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The vapor pressure of ethanol (C2H5OH) at 19 °C is 40.0 torr. A 1.00-g sample of ethanol is placed in a 2.00 L container at 19 °C. If the container is closed and the ethanol is allowed to reach equilibrium with its vapor, how many grams of liquid ethanol remain?

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Nelly Stracke
Nelly StrackeLv2
28 May 2020

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Related questions

Calculate the mass of ethylene glycol (C2H6O2 - molar mass =62.07 g/mol) that must be added to 1.00 kg of ethanol (C2H5OH- molar mass =46.07 g/mol) to reduce its vapor pressure by 10.0 torr at 35 degree C. The vapor pressure of pur ethanol at 35 degree C is 100 torr.

(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.

(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 35°C. The vapor pressure of pure ethanol at 35°C is1.00 multiplied by 102 torr

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