A given mass of a gas collected over water vapour at `25^(@)C` has a pressure of `500mm` `Hg`. Calculate the pressure if its volume is reduced to half of its original volume (aqueous tension at `25^(@)C="24 mm of Hg"`).

Explanation

To solve the problem step by step, we will follow the ideal gas law and account for the vapor pressure of water.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Initial pressure of the gas, \( P_1 = 500 \, \text{mmHg} \)
- Aqueous tension (vapor pressure of water at \( 25^\circ C \)), \( P_{\text{water}} = 24 \, \text{mmHg} \)
- Initial volume of the gas, \( V_1 = V \)
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