The half-life of a first-order reaction is In (2) t1/2 so, first calculate k using the integrated rate equation for a first-order reaction. [A]: = -kt In [A]o If 38.0% of the compound decomposed, then 62.0% remains after 67.0 min.
The half-life of a first-order reaction is In (2) t1/2 so, first calculate k using the integrated rate equation for a first-order reaction. [A]: = -kt In [A]o If 38.0% of the compound decomposed, then 62.0% remains after 67.0 min.
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 63QAP: The uncoiling of deoxyribonucleic acid (DNA) is a first-order reaction. Its activation energy is 420...
Related questions
Question
After 67.0 min,67.0 min, 38.0%38.0% of a compound has decomposed. What is the half‑life of this reaction assuming first‑order kinetics?
I have no idea how to work this out. The homework program has given me hints and I have used them but they aren't giving me the correct answer. I am on my 14th attempt.
![The half-life of a first-order
reaction is
In (2)
t1/2
so, first calculate k using the
integrated rate equation for a
first-order reaction.
[A]:
= -kt
In
[A]o
If 38.0% of the compound
decomposed, then 62.0% remains
after 67.0 min.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1f847689-de5a-49d2-acc2-8d41964079b3%2F9c9cf8aa-f326-43ac-89e2-be9b5400f597%2F2ppkgro.png&w=3840&q=75)
Transcribed Image Text:The half-life of a first-order
reaction is
In (2)
t1/2
so, first calculate k using the
integrated rate equation for a
first-order reaction.
[A]:
= -kt
In
[A]o
If 38.0% of the compound
decomposed, then 62.0% remains
after 67.0 min.
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 3 steps with 3 images
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: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry: Principles and Practice
Chemistry
ISBN:
9780534420123
Author:
Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning