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 carbon tetrachloride (CCl₄) vapor at standard temperature and pressure (STP), we can follow these steps:

### Step 1: Determine the molecular mass of CCl₄
- The molecular mass of carbon (C) is 12 g/mol.
- The molecular mass of chlorine (Cl) is 35.5 g/mol.
- CCl₄ has one carbon atom and four chlorine atoms.

**Calculation:**
\[ \text{Molecular mass of CCl}_4 = 12 + (4 \times 35.5) \]
\[ = 12 + 142 = 154 \text{ g/mol} \]

### Step 2: Use Avogadro's Law to find the volume at STP
- At STP, one mole of any gas occupies 22.4 liters.

### Step 3: Calculate the density
- Density (D) is defined as mass (m) divided by volume (V).
- Here, the mass of one mole of CCl₄ is 154 g, and the volume at STP is 22.4 L.

**Calculation:**
\[ D = \frac{m}{V} = \frac{154 \text{ g}}{22.4 \text{ L}} \]
\[ D \approx 6.875 \text{ g/L} \]

### Step 4: Identify the nearest option
- The calculated density of CCl₄ vapor at STP is approximately 6.875 g/L. We would then look for the option closest to this value.

### Final Answer:
The density of CCl₄ vapor at STP is approximately **6.875 g/L**.

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