An open vessel at `27^@C` is heated until three fifth of the air in it has been expelled। Assuming volume of vessel constant find the temperature to which the vessel has been heated

Explanation

To solve the problem, we will use the ideal gas law, which states that \( PV = nRT \). Given that the vessel is open to the atmosphere, we can assume that the pressure \( P \) remains constant throughout the heating process.

### Step-by-Step Solution:

1. **Identify Initial Conditions**:
- Initial temperature \( T_1 = 27^\circ C \).
- Convert this temperature to Kelvin:
\[
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