For the reaction `CaCO_(3)(s)hArrCaO(s)+CO_(2)(g)` the equilibrium amount of `CO_(2)` can be increased by `:`

Options

A. Adding a suitable catalyst
B. Adding more limestone
C. Increasing volume
D. Adding inert gas at constant volume

Answer

To determine how to increase the equilibrium amount of \( CO_2 \) in the reaction

\[ CaCO_3(s) \rightleftharpoons CaO(s) + CO_2(g) \]

we need to analyze the options provided and apply Le Chatelier's principle.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
The reaction involves calcium carbonate (\( CaCO_3 \)) decomposing into calcium oxide (\( CaO \)) and carbon dioxide (\( CO_2 \)). Here, \( CaCO_3 \) and \( CaO \) are solids, while \( CO_2 \) is a gas.

2. **Identifying the Components**:
In this equilibrium, we have:
- Reactants: \( CaCO_3(s) \) (solid)
- Products: \( CaO(s) \) (solid) and \( CO_2(g) \) (gas)

3. **Applying Le Chatelier's Principle**:
According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium.

4. **Analyzing Each Option**:
- **Option A: Adding a suitable catalyst**:
A catalyst speeds up the rate of both the forward and reverse reactions equally but does not change the position of equilibrium. Thus, this option does not increase \( CO_2 \) concentration.

- **Option B: Adding more limestone (CaCO3)**:
Since \( CaCO_3 \) is a solid, adding more of it does not affect the equilibrium position. Therefore, this option is incorrect.

- **Option C: Increasing the volume**:
Increasing the volume of the system decreases the pressure. According to Le Chatelier's principle, the equilibrium will shift towards the side with more moles of gas to counteract the decrease in pressure. In this case, the right side has one mole of \( CO_2 \) gas, which will increase its concentration. This option is correct.

- **Option D: Adding an inert gas at constant volume**:
Adding an inert gas at constant volume increases the total pressure but does not affect the partial pressures of the gases involved in the reaction. Therefore, it does not shift the equilibrium position and is incorrect.

5. **Conclusion**:
The correct answer is **Option C: Increasing the volume** will increase the equilibrium amount of \( CO_2 \).