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The acid-catalyzed iodination of acetone CH 3 COCH 3 (aq) + I 2 (aq) → CH 3 COCH 2 I(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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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 14, Problem 86IL
Textbook Problem
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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.

Chapter 14, Problem 86IL, The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq)  CH3COCH2I(aq) + HI(aq) is a common

Determine the rate law for this reaction.

Interpretation Introduction

Interpretation:

The rate law should be determined for the given chemical reaction.

Concept Introduction:

Rate law: It is generally the rate equation that consists of the reaction rate with the concentration or the pressures of the reactants and constant parameters.

Rate constant: The rate constant for a chemical reaction is the proportionality term in the chemical reaction rate law which gives the relationship between the rate and the concentration of the reactant present in the chemical reaction.

Explanation of Solution

The rate law is obtained by first determining the order of each reactant present in the given reaction. The order of each reactant is obtained by using the given set of concentration and the rate data as follows,

The order for CH3COCH3 is obtained by considering the experiment 2 and 3 from the given data.

  23isasfollows,[CH3COCH3]2[CH3COCH3]3[H+]2[H+]3[I2]2[I2]3=[Rate]2[Rate]31.330.3230.006651.7×10-50.6670.3230.006657.6×10-6 _2m21

The order for CH3COCH3 is 1.

Similarly, the order for H+ is obtained as follow,

  12isasfollows,[CH3COCH3]1[CH3COCH3]2[H+]1[H+]2[I2]1[I2]2=[Rate]1[Rate]21.330.1620.006658.1×10-61.330.3230.006651

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Chapter 14 Solutions

Chemistry & Chemical Reactivity
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Ch. 14.4 - Using the rate constant for HI decomposition given...Ch. 14.4 - The catalyzed decomposition of hydrogen peroxide...Ch. 14.4 - Americium is used in smoke detectors and in...Ch. 14.4 - The decomposition of N2O5 is a first-order...Ch. 14.4 - Which of the following will confirm that the...Ch. 14.4 - 3. The equation for the decomposition of NO2(g) at...Ch. 14.5 - Rate constants were determined for the...Ch. 14.5 - The colorless gas N2O4, decomposes to the brown...Ch. 14.5 - Which of the following graphs will produce a...Ch. 14.5 - 2. 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