The reaction A C is first order in the reactant A and is known to go to completion. The product C is colored and absorbs light strongly at 550 nm, while the reactant and intermediates are colorless. A solution of A was prepared, and the absorbance of C at 550 nm was measured as a function of time. (Note that the absorbance of C is directly proportional to its concentration.) Use the following data to determine the half-life of the reaction:
The reaction A C is first order in the reactant A and is known to go to completion. The product C is colored and absorbs light strongly at 550 nm, while the reactant and intermediates are colorless. A solution of A was prepared, and the absorbance of C at 550 nm was measured as a function of time. (Note that the absorbance of C is directly proportional to its concentration.) Use the following data to determine the half-life of the reaction:
Chemistry
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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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I'm not really sure how to approach this problem. I thought you could substitute the half life equation into the integrated equation for first order reactions, but that didn't work.

Transcribed Image Text:The reaction A → Cis first order in the reactant A and is known to go to completion.
The product C is colored and absorbs light strongly at 550 nm, while the reactant and
intermediates are colorless. A solution of A was prepared, and the absorbance of C at
550 nm was measured as a function of time. (Note that the absorbance of C is directly
proportional to its concentration.) Use the following data to determine the half-life of
the reaction:
Time (s)
Absorbance
0.000
0.444
10
0.724
1.188
20
100
200
1.200
500
1.200
Expert Solution

Step 1
Given:
wavelength = 550 nm
Time (s) | Absorbance |
0 | 0.000 |
10 | 0.444 |
20 | 0.724 |
100 | 1.188 |
200 | 1.200 |
500 | 1.200 |
formula = [C] =
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