22.4 litre of water vapour at NTP, When condensed to water occupies an approximate volume of

Options

A. 18 litre
B. 1 litre
C. 1 ml
D. 18 ml

Explanation

To solve the problem of finding the volume of water when 22.4 liters of water vapor at NTP is condensed, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Problem**: We are given that 22.4 liters of water vapor condenses into liquid water. We need to find the volume of the water produced.

2. **Identify Molar Volume at NTP**: At Normal Temperature and Pressure (NTP), 1 mole of any ideal gas occupies 22.4 liters. Since we have 22.4 liters of water vapor, we can conclude that this corresponds to 1 mole of water vapor.

3. **Determine the Mass of Water**: The molar mass of water (H₂O) can be calculated as follows:
- Hydrogen (H) has an atomic mass of approximately 1 g/mol. Since there are 2 hydrogen atoms, their total mass is 2 g.
- Oxygen (O) has an atomic mass of approximately 16 g/mol.
- Therefore, the molar mass of water (H₂O) = 2 g (from H) + 16 g (from O) = 18 g/mol.

4. **Calculate the Mass of Water from the Vapor**: Since we have 1 mole of water vapor, the mass of the condensed water will be equal to the molar mass of water, which is 18 grams.

5. **Find the Volume of Water**: To find the volume of water, we can use the formula:
\[ \text{Volume} = \frac{\text{Mass}}{\text{Density}} \]
The density of water is approximately 1 g/mL. Thus, we can substitute the values:
\[ \text{Volume} = \frac{18 \text{ grams}}{1 \text{ g/mL}} = 18 \text{ mL} \]

6. **Final Answer**: Therefore, when 22.4 liters of water vapor at NTP is condensed, it occupies an approximate volume of **18 mL**.