For the equilibrium system
`FeO(s)CO(g)hArrFe(s)+CO_(2)(g)`(Exothermic)
How many of the following changes in condition will cause the equilibrium to shift to the right?
(1) Add `CO_(2)` (2) Add `FeO` (3) Add `CO`
(4) Add positive catalyst (5) Increase temperature

Answer

To determine how many of the given changes in condition will cause the equilibrium of the reaction

\[ \text{FeO(s) + CO(g)} \rightleftharpoons \text{Fe(s) + CO}_2(g) \]

to shift to the right, we will analyze each change based on Le Chatelier's principle. This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.

### Step-by-Step Solution:

1. **Add CO₂**:
- Adding CO₂ increases the concentration of a product. According to Le Chatelier's principle, the system will respond by shifting to the left to reduce the concentration of CO₂.
- **Effect**: Shifts to the left (not to the right).

2. **Add FeO**:
- Adding FeO increases the concentration of a reactant. The system will respond by shifting to the right to consume the added FeO and produce more products (Fe and CO₂).
- **Effect**: Shifts to the right.

3. **Add CO**:
- Adding CO also increases the concentration of a reactant. The system will respond by shifting to the right to consume the added CO and produce more products (Fe and CO₂).
- **Effect**: Shifts to the right.

4. **Add a positive catalyst**:
- A catalyst speeds up the rate of both the forward and reverse reactions equally but does not affect the position of the equilibrium. Therefore, adding a catalyst will not cause a shift in the equilibrium position.
- **Effect**: No shift.

5. **Increase temperature**:
- This reaction is exothermic, meaning heat is released when products are formed. Increasing the temperature will shift the equilibrium to the left, as the system will try to absorb the added heat by favoring the endothermic direction (the reverse reaction).
- **Effect**: Shifts to the left (not to the right).

### Summary of Effects:
- Adding CO₂: Shifts left (incorrect)
- Adding FeO: Shifts right (correct)
- Adding CO: Shifts right (correct)
- Adding a positive catalyst: No shift (incorrect)
- Increasing temperature: Shifts left (incorrect)

### Conclusion:
Out of the five changes, only **two changes (adding FeO and adding CO)** will cause the equilibrium to shift to the right.

### Final Answer:
**2 changes will cause the equilibrium to shift to the right.**

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