Question

Calculate the vapor pressure of a solution containing 36.5 g of glycerol (C3H8O3) and 125 mL of water at 30.0 °C. The vapor pressure of pure water at this temperature is 31.8 torr. Assume that glycerol is not volatile and dissolves molecularly (i.e., it is not ionic) and use a density of 1.00 g/mL for the water.

Answer 1

lytis Psolution = X solvent Psolvent (vapour pressure) X H2O пи,0 in haotinglycerol Xmo x lgx I mol (moles of mo) = 18.016 nog 6093 mol of no mole 36.5 0•396 mol 92.096 bald 125 mLX Х 1 м. (molar mass of glycerol =92-093 g/mol X H2O= moles of moles of mot water t moles of glycerol 0.945 70226 = 6.93 6.93 6.93f00396 Teacher's Signature : CS Scanned with CamScanner

Vapour pressure of pure water = 3 108 toor so Vapour pressure of Psolution X solvent. Psolvent Given. soln = Isolution - 0.945X 31,8 300sl torr Es $canned with Jamscanner