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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 NO 3(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) [fast] NO2(g) + N2O5(g) → 3 NO2(g) + O(g) [slow] NO3(g) + O(g) → NO2(g) O2(g) [fast] IV 2 N2O5(g)=2 NO2(g) + N2O3(g) +3 O(g) [fast] N2O3(g) + O(g) 2 NO2(g) [slow] 2 O(g) → O2(g) [fast] V -> 2 N2O5(g) N4010(g) →> N4O10(g) 4 NO2(g) + O2(g) [slow] [fast] III IV none of the above

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 NO 3(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) [fast] NO2(g) + N2O5(g) → 3 NO2(g) + O(g) [slow] NO3(g) + O(g) → NO2(g) O2(g) [fast] IV 2 N2O5(g)=2 NO2(g) + N2O3(g) +3 O(g) [fast] N2O3(g) + O(g) 2 NO2(g) [slow] 2 O(g) → O2(g) [fast] V -> 2 N2O5(g) N4010(g) →> N4O10(g) 4 NO2(g) + O2(g) [slow] [fast] III IV none of the above

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 23QAP: For a reaction involving the decomposition of Z at a certain temperature, the following data are...
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The reaction and rate law for the gas-phase decomposition of dinitrogen pentaoxide are -> 2N2O5(g) 4NO2(g) + O2(g) Which of the following can be considered valid mechanisms for the reaction? rate = k[N205] I One-step collision II 2 N2O5(g) → 2 NO3(g) + 2 NO2(g) [slow] 2 NO3(g) → 2 NO2(g) +2 O(g) [fast] 2 O(g) → O2(g) [fast] III N2O5(g) NO3(g) + NO2(g) [fast] NO2(g) + N2O5(g) → 3 NO2(g) + O(g) [slow] NO3(g) + O(g) → NO2(g) O2(g) [fast] IV 2 N2O5(g) 2 NO2(g) + N2O3(g) +3 O(g) [fast] N2O3(g) + O(g) → 2 NO2(g) [slow] [fast] 2 O(g) → O2(g) -> V 2 N2O5(g) → N4010(g) N4O10(g) → 4 NO2(g) + O2(g) [slow] [fast] II III IV V none of the above
Transcribed Image Text:The reaction and rate law for the gas-phase decomposition of dinitrogen pentaoxide are -> 2N2O5(g) 4NO2(g) + O2(g) Which of the following can be considered valid mechanisms for the reaction? rate = k[N205] I One-step collision II 2 N2O5(g) → 2 NO3(g) + 2 NO2(g) [slow] 2 NO3(g) → 2 NO2(g) +2 O(g) [fast] 2 O(g) → O2(g) [fast] III N2O5(g) NO3(g) + NO2(g) [fast] NO2(g) + N2O5(g) → 3 NO2(g) + O(g) [slow] NO3(g) + O(g) → NO2(g) O2(g) [fast] IV 2 N2O5(g) 2 NO2(g) + N2O3(g) +3 O(g) [fast] N2O3(g) + O(g) → 2 NO2(g) [slow] [fast] 2 O(g) → O2(g) -> V 2 N2O5(g) → N4010(g) N4O10(g) → 4 NO2(g) + O2(g) [slow] [fast] II III IV V none of the above
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