>Question 6 of 20Attempt 4The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate lawO₂NNH₂ (aq) → N₂O(g) + H₂O(1)rate k[0, NNH,][H+]A proposed mechanism for this reaction isk₁1.0₂NNH₂ (aq) O₂NNH(aq) + H+ (aq)(fast equilibrium)k_1k₂2.0₂NNH(aq) →N₂O(g) + OH(aq) (slow).k33. H+ (aq) + OH(aq) + H₂O(l) (fast)What is the relationship between the observed value of k and the rate constants for the individual steps of the mechanism?Answer Bankk =k₂k₂k=1kıQuestion Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books ▾8:68°F0³»cill4:07 PM6/2/2022O

We have to determine the correct relation for k

The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) - N₂O(g) + H₂O(1) rate k [O,NNH,] [H+] A proposed mechanism for this reaction is k₁ 1.0₂NNH₂ (aq) = O₂NNH(aq) + H+ (aq) (fast equilibrium) k_1 k₂ - 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow). k3 3. H+ (aq) + OH(aq) - -> H₂O(1) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mecha Answer Bank k = k₂ ki k3 k_1

The decomposition of nitramide, O₂NNH₂, in water has the chemical equation and rate law O₂NNH₂(aq) - N₂O(g) + H₂O(1) rate k [O,NNH,] [H+] A proposed mechanism for this reaction is k₁ 1.0₂NNH₂ (aq) = O₂NNH(aq) + H+ (aq) (fast equilibrium) k_1 k₂ - 2.0₂NNH(aq) → N₂O(g) + OH(aq) (slow). k3 3. H+ (aq) + OH(aq) - -> H₂O(1) (fast) What is the relationship between the observed value of k and the rate constants for the individual steps of the mecha Answer Bank k = k₂ ki k3 k_1

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 39QAP: The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction,...

See similar textbooks

Similar questions

Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
What is the difference between average rate, initial rate, and instantaneous rate?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved in chloroform, CHCI3, is 6.2104 min-1. 2N2O54NO2+O2 What is the rate of the reaction when [N2O5] = 0.40 M?
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?