Question

For the following redox reaction, find the correct statement.
\(\text{Sn}^{2+}+2\text{Fe}^{3+}\rightarrow \text{Sn}^{4+}+2\text{Fe}^{2+}\)

• A. \(\text{Sn}^{2+}\) is undergoing oxidation.
• B. \(\text{Fe}^{3+}\) is undergoing oxidation.
• C. It is not a redox reaction.
• D. Both \(\text{Sn}^{2+}\) and \(\text{Fe}^{3+}\) are oxidized.

Hint:

The species that loses electrons is oxidised; Sn goes from +2 to +4.

Answer 1

The Correct Option is A

Step 1: Understanding the Concept
Oxidation is loss of electrons (oxidation number rises). Reduction is gain of electrons (oxidation number falls).

Step 2: Detailed Explanation
\(\text{Sn}^{2+} \rightarrow \text{Sn}^{4+}\): oxidation number goes from +2 to +4, so it loses 2 electrons and is oxidised.
\(\text{Fe}^{3+} \rightarrow \text{Fe}^{2+}\): oxidation number falls from +3 to +2, so it gains an electron and is reduced.
So (A) is correct. (B) reverses the roles, (C) is wrong because electrons are transferred, and (D) is wrong because Fe3+ is reduced.

Final Answer:
Only \(\text{Sn}^{2+}\) is oxidised, option (A). \[ \boxed{\text{Sn}^{2+} \text{ is oxidised}} \]