For the reaction A- products, concentration and time data were collected. I (s) [A] (M) 0.0 3.40 Enter these data into the graphing tool to determine the reaction order. 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data IAl vs.t InjAl vs.t 1/A) vs.t In[A) 1/IA) Add Row 10 total rows What is the reaction order? Calculate the concentration of A after 163 s.

For the reaction A- products, concentration and time data were collected. I (s) [A] (M) 0.0 3.40 Enter these data into the graphing tool to determine the reaction order. 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data IAl vs.t InjAl vs.t 1/A) vs.t In[A) 1/IA) Add Row 10 total rows What is the reaction order? Calculate the concentration of A after 163 s.

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

For the reaction A - products, concentration and time data were collected.
I (s)
[A] (M)
0.0
3.40
Enter these data into the graphing tool to determine the reaction order.
25.0
2.28
50.0
1.53
75.0
1.02
Graphing Tool
Clear All Data
(Al vs.t InAl vs
1/A) vs.t
(A]
In(A)
1/IA)
Add Row
10 total rows
What is the reaction order?
Calculate the concentration of A after 163 s.
[A]163, = 0.6975
M
Incorrect
M

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Reaction Conc. Na2S½O3 Conc. HCI A Abs. A Time (s) Rate (A Abs./ga Time) 1.007568 0.300349 0.01870913 0.02870913 1 0.10 M .30 М 1.3686611 1.358380874 0.10 M .15 M 1.5360817 5.114311671 3 0.050 M .30 M 1.2267196 65.56796601 4 0.025 M .30 M 0.9563164 11.3085840 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. The rate law of the reaction is shown below: Rate = [Na2S2O3]-2