The rusting of iron is an electrochemical process that involves the oxidation of iron in the presence of oxygen and water. Here's a breakdown of the mechanism and the chemical equa... The rusting of iron is an electrochemical process that involves the oxidation of iron in the presence of oxygen and water. Here's a breakdown of the mechanism and the chemical equations involved. Conditions necessary for rusting: Presence of iron: The metal itself is essential. Presence of oxygen: Oxygen acts as the oxidizing agent. Presence of water: Water acts as an electrolyte, facilitating the movement of ions. Mechanism: Anode formation: At certain points on the iron surface, iron atoms lose electrons and become iron(II) ions (oxidation). Equation: Fe(s) → Fe²⁺(aq) + 2e⁻. Cathode formation: At other points on the iron surface, oxygen molecules gain electrons in the presence of water to form hydroxide ions (reduction). Equation: O₂(g) + 2H₂O(l) + 4e⁻ → 4OH⁻(aq). Ion migration: The electrons released at the anode flow through the iron to the cathode. The Fe²⁺ ions migrate through the water towards the cathode, while the OH⁻ ions move towards the anode. Formation of iron(II) hydroxide: At the anode or in the solution near the anode, Fe²⁺ ions react with OH⁻ ions to form iron(II) hydroxide. Equation: Fe²⁺(aq) + 2OH⁻(aq) → Fe(OH)₂(s). Further oxidation: Iron(II) hydroxide is further oxidized by oxygen in the presence of water to form iron(III) oxide-hydroxide (hydrated iron(III) oxide), which is what we commonly call rust. Equation: 4Fe(OH)₂(s) + O₂(g) + 2H₂O(l) → 4Fe(OH)₃(s). Iron(III) oxide-hydroxide can dehydrate to form iron(III) oxide (the most common form of rust): 2Fe(OH)₃(s) → Fe₂O₃(s) + 3H₂O(l). Overall simplified equation: 4Fe(s) + 3O₂(g) + 6H₂O(l) → 4Fe(OH)₃(s) or 4Fe(s) + 3O₂(g) + xH₂O(l) → 2Fe₂O₃.xH₂O(s) where x represents the variable number of water molecules associated with the rust. Key points: Rusting is an electrochemical process requiring the presence of iron, oxygen, and water. The process involves both oxidation (loss of electrons by iron) and reduction (gain of electrons by oxygen). The final product, rust, is a hydrated form of iron(III) oxide.
Understand the Problem
The question is providing a detailed explanation of the rusting process of iron, outlining the necessary conditions, mechanism, chemical equations involved, and the final products in the rusting process.
Answer
4Fe(s) + 3O₂(g) + xH₂O(l) → 2Fe₂O₃.xH₂O(s)
The final answer is: 4Fe(s) + 3O₂(g) + xH₂O(l) → 2Fe₂O₃.xH₂O(s) where x represents the number of water molecules associated with the rust.
Answer for screen readers
The final answer is: 4Fe(s) + 3O₂(g) + xH₂O(l) → 2Fe₂O₃.xH₂O(s) where x represents the number of water molecules associated with the rust.
More Information
Rust formation is an electrochemical process that involves several steps, leading to the formation of hydrated iron(III) oxide, commonly known as rust.
Tips
One common mistake is to overlook the necessity of both oxygen and water for the rusting process.
Sources
- Rusting of Iron - Explanation, Chemical Reaction, Prevention - geeksforgeeks.org
- What is chemical reaction of rusting of iron? - Quora - quora.com
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