We are asked to **determine the value of the equilibrium constant, K** for the cell reaction given its** standard emf** and **number of electrons transferred, n** at 298 K.

The** Nernst Equation **relates the equilibrium constant and cell potential and is given by the equation:

$\overline{){\mathbf{E}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}{\mathbf{=}}\frac{\mathbf{RT}}{\mathbf{nF}}{\mathbf{ln}}{\mathbf{}}{\mathbf{K}}}$

E°_{cell} = cell potential, V

R = gas constant = 8.314 J/(mol·K)

T = temperature, K

n = mole e^{-} transferred

F = Faraday’s constant, 96485 C/mol e^{-}

K_{ }= equilibrium constant

A cell has a standard emf of + 0.151 V at 298 K.

What is the value of the equilibrium constant for the cell reaction if n = 3?

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