(a) Calculate the vapor pressure of water above a solutionprepared by dissolving 33.7 g in glycerin (C3H8O3) to 121 g ofwater at 343 K.
(b) Calculate the mass of ethylene glycol (C2H6O2) that must beadded to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressureby 11.9 torr at 35Â°C. The vapor pressure of pure ethanol at 35Â°C is1.00 multiplied by 102 torr

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Part A

Calculate the vapor pressure of water above a solution prepared by dissolving 28.0 g of glycerin (C3H8O3) in 145 g of water at 343 K. (The vapor pressure of water at 343 K is 233.7 torr.)

PH2O =

torr

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Part B

Calculate the mass of ethylene glycol (C2H6O2) that must be added to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressure by 9.00 torr at 35âC. The vapor pressure of pure ethanol at 35âC is 1.00Ã102 torr.

m =

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(a) Calculate the vapor pressure of water above a solution prepared by dissolving 28.5 g of glycerin (C₃H₈O₃) in 125 g of water at 343 K. (The vapor pressure of water is given in Appendix B.) (b) Calculate the mass of ethylene glycol (C₂H₆O₂) that must be added to 1.00 kg of ethanol (C₂H₅OH) to reduce its vapor pressure by 10.0 torr at 35 °C. The vapor pressure of pure ethanol at 35 °C is 1.00 × 10² torr.