[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = -198 kJ, and Kc = 34.5, at 1.15 x 10³ K: 2SO2(g) + O2(g) = 2SO3(g) If the temperature on the equilibrium system is suddenly decreased: The value of Ke O increases Odecreases O remains the same The value of Qc O is less than Ke Ois greater than Ke O is equal to Ke The reaction must O run in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of O2 will O increase O decrease O remain the same Show Hint Previous Next>
[References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH = -198 kJ, and Kc = 34.5, at 1.15 x 10³ K: 2SO2(g) + O2(g) = 2SO3(g) If the temperature on the equilibrium system is suddenly decreased: The value of Ke O increases Odecreases O remains the same The value of Qc O is less than Ke Ois greater than Ke O is equal to Ke The reaction must O run in the forward direction to reestablish equilibrium Orun in the reverse direction to reestablish equilibrium O remain in the current position, since it is already at equilibrium The concentration of O2 will O increase O decrease O remain the same Show Hint Previous Next>
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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![5
[References]
Use the References to access important values if needed for this question.
Consider the following system at equilibrium where AH = -198 kJ, and
Kc = 34.5, at 1.15 × 10³ K:
2SO2(g) + O2(g) = 2SO3(g)
If the temperature on the equilibrium system is suddenly decreased:
The value of Ke
O increases
Odecreases
O remains the same
T
The value of Q
O is less than Ke
O is greater than K
O is equal to Kc
The reaction must
O run in the forward direction to reestablish equilibrium
Orun in the reverse direction to reestablish equilibrium
O remain in the current position, since it is already at equilibrium
The concentration of O2 will
O increase
O decrease
O remain the same
O
F5
Show Hint
A
6
F6
&
7
U
K
F7
*
8
DII
F8
(
9
F9
)
O
F10
P
Previous
F11
+
Next
Save and Exit
F12
delete](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F028f9fb7-1c19-4c4c-a0ef-3b56d1a3dafb%2Fc71cb508-50e3-4072-b9f1-17e9baa37c99%2F48ycxkl_processed.jpeg&w=3840&q=75)
Transcribed Image Text:5
[References]
Use the References to access important values if needed for this question.
Consider the following system at equilibrium where AH = -198 kJ, and
Kc = 34.5, at 1.15 × 10³ K:
2SO2(g) + O2(g) = 2SO3(g)
If the temperature on the equilibrium system is suddenly decreased:
The value of Ke
O increases
Odecreases
O remains the same
T
The value of Q
O is less than Ke
O is greater than K
O is equal to Kc
The reaction must
O run in the forward direction to reestablish equilibrium
Orun in the reverse direction to reestablish equilibrium
O remain in the current position, since it is already at equilibrium
The concentration of O2 will
O increase
O decrease
O remain the same
O
F5
Show Hint
A
6
F6
&
7
U
K
F7
*
8
DII
F8
(
9
F9
)
O
F10
P
Previous
F11
+
Next
Save and Exit
F12
delete
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