Consider the chemical reaction below.
zn(s)+ 2h*(aq) → zn2+ (aq) + h2(g)
which half reaction correctly represents reduction for this equation?
zn(s) → zn2+ (aq)+2e
2h* (aq)+2e → h2(g)
zn(s) → zn? - (aq)+e"
2h* (aq)+e™ → h2(g)

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.

For the given reactio:

On reactant side:

Oxidation state of zinc= 0

Oxidation state of hydrogen = +21

On product side:

Oxidation state of zinc = +2

Oxidation state of hydrogen = 0

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

Hence, the correct answer is

you need to have a picture of the atom that way we can answer it