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
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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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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