Respuesta :
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.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reactions are defined as the reactions in which a chemical species gains its electrons. The oxidation state of the specie gets reduced.
[tex]X+ne^-\rightarrow X^{n-}[/tex]
For the given reactions:
1.) [tex]Cl^-(aq)\rightarrow Cl_2(g)[/tex]
Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:
[tex]2Cl^-(aq.)\rightarrow Cl_2(g)+2e^-[/tex]
2.) [tex]F^-(aq.)\rightarrow F_2(g)[/tex]
Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:
[tex]2F^-(aq.)\rightarrow F_2(g)+2e^-[/tex]
3.) [tex]S(s)\rightarrow S^{2-}(aq)[/tex]
Here, the oxidation state is getting reduced, therefore it is an reduction reaction. The equation for this follows:
[tex]S(s)+2e^-\rightarrow S^{2-}(aq)[/tex]
4.) [tex]H_2(g)\rightarrow H^+(aq.)[/tex]
Here, the oxidation state is getting increased, therefore it is an oxidation reaction. The equation for this follows:
[tex]H_2(g)\rightarrow 2H^+(aq.)+2e^-[/tex]
5.) [tex]O_2(g)\rightarrow O^{2-}(aq.)[/tex]
Here, the oxidation state is getting reduced, therefore it is an reduction reaction. The equation for this follows:
[tex]O_2(g)+4e^-\rightarrow 2O^{2-}(aq.)[/tex]
