The reaction and rate law for the gas-phase decomposition of dinitrogen pentaoxide are 2N2O5(g) → 4NO2(g) + O2(g) rate = k[N2O5] Which of the following can be considered valid mechanisms for the reaction? I One-step collision II 2 N2O5(g) → 2 NO3(g) + 2 NO2(g) 2 NO3(g) → 2 NO2(g) + 2 O(g) 2 O(g) → O2(g) [slow] [fast] [fast] III N2O5(g) ⇌ NO3(g) + NO2(g) NO2(g) + N2O5(g) → 3 NO2(g) + O(g) NO3(g) + O(g) → NO2(g) O2(g) [fast] [slow] [fast] IV 2 N2O5(g) ⇌ 2 NO2(g) + N2O3(g) + 3 O(g) N2O3(g) + O(g) → 2 NO2(g) 2 O(g) → O2(g) [fast] [slow] [fast] V 2 N2O5(g) → N4O10(g) N4O10(g) → 4 NO2(g) + O2(g) [slow] [fast]