On igniting `Fe_(2)O_(3)` at `1400^(@)`C, the product obtained is

Options

A. `Fe_(2)O_(3)` melts
B. FeO
C. `Fe_(3)O_(4)`
D. metallic iron

Answer

To solve the question of what product is obtained when igniting Fe₂O₃ at 1400°C, we can follow these steps:

### Step 1: Understand the Reaction
When iron(III) oxide (Fe₂O₃) is heated to high temperatures, it can undergo a reduction reaction. This typically involves the presence of a reducing agent, such as carbon.

### Step 2: Write the Reaction
The reaction can be represented as:
\[ \text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO} \]

### Step 3: Balance the Reaction
To balance the equation:
- We have 2 iron (Fe) atoms on the product side from the reaction.
- We have 3 carbon (C) atoms reacting to produce 3 carbon monoxide (CO) molecules.

The balanced equation is:
\[ \text{Fe}_2\text{O}_3 + 3\text{C} \rightarrow 2\text{Fe} + 3\text{CO} \]

### Step 4: Identify the Product
From the balanced reaction, we see that the product formed is metallic iron (Fe) and carbon monoxide (CO). However, the question specifically asks for the product obtained from the ignition of Fe₂O₃.

### Conclusion
Thus, the product obtained when igniting Fe₂O₃ at 1400°C is **metallic iron (Fe)**.

### Final Answer
The product obtained is **metallic iron (Fe)**.

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