Question

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.

Answer 1

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)`

Answer 2

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.