Consider the reaction: A → B.Use the below data to determine the second half-life for experiment 2. Please answer in seconds.Experiment25012[A]0.1 M0.2 MInitial Rate [M/S]0.00250.01Incorrect. We learned in the previous problems that this reaction is second order and k = 0.25 M²¹ s²¹.During the first half-life, [A] decreases by 50% (0.2 M to 0.1M). Now we need to determine how long it will take for [A] decrease byanother 50% (0.1 M to 0.05 M). This means the original concentration for the second half-life of experiment #2 is 0.1 M. Consider the reaction: A → B.Use the below data to determine the first half-life for experiment 1. Please answer in seconds.[A]Experiment4,00012Incorrect.0.1 M0.2 MInitial Rate [M/S]0.00250.01When we double the concentration of A, the rate quadruples. This means that this reaction is second order. Make sure you are usingthe correct half-life equation!*Check to make sure you are using the data from Experiment #1.

Answered: Image /qna-images/answer/ae2e0fc8-151a-4f62-85c3-f98d4e73f18a.jpg

Consider the reaction: A → B. Use the below data to determine the first half-life for experiment 1. Please answer in seconds. Initial Rate [M/s] Experiment 4,000 1 2 Incorrect. [A] 0.1 M 0.2 M 0.0025 0.01

Consider the reaction: A → B. Use the below data to determine the first half-life for experiment 1. Please answer in seconds. Initial Rate [M/s] Experiment 4,000 1 2 Incorrect. [A] 0.1 M 0.2 M 0.0025 0.01

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 49E: The reaction AB+C is known to be zero order in A and to have a rate constant of 5.0 102 mol/L s at...

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Question

Consider the reaction: A → B.
Use the below data to determine the second half-life for experiment 2. Please answer in seconds.
Experiment
250
1
2
[A]
0.1 M
0.2 M
Initial Rate [M/S]
0.0025
0.01
Incorrect. We learned in the previous problems that this reaction is second order and k = 0.25 M²¹ s²¹.
During the first half-life, [A] decreases by 50% (0.2 M to 0.1M). Now we need to determine how long it will take for [A] decrease by
another 50% (0.1 M to 0.05 M). This means the original concentration for the second half-life of experiment #2 is 0.1 M.

Consider the reaction: A → B.
Use the below data to determine the first half-life for experiment 1. Please answer in seconds.
[A]
Experiment
4,000
1
2
Incorrect.
0.1 M
0.2 M
Initial Rate [M/S]
0.0025
0.01
When we double the concentration of A, the rate quadruples. This means that this reaction is second order. Make sure you are using
the correct half-life equation!
*Check to make sure you are using the data from Experiment #1.

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