Two liquids X and Y one mixing form an ideal solution. At `30^(@)C` the vapour pressure of the solution containing 3 moles of X and 1 mole Y is 550 mm Hg. But when 4 moles of X and 1 mole of Y are mixe, the vapour pressur of the solution thus formed is 560 mm Hg. What will be the vapour presure of pure and Pure Y at this temerature ?

Explanation

To solve the problem, we need to find the vapor pressures of pure liquids X and Y at 30°C using the information provided about the vapor pressures of their mixtures. We will use Raoult's Law, which states that the total vapor pressure of an ideal solution is the sum of the partial pressures of each component.

### Step-by-Step Solution:

1. **Identify Given Data:**
- For the first mixture:
- Moles of X (nX1) = 3
- Moles of Y (nY1) = 1
...