Question

Consider the chemical reaction below.

Answer 1

Answer:

A

Explanation:

because we have 2 charges in other Zn to balance the equation we must give the other Zn 2e

Answer 2

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

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:

$Zn(s)+2H^+\rightarrow Zn^{2+}+H_2$

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