Question

Consider the redox reaction below: Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g). Which half reaction correctly describes the oxidation that is taking place?

1) Zn²+(s) + 2e⁻(aq) → Zn(s)
2) Zn(s) → Zn²+(aq) + 2e⁻
3) 2H^+(aq) + 2e⁻ → H₂
4) H₂ + 2e⁻ → 2H^+

Answer 1

The half reaction that correctly describes the oxidation taking place is Zn(s) → Zn²+(aq) + 2e⁻, which shows zinc being oxidized by losing two electrons.

Step-by-step explanation:

Considering the redox reaction Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g), we can identify that zinc atoms are oxidized to Zn²+, where the correct half-reaction for the oxidation process is: Zn(s) → Zn²+(aq) + 2e⁻. A redox reaction consists of two complementary reactions: oxidation, which involves the loss of electrons, and reduction, involving the gain of electrons. In this specific example, Zn(s) is the substance being oxidized, as it loses two electrons to become Zn²+(aq). Option 2) Zn(s) → Zn²+(aq) + 2e⁻ is the correct half reaction for the oxidation occurring in the reaction.