Chemistry

Chemistry

Problem

The table lists standard entropy changes for four gas-phase reactions carried out at 298 K. (1) 2  SO2(g)+O2(g)→2  SO3(g)2\;\text{SO}_2(g)+\text{O}_2(g)\rightarrow 2\;\text{SO}_3(g) ΔS∘=−188  J mol−1 K−1\Delta S^{\circ}=-188\;\text{J mol}^{-1}\,\text{K}^{-1} (2) N2O4(g)→2  NO2(g)\text{N}_2\text{O}_4(g)\rightarrow 2\;\text{NO}_2(g) ΔS∘=+176  J mol−1 K−1\Delta S^{\circ}=+176\;\text{J mol}^{-1}\,\text{K}^{-1} (3) H2O(l)→H2O(g)\text{H}_2\text{O}(l)\rightarrow \text{H}_2\text{O}(g) ΔS∘=+109  J mol−1 K−1\Delta S^{\circ}=+109\;\text{J mol}^{-1}\,\text{K}^{-1} (4) 2  NO(g)+O2(g)→2  NO2(g)2\;\text{NO}(g)+\text{O}_2(g)\rightarrow 2\;\text{NO}_2(g) ΔS∘=−146  J mol−1 K−1\Delta S^{\circ}=-146\;\text{J mol}^{-1}\,\text{K}^{-1} Which reaction best illustrates that an increase in the number of gas molecules can lead to a large positive ΔS∘\Delta S^{\circ}? a) Reaction 1 b) Reaction 3 c) Reaction 2 d) Reaction 4

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