a. What is the order of reaction for the decomposition of hydrogen peroxide? O zero-order O first-order O econd-order b. Find the numerical value of the rate constant at 20°C, including the correct units. (Enter an unrounded value.) c. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t= 0 in the graphs). (Enter an unrounded value.) rate = mol - L-1.s-1
a. What is the order of reaction for the decomposition of hydrogen peroxide? O zero-order O first-order O econd-order b. Find the numerical value of the rate constant at 20°C, including the correct units. (Enter an unrounded value.) c. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t= 0 in the graphs). (Enter an unrounded value.) rate = mol - L-1.s-1
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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![a. What is the order of reaction for the decomposition of hydrogen peroxide?
zero-order
first-order
second-order
b. Find the numerical value of the rate constant at 20°C, including the correct units. (Enter an unrounded value.)
k =
c. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t = 0 in the graphs). (Enter an unrounded value.)
rate =
mol - L-1.s-1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F30b83e10-cc9f-4998-b4fc-42665ab99815%2F2e4b4bc4-603d-46b1-882f-d743fbc79884%2Fkwaz5ru_processed.jpeg&w=3840&q=75)
Transcribed Image Text:a. What is the order of reaction for the decomposition of hydrogen peroxide?
zero-order
first-order
second-order
b. Find the numerical value of the rate constant at 20°C, including the correct units. (Enter an unrounded value.)
k =
c. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t = 0 in the graphs). (Enter an unrounded value.)
rate =
mol - L-1.s-1
![H2O2 (aq) + H20(1) + 1/2 0,(9)
Ordinarily, this reaction proceeds rather slowly, but in the presence of some iodide ions (I), the decomposition is much faster. The decomposition in the presence of iodide was studied at 20°C, and the data were plotted in various ways. Use the graphs below to answer the questions that follow.
М (mol/L)
1-
In[M]
1/M (L/mol)
11-
0.9
10-
0.8
-0.5-
8-
0.74
7.
0.6-
-1-
6-
0.5-
5-
0.4
-1.5-
0.3
3-
0.2-
-2-
0.14
Time (s)
• Time (s)
Time (s)
100
200
300
400
500
600
100
200
300
400
500
600
100
200
300
400
500
600](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F30b83e10-cc9f-4998-b4fc-42665ab99815%2F2e4b4bc4-603d-46b1-882f-d743fbc79884%2Fi4edvmo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:H2O2 (aq) + H20(1) + 1/2 0,(9)
Ordinarily, this reaction proceeds rather slowly, but in the presence of some iodide ions (I), the decomposition is much faster. The decomposition in the presence of iodide was studied at 20°C, and the data were plotted in various ways. Use the graphs below to answer the questions that follow.
М (mol/L)
1-
In[M]
1/M (L/mol)
11-
0.9
10-
0.8
-0.5-
8-
0.74
7.
0.6-
-1-
6-
0.5-
5-
0.4
-1.5-
0.3
3-
0.2-
-2-
0.14
Time (s)
• Time (s)
Time (s)
100
200
300
400
500
600
100
200
300
400
500
600
100
200
300
400
500
600
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