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
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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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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.
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