Question

In: Chemistry

Write the cell reaction and electrode half-reactions and calculate the standard potential of each of the...

Write the cell reaction and electrode half-reactions and calculate the standard potential of each of the following cells:

a) Zn/ZnSO₄(aq)//AgNO₃(aq)/Ag

b) Pt/K₃[Fe(CN)₆](aq), K₄[Fe(CN)₆](aq)//CrCl₃ (aq)/Cr

Please show all steps and clear writing.

Thanks

Solutions

Expert Solution

Zn/ZnSO4 (aq) means redox reaction of Zn²⁺ (aq)/Zn.

And Ag/AgNO3 (aq) means redox system of Ag⁺/Ag.

Redox potential of Zn²⁺ (aq)+ 2e -------> Zn(s) is - 0.76 V.

Redox potential of Ag⁺ (aq)+ e -------> Ag(s) is +0.80 V.

The one with negative reduction potential are good reducing agents and act as anode.

Thus here Zn in ZnSO4 acts as anode and undergoes oxidation.

And Ag in AgNO3 acts as cathode and undergoes reduction.

Anode reaction :

Zn(s) -------->Zn²⁺ (aq)+ 2e

Cathode reaction :

Ag⁺ (aq)+ e -------> Ag(s)

Net cell reaction

Zn(s) + 2 Ag⁺ (aq) -------->Zn²⁺ (aq)+ 2 Ag (s)

E cell = Ecathode - Eanode

= +0.80 V - (-0.76 V) = +1.56 V

When K3[Fe(CN)6](aq) changes to K4[Fe(CN)6](aq) oxidation state of Fe changes from +3 to +2

Redox potential of Fe³⁺ (aq)+ e -------> Fe²⁺(aq) is + 0.77 V.

Redox potential of Cr³⁺ (aq)+ 3 e -------> Cr(s) is - 0.74 V.

Here CrCl3 (aq)/Cracts as anode and undergoes oxidation and

Pt/K3[Fe(CN)6](aq), K4[Fe(CN)6](aq) acts as cathode and undergoes reduction .

Anode reaction :

Cr(s) -------->Cr³⁺ (aq)+ 3 e

Cathode reaction :

Fe⁺³ (aq)+ e -------> Fe²⁺(aq)

Net cell reaction

Cr(s) + 3 Fe³⁺ (aq) -------->Cr³⁺ (aq)+ 3 Fe²⁺(aq)

E cell = Ecathode - Eanode

= +0.77 V - (-0.74 V) = +1.51 V

queen_honey_blossom answered 1 year ago

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