13.54 The rate law for the reaction2H₂(g) + 2NO(g)N₂(g) + 2H₂O(g)is rate = k[H₂][NO]. Which of the following mech-anisms can be ruled out on the basis of the observedrate expression?Mechanism IH₂ + NO→→→→→→ H₂O + NN + NON₂ + OO + H₂H₂OMechanism IIH₂ + 2NO→→→N₂O + H₂ON₂O + H₂N₂ + H₂OMechanism III2NO=N₂0₂N₂O₂ + H₂N₂O + H₂ON₂O + H₂ →→N₂ + H₂O(slow)(fast)(fast)(slow)(fast)(fast equilibrium)(slow)(fast)

Here Given that, Reaction :2H2g + 2NO g →N2g + 2H2O gRate Law :Rate = k. H2NO2

4 The rate law for the reaction 2H₂(g) + 2NO(g) N₂(g) + 2H₂O(g) is rate = k[H₂][NO]. Which of the following mech- anisms can be ruled out on the basis of the observed rate expression? Mechanism I H₂ + NO N + NO O + H₂ H₂O + N N₂ + O H₂O Mechanism II H₂ + 2NON₂O + H₂O N₂O + H₂N₂ + H₂O Mechanism III 2NO-N₂0₂ N₂O₂ + H₂N₂O + H₂O N₂O + H₂ →→→→N₂ + H₂O (slow) (fast) (fast) (slow) (fast) (fast equilibrium) (slow) (fast)

4 The rate law for the reaction 2H₂(g) + 2NO(g) N₂(g) + 2H₂O(g) is rate = k[H₂][NO]. Which of the following mech- anisms can be ruled out on the basis of the observed rate expression? Mechanism I H₂ + NO N + NO O + H₂ H₂O + N N₂ + O H₂O Mechanism II H₂ + 2NON₂O + H₂O N₂O + H₂N₂ + H₂O Mechanism III 2NO-N₂0₂ N₂O₂ + H₂N₂O + H₂O N₂O + H₂ →→→→N₂ + H₂O (slow) (fast) (fast) (slow) (fast) (fast equilibrium) (slow) (fast)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The overall reaction 2 NO (g) + O2 (g) → 2 NO2 (g) is believed to take place in the following steps: 2 NO (g) N2O2 (g) (fast) N2O2 (g) + O2 (g) → 2 NO2 (g) (slow) Obtain a rate expression that corresponds to this proposed mechanism.
2 NO (g) + O₂ (g) --> 2 NO2 (g) The proposed mechanism for the reaction above is 1) NO (g) + NO (g) --> N₂O2(g) 2) N₂O2 (g) + O2 (g) --> 2 NO2 (g) Write the rate law for the mechanism if the first step is fast and the second step is slow.
One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)
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Consider the following reaction for chlorine reacting with chloroform, Cl2 (g) + CHCIl3 (g) HС (g) + СCla (g) a) based on the initial rate data provided (in the table below), determine the rate law for this reaction. b) The following is a proposed mechanism for this reaction. Cl2 (g) = 2 CI (g) CI (g) + CHCI: (g) → HCI (g) + CCl: (g) (slow) CCl: (g) + CI (g) > Сle (g) (fast equilibrium) (fast) Is this an acceptable mechanism based on the rate law you determined in part a? answer should be Yes/No to "is this an acceptable mechanism") Initial Rate [CI,] [CHCI3] 0.00253 | 0.2 0.3 A) Yes 0.00759 0.2 0.9 B) No 0.00506 0.8 0.3
1. The mechanism of a certain non-elementary reaction is given below: (1) NO2Cl = NO2 + Cl k1, k-1 (2) Cl + NO2Cl → NO2 + Cl2 k2 derive (a) Using the steady-state approximation, the differential rate law for the formation of molecular chlorine, Cl2, as a function of time on the basis of the above mechanism.
17. The following overall reaction has a second order rate law as determined by experiment: H₂(g) + 21C1(g) → 12(g) + 2HCl(g) Rate = k[H₂][ICI] Propose a mechanism that is consistent with the experimentally determined rate law.
The decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)–N20(g) + H20(1) is first order in NH,NO2 with a rate constant of 0.0000470 s1. If the initial concentration of NH2NO2 is 0.548 M, the concentration of NH2NO2 will be 0.0986 M after s have passed.
Nn.77. Subject :- Chemistry
The decomposition of nitramide in aqueous solution at 25 °CNH2NO2(aq)N2O(g) + H2O(l)is first order in NH2NO2.During one experiment it was found that when the initial concentration of NH2NO2 was 0.886 M, the concentration of NH2NO2 dropped to 0.103 M after 30353 s had passed.Based on this experiment, the rate constant for the reaction is s-1.
The gas-phase reaction 2NO2Br →2NO2 + Br2 has r = k[NO2Br]. Devise a mechanism consistent with this rate law.
The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °CN2O52 NO2 + ½ O2is first order in N2O5.During one experiment it was found that when the initial concentration of N2O5 was 1.04 M, the concentration of N2O5 dropped to 0.309 M after 210 min had passed.Based on this experiment, the rate constant for the reaction is min-1.