A reaction, 2NO (g) + O2 (g) → 2NO, (g), was run in a laboratory setting. Given the following plausible mechanism, answer the following questions: Step 1: NO (g) + NO (g) N,02 (g) (fast) Step 2: N,O2 (g) + O2 (g) 2NO, (g) (slow) (i) Determine the rate law for the above reaction. (ii) Identify the reaction intermediates. If the speeds of the elementary steps were switched (i.e. elementary step 1 was slow and step 2 was fast), could this reaction mechanism still be plausible? Explain your (ii) answer.

A reaction, 2NO (g) + O2 (g) → 2NO, (g), was run in a laboratory setting. Given the following plausible mechanism, answer the following questions: Step 1: NO (g) + NO (g) N,02 (g) (fast) Step 2: N,O2 (g) + O2 (g) 2NO, (g) (slow) (i) Determine the rate law for the above reaction. (ii) Identify the reaction intermediates. If the speeds of the elementary steps were switched (i.e. elementary step 1 was slow and step 2 was fast), could this reaction mechanism still be plausible? Explain your (ii) answer.

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 23QAP: For a reaction involving the decomposition of Z at a certain temperature, the following data are...

See similar textbooks

Similar questions

Express the rate of the reaction 2N2O(g)2N2(g)+O2(g) in terms of (b) [ N2O ] (a) [ O2 ]
For the reaction A+BC, explain at least two ways in which the rate law could be zero order in chemical A.
Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine: 2 NO2(g) + F2(g) → 2 NO2F(g) Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table: Write the rate law for the reaction. Determine what the order of the reaction is with respect to each reactant and each product. Calculate the rate constant k and express it in appropriate units.
What is the difference between average rate, initial rate, and instantaneous rate?
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.
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)?
Why does a catalyst increase the rate of a reaction? What is the difference between a homogeneous catalyst and a heterogeneous catalyst? Would a given reaction necessarily have the same rate law for both a catalyzed and an uncatalyzed pathway? Explain.
For a reaction involving the decomposition of Z at a certain temperature, the following data are obtained: (a) What is the order of the reaction? (b) Write the rate expression for the decomposition of Z. (c) Calculate k for the decomposition at that temperature.
For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
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?
A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
A reaction has two reactants Q and P. What is the order with respect to each reactant and the overall order of the reaction described by the following rate expressions? (a) rate=k1(b) rate=k2[ P ]2[ Q ] (c) rate=k3[ Q ]2 (d) rate=k4[ P ][ Q ]