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An electrochemical cell has the following standard cell notation.

Mg(s) | Mg^2+ (aq) || Aq^+(aq) | Aq(s)

What is the standard potential for the cell?

Is this a spontaneous or non spontaneous reaction? Explain your answer.

Is this a galvanic cell or an electrolytic cell? Explain your answer.

User Murrayc
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2 Answers

2 votes

Step-by-step 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


Mg(s)\rightarrow Mg^(2+)+2e^-....(1)

Reduction: In this chemical process the electrons are gained by the element to form anion.


Ag^+(aq)+1e^-\rightarrow Ag(s)...(2)

Overall redox reaction: (1)+2 × (2)


Mg(s)+2Ag^+(aq)\rightarrow Mg^(2+)+2Ag(s)

User Martin Vysny
by
8.2k points
1 vote

Answer:

The standard potential for the cell is: 3.17 V

The reaction is spontaneous

It is a galvanic cell

Step-by-step 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.

User Bill Rollins
by
7.7k points
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