Question

Red hot iron absorbs \(SO_2\) giving the product.

• A. FeS + O\(_2\)
• B. FeO + FeS
• C. Fe\(_2\)O\(_3\) + FeS
• D. FeO + S

Hint:

\(SO_2\) is amphoteric in redox behavior → can both oxidize and reduce.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
At very high temperatures (red heat), Sulfur Dioxide (\( \text{SO}_{2} \)) reacts with transition metals like iron to form a mixture of oxides and sulfides.
Step 2: Detailed Explanation:
When Sulfur Dioxide gas is passed over red-hot iron, the iron acts as a reducing agent.
The Oxygen from \( \text{SO}_{2} \) combines with Iron to form Ferrous Oxide (\( \text{FeO} \)).
Simultaneously, the Sulfur from \( \text{SO}_{2} \) combines with Iron to form Ferrous Sulfide (\( \text{FeS} \)).
The balanced chemical equation for the reaction is:
\[ 3\text{Fe} + \text{SO}_{2} \longrightarrow 2\text{FeO} + \text{FeS} \]
This reaction shows that iron absorbs \( \text{SO}_{2} \) to yield a mixture of \( \text{FeO} \) and \( \text{FeS} \).
Step 3: Final Answer:
The product formed is \( \text{FeO} + \text{FeS} \).