Two containers A and B have the same volume. Container A contains 5 moles of `O_(2)` gas. Container B contains 3 moles of He and 2 moles of `N_(2)`. Both the containers are separately kept in vacuum at the same temperature. Both the containers have very small orifices of the same area through which the gases leak out. Compare the rate of effusion of `O_(2)` with that of He gas mixture.

Explanation

To solve the problem of comparing the rate of effusion of \( O_2 \) with that of the He gas mixture in container B, we will use Graham's law of effusion. According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

### Step-by-Step Solution:

1. **Identify the Moles and Molar Masses:**
- Container A (Oxygen):
- Moles of \( O_2 = 5 \) moles
- Molar mass of \( O_2 = 32 \, g/mol \)
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