Consider the hypothetical reaction A + B + 2C 2D + 3E where the rate law is Rate A[A] At k= = k[A][B]² An experiment is carried out where [A] = 1.0 × 10-2 M, [B] = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 × 10-3 M. a. Calculate the value of k for this reaction. L² mol s S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. Concentration = M d. Calculate the concentration of C after 14 seconds. Concentration = -1 M
Consider the hypothetical reaction A + B + 2C 2D + 3E where the rate law is Rate A[A] At k= = k[A][B]² An experiment is carried out where [A] = 1.0 × 10-2 M, [B] = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 × 10-3 M. a. Calculate the value of k for this reaction. L² mol s S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 14.0 seconds. Concentration = M d. Calculate the concentration of C after 14 seconds. Concentration = -1 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
Rate
A[A]
At
k=
=
-2
An experiment is carried out where [A]o = 1.0 × 10−² m, [B]₁ = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 6.0
seconds, the concentration of A is 3.8 × 10-³ M.
a. Calculate the value of k for this reaction.
-2 1
k[A] [B]²
b. Calculate the half-life for this experiment.
Half-life =
Concentration =
L² mol s
S
c. Calculate the concentration of after 14.0 seconds.
Concentration =
M
d. Calculate the concentration of C after 14 seconds.
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08bb2a94-da17-43f2-90ab-4ad444df37b3%2Fbc59e791-6775-4598-9d99-2fd8ac4d0667%2Fv13lu68_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the hypothetical reaction
A + B + 2C → 2D + 3E
where the rate law is
Rate
A[A]
At
k=
=
-2
An experiment is carried out where [A]o = 1.0 × 10−² m, [B]₁ = 8.0 M, and [C] = 2.0 M. The reaction is started, and after 6.0
seconds, the concentration of A is 3.8 × 10-³ M.
a. Calculate the value of k for this reaction.
-2 1
k[A] [B]²
b. Calculate the half-life for this experiment.
Half-life =
Concentration =
L² mol s
S
c. Calculate the concentration of after 14.0 seconds.
Concentration =
M
d. Calculate the concentration of C after 14 seconds.
M
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