A cell exhibits a standard emf of +0.177 V at 298 K?

Question

What is the value of the equilibrium constant for the cell reaction in each of the following cases?

n=1

n=2

n=3

Answer 1

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Answer 2

We know that

Eo = (RT/nF)lnK

Eo = voltage of cell = 0.177

R= 8.314 JK-1mol-1 <-- constant

T = temperature in Kelvins = 298K

n = 1, 2, or 3, depending on your question

F = 96500 J mol-1

K = ??? <-- you want to solve for this

Plug and chug away.

E.g.: for n=2...

Eo = (RT/nF)lnK

0.177 = [(8.314*298)/(2*96500)]lnK

0.177 = 0.0128371606 lnK

13.78809576 = lnK

e^(13.78808576) = K = 9.7E5

Do the same for n=1 and n=3.

[Answer: see above]