We’re being asked to calculate for the ΔG°_{rxn} and E°_{cell} for a redox reaction with n = 3 that has an equilibrium constant of K = 0.050 at 25°C.

**We have two ways (equations) of calculating the Gibbs Free Energy ΔG°:**

**Equation 1:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{\xb0}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RT}}{\mathbf{}}{\mathbf{ln}}{\mathbf{}}{\mathbf{K}}}$

ΔG° = Gibbs Free Energy, J

R = gas constant = 8.314 J/(mol∙K)

T = temperature, K

K = equilibrium constant

**Equation 2:**

Calculate Δ*G°*_{rxn} and *E°*_{cell} for a redox reaction with n = 3 that has an equilibrium constant of K = 0.050 (at 25 °C).

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Our data indicates that this problem or a close variation was asked in Chemistry: A Molecular Approach - Tro 3rd Edition. You can also practice Chemistry: A Molecular Approach - Tro 3rd Edition practice problems.