A mixture of `H_(2)O` vapour, `CO_(2)` and `N_(2)` was trapped in a glass apparatus with a volume of `0.731 mL`. The pressure of the total mixture was `1.74 atm` at `27^(@)C`. The sample was transferred to a bulb in contact with dry ice `(-75^(@)C)` so that the `H_(2)O` vapour was frozen out. When the sample was returned to the measured volume, the pressure was `1.32 mm Hg`. The sample was then transferred to a bulb in contact with liquid nitrogen `(-95^(@)C)` to freeze out the `CO_(2)`. On the measured volume, the pressure was `0.53 mm Hg`. How many moles of each constituent there are in the mixture?

Explanation

To solve the problem step by step, we will use the Ideal Gas Law, which is given by the equation:

\[ PV = nRT \]

Where:
- \( P \) = Pressure in atm
- \( V \) = Volume in liters
- \( n \) = Number of moles
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