QuestionConsider the following system at equilibrium:
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 re Drag the appropriate items to their respective bins.
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Triple [D] and reduce [E] to one third
Decrease [E]
Increase
Triple both and
Increase [F]
Inc出ase [D]
Decrease [D]
Decrease [F]
Leftward shift
Rightward shift
No shift
Studdy Solution
STEP 1
1. We are dealing with a chemical equilibrium system.
2. The equilibrium reaction is: .
3. Le Chatelier's principle will be used to predict the shift in equilibrium.
4. Changes in concentration of reactants or products can cause shifts in the equilibrium position.
STEP 2
1. Understand Le Chatelier's principle.
2. Analyze the effect of changing concentrations on the equilibrium.
3. Classify each action based on its effect on the equilibrium.
STEP 3
Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change and re-establish equilibrium.
STEP 4
Analyze each action:
- **Triple [D] and reduce [E] to one third**: Increasing [D] will shift the equilibrium to the right (towards products) to consume the added D. Reducing [E] will shift the equilibrium to the left (towards reactants) to produce more E. The net effect depends on the relative magnitude of these changes, but typically, reducing a reactant has a stronger effect, causing a leftward shift.
- **Decrease [E]**: Reducing [E] shifts the equilibrium to the left to produce more E.
- **Increase [D]**: Increasing [D] shifts the equilibrium to the right to consume the added D.
- **Triple both [E] and [F]**: Increasing [E] shifts the equilibrium to the right to consume the added E. Increasing [F] shifts the equilibrium to the left to consume the added F. The net effect depends on the relative magnitude of these changes, but typically, increasing a product has a stronger effect, causing a leftward shift.
- **Increase [F]**: Increasing [F] shifts the equilibrium to the left to consume the added F.
- **Decrease [D]**: Reducing [D] shifts the equilibrium to the left to produce more D.
- **Decrease [F]**: Reducing [F] shifts the equilibrium to the right to produce more F.
STEP 5
Classify each action:
- **Leftward shift**:
- Triple [D] and reduce [E] to one third
- Decrease [E]
- Triple both [E] and [F]
- Increase [F]
- Decrease [D]
- **Rightward shift**:
- Increase [D]
- Decrease [F]
- **No shift**: None of the actions result in no shift, as all involve changes in concentration that affect the equilibrium.
The classification of actions is complete.
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