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4 March, 01:47

Calculate the vapor pressure of a solution containing 25.2 gg of glycerin (C3H8O3) (C3H8O3) in 124 mLmL of water at 30.0 ∘C∘C. The vapor pressure of pure water at this temperature is 31.8 torrtorr. Assume that glycerin is not volatile and dissolves molecularly (i. e., it is not ionic) and use a density of 1.00 g/mLg/mL for the water.

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  1. 4 March, 02:06
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    29.256 torr.

    Explanation:

    Number of moles

    Glycerin:

    Molecular weight of glycerin = (12*3) + (1*8) + (16*3)

    = 36 + 8 + 48

    = 92 g/mol

    Number of moles = mass/molar mass

    = 25.2/92

    = 0.274 mol

    Water:

    Converting g/ml to g/l,

    1000 ml = 1 l

    = 1 g/ml * 1000 ml/1l

    = 1000 g/l

    Mass = (density * volume)

    = 1000*0.124

    = 124 g.

    Molar mass of water = (1*2) + 16

    = 18 g/mol

    Number of moles = mass / molar mass

    = 126/18

    = 6.89 mol

    P°solution = xsolvent * P°solvent

    Where,

    xwater = xsolvent = mole fraction of water.

    Mole fraction is defined as the number of moles of a component of a solution divided by the total number of moles present in that solution.

    xwater = mole of water/total mole of solution

    Total mole = 6.89 + 0.274

    = 7.164 moles

    xwater = 6.89/7.164

    = 0.962

    P°solution = xsolvent * P°solvent

    P°solution = 31.8 * 0.962

    = 29.256 torr
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