In a study of the decomposition of nitrous oxide at 565 °C N₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x103 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t=0 s to t = 1.50×10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47×10³ s is (3) Based on these data, the rate constant for this 9.40x10-2 1.04x104 M-1 S-1 order reaction is M-1 S-1. M-1 S-1. s and when the starting

In a study of the decomposition of nitrous oxide at 565 °C N₂O(g) N₂(g) + ½ O₂(g) the following data were obtained: [N₂0], M seconds 0.750 0 0.375 1.50x103 0.188 4.47x10³ Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.750 M is concentration is 0.375 M is S. (2) The average A(1/[N₂0])/ At from t=0 s to t = 1.50×10³ s is The average A(1/[N₂0])/ At from t = 1.50x10³ s to t = 4.47×10³ s is (3) Based on these data, the rate constant for this 9.40x10-2 1.04x104 M-1 S-1 order reaction is M-1 S-1. M-1 S-1. s and when the starting

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 7P

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11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
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)?
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.
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Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. SO2Cl2(g)SO2(g)+Cl2(g)At a certain temperature, the half-life of SO2Cl2 is 7.5102 min. Consider a sealed flask with 122.0 g of SO2Cl2. (a) How long will it take to reduce the amount of SO2Cl2 in the sealed flask to 45.0 g? (b) If the decomposition is stopped after 29.0 h, what volume of Cl2 at 27C and 1.00 atm is produced?
Compare the functions of homogeneous and heterogeneous catalysts.
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.
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.
Hydrogen peroxide (H20i) decomposes into water and oxygen: H,O2(aq) — H,O(f) + ^O2(g) Ordinarily this reaction proceeds rather slowly, hut in the presence of some iodide ions (I-), the decomposition is much faster. Ihe decomposition in the presence of iodide was studied at 20°C, and the data were plotted in various ways. Use the graphs below to answer the questions that follow. What is the order of reaction for the decomposition of hydrogen peroxide? Find the numerical value of the rate constant at 20°C, including the correct units. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t = 0 in the graphs).
The reaction H2(g)+I2(g)2HI(g) may occur by the following mechanism: I2kk12I(fase,equilibrium)I+I+H2k22HI(slow) What rate law is predicted by this mechanism?