At STP , the density of `C Cl_(4)` vapour in g/L will be nearest to

Options

A. 6.87
B. 3.42
C. 10.26
D. 4.57

Explanation

To find the density of CCl₄ vapor at STP (Standard Temperature and Pressure), we can follow these steps:

### Step-by-Step Solution:

1. **Determine the Molar Mass of CCl₄**:
- The molar mass of carbon (C) is approximately 12 g/mol.
- The molar mass of chlorine (Cl) is approximately 35.5 g/mol.
- CCl₄ has one carbon atom and four chlorine atoms.
- Calculate the molar mass:
\[ \text{Molar mass of CCl}_4 = 1 \times 12 + 4 \times 35.5 = 12 + 142 = 154 \text{ g/mol} \]

2. **Use the Ideal Gas Law at STP**:
- At STP, 1 mole of any ideal gas occupies a volume of 22.4 liters.

3. **Calculate the Density**:
- Density (D) is defined as mass (m) divided by volume (V):
\[ D = \frac{m}{V} \]
- For CCl₄ vapor:
\[ D = \frac{154 \text{ g}}{22.4 \text{ L}} \approx 6.87 \text{ g/L} \]

4. **Conclusion**:
- The density of CCl₄ vapor at STP is approximately 6.87 g/L.

### Final Answer:
The density of CCl₄ vapor at STP is nearest to **6.87 g/L**.

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