5. The overall reaction for the oxidation of NO to NO₂ is: 2NO(g) + O₂(g) → 2NO₂(g) The reaction proceeds by the following mechanism: NO + NO → N₂O₂ N₂O₂ → NO + NO N2O2 + O2 → NO₂ + NO₂ ka k'a kb (a) Verify that application of the steady-state approximation to the intermediate, N₂O2, results in the rate law: d[NO₂] 2kak [NO]²[0₂] dt ka + kb [0₂] (b) Show how the rate law simplifies (i) [0₂] is very large, and (ii) if [0₂] is very small. (c) Why might it be important to recognize how the rate law simplifies under the conditions of very large or very small [0₂]?

5. The overall reaction for the oxidation of NO to NO₂ is: 2NO(g) + O₂(g) → 2NO₂(g) The reaction proceeds by the following mechanism: NO + NO → N₂O₂ N₂O₂ → NO + NO N2O2 + O2 → NO₂ + NO₂ ka k'a kb (a) Verify that application of the steady-state approximation to the intermediate, N₂O2, results in the rate law: d[NO₂] 2kak [NO]²[0₂] dt ka + kb [0₂] (b) Show how the rate law simplifies (i) [0₂] is very large, and (ii) if [0₂] is very small. (c) Why might it be important to recognize how the rate law simplifies under the conditions of very large or very small [0₂]?

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...

See similar textbooks

Similar questions

For the overall gas-phase reaction of the formation of phosgene (Cl₂CO) from carbon monoxide and chlorine, the following mechanism has been proposed: Cl₂ + M2CI+M k_1 CI+CO+MCICO + M k_2 k3 CICO + Cl₂C₁₂CO+CI Derive the expected rate law assuming [M] is large and constant, and using: (a) The equilibrium assumption for the first two steps. (b) Instead using the steady state assumption for any intermediates. (c) Why does the reaction become zeroth order in [CO] in the steady state case? (d) The actual rate law is 3/2 order in [Cl₂] and first order in [CO]. Which mechanism is likely correct? (e) Is the other mechanism possible, based on the observed orders?
The rate law for the oxidation reaction 2CO(g) + O2(g) → 2CO2(g) assuming that the reaction occurs by the Langmuir -Hinshelwood mechanism. The over-all rate law for this mechanism is Rate = k3θCOθO2 ΘO2 = (KO2 [O2])1/2 and ΘCO = KCO [CO] --------------------------------- --------------------------------- 1+ (KO2[O2])1/2 + KCO[CO] 1+ (KO2[O2])1/2 + KCO[CO]
For an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 1
The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
Give a reaction rate for the provided mechanism and do not include the intermediates in the final equation. 1. For the spontaneous reaction in water: Re(HzO)z + 2 KCN →Re(CN)z2 + 2K*(aq) + 2 H2O The postulate mechanism is where all species are in aqueous phase k1 Re(H₂O)2 + CN- Re(H₂O)(CN) + H₂O equilibrium Re(H₂O)(CN) + CN-I2 Re(H₂O)(CN)2-² Re(H2O)(CN)2243 Re(CN)22 + H2O k2 slow fast
In a study of the rearrangement of cyclopropane to propene at 500 °C (CH₂)3 CH3CH=CH₂ the concentration of (CH₂)3 was followed as a function of time. It was found that a graph of In[(CH₂)3] versus time in seconds gave a straight line with a slope of -9.38×104 s¹ and a y-intercept of -2.02. Based on this plot, the reaction is order in (CH₂)3 and the rate constant for the reaction is
It has been proposed that the gas NO2C1 decomposes by the mechanism: NO2CI(g) kı NO2(g) + Cl(g) NO2CI(g) + Cl(g) k2 NO2(g) + Cl2(g) Apply the Steady State Approximation to derive an expression for the concentration of the intermediate, Cl(g). Show your working out. States not required.
Determine the rate law of the over all reaction from the mechanism and determine the intermediates in this mechanism
For the gas phase decomposition of 1-chloropropane, CH;CH,CH,CICH;CH=CH, + HC1 the rate constant in s' has been determined at several temperatures. When In k is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.77x10ʻ K and a y-intercept of 31.0. The value of the rate constant for the gas phase decomposition of l-chloropropane at 708 K is (Enter your answer to one significant figure.)
6. To observe the effect of temperature on reaction rate, the reaction between MnO, ag) and C204(ag) in acidic media is performed according to the given redox reaction: 2 MnO4 (aq) + 16 H*(aq) + 5 C204²(aq) → 10 CO2(g) + 2 Mn²"(aq) + 8 H2O(1) At various temperatures, the rate constants were determined experimentally as follows: k (M s') 5.03x105 T (°C) 20 35 3.68×104 60 6.71×103 90 0.119 (a) Determine Ea for this reaction by a graphical method (see the graph given below). (b) Determine E. using Arrhenius equation using tabulated data. (c) Calculate the value of the rate constant, k at 100°C. -2 -4 兰 -6 -8 -10 -12 0.0025 0.0027 0.0029 0.0031 0.0033 0,0035 1/T (K)
Please and thank you ?