I need help with part B The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation lnK=nFERT where n

I need help with part B

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.

Standard reduction potentials

Reduction half-reactionE∘ (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 Part complete

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.

View Available Hint(s)

K = 2.68×106

Submit Previous Answers

Correct

When E∘>0 and K>1 the reaction favors the products.

Part B

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

X(s)+Y+(aq)→X+(aq)+Y(s)

if K = 7.87×10−3.

Express your answer to three significant figures and include the appropriate units.

View Available Hint(s)

E∘ = ?