Certainly! Let's analyze how each action affects the equilibrium of the given chemical reaction:
### The Reaction:
[tex]\[ 2 \text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2 \text{SO}_3(g) \][/tex]
Given equilibrium constant:
[tex]\[ K_c = 1.4 \times 10^1 \][/tex]
### Actions and Effects on the Equilibrium:
1. Increase Volume:
- Effect on Pressure: Increasing the volume of the reaction vessel decreases the pressure.
- Le Chatelier's Principle: The reaction will shift to counteract this change in pressure.
- Analysis of Moles:
In the reaction, reactants (2 SO₂ + 1 O₂) have 3 moles of gas, while the product (2 SO₃) has 2 moles of gas.
- To decrease the pressure, the reaction will shift towards the side with more moles of gas, i.e., shift towards the side of the reactants.
- Conclusion: The equilibrium will shift to the reactants.
2. Add Catalyst:
- Effect on Equilibrium Position: A catalyst speeds up the rate at which equilibrium is achieved but does not change the position of the equilibrium.
- Conclusion: There will be no shift in equilibrium.
3. Add Sulfur Dioxide (SO₂) Gas:
- Effect on Concentration: Adding more SO₂ increases the concentration of one of the reactants.
- Le Chatelier's Principle: The system will counteract this by shifting the equilibrium towards the side that consumes the added reactant, i.e., the product side.
- Conclusion: The equilibrium will shift to the products.
4. Remove Oxygen (O₂) Gas:
- Effect on Concentration: Removing O₂ decreases the concentration of one of the reactants.
- Le Chatelier's Principle: The system will counteract this by shifting the equilibrium towards the side that replenishes the removed reactant, i.e., the reactant side.
- Conclusion: The equilibrium will shift to the reactants.
### Summary:
- Shift to Reactants:
- Increase volume
- Remove oxygen gas
- Shift to Products:
- Add sulfur dioxide gas
- No Shift:
- Add catalyst
You can now place the actions into their respective categories based on these conclusions.
