Question

Red hot iron absorbs SO\(_2\) giving the product

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

Hint:

SO\(_2\) acts as an oxidizing agent here.

Answer 1

The Correct Option is C

To solve this question, we need to understand the chemical reaction between red hot iron and sulfur dioxide (SO\(_2\)).

1. Initially, let's consider the nature of the reactants:
   • Red hot iron is in a reactive state and can react with gases present in the environment.
   • Sulfur dioxide (SO\(_2\)) is a sulfur compound that can oxidize iron.
2. The reaction of red hot iron with sulfur dioxide is known to produce iron(II) oxide and iron(II) sulfide as products. The chemical equation can be represented as:

\(2\text{Fe} + \text{SO}_2 \rightarrow \text{FeO} + \text{FeS}\)

• Iron (Fe) reacts with sulfur dioxide (SO\(_2\)) to form iron(II) oxide (FeO) and iron(II) sulfide (FeS).
• This is a typical reaction where sulfur in SO\(_2\) is reduced to sulfide (S\(^{2-}\)) while iron is partially oxidized to FeO.

1. Examining the given options:
   • Option 1: FeS + O\(_2\) - This does not match the possible reaction products.
   • Option 2: Fe\(_2\)O\(_3\) + FeS - Formation of Fe\(_2\)O\(_3\) requires a different oxidative environment; not just SO\(_2\).
   • Option 3: FeO + FeS - This matches the products formed from red hot iron absorbing SO\(_2\).
   • Option 4: FeO + S - This option lacks the formation of FeS, which is inconsistent given the reduction of SO\(_2\).
2. Based on the analysis above, the correct answer is Option 3: FeO + FeS.
   • This correctly reflects the products of the reaction between red hot iron and sulfur dioxide.

In summary, when red hot iron absorbs SO\(_2\), it results in the formation of iron(II) oxide and iron(II) sulfide, which is represented by the equation: \(2\text{Fe} + \text{SO}_2 \rightarrow \text{FeO} + \text{FeS}\).