Chemistry

Chemistry

Problem

At 310 K, a redox reaction involving n = 1 electron has a standard cell potential of +0.41 V. Using R = 8.314 J·mol⁻¹·K⁻¹ and F = 9.65 × 10⁴ C·mol⁻¹, determine the equilibrium constant K for this reaction at 310 K. Give your answer in scientific notation to two significant figures.
Intuitive explanation

The key is connecting cell potential to thermodynamic favorability through the Nernst equation at equilibrium. When a reaction reaches equilibrium, the cell potential becomes zero, which means all the driving force has been "used up"—that's where ΔG°\Delta G° and KK come in. Use the relationship ΔG°=–nFE°\Delta G° = –nFE° to find the standard free energy, then apply ΔG°=–RTln⁡K\Delta G° = –RT\ln K to extract the equilibrium constant. This bridges electrochemistry and equilibrium in one elegant step.

Intuitive explanation

The key is connecting cell potential to thermodynamic favorability through the Nernst equation at equilibrium. When a reaction reaches equilibrium, the cell potential becomes zero, which means all the driving force has been "used up"—that's where ΔG°\Delta G° and KK come in. Use the relationship ΔG°=–nFE°\Delta G° = –nFE° to find the standard free energy, then apply ΔG°=–RTln⁡K\Delta G° = –RT\ln K to extract the equilibrium constant. This bridges electrochemistry and equilibrium in one elegant step.

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