You are studying the kinetics ofa chemical reaction of the form A+2B 2C+D. Yougather the following data from timing chemical reactions. A has an observable color and itsconcentration is monitored by absorption.You collect the following data:You use 0.100 M solutions of A and B as your stock solutions.Reaction 1: 10 mL A+ 10 mL B+30 mL H,OReaction 2: 20 mL A+ 10 mL B+20 mL HOReaction 3: 30 mL A+ 10 mL B+10 mL H;OReaction 4: 10 mL A+ 20 mLB 20 mL H,OReaction 5: 10 mL A+30 mL B+ 10 mL H,OReaction 6: 20 mL A+ 20 mL B 10 mL H;OT(s)R1R2R30.0400 | 0.0600 0.0200R4 R5R60.02000.02000.0400150.01800.0360 0.0540 0.01600.01400.03200.0338 0.05180.0325 0.0509 0.01160.0317 | 0.05040.0140 0.0312 0.0502 0.00920.0134 0.0308 0.05010.0129 0.0306 0.0501 0.00770.0304 0.0500 0.00710.0122 0.0303 0.0500 | 0.00660.0120 0.0302 0.05000.0117 0.0301 0.0500| 0.0058300.01660.01340.01060.0282456075900.01550.00840.02590.01460.01030.00690.02430.00570.00480.02330.00840.02251051201350.00410.02200.01260.00350.02150.00310.02121500.00610.00270.02091650.00230.0207What is the rate law of the reaction?

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You are studying the kinetics ofa chemical reaction of the form A+2B 2C+D. You gather the following data from timing chemical reactions. A has an observable color and its concentration is monitored by absorption. You collect the following data: You use 0.100 M solutions of A and B as your stock solutions. Reaction 1: 10 mL A+ 10 mL B+30 mL H,O Reaction 2: 20 mL A+ 10 mL B+20 mL H;O Reaction 3: 30 mL A+ 10 mL B+ 10 mL HO Reaction 4: 10 mL A+ 20 mL B-20 mL H;O Reaction 5: 10 mL A+30 mL B+ 10 mL H-O Reaction 6: 20 mL A+ 20 mL B-10 mL H;O T(S) R1 R2 R3 R4 R5 R6 0.0200 0.0400 0.0600 0.0200 0.0200 0.0400 15 0.0180 0.0360 0.0540 0.0160 0.0140 0.0320 30 0.0166 0.0338 | 0.0518 0.0134 0.0106 0.0282 45 60 75 90 105 0.0155 0.0325 0.0509 0.0116 0.0084 0.0259 0.0146 0.0317 0.0504 0.0103 0.0069 0.0243 0.0312 0.0502 0.0308 0.0501 0.0306 0.0501 0.0304 0.0500 0.0071 0.0303 0.0500 | 0.0066 0.0140 0.0092 0.0057 0.0233 0.0134 0.0084 0.0048 0.0225 0.0129 0.0077 0.0041 0.0220 120 135 150 165 0.0126 0.0035 0.0215 0.0122 0.0031 0.0212 0.0120 0.0302 0.0500 0.0061 0.0027 0.0209 0.0117 0.0301 0.0500 0.0058 0.0023 0.0207 What is the rate law of the reaction?

You are studying the kinetics ofa chemical reaction of the form A+2B 2C+D. You gather the following data from timing chemical reactions. A has an observable color and its concentration is monitored by absorption. You collect the following data: You use 0.100 M solutions of A and B as your stock solutions. Reaction 1: 10 mL A+ 10 mL B+30 mL H,O Reaction 2: 20 mL A+ 10 mL B+20 mL H;O Reaction 3: 30 mL A+ 10 mL B+ 10 mL HO Reaction 4: 10 mL A+ 20 mL B-20 mL H;O Reaction 5: 10 mL A+30 mL B+ 10 mL H-O Reaction 6: 20 mL A+ 20 mL B-10 mL H;O T(S) R1 R2 R3 R4 R5 R6 0.0200 0.0400 0.0600 0.0200 0.0200 0.0400 15 0.0180 0.0360 0.0540 0.0160 0.0140 0.0320 30 0.0166 0.0338 | 0.0518 0.0134 0.0106 0.0282 45 60 75 90 105 0.0155 0.0325 0.0509 0.0116 0.0084 0.0259 0.0146 0.0317 0.0504 0.0103 0.0069 0.0243 0.0312 0.0502 0.0308 0.0501 0.0306 0.0501 0.0304 0.0500 0.0071 0.0303 0.0500 | 0.0066 0.0140 0.0092 0.0057 0.0233 0.0134 0.0084 0.0048 0.0225 0.0129 0.0077 0.0041 0.0220 120 135 150 165 0.0126 0.0035 0.0215 0.0122 0.0031 0.0212 0.0120 0.0302 0.0500 0.0061 0.0027 0.0209 0.0117 0.0301 0.0500 0.0058 0.0023 0.0207 What is the rate law of the reaction?

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 86IL: The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common...

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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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The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
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