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 & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.3: Effect Of Concentration On Reaction Rate
Problem 14.3CYU: The initial rate ( [NO]/ t] of the reaction of nitrogen monoxide and oxygen NO(g) + 2O2(g) NO2(g)...
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![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 is
k₁
1. O₂NNH₂(aq) — 0₂NNH¯(aq) + H+ (aq)
O₂NNH(aq) + H+ (aq) (fast equilibrium)
k-1
k₂
2. O₂NNH(aq) → N₂O(g) + OH(aq) (slow)
k3
3. 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?
k1
Answer Bank
k_1
k2
k3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1b99c910-aabd-4bff-9c76-8ab2f9147b49%2F4f272f36-6291-4534-8029-2458dec96b22%2Fol2m6fe_processed.png&w=3840&q=75)
Transcribed Image Text: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 is
k₁
1. O₂NNH₂(aq) — 0₂NNH¯(aq) + H+ (aq)
O₂NNH(aq) + H+ (aq) (fast equilibrium)
k-1
k₂
2. O₂NNH(aq) → N₂O(g) + OH(aq) (slow)
k3
3. 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?
k1
Answer Bank
k_1
k2
k3
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