Question

In the reaction: \[ \text{Zn(s)} + \text{CuSO}_4(aq) \rightarrow \text{ZnSO}_4(aq) + \text{Cu(s)} \] Which of the following is the correct oxidation half-reaction?

• A. \( \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \)
• B. \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \)
• C. \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \)
• D. \( \text{Cu} \rightarrow \text{Cu}^{2+} + 2e^- \)

Hint:

In redox reactions, oxidation involves the loss of electrons, and reduction involves the gain of electrons. The oxidation half-reaction always shows the species losing electrons.

Answer 1

The Correct Option is A

In this redox reaction, zinc (Zn) is oxidized and copper ions (\( \text{Cu}^{2+} \)) are reduced. Oxidation involves the loss of electrons. Zinc is losing two electrons to form \( \text{Zn}^{2+} \): \[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \] Thus, the oxidation half-reaction is: \[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \] Therefore, the correct oxidation half-reaction is option (1).