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O2 4 e 2 H2O 4 OH Here oxygen gains electrons thus it is oxidizing agent.
Rusting of iron reaction. Many other metals undergo similar corrosion but the resulting oxides are not commonly called rust. The familiar red form of rust is Fe 2 O 3 but iron has other oxidation states so it can form other colors of rust. Water is also required for this reaction to occur but because the total amount of water does not change it is not included in the equation.
For iron to rust oxygen and water must be present. The rusting of iron is an electrochemical process that begins with the transfer of electrons from iron to oxygen. During rusting iron combines with oxygen in the presence of water.
When some grease or oil is applied to the surface of an iron object then air and moisture cannot come in contact with it and hence rusting is prevented. Rusting is the common term for corrosion of iron and its alloys such as steel. Rusting is a redox reaction whereby oxygen acts as the oxidising agent and iron acts as the reducing agent.
For example to avoid corrosion iron and steel tools and machine parts are rubbed with grease or oil. Page 4 of 17 INTRODUCTION Rust is an iron oxide usually red oxide formed by the redox reaction of iron and oxygen in the presence of water or air moisture. Therefore at each anode neutral iron atoms are oxidised to ferrous ions.
Rust is mostly made up of two different oxides of iron that vary in the oxidation state of the iron. Associated Reactions The rusting of iron is an electrochemical process that begins with the transfer of electrons from iron to oxygen. Rusting of iron is an example of a redox reaction.
The iron reacts with water and oxygen to form hydrated iron III oxide which we see as rust. Rust forms when iron or its alloys are exposed to moist air. The iron is the reducing agent gives up electrons while the oxygen is the oxidising agent gains electrons.
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