At STP , the density of` C O_(2) `vapour in g/L will be nearest to

Options

A. 2
B. 2.45
C. 1.5
D. 7.5

Answer

To find the density of CO₂ vapor at STP (Standard Temperature and Pressure), we can follow these steps:

### Step 1: Calculate the molar mass of CO₂
The molar mass of CO₂ can be calculated by adding the atomic masses of its constituent elements:
- Carbon (C): 12 g/mol
- Oxygen (O): 16 g/mol (and there are 2 oxygen atoms in CO₂)

So, the molar mass of CO₂ is:
\[ \text{Molar mass of CO₂} = 12 \, \text{g/mol} + 2 \times 16 \, \text{g/mol} = 12 + 32 = 44 \, \text{g/mol} \]

### Step 2: Use the molar volume of a gas at STP
At STP, one mole of any ideal gas occupies a volume of 22.4 liters.

### Step 3: Calculate the density of CO₂
Density (D) is defined as mass (m) divided by volume (V):
\[ D = \frac{m}{V} \]
For CO₂:
- Mass (m) = 44 g (from Step 1)
- Volume (V) = 22.4 L (from Step 2)

Substituting these values into the density formula:
\[ D = \frac{44 \, \text{g}}{22.4 \, \text{L}} \]

### Step 4: Perform the calculation
Now, we perform the division:
\[ D = \frac{44}{22.4} \approx 1.9643 \, \text{g/L} \]

### Step 5: Round the result
Rounding 1.9643 to the nearest whole number gives us approximately 2 g/L.

### Final Answer
Thus, the density of CO₂ vapor at STP is approximately **2 g/L**.

---