Chemistry

Chemistry

Problem

At 298\,K a particular reaction R has an equilibrium constant KR=1.2×10−4K_R = 1.2\times10^{-4}. Reaction S is produced by reversing reaction R and then doubling every stoichiometric coefficient. Which of the following correctly describes the sign of the standard Gibbs free energy change ΔGS∘\Delta G^{\circ}_{\text{S}} for reaction S? a) ΔGS∘>0\Delta G^{\circ}_{\text{S}} > 0 b) ΔGS∘<0\Delta G^{\circ}_{\text{S}} < 0 c) The sign of ΔGS∘\Delta G^{\circ}_{\text{S}} cannot be determined from the information provided. d) ΔGS∘=0\Delta G^{\circ}_{\text{S}} = 0

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