For a particular reaction, AH = 73.5 kJ and AS = 193.7 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? PT= Incorrect Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than O greater than K
For a particular reaction, AH = 73.5 kJ and AS = 193.7 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? PT= Incorrect Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than O greater than K
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 102CP
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For a particular reaction, AH = 73.5 kJ and AS - 193.7 J/K. Assuming these values change very little with temperature, at
what temperature does the reaction change from nonspontaneous to spontaneous?
T-
Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature?
H
Incorrect
less than
Ogreater than
▬▬
Search
A
3
50
F10
*-
F11
F12
PrtSc
Insert
K
Delete](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9437567b-8da5-455d-a4fe-2bd0f454b63f%2F5f072b51-e3d8-490a-99e3-817934bd6443%2Fxt8lxn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:√
Macmillan Learning
For a particular reaction, AH = 73.5 kJ and AS - 193.7 J/K. Assuming these values change very little with temperature, at
what temperature does the reaction change from nonspontaneous to spontaneous?
T-
Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature?
H
Incorrect
less than
Ogreater than
▬▬
Search
A
3
50
F10
*-
F11
F12
PrtSc
Insert
K
Delete
![General Chemistry 4th Edition
FANA
The equation represents the decomposition of a generic diatomic element in its standard state.
X₂(g) →X(g)
Assume that the standard molar Gibbs energy of formation of X(g) is 5.97 kJ-mol-¹ at 2000. K and -52.12 kJ-mol-¹ at 3000. K.
Determine the value of K (the thermodynamic equilibrium constant) at each temperature.
K at 2000. K =
K at 3000. K =
Assuming that AHin is independent of temperature, determine the value of AHin from this data.
AHin =
O Search
&
F8
8
F9
08
F10
*-
F11
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presented by Macmillan Learning
*+
F12
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kJ-mol-1
Question Source: McQuarrie, Rock, And Gallop
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Transcribed Image Text:General Chemistry 4th Edition
FANA
The equation represents the decomposition of a generic diatomic element in its standard state.
X₂(g) →X(g)
Assume that the standard molar Gibbs energy of formation of X(g) is 5.97 kJ-mol-¹ at 2000. K and -52.12 kJ-mol-¹ at 3000. K.
Determine the value of K (the thermodynamic equilibrium constant) at each temperature.
K at 2000. K =
K at 3000. K =
Assuming that AHin is independent of temperature, determine the value of AHin from this data.
AHin =
O Search
&
F8
8
F9
08
F10
*-
F11
University Science Books
presented by Macmillan Learning
*+
F12
PrtSc
kJ-mol-1
Question Source: McQuarrie, Rock, And Gallop
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Delete
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