from very slow (as in the case of the rusting of iron) to very fast (such as the burning of eg wood). Examples of applications where redox reactions take place are batteries and accumulators. Redox reactions are also used in electrodeposition to gild materials (of jewelry), silver (of cutlery), electroplating (of steel) or chrome plating (of car parts). Many examples of redox reactions can also be found in biology, such as: cell respiration (oxidation of glucose to CO₂and reduction of oxygen to water) and photosynthesis (reduction of CO₂ to sugars and oxidation of water to oxygen gas).