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please show work and explain the problem The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) N₂O(g) + H₂O(1) 10₂NNH₂] [H+] A proposed mechanism for this reaction is ki 1.0, NNH₂ (aq) O₂NNH (aq) + H+ (aq) (fast equilibrium) k.1 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(l) (fast) k= rate = k What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism k₁ k₂ Answer Bank ki

please show work and explain the problem The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) N₂O(g) + H₂O(1) 10₂NNH₂] [H+] A proposed mechanism for this reaction is ki 1.0, NNH₂ (aq) O₂NNH (aq) + H+ (aq) (fast equilibrium) k.1 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(l) (fast) k= rate = k What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism k₁ k₂ Answer Bank ki

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...
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please show work and explain the problem The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) N₂O(g) + H₂O(1) [O₂NNH₂] [H+] A proposed mechanism for this reaction is ki 1.0₂NNH₂ (aq) O₂NNH (aq) + H+ (aq) (fast equilibrium) k.1 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(l) (fast) k= rate = k What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k₁ k₂ Answer Bank ki
Transcribed Image Text:please show work and explain the problem The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) N₂O(g) + H₂O(1) [O₂NNH₂] [H+] A proposed mechanism for this reaction is ki 1.0₂NNH₂ (aq) O₂NNH (aq) + H+ (aq) (fast equilibrium) k.1 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow) 3. H* (aq) + OH-(aq) → H₂O(l) (fast) k= rate = k What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism? k₁ k₂ Answer Bank ki
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