Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is A[A] At Rate == = k[A][B]² An experiment is carried out where [A]o = 1.0 × 10-2² 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 3.8 × 10-³ M. a. Calculate the value of k for this reaction. L² mol 2S-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = d. Calculate the concentration of C after 19 seconds. Concentration = M M
Consider the hypothetical reaction A+B+ 2C 2D + 3E where the rate law is A[A] At Rate == = k[A][B]² An experiment is carried out where [A]o = 1.0 × 10-2² 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 3.8 × 10-³ M. a. Calculate the value of k for this reaction. L² mol 2S-1 k= b. Calculate the half-life for this experiment. Half-life = S c. Calculate the concentration of A after 19.0 seconds. Concentration = d. Calculate the concentration of C after 19 seconds. Concentration = M M
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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![Consider the hypothetical reaction
A+B+ 2C 2D + 3E
where the rate law is
Δ[Α]
At
=
An experiment is carried out where
[A]o
1.0 × 10-² M,
Rate
=
Blo
3.0 M, and
[C]o
2.0 M. The reaction is started, and after 6.0 seconds,
the concentration of
A is
3.8 × 10-3
=
= k[A][B]²
M.
a. Calculate the value of k for this reaction.
L² mol 2S-1
k=
b. Calculate the half-life for this experiment.
Half-life =
S
c. Calculate the concentration of A after
19.0 seconds.
Concentration =
d. Calculate the concentration of C after
19 seconds.
Concentration =
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdb5c194b-e795-4bc8-bd29-1bd3357aeff1%2F9a9902cb-9dbe-47e7-abfb-13def9cd6a31%2Fvp5it9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the hypothetical reaction
A+B+ 2C 2D + 3E
where the rate law is
Δ[Α]
At
=
An experiment is carried out where
[A]o
1.0 × 10-² M,
Rate
=
Blo
3.0 M, and
[C]o
2.0 M. The reaction is started, and after 6.0 seconds,
the concentration of
A is
3.8 × 10-3
=
= k[A][B]²
M.
a. Calculate the value of k for this reaction.
L² mol 2S-1
k=
b. Calculate the half-life for this experiment.
Half-life =
S
c. Calculate the concentration of A after
19.0 seconds.
Concentration =
d. Calculate the concentration of C after
19 seconds.
Concentration =
M
M
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