Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Δ[Α] At = Rate = = An experiment is carried out where [A]o 1.0 × 10-² M, [B]o 3.0 M, and [C]o = 2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is -3 3.8 × 10-³ a. M. = k[A][B]² = k= Calculate the value of k for this reaction. L² mol 2S-1 b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = M d. Calculate the concentration of C after 19 seconds. Concentration = M
Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is Δ[Α] At = Rate = = An experiment is carried out where [A]o 1.0 × 10-² M, [B]o 3.0 M, and [C]o = 2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is -3 3.8 × 10-³ a. M. = k[A][B]² = k= Calculate the value of k for this reaction. L² mol 2S-1 b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = M d. Calculate the concentration of C after 19 seconds. Concentration = 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
Δ[Α]
At
Rate =
= k[A] [B]²
An experiment is carried out where
[A] = 1.0 × 10-² M,
=
-3
3.8 × 10-³ M.
=
[Blo
3.0 M, and
[C]o
= 2.0 M. The reaction is started, and after 6.0 seconds,
the concentration of
A is
k=
a. Calculate the value of k for this reaction.
-2
L² mol s
b. Calculate the half-life for this experiment.
Half-life =
S
c. Calculate the concentration of A after
19.0 seconds.
Concentration =
M
d. Calculate the concentration of C after
19 seconds.
Concentration =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fac5c0af2-5f1c-4dfc-8647-f9548fdbda76%2F9fa645e2-1eb5-4511-bccd-fe558be3afbc%2Fjk9f8f5q_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the hypothetical reaction
A + B + 2C 2D + 3E
where the rate law is
Δ[Α]
At
Rate =
= k[A] [B]²
An experiment is carried out where
[A] = 1.0 × 10-² M,
=
-3
3.8 × 10-³ M.
=
[Blo
3.0 M, and
[C]o
= 2.0 M. The reaction is started, and after 6.0 seconds,
the concentration of
A is
k=
a. Calculate the value of k for this reaction.
-2
L² mol s
b. Calculate the half-life for this experiment.
Half-life =
S
c. Calculate the concentration of A after
19.0 seconds.
Concentration =
M
d. Calculate the concentration of C after
19 seconds.
Concentration =
M
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