Problems requiring More Work 1. The decomposition of hydrogen peroxide was studied and the data below was collected and graphed as shown in the 3 graphs. 2 H2O2 (I) → 2 H2O (I) + 02(g) time, s [H,O,1,mol/L In[H;O] 1/[H;O;] 25 y = 0.004596x - 0.847 R = 0.872 1 20 120 0.91 -0.09431 1.098901 15 300 0.78 -0,24846 1.282051 600 0.59 -0.52763 1.694915 10 1200 0.37 -0.99425 2.702703 1800 0.22 -1.51413 4.545455 2400 0.13 -2.04022 7.692308 1000 2000 3000 4000 3000 0.082 -2.50104 12.19512 -5 time, s 3600 0.05 -2.99573 20 1.5 .1000 2000 3000 4000 y=-0.000264x+0.841 R2 = 0,889 1 -1 0.5 -2 y = -0.000835x - 0.00493 R = 0.99978 %3D 1000 2000 3000 4000 -0.5 -4 time, s time, s a. Write the general form of the rate law for the decomposition of hydrogen peroxide with respect to the disappearance of the hydrogen peroxide. b. What is the order of reaction with respect to [H2O2]? How did you determine this? c. Write the integrated rate law, including the value of the rate constant with units. d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the integrated rate law from c and show your work.) e. Calculate the half life of this reaction [H,O;] , M 1/[H,O,] , M-1
Problems requiring More Work 1. The decomposition of hydrogen peroxide was studied and the data below was collected and graphed as shown in the 3 graphs. 2 H2O2 (I) → 2 H2O (I) + 02(g) time, s [H,O,1,mol/L In[H;O] 1/[H;O;] 25 y = 0.004596x - 0.847 R = 0.872 1 20 120 0.91 -0.09431 1.098901 15 300 0.78 -0,24846 1.282051 600 0.59 -0.52763 1.694915 10 1200 0.37 -0.99425 2.702703 1800 0.22 -1.51413 4.545455 2400 0.13 -2.04022 7.692308 1000 2000 3000 4000 3000 0.082 -2.50104 12.19512 -5 time, s 3600 0.05 -2.99573 20 1.5 .1000 2000 3000 4000 y=-0.000264x+0.841 R2 = 0,889 1 -1 0.5 -2 y = -0.000835x - 0.00493 R = 0.99978 %3D 1000 2000 3000 4000 -0.5 -4 time, s time, s a. Write the general form of the rate law for the decomposition of hydrogen peroxide with respect to the disappearance of the hydrogen peroxide. b. What is the order of reaction with respect to [H2O2]? How did you determine this? c. Write the integrated rate law, including the value of the rate constant with units. d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the integrated rate law from c and show your work.) e. Calculate the half life of this reaction [H,O;] , M 1/[H,O,] , M-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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![Problems requiring More Work
1. The decomposition of hydrogen peroxide was studied and the data below was collected and
graphed as shown in the 3 graphs.
2 H2O2 (I) → 2 H2O (I) + 02(g)
time, s
[H,O,1,mol/L
In[H;O]
1/[H;O;]
25
y = 0.004596x - 0.847
R = 0.872
1
20
120
0.91
-0.09431
1.098901
15
300
0.78
-0,24846
1.282051
600
0.59
-0.52763
1.694915
10
1200
0.37
-0.99425
2.702703
1800
0.22
-1.51413
4.545455
2400
0.13
-2.04022
7.692308
1000
2000
3000
4000
3000
0.082
-2.50104
12.19512
-5
time, s
3600
0.05
-2.99573
20
1.5
.1000
2000
3000
4000
y=-0.000264x+0.841
R2 = 0,889
1
-1
0.5
-2
y = -0.000835x - 0.00493
R = 0.99978
%3D
1000
2000
3000
4000
-0.5
-4
time, s
time, s
a. Write the general form of the rate law for the decomposition of hydrogen peroxide with
respect to the disappearance of the hydrogen peroxide.
b. What is the order of reaction with respect to [H2O2]? How did you determine this?
c. Write the integrated rate law, including the value of the rate constant with units.
d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the
integrated rate law from c and show your work.)
e. Calculate the half life of this reaction
[H,O;] , M
1/[H,O,] , M-1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb987d8c1-664b-448b-b573-1ab7f66094f6%2F3826cb67-8611-4b8d-b644-004e439db372%2F6zw9bc_processed.png&w=3840&q=75)
Transcribed Image Text:Problems requiring More Work
1. The decomposition of hydrogen peroxide was studied and the data below was collected and
graphed as shown in the 3 graphs.
2 H2O2 (I) → 2 H2O (I) + 02(g)
time, s
[H,O,1,mol/L
In[H;O]
1/[H;O;]
25
y = 0.004596x - 0.847
R = 0.872
1
20
120
0.91
-0.09431
1.098901
15
300
0.78
-0,24846
1.282051
600
0.59
-0.52763
1.694915
10
1200
0.37
-0.99425
2.702703
1800
0.22
-1.51413
4.545455
2400
0.13
-2.04022
7.692308
1000
2000
3000
4000
3000
0.082
-2.50104
12.19512
-5
time, s
3600
0.05
-2.99573
20
1.5
.1000
2000
3000
4000
y=-0.000264x+0.841
R2 = 0,889
1
-1
0.5
-2
y = -0.000835x - 0.00493
R = 0.99978
%3D
1000
2000
3000
4000
-0.5
-4
time, s
time, s
a. Write the general form of the rate law for the decomposition of hydrogen peroxide with
respect to the disappearance of the hydrogen peroxide.
b. What is the order of reaction with respect to [H2O2]? How did you determine this?
c. Write the integrated rate law, including the value of the rate constant with units.
d. Calculate the concentration of H2O2 after the reaction has run for 45.0 minutes. (Use the
integrated rate law from c and show your work.)
e. Calculate the half life of this reaction
[H,O;] , M
1/[H,O,] , M-1
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