Question

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)

Answer 1

2H+(aq) + 2e– → H2(g) or B.)

on edge 2023

Answer 2

Answer:
`2H^++2e^-\rightarrow H_2(g)`

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.

For the given reactio:

`Zn(s)+2H^+\rightarrow Zn^(2+)+H_2`

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
`2H^++2e^-\rightarrow H_2(g)`