In the aluminothermite process, aluminium is

Options

A. Oxidising agent
B. Flux
C. Reducing agent
D. Solder

Answer

**Step-by-Step Solution:**

1. **Understanding the Aluminothermite Process**:
The aluminothermite process is a metallurgical reaction where aluminum is used to reduce certain metal oxides to their respective metals. This process is particularly useful for metals that cannot be reduced effectively by carbon.

2. **Identifying the Role of Aluminum**:
In this process, aluminum serves as a reducing agent. A reducing agent is a substance that donates electrons to another substance, causing the reduction of that substance while itself being oxidized.

3. **Example Reaction**:
A common example is the reduction of iron(III) oxide (Fe2O3) using aluminum. The reaction can be represented as:
\[ Fe2O3 + 2Al \rightarrow 2Fe + Al2O3 \]
In this reaction, Fe2O3 is reduced to Fe, while aluminum (Al) is oxidized to aluminum oxide (Al2O3).

4. **Balancing the Reaction**:
The reaction is balanced by ensuring that the number of atoms of each element is the same on both sides. In this case, we have 2 iron atoms, 3 oxygen atoms, and 2 aluminum atoms balanced appropriately.

5. **Conclusion**:
Since aluminum is responsible for reducing Fe2O3 to Fe while itself being oxidized, it acts as a reducing agent in the aluminothermite process.

**Final Answer**: Aluminum is used as a **reducing agent** in the aluminothermite process.

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