For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction. Express your answer in M−1⋅min−1 to three significant figures.
For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction. Express your answer in M−1⋅min−1 to three significant figures.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.10QP
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Part B Please
Part A:
Consider the second-order reaction:
2HI(g)→H2(g)+I2(g)
Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 3.58×1010 s ([HI]t) for a reaction starting under the condition in the simulation?
Answer: 4.36×10−3 mol/L
Part B:
For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction.
Express your answer in M−1⋅min−1 to three significant figures.
![Most of the time, the rate of a reaction depends on
the concentration of the reactant. In the case of
Characteristics of second-order reactions
second-order reactions, the rate is proportional to
the square of the concentration of the reactant.
For a second-order reaction, [A]→products, the rate of the reaction is given as rate = kA]², where k is the rate constant
1
= kt+
Select the image to explore the simulation, which
will help you to understand how second-order
reactions are identified by the nature of their plots.
You can also observe the rate law for different
and [A is the concentration of reactant A. The integrated rate law for second-order reactions is
[A],
where
TAlo
[At is the concentration of reactant A at time t, k is the rate constant, and Ao is the initial concentration of reactant A.
This equation is of the type y = mx +b. Therefore, the plot of
1
versus time is always a straight line with a slope k and
reactions.
1
a y intercept
[A]
(HI] mol/1
concentration, mol
1L
[A]; mol
2H1 H; + :
Rane lrw: N{HT
-64-10 (mol s) 500 K
Initial rate- 1.6-10' mol(]-s)
19 5 20 25
lime, 10s
slope =k
Start
O Plet (1) vs. time
O Piet InHT] vs. ime
OPlet 1/THT) vs time
Kese
1
[A]o
In the simulation, you can select one of the three
different kinds of plots. You may use the Start,
Stop, and Reset buttons to observe the
corresponding changes in the plot for different
kinds of reactions. You can also select six different
time, s
reactions using the drop-down menu and observe
three different types of plots for each reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffc8e52c4-de61-4660-8309-2c98ec96e370%2Fd14c8eee-cae7-4143-9e9f-5b596fe486b7%2F7xksv0g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Most of the time, the rate of a reaction depends on
the concentration of the reactant. In the case of
Characteristics of second-order reactions
second-order reactions, the rate is proportional to
the square of the concentration of the reactant.
For a second-order reaction, [A]→products, the rate of the reaction is given as rate = kA]², where k is the rate constant
1
= kt+
Select the image to explore the simulation, which
will help you to understand how second-order
reactions are identified by the nature of their plots.
You can also observe the rate law for different
and [A is the concentration of reactant A. The integrated rate law for second-order reactions is
[A],
where
TAlo
[At is the concentration of reactant A at time t, k is the rate constant, and Ao is the initial concentration of reactant A.
This equation is of the type y = mx +b. Therefore, the plot of
1
versus time is always a straight line with a slope k and
reactions.
1
a y intercept
[A]
(HI] mol/1
concentration, mol
1L
[A]; mol
2H1 H; + :
Rane lrw: N{HT
-64-10 (mol s) 500 K
Initial rate- 1.6-10' mol(]-s)
19 5 20 25
lime, 10s
slope =k
Start
O Plet (1) vs. time
O Piet InHT] vs. ime
OPlet 1/THT) vs time
Kese
1
[A]o
In the simulation, you can select one of the three
different kinds of plots. You may use the Start,
Stop, and Reset buttons to observe the
corresponding changes in the plot for different
kinds of reactions. You can also select six different
time, s
reactions using the drop-down menu and observe
three different types of plots for each reaction.
0.00
0.500
20.0
0.382
40.0
0.310
60.0
0.260
80.0
0.224](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffc8e52c4-de61-4660-8309-2c98ec96e370%2Fd14c8eee-cae7-4143-9e9f-5b596fe486b7%2F91ykeer_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Examine experimental data
Consider a second-order reaction in which reactant A decomposes according to the chemical equation 2A-products.
The data given below is the time, in minutes, and the corresponding change in the concentration of reactant A for this
reaction.
t (min)
[A](M)
0.00
0.500
20.0
0.382
40.0
0.310
60.0
0.260
80.0
0.224
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