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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The first order reaction AB, has k = 8.00s-¹. If [A]o = 0.500 M, how long will it take when [A] = 0.200 M?
O 0.488 s
8.18 S
0.115 S
O 0.244 S
7
0.100 S
DELL](https://content.bartleby.com/qna-images/question/0c8889e4-511f-4485-9631-829312b0ab2d/d07d2c75-a851-46a0-8919-198119ccab79/pb65xhe_thumbnail.jpeg)
Transcribed Image Text:marked out 31 10.00 PFlag question
The first order reaction AB, has k = 8.00s-¹. If [A]o = 0.500 M, how long will it take when [A] = 0.200 M?
O 0.488 s
8.18 S
0.115 S
O 0.244 S
7
0.100 S
DELL
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- The rate constant for the reaction is 0.200 M-! · s-! at 200 °C. A products If the initial concentration of A is 0.00780 M, what will be the concentration after 105 s? [A] = M * TOOLS x10arrow_forward11. A reaction has a rate constant of k = 3.40 L2 mol-2 min -1, What is the overall reaction order? 1. 1 st order 2. 2nd order 3. 3rd order 4. 4th order 5. none of the abovearrow_forwardIn 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?arrow_forward
- 6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179arrow_forwardIf the order of the reaction is first order for both reagents then using the rate law and the following data solve for K. Rate 1.9 X 10^-6 [I-] = 0.45 M [H2O2] = 0.125 M O A. 1.1 X 10^-5 O B.3.4 X 10^-5 O C. 3.4 X 10^-4 O D. 1.1 X 10^-7arrow_forwardIn 2nd order reaction 2OH →→ H2O + O k = 1.47 x 1010 M-1 s-1. There is an initial OH concentration of [OH]0 = 1.88×10−4M. a)How long will it take for the OH concentration to decrease to 6.0997×10−5M?arrow_forward
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