Chemistry

Chemistry

Problem

Identify the correct description for a redox reaction with a positive standard electrode potential: ΔG⊖=−nFE⊖\Delta G^\ominus = -nFE^\ominus and ΔG⊖=−RTln⁡K\Delta G^\ominus = -RT \ln K a. ΔG⊖\Delta G^\ominus is negative and KK is less than 1. b. ΔG⊖\Delta G^\ominus is negative and KK is greater than 1. c. ΔG⊖\Delta G^\ominus is positive and KK is less than 1. d. ΔG⊖\Delta G^\ominus is positive and KK is greater than 1.
Intuitive explanation

A positive standard electrode potential (E°E°) means the reaction is thermodynamically favorable and will proceed spontaneously under standard conditions. The key insight is that E°>0E° > 0 makes ΔG°\Delta G° negative (since ΔG°=−nFE°\Delta G° = -nFE°), which corresponds to a large equilibrium constant KK — the reaction strongly favors products. This connection between electrode potential, free energy, and equilibrium tells you that spontaneous redox reactions are those that "want" to happen because they release energy.

Intuitive explanation

A positive standard electrode potential (E°E°) means the reaction is thermodynamically favorable and will proceed spontaneously under standard conditions. The key insight is that E°>0E° > 0 makes ΔG°\Delta G° negative (since ΔG°=−nFE°\Delta G° = -nFE°), which corresponds to a large equilibrium constant KK — the reaction strongly favors products. This connection between electrode potential, free energy, and equilibrium tells you that spontaneous redox reactions are those that "want" to happen because they release energy.

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