Chemistry

Chemistry

Problem

At 298 K, a particular reaction has an equilibrium constant of K=3.0×105K=3.0\times10^{5}. Which statement best describes the standard Gibbs free-energy change ΔG∘\Delta G^{\circ} for this reaction? a) ΔG∘\Delta G^{\circ} is large and positive (magnitude about 30  kJ mol−130\;\text{kJ mol}^{-1}). b) ΔG∘\Delta G^{\circ} is approximately zero (within ±3  kJ mol−1\pm 3\;\text{kJ mol}^{-1}). c) ΔG∘\Delta G^{\circ} is large and negative (magnitude about 30  kJ mol−130\;\text{kJ mol}^{-1}). d) ΔG∘\Delta G^{\circ} is moderately negative (between 00 and 20  kJ mol−120\;\text{kJ mol}^{-1} in magnitude).

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