Table 3. Data for the Graphical Analysis Time, s Pcoz InP co2 YP coz [CO2] vs Time 1 1.00E+00 1.00E+00 1.20E+00 2 0.271 7.63E-01 -0.2711357 1.31E+00 1.00E+00 3 0.542 5.81E-01 -0.5422716 1.72E+00 8.00E-01 4 0.813 4.43E-01 -0.813407 2.26E+00 v=-0.3187x +0.7952 R = 0.8819 5 1.084 3.38E-01 -1.0845437 2.96E+00 6.00E-01 6 1.355 2.58E-01 -1.3556798 3.88E +00 4.00E-01 7 1.626 1.97E-01 -1.626813 5.09E+00 2.00E-01 1.897 1.50E-01 -1.897947 6.67E+00 0.00E+00 9 2.168 1.14E-01 -2.1690862 8.75E+00 1 15 2 2.5 -2.00E-01 10 2.439 8.71E-02 -2.4402197 1.15E+01 Time, s 11 2.709 6.65E-02 -2.7103549 1.50E+01 Graph 3. P vs t. Show trendline equation, R', give it a proper title. In[CO2] vs Time 1/[CO2] vs Time 1.60E+01 ois 15 2,5 1.40E+01 -05 1.20E+01 y=4.7936x - 1.0271 R=0.8819 -1 1.00E+01 me 8.00E+00 -15 6.00E+00 y=-1.0005x- 6E-07 R =1 -2 4.00E+00 2.00E+00 -25 0,00E+00 1,5 2 25 -3 -2.00E+00 Time, s Time, s Graph 4. InP vs t. Show trendline equation, R', give it a proper ti Graph 5. 11P vs t. Show trendline equation, R', give it a proper title Compare the trendline equations alone with R? for three graphs and make a conclusion about the order of reaction The order with respect to CO, is: First Order The rate constant is (use correct units): k=1.0005s^-1 The integrated rate law is: [A)=[A]0e^(-kt) In[CO2] (co2] 1/[CO2]
Table 3. Data for the Graphical Analysis Time, s Pcoz InP co2 YP coz [CO2] vs Time 1 1.00E+00 1.00E+00 1.20E+00 2 0.271 7.63E-01 -0.2711357 1.31E+00 1.00E+00 3 0.542 5.81E-01 -0.5422716 1.72E+00 8.00E-01 4 0.813 4.43E-01 -0.813407 2.26E+00 v=-0.3187x +0.7952 R = 0.8819 5 1.084 3.38E-01 -1.0845437 2.96E+00 6.00E-01 6 1.355 2.58E-01 -1.3556798 3.88E +00 4.00E-01 7 1.626 1.97E-01 -1.626813 5.09E+00 2.00E-01 1.897 1.50E-01 -1.897947 6.67E+00 0.00E+00 9 2.168 1.14E-01 -2.1690862 8.75E+00 1 15 2 2.5 -2.00E-01 10 2.439 8.71E-02 -2.4402197 1.15E+01 Time, s 11 2.709 6.65E-02 -2.7103549 1.50E+01 Graph 3. P vs t. Show trendline equation, R', give it a proper title. In[CO2] vs Time 1/[CO2] vs Time 1.60E+01 ois 15 2,5 1.40E+01 -05 1.20E+01 y=4.7936x - 1.0271 R=0.8819 -1 1.00E+01 me 8.00E+00 -15 6.00E+00 y=-1.0005x- 6E-07 R =1 -2 4.00E+00 2.00E+00 -25 0,00E+00 1,5 2 25 -3 -2.00E+00 Time, s Time, s Graph 4. InP vs t. Show trendline equation, R', give it a proper ti Graph 5. 11P vs t. Show trendline equation, R', give it a proper title Compare the trendline equations alone with R? for three graphs and make a conclusion about the order of reaction The order with respect to CO, is: First Order The rate constant is (use correct units): k=1.0005s^-1 The integrated rate law is: [A)=[A]0e^(-kt) In[CO2] (co2] 1/[CO2]
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
Please help me determine the integrated rate law and justify the answer
![Table 3. Data for the Graphical Analysis
Time, s
Pcoz
InP
co2
YP
coz
[CO2] vs Time
1
1.00E+00
1.00E+00
1.20E+00
2
0.271
7.63E-01
-0.2711357
1.31E+00
1.00E+00
3
0.542
5.81E-01
-0.5422716
1.72E+00
8.00E-01
4
0.813
4.43E-01
-0.813407
2.26E+00
v=-0.3187x +0.7952
R = 0.8819
5
1.084
3.38E-01
-1.0845437
2.96E+00
6.00E-01
6
1.355
2.58E-01
-1.3556798
3.88E +00
4.00E-01
7
1.626
1.97E-01
-1.626813 5.09E+00
2.00E-01
1.897
1.50E-01
-1.897947
6.67E+00
0.00E+00
9
2.168
1.14E-01
-2.1690862 8.75E+00
1
15
2
2.5
-2.00E-01
10
2.439
8.71E-02
-2.4402197
1.15E+01
Time, s
11
2.709
6.65E-02
-2.7103549
1.50E+01
Graph 3. P vs t. Show trendline equation, R', give it a proper title.
