The vapour density of a gas is 11.2. Calculate the volume occupied by 11.2 g of the gas at NTP.
[Hint: mol. Wt `=2 xx` V.D]

Answer

To solve the problem, we will follow these steps:

### Step 1: Understand the relationship between vapor density and molecular weight.
The vapor density (VD) of a gas is related to its molecular weight (M) by the formula:
\[ M = 2 \times \text{VD} \]

### Step 2: Calculate the molecular weight of the gas.
Given that the vapor density of the gas is 11.2, we can substitute this value into the formula:
\[ M = 2 \times 11.2 = 22.4 \text{ g/mol} \]

### Step 3: Use the molecular weight to find the number of moles of the gas.
To find the number of moles (n) of the gas, we use the formula:
\[ n = \frac{\text{mass}}{\text{molecular weight}} \]
Given that the mass of the gas is 11.2 g, we can substitute the values:
\[ n = \frac{11.2 \text{ g}}{22.4 \text{ g/mol}} = 0.5 \text{ moles} \]

### Step 4: Calculate the volume occupied by the gas at NTP.
At Normal Temperature and Pressure (NTP), 1 mole of gas occupies 22.4 liters. Therefore, the volume (V) occupied by the gas can be calculated as:
\[ V = n \times 22.4 \text{ L} \]
Substituting the number of moles we calculated:
\[ V = 0.5 \text{ moles} \times 22.4 \text{ L/mole} = 11.2 \text{ L} \]

### Final Answer:
The volume occupied by 11.2 g of the gas at NTP is **11.2 liters**.

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