Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 0.9563164 1.007568 0.300349 0.01870913 0.02870913 .30 M .15 M 1 0.10 M 1.358380874 2 0.10 M 5.114311671 .30 M .30 M 3 0.050 M 65.56796601 4 0.025 M 11.3085840 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 = [NazS203]¬2
Reaction Conc. Na2S203 Conc. HCI A Abs. A Time (s) Rate (A Abs./BA Time) 1.3686611 1.5360817 1.2267196 0.9563164 1.007568 0.300349 0.01870913 0.02870913 .30 M .15 M 1 0.10 M 1.358380874 2 0.10 M 5.114311671 .30 M .30 M 3 0.050 M 65.56796601 4 0.025 M 11.3085840 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 = [NazS203]¬2
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
![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff1aaab1d-8ba4-46f3-ada9-df467e4ce664%2Ffeed4d2b-cc59-42b1-bfde-af19d1c6f2df%2Fniqm70n_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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
Expert Solution
Introduction
The rate of a reaction can be defined as the rate of decrease in concentration of reactants or the rate of increase in concentration of product.
The rate law can be expressed in terms of powers of concentration of reactants, and the reaction constant K.
That is
For this simple reaction
nA→B
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