X litres of carbon monoxide is present at S.T.P. It is completely oxidised to `CO_(2)`. The volume of `CO_(2)` formed is 11.207 L at S.T.P. What is the value of X in litres?

Options

A. 22.414 L
B. 11.207 L
C. 5.6035L
D. 44.828 L

Explanation

To solve the problem, we need to determine the volume of carbon monoxide (CO) that was oxidized to produce a given volume of carbon dioxide (CO₂) at standard temperature and pressure (S.T.P.).

### Step-by-Step Solution:

1. **Understand the Reaction**: The balanced chemical reaction for the oxidation of carbon monoxide to carbon dioxide is:
\[ 2 \text{CO} + \text{O}_2 \rightarrow 2 \text{CO}_2 \]
This indicates that 2 volumes of CO react with 1 volume of O₂ to produce 2 volumes of CO₂.

2. **Volume Relationship at STP**: At standard temperature and pressure (S.T.P.), 1 mole of any gas occupies 22.4 liters. Therefore, the volume ratios of gases involved in the reaction can be directly compared.

3. **Given Data**: We know that the volume of CO₂ produced is 11.207 liters.

4. **Determine Volume of CO Required**: From the balanced reaction, we see that 1 volume of CO produces 1 volume of CO₂. Therefore, if we produce 11.207 liters of CO₂, we must have started with the same volume of CO:
\[ \text{Volume of CO} = \text{Volume of CO₂} = 11.207 \text{ liters} \]

5. **Conclusion**: Thus, the value of X, which represents the volume of carbon monoxide initially present, is:
\[ X = 11.207 \text{ liters} \]

### Final Answer:
The value of X is **11.207 liters**.