At `20^(@)C`, two balloons of equal volume and porosity are filled to a pressure of `2atm`, one with `14 kg N_(2)` and the other with `1 Kg` of `H_(2)`.The `N_(2)` balloon leaks to a pressure of `1//2 atm` in `1 hour`. How long will it take for the `H_(2)` balloon to reach a pressure of `1//2 atm`?

Explanation

To solve the problem, we will use Graham's Law of Effusion, which states that 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 Given Data:**
- For the nitrogen (N₂) balloon:
- Initial pressure = 2 atm
- Final pressure = 0.5 atm
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