The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law[O₂NNH₂][H+]O₂NNH₂ (aq) →→→ N₂O(g) + H₂O(1)A proposed mechanism for this reaction isk₁1. O₂NNH₂(aq) — 0₂NNH¯(aq) + H+ (aq)O₂NNH(aq) + H+ (aq) (fast equilibrium)k-1k₂2. O₂NNH(aq) → N₂O(g) + OH(aq) (slow)k33. H+ (aq) + OH(aq) → H₂O(l) (fast)rate =k =k.What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?k1Answer Bankk_1k2k3

Overall reaction : O2NNH2(aq) → N2O(g) +H2O(I) Rate : r= k [O2NNH2][H+]

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 k₁ 1. O₂NNH₂ (aq) = O₂NNH(aq) + H+ (aq) (fast equilibrium) k_1 k₂ 2. O₂NNH¯(aq) +² N₂O(g) + OH¯(aq) (slow) 3. H+ (aq) + OH-(aq) rate = k k3 H₂O(1) (fast)

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 k₁ 1. O₂NNH₂ (aq) = O₂NNH(aq) + H+ (aq) (fast equilibrium) k_1 k₂ 2. O₂NNH¯(aq) +² N₂O(g) + OH¯(aq) (slow) 3. H+ (aq) + OH-(aq) rate = k k3 H₂O(1) (fast)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.7: Reaction Mechanisms

Problem 11.12E

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