Question

Which of the following reaction is possible at anode?

• A. \(\text{F}_2+2e^-\rightarrow 2\text{F}^-\)
• B. \(2\text{H}^++\frac{1}{2}\text{O}_2+2e^-\rightarrow \text{H}_2\text{O}\)
• C. \(\text{Fe}^{2+}\rightarrow \text{Fe}^{3+}+1e^-\)
• D. \(\text{Cu}^{2+}+2e^-\rightarrow \text{Cu}(s)\)

Hint:

Oxidation (loss of electrons) takes place at the anode.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept:
The anode is the electrode where oxidation happens, meaning that electrons are lost.

Step 2: Check each:
A: \(\text{F}_2 + 2e^- \to 2\text{F}^-\) gains electrons, so it is reduction (cathode).
B: \(\text{O}_2\) with \(2e^-\) gives water, again reduction.
C: \(\text{Fe}^{2+} \to \text{Fe}^{3+} + e^-\) loses an electron, so it is oxidation. This occurs at the anode.
D: \(\text{Cu}^{2+} + 2e^- \to \text{Cu}\) gains electrons, so it is reduction.

Final Answer:
Only \(\text{Fe}^{2+}\to\text{Fe}^{3+}+e^-\) is an anode reaction, option (C). \[ \boxed{\text{Fe}^{2+}\to\text{Fe}^{3+}+e^-} \]