Chemistry

Chemistry

Problem

The overall reaction 2 NO(g)+O2(g)→2 NO2(g)2\,\text{NO}(g)+\text{O}_{2}(g)\rightarrow2\,\text{NO}_{2}(g) obeys the experimental rate law rate=k[NO]2[O2]\text{rate}=k[\text{NO}]^{2}[\text{O}_{2}]. Four mechanisms are proposed. A. Slow: 2 NO+O2→2 NO22\,\text{NO}+\text{O}_{2}\rightarrow2\,\text{NO}_{2} (termolecular) B. Fast equilibrium: NO+NO⇌N2O2\text{NO}+\text{NO}\rightleftharpoons\text{N}_{2}\text{O}_{2} Slow: N2O2+O2→2 NO2\text{N}_{2}\text{O}_{2}+\text{O}_{2}\rightarrow2\,\text{NO}_{2} (bimolecular) C. Slow: NO+O2→NO3\text{NO}+\text{O}_{2}\rightarrow\text{NO}_{3} Fast: NO+NO3→2 NO2\text{NO}+\text{NO}_{3}\rightarrow2\,\text{NO}_{2} D. Slow: NO+NO2→N2O3\text{NO}+\text{NO}_{2}\rightarrow\text{N}_{2}\text{O}_{3} Fast: N2O3+O2→2 NO2\text{N}_{2}\text{O}_{3}+\text{O}_{2}\rightarrow2\,\text{NO}_{2} Which mechanism is MOST consistent with both the observed rate law and the relative rarity of simultaneous three-body collisions? a) Mechanism D b) Mechanism B c) Mechanism A d) Mechanism C

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