Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 °C: 3I₂(s) + 2Fe(s) → 2Fe³⁺(aq) + 6I⁻(aq)
E°(I₂/I^-) = + 0.54 V and E°(Fe³⁺/Fe) = -0.036 V

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The equilibrium constant (K) for a redox reaction can be calculated using the Nernst equation:E°cell = E°red - E°oxidwhere E°cell is the standard cell potential, E°red is the standard reduction potential of the reduction half-reaction, and E°oxid is the standard oxidation potential of the oxidation half-reaction.In this case, the reduction half-reaction is:I₂(s) + 2e⁻ → 2I⁻(aq)and the oxidation half-reaction is:Fe(s) → Fe³⁺(aq) + 3e⁻The standard cell potential is:E°cell = E°red - E°oxid = 0.54 V - (-0.036 V) = 0.576 VThe equilibrium constant is related to the standard cell potential by the equation:K = e^(nE°cell/RT)where n is the number of electrons transferred in the balanced redox reaction, R is the gas constant (8.314 J/mol·K), and T is the temperature in Kelvin (298 K).In this case, n = 6, so:K = e^(6 * 0.576 V / (8.314 J/mol·K * 298 K)) = 2.4 × 10^58

Use the Tabulated Half-Cell Potentials to Calculate the Equilibrium Constant