The volume of phosgene formed at STP when 11.2 lit of chlorine reacts with carbon monoxide is

Options

A. 11.2 litre
B. 22.4 lit
C. 5.6 lit
D. 44.8 lit

Explanation

To solve the problem of finding the volume of phosgene (COCl2) formed at STP when 11.2 liters of chlorine (Cl2) reacts with carbon monoxide (CO), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**:
The reaction between chlorine (Cl2) and carbon monoxide (CO) to form phosgene (COCl2) can be represented as:
\[ \text{CO} + \text{Cl}_2 \rightarrow \text{COCl}_2 \]

2. **Determine the Volume of Chlorine**:
We are given that the volume of chlorine (Cl2) is 11.2 liters.

3. **Use the Molar Volume at STP**:
At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters.

4. **Calculate Moles of Chlorine**:
To find the number of moles of chlorine, we can use the formula:
\[ \text{Number of moles} = \frac{\text{Volume of gas}}{\text{Molar volume at STP}} = \frac{11.2 \, \text{liters}}{22.4 \, \text{liters/mole}} = 0.5 \, \text{moles} \]

5. **Determine Moles of Phosgene Formed**:
From the balanced reaction, we see that 1 mole of Cl2 produces 1 mole of COCl2. Therefore, if we have 0.5 moles of Cl2, it will produce:
\[ 0.5 \, \text{moles of COCl}_2 \]

6. **Calculate the Volume of Phosgene**:
Now, we can find the volume of phosgene formed using the same molar volume:
\[ \text{Volume of COCl}_2 = \text{Number of moles of COCl}_2 \times \text{Molar volume at STP} = 0.5 \, \text{moles} \times 22.4 \, \text{liters/mole} = 11.2 \, \text{liters} \]

### Final Answer:
The volume of phosgene (COCl2) formed at STP when 11.2 liters of chlorine reacts with carbon monoxide is **11.2 liters**.

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