Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 0.0744 s : CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HCl (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.270M. Calculate the concentration of CICH₂CH₂Cl in the vessel 9.70 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0
Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 0.0744 s : CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HCl (g) Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.270M. Calculate the concentration of CICH₂CH₂Cl in the vessel 9.70 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0
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...
Related questions
Question
100%
![- с
Gmail
|||
=
YouTube Translate
www-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-UibwdleAUz2IYCcR4NM7yr_IpMriNwxObE8AQh1KpvSelejev-TduPS6C7h-fsNAPGB1ZaRgTTPXJcYxzQV8...
O KINETICS AND EQUILIBRIUM
Using an integrated rate law for a first-order reaction
At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 0.0744 s
CICH₂CH₂Cl (g) → CH₂CHCI (g) + HCl (g)
M
Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.270 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 9.70 seconds later. You may
assume no other reaction is important.
Round your answer to 2 significant digits.
82°F
Mostly cloudy
Explanation
Check
Q Search
F
i
1/5
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A-
O
<)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6a19bf2-47f2-4e82-bd9e-871794366298%2F34a25350-67d2-4ff7-ac32-a24b76d95af9%2Fy6cfwor_processed.jpeg&w=3840&q=75)
Transcribed Image Text:- с
Gmail
|||
=
YouTube Translate
www-awu.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-UibwdleAUz2IYCcR4NM7yr_IpMriNwxObE8AQh1KpvSelejev-TduPS6C7h-fsNAPGB1ZaRgTTPXJcYxzQV8...
O KINETICS AND EQUILIBRIUM
Using an integrated rate law for a first-order reaction
At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 0.0744 s
CICH₂CH₂Cl (g) → CH₂CHCI (g) + HCl (g)
M
Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.270 M. Calculate the concentration of CICH₂CH₂Cl in the vessel 9.70 seconds later. You may
assume no other reaction is important.
Round your answer to 2 significant digits.
82°F
Mostly cloudy
Explanation
Check
Q Search
F
i
1/5
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | A-
O
<)
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
Step 1
Given,
ClCH2CH2Cl(g) ----> CH2CHCl(g) + HCl(g)
Reaction follows first order kinetics.
Rate constant (k) = 0.0744 s-1
Time (t) = 9.70 s
Initial concentration of ClCH2CH2Cl = [ClCH2CH2Cl]0 = 0.270 M
concentration of ClCH2CH2Cl after 9.70 s = [ClCH2CH2Cl]t = ? M
Step by step
Solved in 3 steps
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY