3. The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant of 5.00 x 10³ cm-1 M-1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The data from the experiment are given in the table below. Calculate the initial concentration of the colored species. a. [X] (M) ? 4.00 x 10-5 3.00 x 10-5 1.50 x 10-5 Absorbance 0.600 0.200 0.150 0.075 Time (min) C. Calculate the number of minutes it takes for the absorbance to drop from 0.600 to 0.075. 0.0 35.0 44.2 ? b. Calculate the rate constant for the first-order reaction using the values given for concentration and time. Include units with your answer.
3. The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant of 5.00 x 10³ cm-1 M-1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The data from the experiment are given in the table below. Calculate the initial concentration of the colored species. a. [X] (M) ? 4.00 x 10-5 3.00 x 10-5 1.50 x 10-5 Absorbance 0.600 0.200 0.150 0.075 Time (min) C. Calculate the number of minutes it takes for the absorbance to drop from 0.600 to 0.075. 0.0 35.0 44.2 ? b. Calculate the rate constant for the first-order reaction using the values given for concentration and time. Include units with your answer.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 85IL: The color change accompanying the reaction of phenolphthalein with strong base is illustrated below....
Related questions
Question
![3. The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a
spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant
of 5.00 x 10³ cm-1 M-1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The
data from the experiment are given in the table below.
Calculate the initial concentration of the colored species.
a.
[X]
(M)
4.00 x 10-5
3.00 x 10-5.
1.50 x 10-5
Absorbance
0.600
0.200
0.150
0.075
Time
(min)
C. Calculate the number of minutes it takes for the absorbance to drop from 0.600 to 0.075.
0.0
35.0
44.2
?
b. Calculate the rate constant for the first-order reaction using the values given for concentration and time.
Include units with your answer.
O2 from
4005
J](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F50de52e1-7d33-4b3c-a050-8482f7f33c6d%2F42b012d6-fe56-44a7-bf4e-405af1c73cc6%2F5sxyc2i_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3. The first-order decomposition of a colored chemical species, X, into colorless products is monitored with a
spectrophotometer by measuring changes in absorbance over time. Species X has a molar absorptivity constant
of 5.00 x 10³ cm-1 M-1 and the path length of the cuvette containing the reaction mixture is 1.00 cm. The
data from the experiment are given in the table below.
Calculate the initial concentration of the colored species.
a.
[X]
(M)
4.00 x 10-5
3.00 x 10-5.
1.50 x 10-5
Absorbance
0.600
0.200
0.150
0.075
Time
(min)
C. Calculate the number of minutes it takes for the absorbance to drop from 0.600 to 0.075.
0.0
35.0
44.2
?
b. Calculate the rate constant for the first-order reaction using the values given for concentration and time.
Include units with your answer.
O2 from
4005
J
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning