Question

[15 Points, Heeeeelp]

Answer 1

Answer: The half reactions are given below.

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:

$O_2(g)+4e^-\rightarrow 2O^{2-}(aq.)$