Chemistry

Chemistry

Problem

Three gaseous reactions are carried out at 298\,K under standard-state conditions. Standard molar free-energy changes are given below. I. N2O4(g)→2 NO2(g)\text{N}_2\text{O}_4(g) \rightarrow 2\,\text{NO}_2(g) ; ΔG∘=+5.3 kJ mol−1\Delta G^{\circ}=+5.3\,\text{kJ\,mol}^{-1} II. NH4+(aq)+OH−(aq)→NH3(aq)+H2O(l)\text{NH}_4^{+}(aq)+\text{OH}^{-}(aq) \rightarrow \text{NH}_3(aq)+\text{H}_2\text{O}(l) ; ΔG∘=−9.2 kJ mol−1\Delta G^{\circ}=-9.2\,\text{kJ\,mol}^{-1} III. 2 SO2(g)+12 O2(g)→SO3(g)2\,\text{SO}_2(g)+\tfrac12\,\text{O}_2(g) \rightarrow \text{SO}_3(g) ; ΔG∘=−142 kJ mol−1\Delta G^{\circ}=-142\,\text{kJ\,mol}^{-1} Use these data to analyze how the position of equilibrium differs among the three reactions. (a) List the three reactions in order of decreasing equilibrium constant KK (largest KK first). (b) Provide a concise justification for your ranking that references both the sign and the magnitude of the given ΔG∘\Delta G^{\circ} values. (c) Identify which reaction’s equilibrium lies farthest toward reactants and explain how the numerical value of ΔG∘\Delta G^{\circ} supports that conclusion.

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