An open vessel at `27^(@)C` is heated until three-fifths of the air in it has been expelled. Assuming the volume of the vessle remains constant, find the temperature to which the vessle has to be heated.

Explanation

To solve the problem, we will use the ideal gas law and the relationship between the number of moles and temperature. Here’s a step-by-step solution:

### Step 1: Understand the Initial Conditions
We start with an open vessel at a temperature of \(27^\circ C\). We need to convert this temperature to Kelvin for our calculations.

**Hint:** Remember that to convert Celsius to Kelvin, you add 273.15.

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