In[CO2] vs Time
1/[CO2] vs Time
1.60E+01
ois
15
2,5
1.40E+01
-05
1.20E+01
y=4.7936x - 1.0271
R=0.8819
-1
1.00E+01
me
8.00E+00
-15
6.00E+00
y=-1.0005x- 6E-07
R =1
-2
4.00E+00
2.00E+00
-25
0,00E+00
1,5
2
25
-3
-2.00E+00
Time, s
Time, s
Graph 4. InP vs t. Show trendline equation, R', give it a proper ti
Graph 5. 11P vs t. Show trendline equation, R', give it a proper title
Compare the trendline equations alone with R? for three graphs and make a conclusion about the order
of reaction
The order with respect to CO, is:
First Order
The rate constant is (use correct units): k=1.0005s^-1
The integrated rate law is:
[A)=[A]0e^(-kt)
In[CO2]
(co2]
1/[CO2]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F435327ce-ad1d-47b0-9d05-42b05e19b7ae%2Fccd261f4-48ff-4aff-8820-631f4734ffa6%2Fnmgu0sw_processed.png&w=3840&q=75)
Transcribed Image Text:Table 3. Data for the Graphical Analysis
Time, s
Pcoz
InP
co2
YP
coz
[CO2] vs Time
1
1.00E+00
1.00E+00
1.20E+00
2
0.271
7.63E-01
-0.2711357
1.31E+00
1.00E+00
3
0.542
5.81E-01
-0.5422716
1.72E+00
8.00E-01
4
0.813
4.43E-01
-0.813407
2.26E+00
v=-0.3187x +0.7952
R = 0.8819
5
1.084
3.38E-01
-1.0845437
2.96E+00
6.00E-01
6
1.355
2.58E-01
-1.3556798
3.88E +00
4.00E-01
7
1.626
1.97E-01
-1.626813 5.09E+00
2.00E-01
1.897
1.50E-01
-1.897947
6.67E+00
0.00E+00
9
2.168
1.14E-01
-2.1690862 8.75E+00
1
15
2
2.5
-2.00E-01
10
2.439
8.71E-02
-2.4402197
1.15E+01
Time, s
11
2.709
6.65E-02
-2.7103549
1.50E+01
Graph 3. P vs t. Show trendline equation, R', give it a proper title.
In[CO2] vs Time
1/[CO2] vs Time
1.60E+01
ois
15
2,5
1.40E+01
-05
1.20E+01
y=4.7936x - 1.0271
R=0.8819
-1
1.00E+01
me
8.00E+00
-15
6.00E+00
y=-1.0005x- 6E-07
R =1
-2
4.00E+00
2.00E+00
-25
0,00E+00
1,5
2
25
-3
-2.00E+00
Time, s
Time, s
Graph 4. InP vs t. Show trendline equation, R', give it a proper ti
Graph 5. 11P vs t. Show trendline equation, R', give it a proper title
Compare the trendline equations alone with R? for three graphs and make a conclusion about the order
of reaction
The order with respect to CO, is:
First Order
The rate constant is (use correct units): k=1.0005s^-1
The integrated rate law is:
[A)=[A]0e^(-kt)
In[CO2]
(co2]
1/[CO2]
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