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)

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...

See similar textbooks

Similar questions

The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
(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?
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
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?
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
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 thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.