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?

A) Zn2+(s)+2e−→Zn(s)
B) Zn(s)→Zn2+(aq)+2e−
C) 2H++2e−→H2​
D) H2​+2e−→2H+

Answer 1

The oxidation half-reaction for the given equation is B) Zn(s) → Zn2+(aq) + 2e−, representing the loss of electrons as zinc is oxidized to Zn2+.

Step-by-step explanation:

The oxidation half-reaction that correctly describes the oxidation occurring in the reaction Zn(s) + 2HCl(aq) → ZnCl2​(aq) + H2​(g) is B) Zn(s) → Zn2+(aq) + 2e−. In a redox reaction, the substance that loses electrons is said to be oxidized. Here, zinc atoms are oxidized to Zn2+, showing a loss of two electrons which are then written as products, transforming neutral zinc into a 2+ ion.

In the provided reaction, zinc acts as the reductant as it loses electrons during the reaction. This process of zinc losing electrons corresponds to the half-equation Zn(s) → Zn2+(aq) + 2e−. It's important to note that the overall charge is balanced on both sides of the half-reaction.