Question

In this reaction, what is the substance oxidized? zn(s) + 2 hcl(aq) → zncl2(aq) + h2(g) zinc chloride chlorine hydrogen zn oxygen

Answer 1

Answer: Zinc (Zn)

Step-by-step explanation:

Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.

Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.

Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.

`Zn(s)+2HCl(aq)\rightarrow ZnCl_2(aq)+H_2(g)`

On reactant side:

Oxidation state of zinc = 0

Oxidation state of hydrogen = +1

On product side:

Oxidation state of zinc = +2

Oxidation state of hydrogen = 0

The oxidation state of zinc increases from 0 to +2, it is getting oxidized and it undergoes oxidation reaction.

The oxidation state of hydrogen decreases from +1 to 0. Thus, it is getting reduced and it undergoes reduction reaction.

Answer 2

Zn(s) + 2 HCl(aq) → ZnCl₂(aq) + H₂(g)
Oxidation means lose of electrons and increase of positive charge so the part which oxidized in this equation is Zn(s) because it converted to Zn²⁺ (i.e. lost two electrons)