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: Idea:
Look at which side the electrons appear. Electrons on the product side means oxidation.

Step 2: Result:
Only option C writes the electron on the right-hand side, so only it is an oxidation half reaction and can occur at the anode.

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