Question

[15 Points, Heeeeelp]

Complete the half equations by balancing it and identify as either oxidation or reduction.

Cl^- (aq) → Cl2 (g)

F^- (aq) → F2 (g)

S (s) → S^2- (aq)

H2 (g) → H^+ (aq)

O2 (g) → O^2 (aq) ​

Answer 1

Answer: The half reactions are given below.

Step-by-step explanation:

Oxidation reactions are defined as the reactions in which a chemical species looses its electrons. The oxidation state of the specie increases.

`X\rightarrow X^(n+)+ne^-`

Reduction reactions are defined as the reactions in which a chemical species gains its electrons. The oxidation state of the specie gets reduced.

`X+ne^-\rightarrow X^(n-)`

For the given reactions:

1.)
`Cl^-(aq)\rightarrow Cl_2(g)`

Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:

`2Cl^-(aq.)\rightarrow Cl_2(g)+2e^-`

2.)
`F^-(aq.)\rightarrow F_2(g)`

Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:

`2F^-(aq.)\rightarrow F_2(g)+2e^-`

3.)
`S(s)\rightarrow S^(2-)(aq)`

Here, the oxidation state is getting reduced, therefore it is an reduction reaction. The equation for this follows:

`S(s)+2e^-\rightarrow S^(2-)(aq)`

4.)
`H_2(g)\rightarrow H^+(aq.)`

Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:

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

5.)
`O_2(g)\rightarrow O^(2-)(aq.)`

Here, the oxidation state is getting reduced, therefore it is an reduction reaction. The equation for this follows:

`O_2(g)+4e^-\rightarrow 2O^(2-)(aq.)`