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Solution: The overall equation and rate law for the gas-phase decomposition of dinitrogen pentoxide are2 N2O5(g) ⟶ 4 NO2(g) + O 2(g)               rate = k[N  2O5]Which of the following can be considered valid mechanisms for the reaction?I – One-step collisionII – 2 N 2O5(g) ⟶ 2 NO 3(g) + 2 NO 2(g)     [slow]      2 NO 3(g) ⟶ 2 NO 2(g) + 2 O (g)     [fast]               2 O  (g) ⟶ O 2(g)      [fast]III – N 2O5(g) ⇌ NO 3(g) + NO 2(g)     [fast]       NO 2(g) + N 2O5(g) ⟶ 3 NO 2(g) + O(g)     [slow]                 NO 3(g) + O(g) ⟶ NO2(g) + O2(g)     [fast]IV – 2 N 2O5(g) ⇌ 2 NO 2(g) + N2O3(g) + 3 O (g)     [fast]        N 2O3(g) + O(g) ⟶ 2 NO 2(g)     [slow]        2 O (g) ⟶ O 2(g)     [fast]V – 2 N2O5(g) ⟶ N4O10(g)               [slow]       N 4O10(g) ⟶ 4 NO2(g) + O 2(g)     [fast]

Problem

The overall equation and rate law for the gas-phase decomposition of dinitrogen pentoxide are

2 N2O5(g) ⟶ 4 NO2(g) + O 2(g)               rate = k[N  2O5]

Which of the following can be considered valid mechanisms for the reaction?

I – One-step collision

II – 2 N 2O5(g) ⟶ 2 NO 3(g) + 2 NO 2(g)     [slow]

      2 NO 3(g) ⟶ 2 NO 2(g) + 2 O (g)     [fast]

               2 O  (g) ⟶ O 2(g)      [fast]

III – N 2O5(g) ⇌ NO 3(g) + NO 2(g)     [fast]

       NO 2(g) + N 2O5(g) ⟶ 3 NO 2(g) + O(g)     [slow]

                 NO 3(g) + O(g) ⟶ NO2(g) + O2(g)     [fast]

IV – 2 N 2O5(g) ⇌ 2 NO 2(g) + N2O3(g) + 3 O (g)     [fast]

        N 2O3(g) + O(g) ⟶ 2 NO 2(g)     [slow]

        2 O (g) ⟶ O 2(g)     [fast]

V – 2 N2O5(g) ⟶ N4O10(g)               [slow]

       N 4O10(g) ⟶ 4 NO2(g) + O 2(g)     [fast]