Which of the following is not true of the rusting of iron?
The statement that is not true about the rusting of iron is that "rusting is a reduction process." Rusting is actually an oxidation process, which means that it involves the loss of electrons from the iron atoms in the metal. This loss of electrons causes the iron to become positively charged, which allows it to react with oxygen in the air and water molecules to form hydrated iron oxide, which is the main component of rust.
Rusting occurs when iron is exposed to both oxygen and moisture. In the presence of oxygen, iron undergoes a chemical reaction called oxidation, which produces iron oxide or rust. This process is accelerated by the presence of water, which provides the necessary electrons for the reaction to occur more quickly.
Rust is typically reddish-brown in color and is composed mainly of hydrated iron (III) oxide, which has the chemical formula Fe2O3•xH2O. The "x" in the formula represents the number of water molecules that can bond to each iron atom in the rust.
While rusting may look similar to burning, it is actually a different process. Burning involves a rapid oxidation reaction that produces heat and light, whereas rusting is a slower process that does not produce heat or light.