Part B. Activation Energy Temp. Temp. 1/T Reaction Time Rate of Reaction 2.8 x 10-5/time k oC K K-1 sec. M/sec 40.05 313.20 0.00319 79.40 1.40*10-5 20.0 293.15 0.00341 213.28 5.20*10-6 16.7 289.85 0.00345 155.58 7.14*10-6 9.8 282.95 0.00353 209.90 5.29*10-6 Rate= k[I-]m[BrO3-]n[H+]p Reactant order: m = 2 n=1 p=2 concentration: I = 3.33 x 10-3 ; BrO3 = 6.67 x 10-3; H+=1.67 x 10-2 Find the rate constant k with proper units
Part B. Activation Energy Temp. Temp. 1/T Reaction Time Rate of Reaction 2.8 x 10-5/time k oC K K-1 sec. M/sec 40.05 313.20 0.00319 79.40 1.40*10-5 20.0 293.15 0.00341 213.28 5.20*10-6 16.7 289.85 0.00345 155.58 7.14*10-6 9.8 282.95 0.00353 209.90 5.29*10-6 Rate= k[I-]m[BrO3-]n[H+]p Reactant order: m = 2 n=1 p=2 concentration: I = 3.33 x 10-3 ; BrO3 = 6.67 x 10-3; H+=1.67 x 10-2 Find the rate constant k with proper 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...
Related questions
Question
|
Part B. Activation Energy |
||||||
|
Temp. |
Temp. |
1/T |
Reaction Time |
Rate of Reaction 2.8 x 10-5/time |
k |
|
|
oC |
K |
K-1 |
sec. |
M/sec |
|
|
|
40.05 |
313.20 |
0.00319 |
79.40 |
1.40*10-5 |
|
|
|
20.0 |
293.15 |
0.00341 |
213.28 |
5.20*10-6 |
|
|
|
16.7 |
289.85 |
0.00345 |
155.58 |
7.14*10-6 |
|
|
|
9.8 |
282.95 |
0.00353 |
209.90 |
5.29*10-6 |
|
|
Rate= k[I-]m[BrO3-]n[H+]p
Reactant order: m = 2 n=1 p=2
concentration: I = 3.33 x 10-3 ; BrO3 = 6.67 x 10-3; H+=1.67 x 10-2
Find the rate constant k with proper units
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