When iron is rusted, it is

Options

A. Oxidised
B. Reduced
C. Evaporated
D. Decomposed

Explanation

To solve the question "When iron is rusted, it is," we need to analyze the rusting process of iron, which involves redox reactions. Here’s a step-by-step solution:

### Step 1: Understanding Rusting
Rusting is a chemical process where iron reacts with oxygen and moisture (water) in the environment to form rust, primarily composed of iron(III) oxide (Fe2O3) and water (H2O).

### Step 2: Writing the Oxidation Reaction
The first step in rusting involves the oxidation of iron (Fe) to iron ions (Fe²⁺). The half-reaction for this oxidation can be written as:
\[ \text{Fe (s)} \rightarrow \text{Fe}^{2+} + 2e^- \]
Here, iron loses electrons, indicating that it is being oxidized.

### Step 3: Writing the Reduction Reaction
The second part of the rusting process involves the reduction of oxygen (O2) in the presence of water (H2O). The half-reaction for this reduction can be written as:
\[ \text{O}_2 + 4\text{H}^+ + 4e^- \rightarrow 2\text{H}_2\text{O} \]
In this step, oxygen gains electrons, indicating that it is being reduced.

### Step 4: Combining the Half-Reactions
To find the overall reaction, we need to combine the oxidation and reduction half-reactions. The balanced overall reaction for rusting can be summarized as:
\[ 4\text{Fe (s)} + 3\text{O}_2 + 6\text{H}_2\text{O} \rightarrow 4\text{Fe}_2\text{O}_3 \cdot 3\text{H}_2\text{O} \]
This shows that iron reacts with oxygen and water to form rust (Fe2O3·xH2O).

### Step 5: Conclusion
From the above reactions, we can conclude that when iron is rusted, it undergoes oxidation. Therefore, the correct answer to the question is that iron is oxidized during the rusting process.

### Final Answer
When iron is rusted, it is oxidized.

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