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.

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.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction

Section: Chapter Questions

Problem 2ASA

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Question

Reaction Conc, Na,d O3| Cune. HCI 4Als.
|
AIme (3) Rabe
I1.3085840
0.10M
•30M 0.4563/64 |0.028 F0913
15 M 12267196 | 0,01870913
30M 1.5360817 0.300349
2
65.56796607
5. 11431671
O.10 M
3
0.050 M
4
0.025 M
0:30M 1.54866|1
1.007568
1,358380874
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.
-1-4
-2:5
Rate= k [ Naz s03] [Hc1]

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