Consider the hypothetical reaction A +B+ 2C –→ 2D + 3E where the rate law is A[A] k[A][B}* At Rate = - %3D An experiment is carried out where [A], = 1.0 x 10-2 M, B. = 7.0 M, and [C], = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k = 5.4x10^-3 L² mols-1 b. Calculate the half-life for this experiment. Half-life = 3.6 c. Calculate the concentration of A after 18.0 seconds. Concentration = d. Calculate the concentration of C after 18 seconds. Concentration = 2.0 M
Consider the hypothetical reaction A +B+ 2C –→ 2D + 3E where the rate law is A[A] k[A][B}* At Rate = - %3D An experiment is carried out where [A], = 1.0 x 10-2 M, B. = 7.0 M, and [C], = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k = 5.4x10^-3 L² mols-1 b. Calculate the half-life for this experiment. Half-life = 3.6 c. Calculate the concentration of A after 18.0 seconds. Concentration = d. Calculate the concentration of C after 18 seconds. Concentration = 2.0 M
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...
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![Consider the hypothetical reaction
A + B+ 2C –→ 2D + 3E
where the rate law is
A[A]
k[A][B]?
At
Rate
An experiment is carried out where
[A], = 1.0 x 10-2 M,
7.0 M, and
[Blo
[C), = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of
A is
-3
3.8 x 10 M.
a. Calculate the value of k for this reaction.
k =
L? mols-1
5.4x10^-3
b. Calculate the half-life for this experiment.
Half-life =
3.6
S
c. Calculate the concentration of A after 18.0 seconds.
Concentration =
M
d. Calculate the concentration of C after 18 seconds.
Concentration =
2.0
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f79bd48-9cb9-4531-8b82-3e5c7476c17a%2Fd006a5d4-95f4-4f36-a367-54534eecd9b1%2Fdnb3pi8_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the hypothetical reaction
A + B+ 2C –→ 2D + 3E
where the rate law is
A[A]
k[A][B]?
At
Rate
An experiment is carried out where
[A], = 1.0 x 10-2 M,
7.0 M, and
[Blo
[C), = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of
A is
-3
3.8 x 10 M.
a. Calculate the value of k for this reaction.
k =
L? mols-1
5.4x10^-3
b. Calculate the half-life for this experiment.
Half-life =
3.6
S
c. Calculate the concentration of A after 18.0 seconds.
Concentration =
M
d. Calculate the concentration of C after 18 seconds.
Concentration =
2.0
M
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