We are asked to calculate for the standard potential (E°cell) of the reaction. We will use the Nernst Equation to calculate for the ratio. The Nernst Equation relates the concentrations of compounds and cell potential.
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
Let’s first determine how many electrons were transferred in the reaction:
Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K.
X(s) + Y2+(aq) ⇌ X2+(aq) + Y(s) K= 9.49 x 105
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