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3 May, 15:47

If 651 grams of ethylene glycol, HOCH2CH2OH, is dissolved in 1.50 kg of water at 90.°C, what is the vapor pressure of the water in the solution?

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  1. 3 May, 15:55
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    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
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