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In the process of iron rusting, what role does iron play, and what role does oxygen gas play?
In the process of iron rusting, what role does iron play, and what role does oxygen gas play?
Iron acts as the reducing agent, and oxygen gas acts as the oxidizing agent.
Explain why the edge of a water droplet on an iron surface acts as the cathode in the rusting process.
Explain why the edge of a water droplet on an iron surface acts as the cathode in the rusting process.
The edge of the water droplet acts as the cathode because the concentration of soluble oxygen is higher on the edge than in the droplet's center. Oxygen is needed for the reduction reaction which occurs at the cathode.
Write the equation for the oxidation of iron at the anode during rusting.
Write the equation for the oxidation of iron at the anode during rusting.
Fe → $Fe^{2+}$ + 2e
Write the equation that describes how soluble oxygen in the water accepts electrons at the cathode area to form hydroxide ions.
Write the equation that describes how soluble oxygen in the water accepts electrons at the cathode area to form hydroxide ions.
What is the chemical formula of the initial product formed when iron(II) ions combine with hydroxide ions?
What is the chemical formula of the initial product formed when iron(II) ions combine with hydroxide ions?
Write the balanced chemical equation for the oxidation of iron(II) hydroxide to form iron(III) hydroxide.
Write the balanced chemical equation for the oxidation of iron(II) hydroxide to form iron(III) hydroxide.
What is the general formula for hydrated iron(III) oxide, which is formed by the decomposition of iron(III) hydroxide, and what is its common name?
What is the general formula for hydrated iron(III) oxide, which is formed by the decomposition of iron(III) hydroxide, and what is its common name?
If $x = 3$ in the formula $Fe_2O_3•xH_2O$, what would be the molecular weight of the hydrated iron(III) oxide?
If $x = 3$ in the formula $Fe_2O_3•xH_2O$, what would be the molecular weight of the hydrated iron(III) oxide?
Briefly explain the role of water in the rusting process of iron.
Briefly explain the role of water in the rusting process of iron.
Write the overall equation for the rusting of iron.
Write the overall equation for the rusting of iron.
Flashcards
Rusting: Roles of Iron and Oxygen
Rusting: Roles of Iron and Oxygen
In rusting, iron loses electrons, acting as the reducing agent. Oxygen gas gains electrons, acting as the oxidising agent.
Anode in Rusting
Anode in Rusting
The region on the iron surface exposed to water where oxidation occurs, forming iron(II) ions.
Cathode in Rusting
Cathode in Rusting
The region on the water droplet edge where reduction occurs; soluble oxygen accepts electrons to form hydroxide ions.
Oxidation of Iron
Oxidation of Iron
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Electron Flow in Rusting
Electron Flow in Rusting
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Formation of Iron(II) Hydroxide
Formation of Iron(II) Hydroxide
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Formation of Iron(III) Hydroxide
Formation of Iron(III) Hydroxide
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Formation of Rust
Formation of Rust
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Overall Rusting Equation
Overall Rusting Equation
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Study Notes
- In the rusting of iron, iron acts as the reducing agent and oxygen gas acts as the oxidising agent.
Rusting Process
- The surface of iron exposed to water droplets experiences oxidation at the center of the droplets, known as the anode.
- Reduction occurs at the edge of the water droplets, referred to as the cathode, due to the higher concentration of soluble oxygen at the edge compared to the center.
- At the anode, metal iron undergoes oxidation to produce iron(II) ions, with the loss of electrons per the equation Fe → Fe2+ + 2e.
- Electrons freed at the anode move through the metal iron to the cathode area.
- Soluble oxygen in the water accepts electrons to form hydroxide ions, shown as O2 + 2H2O + 4e → 4OH-.
- Iron(II) ions combine with hydroxide ions to create iron(II) hydroxide, as per Fe2+ + OH- → Fe(OH)2.
- Iron(II) hydroxide then gets oxidised by oxygen to produce iron(III) hydroxide, following 4Fe(OH)2 + 2H2O + O2 → 4Fe(OH)3.
- Iron(III) hydroxide decomposes into hydrated iron(III) oxide (Fe2O3•xH2O) by oxygen in the air, demonstrated by the equation 4Fe(OH)3 → Fe2O3•XH2O.
- Hydrated iron(III) oxide is brown and known as rust.
- The overall equation for the rusting of iron is 4Fe + 3O2 +2xH2O → 2Fe2O3•XH2O.
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