6. 0.156 = k [0.000255) 2. The catalyzed decomposition of hydrogen peroxide, H₂O2(aq), is represented by the following equation. -0.05 2 H₂O2(sq) 2 H₂O(L) + O2(g) -0.06 0.11 The kinetics of the decomposition reaction were studied and the analysis of the results show that it is a first-order reaction. Some of the experimental data are shown in the table to the right. ola catalyst 0/2 (a) During the analysis of the data, the graph to the right was produced. Label the vertical axis of this graph. Dash in a second line that represents the plot of the uncatalyzed first-order decomposition of 1.00 M H₂O2(aq). 0.22 - 0.17 concentration. 6253444 mol L-1 rate = k 0.6084 [H₂O₂] (mol L ¹) 1.00 0.78 (13 0.61 0.50 time (minutes) suse your Integrated rate (b) Use the data in the table to calculate the rate constat, k, and specify the units. Be sure to show the method you used in your calculations. laws! = 1 (5) 2 rate = k [H₂0₂] ² rate = K [1.00]² nate = k 1 rate = k [1.00] 1 Time (minutes) 1 (0.78] 5.0 10.0 ? rate=1 [0.78] ² rate -1 [2084] (c) Calculate the time that is missing from the table. Be certain to show all work you used to make this calculation. 0/2 Juster 45 +5 +5 1 - 1.28705 = 1(5) -0.28 205 = k/s) 5 B 12=-0.06
6. 0.156 = k [0.000255) 2. The catalyzed decomposition of hydrogen peroxide, H₂O2(aq), is represented by the following equation. -0.05 2 H₂O2(sq) 2 H₂O(L) + O2(g) -0.06 0.11 The kinetics of the decomposition reaction were studied and the analysis of the results show that it is a first-order reaction. Some of the experimental data are shown in the table to the right. ola catalyst 0/2 (a) During the analysis of the data, the graph to the right was produced. Label the vertical axis of this graph. Dash in a second line that represents the plot of the uncatalyzed first-order decomposition of 1.00 M H₂O2(aq). 0.22 - 0.17 concentration. 6253444 mol L-1 rate = k 0.6084 [H₂O₂] (mol L ¹) 1.00 0.78 (13 0.61 0.50 time (minutes) suse your Integrated rate (b) Use the data in the table to calculate the rate constat, k, and specify the units. Be sure to show the method you used in your calculations. laws! = 1 (5) 2 rate = k [H₂0₂] ² rate = K [1.00]² nate = k 1 rate = k [1.00] 1 Time (minutes) 1 (0.78] 5.0 10.0 ? rate=1 [0.78] ² rate -1 [2084] (c) Calculate the time that is missing from the table. Be certain to show all work you used to make this calculation. 0/2 Juster 45 +5 +5 1 - 1.28705 = 1(5) -0.28 205 = k/s) 5 B 12=-0.06
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 61AP
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Lock And Key Model
The lock-and-key model is used to describe the catalytic enzyme activity, based on the interaction between enzyme and substrate. This model considers the lock as an enzyme and the key as a substrate to explain this model. The concept of how a unique distinct key only can have the access to open a particular lock resembles how the specific substrate can only fit into the particular active site of the enzyme. This is significant in understanding the intermolecular interaction between proteins and plays a vital role in drug interaction.
Question
Can someone please help, I got these wrong and I don't know how? Thanks
![6.
0.156 = k [0.000255)
2. The catalyzed decomposition of hydrogen peroxide, H₂O2(aq), is represented by the
following equation.
-0.05
2 H₂O2(sq)
2 H₂O(L) + O2(g)
-0.06
0.11
The kinetics of the decomposition reaction were studied and the analysis of the results
show that it is a first-order reaction. Some of the experimental data are shown in the
table to the right.
ola
catalyst
0/2
(a) During the analysis of the data, the graph to the right was
produced.
Label the vertical axis of this graph.
Dash in a second line that represents the plot of the
uncatalyzed first-order decomposition of 1.00 M
H₂O2(aq).
0.22
- 0.17
concentration.
6253444
mol L-1
rate = k
0.6084
[H₂O₂]
(mol L ¹)
1.00
0.78
(13
0.61
0.50
time (minutes)
suse your Integrated rate
(b) Use the data in the table to calculate the rate constat, k, and specify the units. Be sure to show the method
you used in your calculations.
laws!
= 1 (5)
2
rate = k [H₂0₂] ² rate = K [1.00]² nate = k
1
rate = k [1.00]
1
Time
(minutes)
1
(0.78]
5.0
10.0
?
rate=1 [0.78] ²
rate -1 [2084]
(c) Calculate the time that is missing from the table. Be certain to show all work you used to make this
calculation.
0/2
Juster
45
+5
+5
1 - 1.28705 = 1(5)
-0.28 205 = k/s)
5
B
12=-0.06](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff959d43b-03bc-4e94-98b8-551f4a725169%2Fe2f2d6d2-75d9-445f-87c0-3b90b7faf944%2Fmlypxv_processed.png&w=3840&q=75)
Transcribed Image Text:6.
0.156 = k [0.000255)
2. The catalyzed decomposition of hydrogen peroxide, H₂O2(aq), is represented by the
following equation.
-0.05
2 H₂O2(sq)
2 H₂O(L) + O2(g)
-0.06
0.11
The kinetics of the decomposition reaction were studied and the analysis of the results
show that it is a first-order reaction. Some of the experimental data are shown in the
table to the right.
ola
catalyst
0/2
(a) During the analysis of the data, the graph to the right was
produced.
Label the vertical axis of this graph.
Dash in a second line that represents the plot of the
uncatalyzed first-order decomposition of 1.00 M
H₂O2(aq).
0.22
- 0.17
concentration.
6253444
mol L-1
rate = k
0.6084
[H₂O₂]
(mol L ¹)
1.00
0.78
(13
0.61
0.50
time (minutes)
suse your Integrated rate
(b) Use the data in the table to calculate the rate constat, k, and specify the units. Be sure to show the method
you used in your calculations.
laws!
= 1 (5)
2
rate = k [H₂0₂] ² rate = K [1.00]² nate = k
1
rate = k [1.00]
1
Time
(minutes)
1
(0.78]
5.0
10.0
?
rate=1 [0.78] ²
rate -1 [2084]
(c) Calculate the time that is missing from the table. Be certain to show all work you used to make this
calculation.
0/2
Juster
45
+5
+5
1 - 1.28705 = 1(5)
-0.28 205 = k/s)
5
B
12=-0.06
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