For questions 1. to 5.The following data were collected from the reaction of:A + B+CPRODUCTS[A] (M)[B] (M)[C] (M)Initial Rate M/sec0.100.100.100.0200.200.200.200.1600.400.200.400.6400.400.400.801.2801. What is the order of the reaction with respect to [A]?(A) 0(В) 1(C) 2(D) 32. What is the order of the reaction with respect to [B]?(A) 0(В) 1(C) 2(D) 33. What is the order of the reaction with respect to [C]?(A) 0(В) 1(С) 2(D) 34. What is the rate law of this reaction?(A) Rate = k [A][B][C](B) Rate = k [A][B]² [C](C) Rate = k [A]² [B](D) Rate = k [A][BJ° [C]?(E) Rate = k [A]² [C]5. What is the rate constant of this reaction?(A) 0.200 § -1(B) 20.0 M-² s -(C) 200.0 M³ s -(D) 2.00 M-' s´6. What is the unit for the rate constant of the second order reaction?(A) M.s'(В) M- s -1(С) М' s(D) s -l(E) M-'7. Consider the following data and state whether the reaction is zero order, first or second order. Calculate theTime (sec)value of the rate constant.[A] (M)Reaction:A → B0.3200.000.20210.0(A) 0.0031 M. s(B) 0.884 M-' s -(С) 15s0.16015.0(D) 0.0462 s ·'(E) None of these above0.040045.08. The rate of appearance of oxygen O2 is 0.0320 M.s-', what is the rate of disappearance of N2O5?2 N2O5(g)4 NO2(g) + O2(g)(A) 0.0160 M. s'(B) 0.0320 M. s '(C) 0.0640 M. sl(D) 0.0200 M. s -'(E) 0.128 M. s¯

Answered: Image /qna-images/answer/79940119-10ac-4b79-bb07-89813cb36a9d.jpg

For questions 1. to 5. The following data were collected from the reaction of: A + B +C PRODUCTS [A] (M) [B] (M) [C] (M) Initial Rate M/sec 0.10 0.10 0.10 0.020 0.20 0.20 0.20 0.160 0.40 0.20 0.40 0.640 0.40 0.40 0.80 1.280 1. What is the order of the reaction with respect to [A]? (A) 0 (B) 1 (C) 2 (D) 3 2. What is the order of the reaction with respect to [B]? (A) 0 (B) 1 (C) 2 (D) 3 3. What is the order of the reaction with respect to [C]? (A) 0 (B) 1 (C) 2 (D) 3 4. What is the rate law of this reaction? (A) Rate = k [A][B][C] (B) Rate = k [A][B]² [C] (C) Rate = k [A]² [B] (D) Rate = k [A][B] [C} (E) Rate = k [A]² [C] 5. What is the rate constant of this reaction? (A) 0.200 § -1 (B) 20.0 M² s -l (C) 200.0 M-³ s (D) 2.00 M-' s -l

For questions 1. to 5. The following data were collected from the reaction of: A + B +C PRODUCTS [A] (M) [B] (M) [C] (M) Initial Rate M/sec 0.10 0.10 0.10 0.020 0.20 0.20 0.20 0.160 0.40 0.20 0.40 0.640 0.40 0.40 0.80 1.280 1. What is the order of the reaction with respect to [A]? (A) 0 (B) 1 (C) 2 (D) 3 2. What is the order of the reaction with respect to [B]? (A) 0 (B) 1 (C) 2 (D) 3 3. What is the order of the reaction with respect to [C]? (A) 0 (B) 1 (C) 2 (D) 3 4. What is the rate law of this reaction? (A) Rate = k [A][B][C] (B) Rate = k [A][B]² [C] (C) Rate = k [A]² [B] (D) Rate = k [A][B] [C} (E) Rate = k [A]² [C] 5. What is the rate constant of this reaction? (A) 0.200 § -1 (B) 20.0 M² s -l (C) 200.0 M-³ s (D) 2.00 M-' s -l

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 115QRT

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
The uncoiling of deoxyribonucleic acid (DNA) is a first-order reaction. Its activation energy is 420 kJ. At 37C, the rate constant is 4.90104min1 (a) What is the half-life of the uncoiling at 37C (normal body temperature)? (b) What is the half-life of the uncoiling if the organism has a temperature of 40C(104F)? (c) By what factor does the rate of uncoiling increase (per C) over this temperature interval?
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?
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.
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For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
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