Run # [10,1 [1] [H] Time (s) Rate* 0.05 0.00002 17.7 2.0x1-5 S00S 0.005 1. 1. 0.05 0.00002 17.8 0.01 0.05 0.00002 8.9 5.3x10^-5 8.7 0.005 0.01 0.00002 5.2 9.2x10^-5 5.5 4 0.005 0.05 0.00001 1.8 0.7x10^5 4. 2.0 *Rate = 3. The value of [HASO,lo, the initial concentration of arsenlous acid, can be found by looking carefully at the Experiment page online. 15. Determine the exponent in the rate law for each reactant by comparing the change in concentration with the change in rate. See Example 13.3 In your ebook. rate = k[10, 1. (1].'H*]." a (order with respect to I0, ) 2. b (order with respect to I) 2 c (order with respect to H) 1 16. Once you have found the values of a, b, and c, you can calculate the rate constant k for each run. Fill in these values in the table above. 17. Finally, calculate the average value of k. Include units! I
Run # [10,1 [1] [H] Time (s) Rate* 0.05 0.00002 17.7 2.0x1-5 S00S 0.005 1. 1. 0.05 0.00002 17.8 0.01 0.05 0.00002 8.9 5.3x10^-5 8.7 0.005 0.01 0.00002 5.2 9.2x10^-5 5.5 4 0.005 0.05 0.00001 1.8 0.7x10^5 4. 2.0 *Rate = 3. The value of [HASO,lo, the initial concentration of arsenlous acid, can be found by looking carefully at the Experiment page online. 15. Determine the exponent in the rate law for each reactant by comparing the change in concentration with the change in rate. See Example 13.3 In your ebook. rate = k[10, 1. (1].'H*]." a (order with respect to I0, ) 2. b (order with respect to I) 2 c (order with respect to H) 1 16. Once you have found the values of a, b, and c, you can calculate the rate constant k for each run. Fill in these values in the table above. 17. Finally, calculate the average value of k. Include units! I
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 5PS: Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data;...
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I need to calculate the average value of K. Could you please show all the steps.
![Run #
[10,1
[1]
[H]
Time (s)
Rate*
0.05
0.00002
17.7
2.0x1-5
S00S
0.005
1.
1.
0.05
0.00002
17.8
0.01
0.05
0.00002
8.9
5.3x10^-5
8.7
0.005
0.01
0.00002
5.2
9.2x10^-5
5.5
4
0.005
0.05
0.00001
1.8
0.7x10^5
4.
2.0
*Rate =
3.
The value of [HASO,lo, the initial concentration of arsenlous acid, can be found by looking
carefully at the Experiment page online.
15. Determine the exponent in the rate law for each reactant by comparing the change in concentration with
the change in rate. See Example 13.3 In your ebook.
rate = k[10, 1. (1].'H*]."
a (order with respect to I0, )
2.
b (order with respect to I)
2
c (order with respect to H)
1
16. Once you have found the values of a, b, and c, you can calculate the rate constant k for each run.
Fill in these values in the table above.
17. Finally, calculate the average value of k. Include units!
I](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F514f8385-760c-4081-bafc-6b418d632275%2Fe57a2601-13e0-4c30-82d0-48b300288f2b%2Fdlp9qtb.jpeg&w=3840&q=75)
Transcribed Image Text:Run #
[10,1
[1]
[H]
Time (s)
Rate*
0.05
0.00002
17.7
2.0x1-5
S00S
0.005
1.
1.
0.05
0.00002
17.8
0.01
0.05
0.00002
8.9
5.3x10^-5
8.7
0.005
0.01
0.00002
5.2
9.2x10^-5
5.5
4
0.005
0.05
0.00001
1.8
0.7x10^5
4.
2.0
*Rate =
3.
The value of [HASO,lo, the initial concentration of arsenlous acid, can be found by looking
carefully at the Experiment page online.
15. Determine the exponent in the rate law for each reactant by comparing the change in concentration with
the change in rate. See Example 13.3 In your ebook.
rate = k[10, 1. (1].'H*]."
a (order with respect to I0, )
2.
b (order with respect to I)
2
c (order with respect to H)
1
16. Once you have found the values of a, b, and c, you can calculate the rate constant k for each run.
Fill in these values in the table above.
17. Finally, calculate the average value of k. Include units!
I
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