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Calculate E for the following electrochemical cell at 25°C, Cu | Cu2+ (0.100 M) || Zn2+ (0.0750 M) | Zn if E° (Cu2+) = +0.339 V and E° (Zn2+) = −0.762 V. (R = 8.31 J/K⋠mol, F = 96480 C/mol e− )

a. −1.105 V

b. −0.919 V

c. −0.486 V

d. −0.259 V

e. +0.486 V

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Related questions

8. What is the copper(II)-ion concentration at 25°C in the cell- Zn(s) | Zn2+(1.0 M) || Cu2+(aq) (? M) | Cu(s) if the measured cell potential is 1.01 V? The standard cell potential is 1.10 V. A) 0.030 M B) 0.99 M C) 0.00091 M D) 1.0 M E) 0.99 M

the questions arent supposed to be numbered like that so the question is starting where i crossed out 22 and the directions are 21

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∘ =

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