QuestionReview I Constants I Period
Consider 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 reaction.
Drag the appropriate items to their respective bins.
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Triple [D] and reduce [E] to one third
Decrease [E]
Increase [E]
Triple both and
Increase [F]
Increase [D]
Decrease [D]
Decrease [F]
Leftward shift
Rightward shift
No shift
Studdy Solution
STEP 1
1. The system is at equilibrium initially.
2. The equilibrium reaction is: .
3. Le Chatelier's principle applies to predict the direction of the shift when changes are made to the system.
STEP 2
1. Analyze the effect of concentration changes on the equilibrium position.
2. Classify each action as causing a leftward shift, rightward shift, or no shift.
STEP 3
According to Le Chatelier's principle, if the concentration of a reactant or product is changed, the equilibrium will shift to counteract the change.
STEP 4
Evaluate each action:
- **Triple [D] and reduce [E] to one third**:
- Increasing [D] tends to shift the equilibrium to the right.
- Reducing [E] tends to shift the equilibrium to the left.
- The net effect depends on the relative magnitude of changes, but generally, reducing a reactant has a stronger effect, causing a **leftward shift**.
- **Decrease [E]**:
- Reducing a reactant concentration shifts the equilibrium to the left to produce more reactants.
- **Leftward shift**.
- **Increase [E]**:
- Increasing a reactant concentration shifts the equilibrium to the right to produce more products.
- **Rightward shift**.
- **Triple both [E] and [F]**:
- Increasing [E] shifts the equilibrium to the right.
- Increasing [F] shifts the equilibrium to the left.
- The net effect is likely **no shift** if changes are balanced.
- **Increase [F]**:
- Increasing a product concentration shifts the equilibrium to the left to reduce the product concentration.
- **Leftward shift**.
- **Increase [D]**:
- Increasing a reactant concentration shifts the equilibrium to the right to produce more products.
- **Rightward shift**.
- **Decrease [D]**:
- Reducing a reactant concentration shifts the equilibrium to the left to produce more reactants.
- **Leftward shift**.
- **Decrease [F]**:
- Reducing a product concentration shifts the equilibrium to the right to produce more products.
- **Rightward shift**.
The classification of actions is as follows:
- **Leftward shift**: Triple [D] and reduce [E] to one third, Decrease [E], Increase [F], Decrease [D]
- **Rightward shift**: Increase [E], Increase [D], Decrease [F]
- **No shift**: Triple both [E] and [F]
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