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vapor pressure question in chemistry?
What is the vapor pressure (in mm Hg) of a solution of 18.2 of glucose (C6H12O6) in 94.6 of methanol (CH3OH) at 27 degrees Celsius? The vapor pressure of pure methanol at 27 degrees Celsius is 140 mm Hg, I need to know how to set up the problem as well as get the answer. Thank you.
1 Answer
- skipperLv 71 decade agoFavorite Answer
mole fraction of methanol x 140 mm Hg = vapor pressure of solution
moles of glucose = 18.2 g / 180.2 g/mole = 0.101 mole
moles of methanol = 94.6 g / 32.04 g/mole = 2.953 mole
moles fraction of methanol = 2.953 / (0.101 + 2.953) = 0.967
vapor pressure of solution = 0.967 x 140 mm Hg = 135 mm Hg
