Problem: Calculate ΔG°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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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:

G°=-RT ln K

ΔG° = Gibbs Free Energy, J
R = gas constant = 8.314 J/(molK)
T = temperature, K
K = equilibrium constant


Equation 2:

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Problem Details

Calculate Δrxn and cell for a redox reaction with n = 3 that has an equilibrium constant of K = 0.050 (at 25 °C).

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Based on our data, we think this problem is relevant for Professor Negroni's class at MONTGOMERY COLLEGE.

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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.