In a galvanic cell operating in an acidic solution, which of the following represents the correct half-reaction occurring at the anode?

• A. 2H⁺ + 2e⁻ → H₂
• B. Cu²⁺ + 2e⁻ → Cu
• C. Zn → Zn²⁺ + 2e⁻
• D. O₂ + 4H⁺ + 4e⁻ → 2H₂O

Answer: (C)

Verified step by step guidance

1. Identify the role of the anode in a galvanic cell. The anode is where oxidation occurs, meaning it loses electrons.
2. Examine each given half-reaction to determine which one involves oxidation. Oxidation is characterized by the loss of electrons.
3. Analyze the half-reaction '2H⁺ + 2e⁻ → H₂'. This reaction involves the gain of electrons (reduction), so it cannot occur at the anode.
4. Consider the half-reaction 'Cu²⁺ + 2e⁻ → Cu'. This also involves the gain of electrons (reduction), so it is not the anode reaction.
5. Evaluate the half-reaction 'Zn → Zn²⁺ + 2e⁻'. This reaction involves the loss of electrons, indicating oxidation, which is consistent with the process occurring at the anode in a galvanic cell.