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13 October, 20:07

What is the vapor pressure (in mm Hg) of a solution of 17.5 g of glucose (C6H12O6) in 82.0 g of methanol (CH3OH) at 27∘C? The vapor pressure of pure methanol at 27∘C is 1.40*102 mm H

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  1. 14 October, 00:07
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    134.8 mmHg is the vapor pressure for solution

    Explanation:

    We must apply the colligative property of lowering vapor pressure, which formula is: P° - P' = P°. Xm

    P° → Vapor pressure of pure solvent

    P' → Vapor pressure of solution

    Xm → Mole fraction for solute

    Let's determine the moles of solute and solvent

    17.5 g. 1 mol/180 g = 0.0972 moles

    82 g. 1mol / 32 g = 2.56 moles

    Total moles → moles of solute + moles of solvent → 2.56 + 0.0972 = 2.6572 moles

    Xm → moles of solute / total moles = 0.0972 / 2.6572 = 0.0365

    We replace the data in the formula

    140 mmHg - P' = 140 mmHg. 0.0365

    P' = - (140 mmHg. 0.0365 - 140mmHg)

    P' = 134.8 mmHg
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