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: Track oxidation numbers
Sn: +2 to +4 (increase). Fe: +3 to +2 (decrease).

Step 2: Interpret
An increase means loss of electrons, which is oxidation, so Sn2+ is oxidised and acts as the reducing agent. Fe3+ is reduced and acts as the oxidising agent.

Step 3: Pick
This is option (A). The reaction clearly has electron transfer, so it is a redox reaction.

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