Decomposition of ozone to oxygen occurs as a series of radical reactions. The Individual reactions in this series are listed below but they are not in the correct order. Use the labels on the right to correct the order of the reactions. 1st 3rd 5th 2nd 4th CIOO Cl• + 0₂ - 2 Cl. +203->> CIOOCI CI F-C-Cl F UV photon 2 CIQ. +20₂ ►CIOO + Cl CI 1 F-C+Cl UV photon A 220 nm 2 CIO- -CIOOCI F

Decomposition of ozone to oxygen occurs as a series of radical reactions. The Individual reactions in this series are listed below but they are not in the correct order. Use the labels on the right to correct the order of the reactions. 1st 3rd 5th 2nd 4th CIOO Cl• + 0₂ - 2 Cl. +203->> CIOOCI CI F-C-Cl F UV photon 2 CIQ. +20₂ ►CIOO + Cl CI 1 F-C+Cl UV photon A 220 nm 2 CIO- -CIOOCI F

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 41E: The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was...

See similar textbooks

Similar questions

The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
11.93 On a particular day, the ozone level in Milwaukee exceeded the EPAs 1-hour standard of 0.12 ppin by 10 ppb. How many ozone molecules would be present in 1 liter of air at the detection site?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 4.00 105 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 102 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 102 M C2H5OH to decompose?
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
11. The lifetime of the VOC called glyoxal in the atmosphere is controlled by its reaction with the OH radical and photolysis. The rate constants for these reactions have been measured as kos=3.7x 10* cm molecules'and ka =12 min". What would the overall lifetime of glyoxal under these conditions with an [OH] =1.6x 10 molecule cm.
3. The decomposition of N2O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO2 (g) + O2(g) The following results were collected: find nature) N2O5] 0.1000 Ln[N2O5] -2.30 2.65 2.99 -3.69 -4.38 -5.08 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Time (s) 10g. (LN) 0.0707 0.0500 50 0.0250 100 0.0125 200 0.00625 300 400 Ln[N2O5] versus time. Determine the value of k. Which graph did you use? graph *b. On your graph of [N2O5] versus time, highlight the times it takes for each halving of the reactant concentration. What is the half-life? Using this half-life calculate k. design experiments to find the activation energy,
но HO Но HO co + ½ 0, - + H,O H" H но Он ascorbic acid dehydroascorbic acid Vitamin C is oxidized slowly to dehydroascorbic acid by the oxygen in air. It is catalyzed by ions such as Cu*2 and Fe*3. The reaction can be followed by measuring the ultraviolet absorbance at 243 nm. Time (hours) Absorbance (A) 1/A In A - In A 0.75 1.3 -0.29 0.29 1 0.38 2.6 -0.97 0.97 0.19 5.3 - 1.7 1.7 3 0.095 11 - 2.4 2.4 27. Which of the following is the best interpretation of the data given above? (A) The data support a zero-order reaction. (B) The data support a first-order reaction. (C) The data support a second-order reaction. (D) The overall order is third. 28. A new compound is synthesized and found to be a monoprotic acid with a molar mass of 248 g/mole. When 0.0050 moles of this acid are dissolved in 0.500L of water, the pH is measured as 2.94. What is the pk, of this acid? (A) (В) (C) (D) 2.33 3.89 5.78 7.78 29. What is the hybridization of carbon 1 (far left) and carbon 2 (middle) in this…