Four one litre flaske are separately filled with the gases `H_(2), He, O_(2) "and" O_(3)` at the same temperature and pressure. The ratio of total number of atoms of these gases present in different flask would be:

Options

A. `1:1:1:1`
B. `1:2:2:3`
C. `2:1:2:3`
D. `3:2:2:1`

Explanation

To solve the problem, we need to determine the total number of atoms present in each of the gases (H₂, He, O₂, and O₃) when they are filled in one-litre flasks at the same temperature and pressure.

### Step-by-step Solution:

1. **Understand the concept of moles**: Since the volume, temperature, and pressure are the same for all gases, the number of moles of each gas will also be the same.

2. **Identify the number of molecules**: For one mole of any gas, the number of molecules is Avogadro's number (approximately \(6.022 \times 10^{23}\)). Therefore, each flask contains the same number of molecules.

3. **Determine the number of atoms in each gas**:
- For **Hydrogen (H₂)**: Each molecule has 2 atoms. Therefore, the total number of atoms from H₂ in one flask is \(2 \times n\), where \(n\) is the number of moles.
- For **Helium (He)**: Each molecule has 1 atom. Therefore, the total number of atoms from He in one flask is \(1 \times n\).
- For **Oxygen (O₂)**: Each molecule has 2 atoms. Therefore, the total number of atoms from O₂ in one flask is \(2 \times n\).
- For **Ozone (O₃)**: Each molecule has 3 atoms. Therefore, the total number of atoms from O₃ in one flask is \(3 \times n\).

4. **Calculate the total number of atoms**:
- Total atoms from H₂: \(2n\)
- Total atoms from He: \(1n\)
- Total atoms from O₂: \(2n\)
- Total atoms from O₃: \(3n\)

5. **Formulate the ratio of total atoms**:
- The ratio of total number of atoms in the flasks containing H₂, He, O₂, and O₃ is:
\[ \text{Ratio} = 2n : 1n : 2n : 3n \]
- Simplifying this, we get:
\[ \text{Ratio} = 2 : 1 : 2 : 3 \]

### Final Answer:
The ratio of the total number of atoms of the gases in the flasks is **2 : 1 : 2 : 3**.