Applying Le Châtelier's Principle 12 of 22 <> N Review | Constants | Periodic Table Consider the following system at equilibrium: D(aq) + E(aq) 2F(aq) When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help Increase (D] If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the Decrease [F] Decrease (E) Decrease (D] Increase (F] stress. Triple (D] and reduce [E] to one third Triple both (E] and (F] Increase (E] Leftward shift Rightward shift No shift
Applying Le Châtelier's Principle 12 of 22 <> N Review | Constants | Periodic Table Consider the following system at equilibrium: D(aq) + E(aq) 2F(aq) When a chemical reaction is at equilibrium, Q (the reaction quotient) is equal to K (the equilibrium constant). If a stress is applied to the mixture that changes the value of Q, then the system is no longer at equilibrium. To regain equilibrium, the reaction will either proceed forward or in reverse until Q is equal to K once again. Alternatively, equilibrium can be disrupted by a change in temperature, which changes the value of K The result however is the same, and the reaction will proceed forward or in reverse until Q is equal to the new K. Le Châtelier's principle summarizes this idea: Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction. Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help Increase (D] If a stress is applied to a reaction mixture at equilibrium, a net reaction occurs in the direction that relieves the Decrease [F] Decrease (E) Decrease (D] Increase (F] stress. Triple (D] and reduce [E] to one third Triple both (E] and (F] Increase (E] Leftward shift Rightward shift No shift
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
![<Homework #4 - Chapter 15 - Chemical Equilibrium
Applying Le Châtelier's Principle
12 of 22
I Review | Constants | Periodic Table
Consider the following system at equilibrium:
D(aq) + E(aq) = 2F(aq)
When a chemical reaction is at equilibrium, Q (the
reaction quotient) is equal to K (the equilibrium
constant). If a stress is applied to the mixture that
changes the value of Q, then the system is no longer at
equilibrium. To regain equilibrium, the reaction will either
proceed forward or in reverse until Q is equal to K once
again. Alternatively, equilibrium can be disrupted by a
change in temperature, which changes the value of K.
The result however is the same, and the reaction will
proceed forward or in reverse until Q is equal to the new
K. Le Châtelier's principle summarizes this idea:
Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.
Drag the appropriate items to their respective bins.
• View Available Hint(s)
Reset
Help
Increase [D]
Decrease [F]
Decrease [E]
Decrease [D]
Increase [F]
If a stress is applied to a reaction mixture at equilibrium,
a net reaction occurs in the direction that relieves the
stress.
Triple [D] and
reduce [E] to one third
Triple both [E] and [F]
Increase [E]
Leftward shift
Rightward shift
No shift](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87faf35d-bdff-4fde-b9fe-6459d170f061%2F686bc8ff-b591-4cca-8bed-476d3216ea84%2Fqkkllpo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:<Homework #4 - Chapter 15 - Chemical Equilibrium
Applying Le Châtelier's Principle
12 of 22
I Review | Constants | Periodic Table
Consider the following system at equilibrium:
D(aq) + E(aq) = 2F(aq)
When a chemical reaction is at equilibrium, Q (the
reaction quotient) is equal to K (the equilibrium
constant). If a stress is applied to the mixture that
changes the value of Q, then the system is no longer at
equilibrium. To regain equilibrium, the reaction will either
proceed forward or in reverse until Q is equal to K once
again. Alternatively, equilibrium can be disrupted by a
change in temperature, which changes the value of K.
The result however is the same, and the reaction will
proceed forward or in reverse until Q is equal to the new
K. Le Châtelier's principle summarizes this idea:
Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.
Drag the appropriate items to their respective bins.
• View Available Hint(s)
Reset
Help
Increase [D]
Decrease [F]
Decrease [E]
Decrease [D]
Increase [F]
If a stress is applied to a reaction mixture at equilibrium,
a net reaction occurs in the direction that relieves the
stress.
Triple [D] and
reduce [E] to one third
Triple both [E] and [F]
Increase [E]
Leftward shift
Rightward shift
No shift
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