Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec
Consider the following data concerning the equation: H2O2 + 3I– + 2H+ → I3– + 2H2O [H2O2] [I–] [H+] rate I 0.100 M 5.00 × 10–4 M 1.00 × 10–2 M 0.137 M/sec II. 0.100 M 1.00 × 10–3 M 1.00 × 10–2 M 0.268 M/sec III. 0.200 M 1.00 × 10–3 M 1.00 × 10–2 M 0.542 M/sec IV. 0.400 M 1.00 × 10–3 M 2.00 × 10–2 M 1.084 M/sec
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
Consider the following data concerning the equation:
H2O2 + 3I– + 2H+ → I3– + 2H2O
|
|
[H2O2] |
[I–] |
[H+] |
rate |
|
|
I |
0.100 M |
5.00 × 10–4 M |
1.00 × 10–2 M |
0.137 M/sec |
|
|
II. |
0.100 M |
1.00 × 10–3 M |
1.00 × 10–2 M |
0.268 M/sec |
|
|
III. |
0.200 M |
1.00 × 10–3 M |
1.00 × 10–2 M |
0.542 M/sec |
|
|
IV. |
0.400 M |
1.00 × 10–3 M |
2.00 × 10–2 M |
1.084 M/sec |
The rate law for this reaction is
| a. |
rate = k[H2O2][I–][H+]
|
|
| b. |
rate = k[H2O2][H+]
|
|
| c. |
rate = k[H2O2]2[I–]2[H+]2
|
|
| d. |
None of these
|
|
| e. |
rate = k[H2O2][I–]
|
|
| f. |
rate = k[I–][H+]
|
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