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Calculate the vapor pressure of a solution containing 25.3 g of glycerin (C3H8O3) in 119 mL...

Calculate the vapor pressure of a solution containing 25.3 g of glycerin (C3H8O3) in 119 mL of water at 30.0 ∘C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerin is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.

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Expert Solution

molar mass of glycerine = 92

no of moles of glycerine = W/GMM

                                        = 25.3/92 = 0.275moles

mass of water = volume * density

                       = 119*1 = 119g

no of moles of water = W/GMM

                                 = 119/18 = 6.6moles

total no of mole   = ngly + nwater

                           = 0.275 + 6.6 = 6.875

mole fraction of water Xwater = nwater/ ngly + nwater

                                                                 = 6.6/6.875 = 0.96

pressure of solution = molefraction of water* pressure of water

                                   = 0.96*31.8 = 30.528torr

queen_honey_blossom answered 7 months ago
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