Answer:
Vapor pressure of solution = 467.9 Torr
Explanation:
This about a colligative property, vapor pressure lowering.
ΔP = P° . Xm
ΔP = Vapor pressure of pure solvent - Vapor pressure of solution
Xm = Mole fraction, for solute.
Let's convert the mass of solute and solvent to moles (mass / molar mass)
651 g / 62.07 g/m = 10.5 moles of ethylene glycol
1500 g / 18 g/m = 83.3 moles of water
Total moles = 10.5 moles of solute + 83.3 moles of solvent ⇒ 93.8 moles
Mole fraction of solute = 10.5 / 93.8 = 0.11
Vapor pressure of water at 90°C is 525.8 Torr
525.8 Torr - Vapor pressure of solution = 525.8 Torr . 011
Vapor pressure of solution = 525.8 Torr . 011 - 525.8 Torr
Vapor pressure of solution = 467.9 Torr
