A)Calculate vaporpressure of water above a solution preparedby dissovling 36.5g

Question

A)Calculate vaporpressure of water above a solution preparedby dissovling 36.5g in C3H6O2 to187g of water at 343K. B) Calculate the mass ofC3H6O2 that must be added to1.00kg of C3H5OH to reduce its vapor pressureby 13.7 torr at 35*C. the vapor pressure of pure ethanol at 35*C is1.00x102 torr A)Calculate vaporpressure of water above a solution preparedby dissovling 36.5g in C3H6O2 to187g of water at 343K. B) Calculate the mass ofC3H6O2 that must be added to1.00kg of C3H5OH to reduce its vapor pressureby 13.7 torr at 35*C. the vapor pressure of pure ethanol at 35*C is1.00x102 torr

Explanation / Answer

a) 187 g / 18 g/ mol = 10.34 mol of water 36.5 g / 74 g/mol = .493 mol C3H6O2 10.34 mol / (10.34+.493 mol) = .955 mol Vapor pressure = (Pressure of pure water at 343)(mole fraction) Look up for pressure of water at 343: 226.8 torr Vapor Pressure = (226.8) (.955) = 216.5 torr b) p = p° X (100-13.7) = 100 X .863 = x = mole fraction 1000 g / 58 g/mol = 17.24 mol C3H5OH .863 = 17.24 / (17.24 + X mole C3H6O2) X = 2.74 mol Mass = 2.74 mol x 74 g/mol = 202.5 grams

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