Explanation:
The given following standard cell notation.
Mg(s) | Mg^2+ (aq) || Aq^+(aq) | Aq(s)
Oxidation: In this chemical process the electrons are lost by the element to form cation
[tex]Mg(s)\rightarrow Mg^{2+}+2e^-[/tex]....(1)
Reduction: In this chemical process the electrons are gained by the element to form anion.
[tex]Ag^+(aq)+1e^-\rightarrow Ag(s)[/tex]...(2)
Overall redox reaction: (1)+2 × (2)
[tex]Mg(s)+2Ag^+(aq)\rightarrow Mg^{2+}+2Ag(s)[/tex]
Answer:
The standard potential for the cell is: 3.17 V
The reaction is spontaneous
It is a galvanic cell
Explanation:
The half-reactions for each process are:
Oxidation: Mg(s) -> Mg^2+ (aq) + 2e^- E^0 = 2.37
Reduction: Ag^+ (aq) + 1e^- -> Ag(s) E^0 = 0.8
The standard potential for the cell is:
E^0 cell = E^0 reduction + E^0 oxidation = 2.37 + 0.8 = 3.17 V
The reaction is spontaneous because the standard potential for the cell is positive.
It is a galvanic cell. In a galvanic cell, spontaneous redox processes occur allowing the continuous flow of electrons through the conductor, whereas, in an electrolytic cell, the non-spontaneous redox reactions are promoted by an external source of current.
