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**Problem**: 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

###### FREE Expert Solution

###### FREE Expert Solution

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:**

###### Problem Details

Calculate the standard potential, E°, for this reaction from its equilibrium constant at 298 K.

X(s) + Y^{2+}(aq) ⇌ X^{2+}(aq) + Y(s) *K*= 9.49 x 10^{5}

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