Final Reactant Concentrations and Reaction Rates [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 3.876 x 10^-6 2 0.0033 0.0666 0.0166 135 7.40 x 10^-6 3 0.00166 0.0133 0.0166 132 7.576 x 10^-6 4 0.00166 0.0066 0.033 78 1.282 x 10^-5 Using the general rate law equation below and your orders determined, calculate the rate constant for each experiment and then the average. Rate= k[I-]m[BrO3-]n[H+]p k______________ k________________ k________________ k ____________ Average value of k __________________ Units of k__________________ Rewrite the final rate law including values for m, n, p and the average value of k and units:
Final Reactant Concentrations and Reaction Rates [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258 3.876 x 10^-6 2 0.0033 0.0666 0.0166 135 7.40 x 10^-6 3 0.00166 0.0133 0.0166 132 7.576 x 10^-6 4 0.00166 0.0066 0.033 78 1.282 x 10^-5 Using the general rate law equation below and your orders determined, calculate the rate constant for each experiment and then the average. Rate= k[I-]m[BrO3-]n[H+]p k______________ k________________ k________________ k ____________ Average value of k __________________ Units of k__________________ Rewrite the final rate law including values for m, n, p and the average value of k and units:
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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Final Reactant Concentrations and Reaction Rates |
|||||
|
|
[I-] |
[BrO3-] |
[H+] |
Reaction Time |
|
|
Expt. # |
M |
M |
M |
sec. |
M/sec |
|
1 |
0.00166 |
0.0066 |
0.0166 |
258 |
3.876 x 10^-6 |
|
2 |
0.0033 |
0.0666 |
0.0166 |
135 |
7.40 x 10^-6 |
|
3 |
0.00166 |
0.0133 |
0.0166 |
132 |
7.576 x 10^-6 |
|
4 |
0.00166 |
0.0066 |
0.033 |
78 |
1.282 x 10^-5
|
Using the general rate law equation below and your orders determined, calculate the rate constant for each experiment and then the average.
Rate= k[I-]m[BrO3-]n[H+]p
k______________ k________________ k________________ k ____________
Average value of k __________________
Units of k__________________
Rewrite the final rate law including values for m, n, p and the average value of k and units:
_________________________________
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