Question

The below reaction takes place in the presence of________
$4Fe(s) + 3{O_2}(G) \to 2F{e_2}{O_3}(s)$

Answer 1

Hint: To understand this we must know what rusting is. Rusting is an oxidation reaction. The iron reacts with water and oxygen to form hydrated iron oxide, which we see as rust. This prevents the metal below from coming into contact with air (containing oxygen).

Complete answer:
$4Fe(s) + 3{O_2}(G) \to 2F{e_2}{O_3}(s)$
The above reaction takes place in the presence of moisture.
The rusting of iron is an electrochemical process that begins with the transfer of electrons from iron to oxygen. The iron is the reducing agent while the oxygen is the oxidizing agent.
The exposure of iron to oxygen in the presence of moisture leads to the formation of rust. This phenomenon takes place in the presence of moisture and air. So, the presence of air and water vapor in air are two necessary conditions for the rusting of iron.
The iron reacts with water and oxygen to form hydrated iron oxide. Iron and steel rust when they come into contact with water and oxygen both are needed for rusting to occur. This prevents the metal below from coming into contact with air

Additional information:
There are three types of rusts
Yellow Rust. Iron oxide-hydroxide $FeO(OH).{H_2}O$ Yellow rust is present in metals that are found in large amounts of standing water.
Brown Rust. Oxide $F{e_2}{O_3}$.
Black Rust. Iron oxide $F{e_3}{O_4}$

Note:
Rust may be treated with commercial products known as rust converter which contain tannic acid or phosphoric acid which combines with rust removed with organic acids like citric acid and vinegar or the stronger hydrochloric acid or removed with chelating agents as in some commercial formulations or even a solution of molasses.