A ballon is filled with hydrogen at room temperature. It will burst if pressure exceeds `0.2 "bar"`. If at `I` bar pressure, the gas occupies `2.27 L` volume, up to what volume can the balloon be expanded?

Explanation

To solve the problem step by step, we will use Boyle's Law, which states that for a given mass of gas at constant temperature, the product of pressure and volume is constant. This can be mathematically expressed as:

\[ P_1 V_1 = P_2 V_2 \]

### Step 1: Identify the given values
- Initial pressure, \( P_1 = 1 \, \text{bar} \)
- Initial volume, \( V_1 = 2.27 \, \text{L} \)
- Maximum pressure before bursting, \( P_2 = 0.2 \, \text{bar} \)
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