Respuesta :
Answer:
For (i): Magnesium is getting oxidized and zinc is getting reduced.
For (ii): The half reactions are given below.
For (iii): Magnesium will act as anode and zinc act as cathode.
Explanation:
- For (i):
[tex]E^o_{(Mg^{2+}/Mg)}=-2.37V\\E^o_{(Zn^{2+}/Zn)}=-0.76V[/tex]
The substance having highest positive [tex]E^o[/tex] potential will always get reduced and will undergo reduction reaction. Here, zinc will always undergo reduction reaction will get reduced.
Magnesium will undergo oxidation reaction and will get oxidized.
- For (ii):
Oxidation reaction is defined as the reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reaction is defined as the reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
Oxidation half reaction: [tex]Mg\rightarrow Mg^{2+}+2e^-[/tex]
Reduction half reaction: [tex]Zn^{2+}+2e^-\rightarrow Zn[/tex]
- For (iii):
Oxidation reaction always occurs on anode side and thus, magnesium is acting as anode.
Reduction reaction always occurs on cathode side and thus, zinc is acting as cathode.
