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10 Nov 2019

Based on the following electrochemical cell, what is the standard reduction potential of metal M at 298 K? (R = 8.314 J/K • mol, F = 96500 C/mol)
Half-Reaction E° (V)
Fe2+(aq) + 2e– → Fe(s) –0.44

A) –0.54 V

B) +0.60 V

C) –0.30 V

D) +0.56 V

E) –0.28 V

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Related questions

The equilibrium constant, K, for a redox reaction is related to the standard potential, E∘, by the equation

lnK=nFE∘RT

where n is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e−) , R (the gas constant) is equal to 8.314 J/(mol⋠K) , and T is the Kelvin temperature.

Reduction half-reaction E∘ (V)
Ag+(aq)+e−→Ag(s) 0.80
Cu2+(aq)+2e−→Cu(s) 0.34
Sn4+(aq)+4e−→Sn(s) 0.15
2H+(aq)+2e−→H2(g) 0
Ni2+(aq)+2e−→Ni(s) −0.26
Fe2+(aq)+2e−→Fe(s) −0.45
Zn2+(aq)+2e−→Zn(s) −0.76
Al3+(aq)+3e−→Al(s) −1.66
Mg2+(aq)+2e−→Mg(s) −2.37

Part A

Use the table of standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 ∘C) for the following reaction:

Fe(s)+Ni2+(aq)→Fe2+(aq)+Ni(s)

Express your answer numerically.

K =

Part B

Calculate the standard cell potential (E∘) for the reaction

X(s)+Y+(aq)→X+(aq)+Y(s)

if K = 4.04×10−3.

Express your answer numerically in volts.
E∘ =

Calculate the standard cell potential for each of the following electrochemical cells.

Standard Electrode Potentials at 25 ∘C
Reduction half-reaction E∘(V)
Ag+(aq)+e− →Ag(s) 0.80
Sn2+(aq)+2e− →Sn(s) -0.14
ClO2(g)+e− →ClO2−(aq) 0.95
I2(s)+2e− →2I−(aq) 0.54
Ni2+(s)+2e− →Ni(s) -0.23
O2(g)+4H+(aq)+2e− →2H2O(l)

1.23

1. 2Ag+(aq)+Sn(s)→2Ag(s)+Sn2+(aq)

2. 2ClO2(g)+2I−(aq)→2ClO−2(aq)+I2(s)

3. O2(g)+4H+(aq)+2Ni(s)→2H2O(l)+2Ni2+(aq)
Free-energy change, ΔG∘, is related to cell potential, E∘, by the equation

ΔG∘=−nFE∘

where n is the number of moles of electrons transferred and F=96,500C/(mol e−) is the Faraday constant. When E∘ is measured in volts and can be determined from half-reaction potentials as given in the table below. ΔG∘ must be in joules since 1 J=1 C⋠V.
Reduction half-reaction E∘ (V)
Ag+(aq)+e−→Ag(s) 0.80
Cu2+(aq)+2e−→Cu(s) 0.34
Sn4+(aq)+4e−→Sn(s) 0.15
2H+(aq)+2e−→H2(g) 0
Ni2+(aq)+2e−→Ni(s) −0.26
Fe2+(aq)+2e−→Fe(s) −0.45
Zn2+(aq)+2e−→Zn(s) −0.76
Al3+(aq)+3e−→Al(s) −1.66
Mg2+(aq)+2e−→Mg(s) −2.37

Part A

Calculate the standard free-energy change at 25 ∘C for the following reaction using the table in the introduction:

Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)

Express your answer numerically in joules.
ΔG∘ = J

Part B

Calculate the standard cell potential at 25 ∘C for the reaction

X(s)+2Y+(aq)→X2+(aq)+2Y(s)

where ΔH∘ = -923 kJ and ΔS∘ = -123 J/K .

Express your answer numerically in volts.
E∘ = V

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