70% iPad 11:35 PM 51_Kinetic_Homework.pdf 4. A reaction in which X and Y reacts to form product Z is a first order in X, and 2 order in Y. a) Write the rate law for this reaction b) What is the overall order of this reaction. c) By what factor does the reaction rate change if [X] is doubled and [Y] stays the same? d) By what factor does the reaction rate change if [Y] is doubled and [X] stays the same? e) By what factor does the reaction rate change if [X] is doubled and [Y] is halved? 5. Consider the reaction: H2(g) Br2(g) HBr(g) This reaction is first order reaction. k = .053s1 a) Calculate the rate of the reaction when [HBr] = 0.055M b) Calculate the half-life of this reaction c) What is the new rate for this reaction if the reaction was to be a second order reaction? 6. A reaction has a rate constant of 0.0117 M/s at 400.0K and 0.689 M/s at 450.0K. What is the activation energy of the reaction? 7. Consider the reaction: HBr(g) H2(g) Br2(g) y = -0.0236x + 0.897 Time (s) a. Calculate the concentration of HgO after 1 minute b. Calculate the concentration of Hg after 1 minute. c. Sketch how the plot would look if the reaction was performed at a much hotter and colder temperature To Do Notifications Inbox Dashboard Calendar In [HgO]
70% iPad 11:35 PM 51_Kinetic_Homework.pdf 4. A reaction in which X and Y reacts to form product Z is a first order in X, and 2 order in Y. a) Write the rate law for this reaction b) What is the overall order of this reaction. c) By what factor does the reaction rate change if [X] is doubled and [Y] stays the same? d) By what factor does the reaction rate change if [Y] is doubled and [X] stays the same? e) By what factor does the reaction rate change if [X] is doubled and [Y] is halved? 5. Consider the reaction: H2(g) Br2(g) HBr(g) This reaction is first order reaction. k = .053s1 a) Calculate the rate of the reaction when [HBr] = 0.055M b) Calculate the half-life of this reaction c) What is the new rate for this reaction if the reaction was to be a second order reaction? 6. A reaction has a rate constant of 0.0117 M/s at 400.0K and 0.689 M/s at 450.0K. What is the activation energy of the reaction? 7. Consider the reaction: HBr(g) H2(g) Br2(g) y = -0.0236x + 0.897 Time (s) a. Calculate the concentration of HgO after 1 minute b. Calculate the concentration of Hg after 1 minute. c. Sketch how the plot would look if the reaction was performed at a much hotter and colder temperature To Do Notifications Inbox Dashboard Calendar In [HgO]
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 98CWP: A certain reaction has the form aAProducts At a particular temperature, concentration versus time...
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iPad
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51_Kinetic_Homework.pdf
4. A reaction in which X and Y reacts to form product Z is a first order in X, and 2 order in
Y.
a) Write the rate law for this reaction
b) What is the overall order of this reaction.
c) By what factor does the reaction rate change if [X] is doubled and [Y] stays the same?
d) By what factor does the reaction rate change if [Y] is doubled and [X] stays the same?
e) By what factor does the reaction rate change if [X] is doubled and [Y] is halved?
5. Consider the reaction:
H2(g)
Br2(g)
HBr(g)
This reaction is first order reaction. k = .053s1
a) Calculate the rate of the reaction when [HBr] = 0.055M
b) Calculate the half-life of this reaction
c) What is the new rate for this reaction if the reaction was to be a second order
reaction?
6. A reaction has a rate constant of 0.0117 M/s at 400.0K and 0.689 M/s at 450.0K. What is
the activation energy of the reaction?
7. Consider the reaction:
HBr(g) H2(g)
Br2(g)
y = -0.0236x + 0.897
Time (s)
a. Calculate the concentration of HgO after 1 minute
b. Calculate the concentration of Hg after 1 minute.
c. Sketch how the plot would look if the reaction was performed at a much hotter and
colder temperature
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Inbox
Dashboard
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In [HgO]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7d23c96d-31a9-42e5-b3a5-12aac80129ac%2Ffb414575-2ebd-4f50-9edf-abe4c8c17f58%2Fmlvk1e.png&w=3840&q=75)
Transcribed Image Text:70%
iPad
11:35 PM
51_Kinetic_Homework.pdf
4. A reaction in which X and Y reacts to form product Z is a first order in X, and 2 order in
Y.
a) Write the rate law for this reaction
b) What is the overall order of this reaction.
c) By what factor does the reaction rate change if [X] is doubled and [Y] stays the same?
d) By what factor does the reaction rate change if [Y] is doubled and [X] stays the same?
e) By what factor does the reaction rate change if [X] is doubled and [Y] is halved?
5. Consider the reaction:
H2(g)
Br2(g)
HBr(g)
This reaction is first order reaction. k = .053s1
a) Calculate the rate of the reaction when [HBr] = 0.055M
b) Calculate the half-life of this reaction
c) What is the new rate for this reaction if the reaction was to be a second order
reaction?
6. A reaction has a rate constant of 0.0117 M/s at 400.0K and 0.689 M/s at 450.0K. What is
the activation energy of the reaction?
7. Consider the reaction:
HBr(g) H2(g)
Br2(g)
y = -0.0236x + 0.897
Time (s)
a. Calculate the concentration of HgO after 1 minute
b. Calculate the concentration of Hg after 1 minute.
c. Sketch how the plot would look if the reaction was performed at a much hotter and
colder temperature
To Do
Notifications
Inbox
Dashboard
Calendar
In [HgO]
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