For the reaction
`CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)`
at a given temperature, the equilibrium amount of `CO_(2)(g)` can be increased by

Options

A. Adding a suitable catalyst
B. Adding an inert gas
C. Decreasing the volume of the container
D. Increasing the amount of `CO(g)`

Explanation

To solve the question regarding the equilibrium reaction:

\[ \text{CO(g)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO}_2\text{(g)} + \text{H}_2\text{(g)} \]

we need to determine how to increase the equilibrium amount of \(\text{CO}_2\) at a given temperature.

### Step-by-Step Solution:

1. **Identify the Reaction Components**:
- The reactants are \(\text{CO(g)}\) and \(\text{H}_2\text{O(g)}\).
- The products are \(\text{CO}_2\text{(g)}\) and \(\text{H}_2\text{(g)}\).

2. **Calculate \(\Delta N_g\)**:
- \(\Delta N_g\) is the change in the number of moles of gas from reactants to products.
- For the given reaction:
- Moles of gas on the reactant side = 2 (1 mole of CO + 1 mole of H₂O)
- Moles of gas on the product side = 2 (1 mole of CO₂ + 1 mole of H₂)
- Therefore, \(\Delta N_g = 2 - 2 = 0\).

3. **Analyze the Effect of \(\Delta N_g = 0\)**:
- When \(\Delta N_g = 0\), changes in pressure or volume do not affect the equilibrium position. Thus, options involving changes in pressure or volume will not increase the amount of \(\text{CO}_2\).

4. **Evaluate Each Option**:
- **Option 1: Adding a suitable catalyst**:
- Incorrect. A catalyst speeds up the rate of reaching equilibrium but does not change the equilibrium concentrations.
- **Option 2: Adding an inert gas**:
- Incorrect. Adding an inert gas at constant temperature and pressure does not change the partial pressures of the reactants or products, hence does not affect the equilibrium.
- **Option 3: Decreasing the volume of the container**:
- Incorrect. Since \(\Delta N_g = 0\), decreasing the volume does not favor either side of the reaction.
- **Option 4: Increasing the amount of CO**:
- Correct. By increasing the concentration of \(\text{CO}\), the reaction will shift to the right (towards products) to re-establish equilibrium, thus increasing the amount of \(\text{CO}_2\).

5. **Conclusion**:
- The equilibrium amount of \(\text{CO}_2\) can be increased by increasing the amount of \(\text{CO}\).

### Final Answer:
The equilibrium amount of \(\text{CO}_2\) can be increased by increasing the amount of \(\text{CO}\).

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