a) The reaction of NO2 has been studied as a function of temperature. For the following decompositionreactions, the rate constant is 2.7 × 10-2M-'s-1 at 227 °C and 2.4 x 10-1M-1s-1 at 305 °C.9.2 NO2 → 2 N0 + 02Calculate the activation energy for this reaction.9.b) Nitrogen oxide converts ozone into molecular oxygen as follows:Оз + NO -> 02 + NO2The experimental rate law is: Rate = k[03][NO]. Show which of the followingmechanism/mechanisms are consistent with the experimental rate law.Mechanism 1:03 + NO → 02 + NO3(slow)0 + 03 → 2 02(fast)NO3 + NO → 2 NO2(fast)Mechanism 2:032 02 + 0(fast)NO +0 → N02(slow)Mechanism 3:03 + NO → 02 + NO2(slow)

Minimum energy required for reacting species to react to form products

a) The reaction of NO2 has been studied as a function of temperature. For the following decomposition reactions, the rate constant is 2.7 × 10-2M-1s-1 at 227 °C and 2.4 x 10-1M-1s-1 at 305 °C. 9. 2 NO2 → 2 NO + 02 Calculate the activation energy for this reaction. 9. b) Nitrogen oxide converts ozone into molecular oxygen as follows: 03 + NO → 02 + NO2 k[03][NO]. Show which of the following The experimental rate law is: Rate = mechanism/mechanisms are consistent with the experimental rate law. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 03 = 02 + 0 (fast) NO + 0 → N02 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)

a) The reaction of NO2 has been studied as a function of temperature. For the following decomposition reactions, the rate constant is 2.7 × 10-2M-1s-1 at 227 °C and 2.4 x 10-1M-1s-1 at 305 °C. 9. 2 NO2 → 2 NO + 02 Calculate the activation energy for this reaction. 9. b) Nitrogen oxide converts ozone into molecular oxygen as follows: 03 + NO → 02 + NO2 k[03][NO]. Show which of the following The experimental rate law is: Rate = mechanism/mechanisms are consistent with the experimental rate law. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 03 = 02 + 0 (fast) NO + 0 → N02 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 108CP: The decomposition of NO2(g) occurs by the following bimolecular elementary reaction:...

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11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
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.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
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)?
(Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a 10-K rise in temperature increases the reaction rate by two to four times. Use an average increase of three times to answer the questions below. (a) What is the approximate activation energy of a typical chemical reaction at 298 K? (b) If a catalyst increases a chemical reactions rate by providing a mechanism that has a lower activation energy, then what change do you expect a 10-K increase in temperature to make in the rate of a reaction whose uncatalyzed activation energy of 75 kJ/mol has been lowered to one half this value (at 298 K) by addition of a catalyst?
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
The decomposition of NO2(g) occurs by the following bimolecular elementary reaction: 2NO2(g)2NO(g)+O2(g) The rate constant at 273 K is 2.3 1012 L/mol s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 2.5 atm to 1.5 atm at 500. K? Assume ideal gas behavior.
In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were obtained: Initial Concentration of Azomethane Initial Rate Exp. 1 1.13 102 M 2.8 106 M/s Exp. 2 2.26 102 M 5.6 106 M/s What is the rate law? What is the value of the rate constant?

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