Chemistry

Chemistry

Problem

Standard entropy changes for four reactions at 298 K are shown. A. 2  CO(g)+O2(g)→2  CO2(g)2\;\text{CO}(g)+\text{O}_2(g)\rightarrow 2\;\text{CO}_2(g) ΔS∘=−173  J mol−1 K−1\Delta S^{\circ}=-173\;\text{J mol}^{-1}\,\text{K}^{-1} B. 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} C. H2(g)+F2(g)→2  HF(g)\text{H}_2(g)+\text{F}_2(g)\rightarrow 2\;\text{HF}(g) ΔS∘=−186  J mol−1 K−1\Delta S^{\circ}=-186\;\text{J mol}^{-1}\,\text{K}^{-1} D. 2  H2O2(l)→2  H2O(l)+O2(g)2\;\text{H}_2\text{O}_2(l)\rightarrow 2\;\text{H}_2\text{O}(l)+\text{O}_2(g) ΔS∘=+70  J mol−1 K−1\Delta S^{\circ}=+70\;\text{J mol}^{-1}\,\text{K}^{-1} If two of these reactions occur sequentially, which pairing would result in an overall ΔS∘\Delta S^{\circ} closest to zero? a) B + C b) C + D c) A + B d) A + D

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