he reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0359 0.0359 0.0209 2 0.0359 0.0718 0.0418 3 0.0718 0.0359 0.0837 4 0.0718 0.0718 0.167 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate = k [ClO2(aq)]4 [OH-(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of ClO2(aq) is 0.0640 M and that of OH-(aq) is 0.0732 M if the temperature is the same as that used to obtain the data shown above? M/s
he reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results: Experiment [ClO2(aq)] (M) [OH-(aq)] (M) Rate (M/s) 1 0.0359 0.0359 0.0209 2 0.0359 0.0718 0.0418 3 0.0718 0.0359 0.0837 4 0.0718 0.0718 0.167 (a) What is the rate law for this reaction? Rate = k [ClO2(aq)] [OH-(aq)] Rate = k [ClO2(aq)]2 [OH-(aq)] Rate = k [ClO2(aq)] [OH-(aq)]2 Rate = k [ClO2(aq)]2 [OH-(aq)]2 Rate = k [ClO2(aq)] [OH-(aq)]3 Rate = k [ClO2(aq)]4 [OH-(aq)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of ClO2(aq) is 0.0640 M and that of OH-(aq) is 0.0732 M if the temperature is the same as that used to obtain the data shown above? M/s
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
he reaction 2 ClO2(aq) + 2 OH-(aq) ClO3-(aq) + ClO3-(aq) + H2O(l) was studied at a certain temperature with the following results:
Experiment | [ClO2(aq)] (M) | [OH-(aq)] (M) | Rate (M/s) |
---|---|---|---|
1 | 0.0359 | 0.0359 | 0.0209 |
2 | 0.0359 | 0.0718 | 0.0418 |
3 | 0.0718 | 0.0359 | 0.0837 |
4 | 0.0718 | 0.0718 | 0.167 |
(a) What is the rate law for this reaction?
Rate = k [ClO2(aq)] [OH-(aq)]
Rate = k [ClO2(aq)]2 [OH-(aq)]
Rate = k [ClO2(aq)] [OH-(aq)]2
Rate = k [ClO2(aq)]2 [OH-(aq)]2
Rate = k [ClO2(aq)] [OH-(aq)]3
Rate = k [ClO2(aq)]4 [OH-(aq)]
(b) What is the value of the rate constant?
(c) What is the reaction rate when the concentration of ClO2(aq) is 0.0640 M and that of OH-(aq) is 0.0732 M if the temperature is the same as that used to obtain the data shown above?
M/s
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