Question

Identify the species that is oxidized and the species that is reduced: Zn(s) + 2 HCl(aq) ZnCl₂(aq) + H2(g).

a) Zn is oxidized, H+ is reduced
b) Zn is reduced, Cl- is oxidized
c) Zn is oxidized, Cl- is reduced
d) Zn is reduced, H+ is oxidized

Answer 1

The species that is oxidized in the reaction Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g) is zinc (Zn), and the species that is reduced is the hydrogen ion (H+).

Step-by-step explanation:

The correct option for the redox reaction for the equation Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g) is (a) Zn is oxidized, H+ is reduced. The species that is oxidized is zinc (Zn), represented by Zn(s), which loses electrons to form Zn²+ (zinc ion). This transition from 0 to +2 oxidation state is considered oxidation.

On the other side, the species that is reduced is the hydrogen ion, H+, which gains electrons to form H₂ (hydrogen gas). This transition from +1 to 0 oxidation state is considered reduction. The chloride ion, Cl-, does not change its oxidation state in this reaction and thus is neither oxidized nor reduced.