`Fe_(2)O_(3) + 2Al rarr Al_(2)O_(3) + 2Fe`
The above reaction is an example of a
(i) combination reaction.
(ii) double displacement reaction
(iii) decomposition reaction.
(iv) displacement reaction.

Options

A. combination reaction.
B. double displacement reaction
C. decomposition reaction.
D. displacement reaction.

Explanation

To determine the type of reaction represented by the equation:

\[ \text{Fe}_2\text{O}_3 + 2\text{Al} \rightarrow \text{Al}_2\text{O}_3 + 2\text{Fe} \]

we can follow these steps:

### Step 1: Identify the Reactants and Products
- The reactants in this reaction are ferric oxide (\( \text{Fe}_2\text{O}_3 \)) and aluminum (\( \text{Al} \)).
- The products of the reaction are aluminum oxide (\( \text{Al}_2\text{O}_3 \)) and iron (\( \text{Fe} \)).

### Step 2: Analyze the Reaction
- In this reaction, aluminum is reacting with ferric oxide.
- During the reaction, aluminum displaces iron from its oxide, resulting in the formation of aluminum oxide and elemental iron.

### Step 3: Determine the Type of Reaction
- A **combination reaction** involves two or more substances combining to form a single product.
- A **double displacement reaction** involves the exchange of ions between two compounds.
- A **decomposition reaction** involves a single compound breaking down into two or more simpler substances.
- A **displacement reaction** (or single displacement reaction) occurs when one element displaces another in a compound.

### Step 4: Conclusion
- Since aluminum displaces iron from ferric oxide, this reaction is classified as a **displacement reaction**.

### Final Answer
The above reaction is an example of a **(iv) displacement reaction**.

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