Question

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

1) Zn��+(s) + 2e���(aq) ��� Zn(s)
2) Zn(s) ��� Zn��+(aq) + 2e���
3) 2H^+(aq) + 2e��� ��� H���
4) Cannot be determined

Answer 1

The correct oxidation half-reaction for the oxidation of zinc in the given redox reaction is Zn(s) → Zn²⁺(aq) + 2e⁻.

Step-by-step explanation:

To determine which half-reaction correctly describes the oxidation taking place in the reaction Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g), we need to identify the species that is losing electrons. In this reaction, zinc atoms are oxidized to Zn²⁺. The correct oxidation half-reaction for zinc is Zn(s) → Zn²⁺(aq) + 2e⁻. Hence the apt half reaction from the given options is number 2) Zn(s) → Zn²⁺(aq) + 2e⁻.