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: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.94QE

See similar textbooks

Similar questions

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
Assuming that the mechanism for the hydrogenation of C2H4 given in Section 11-7 is correct, would you predict that the product of the reaction of C2H4. with D2 would be CH2DCH2D or CHD2CH3? How could the reaction of C2H4 with D2 be used to confirm the mechanism for the hydrogenation of C2H4 given in Section 11-7?
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
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.