b Calculate the values of the rate constants k1 and k2. k1 L mol-1 min-1 k2 L? mol-2 min-1 Hydrogen peroxide and the iodide ion react in acidic solution as follows: H2O2 (ag) + 31 (aq) + 2H† (ag) → I3 (aq) + 2H2O(1) The kinetics of this reaction were studied by following the decay of the concentration of H2 O2 and constructing plots of In[H2O2] versus time. All the plots were linear and all solutions had [H2O2]o concentrations of I and H†. The results follow: = 8.0 x 10-4 mol/L. The slopes of these straight lines depended on the initial [I], (mol/L) [H*], (mol/L) Slope (min-1) 0.1000 0.0400 -0.120 0.3000 0.0400 -0.360 0.4000 0.0400 -0.480 0.0750 0.0200 -0.0760 0.0750 0.0800 -0.118 0.0750 0.1600 -0.174 The rate law for this reaction has the form -d[H2O2] (kı + k2 [H*])[I¯]™" [H2O2]* Rate dt

b Calculate the values of the rate constants k1 and k2. k1 L mol-1 min-1 k2 L? mol-2 min-1 Hydrogen peroxide and the iodide ion react in acidic solution as follows: H2O2 (ag) + 31 (aq) + 2H† (ag) → I3 (aq) + 2H2O(1) The kinetics of this reaction were studied by following the decay of the concentration of H2 O2 and constructing plots of In[H2O2] versus time. All the plots were linear and all solutions had [H2O2]o concentrations of I and H†. The results follow: = 8.0 x 10-4 mol/L. The slopes of these straight lines depended on the initial [I], (mol/L) [H], (mol/L) Slope (min-1) 0.1000 0.0400 -0.120 0.3000 0.0400 -0.360 0.4000 0.0400 -0.480 0.0750 0.0200 -0.0760 0.0750 0.0800 -0.118 0.0750 0.1600 -0.174 The rate law for this reaction has the form -d[H2O2] (kı + k2 [H])[I¯]™" [H2O2]* Rate dt

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

n=1

and m=1

b Calculate the values of the rate constants k1 and k2.
k1
L mol-1 min-1
k2
L? mol-2 min-1

Hydrogen peroxide and the iodide ion react in acidic solution as follows:
H2O2 (ag) + 31 (aq) + 2H† (ag) → I3 (aq) + 2H2O(1)
The kinetics of this reaction were studied by following the decay of the concentration of H2 O2 and constructing plots of In[H2O2] versus time.
All the plots were linear and all solutions had [H2O2]o
concentrations of I and H†. The results follow:
= 8.0 x 10-4 mol/L. The slopes of these straight lines depended on the initial
[I], (mol/L) [H*], (mol/L) Slope (min-1)
0.1000
0.0400
-0.120
0.3000
0.0400
-0.360
0.4000
0.0400
-0.480
0.0750
0.0200
-0.0760
0.0750
0.0800
-0.118
0.0750
0.1600
-0.174
The rate law for this reaction has the form
-d[H2O2]
(kı + k2 [H*])[I¯]™" [H2O2]*
Rate
dt

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