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10 Nov 2019

Calculate the mass of ethylene glycol (C2H6O2) that must beadded to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressureby 9.00torr at 35âC. The vapor pressure of pure ethanol at 35âC is1.00Ã102 torr.

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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.

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Calculate the mass of ethylene glycol (C2H6O2) that must be added to 1.00kg of ethanol (C2H5OH) to reduce its vapor pressure by9.00torr at35?C.The vapor pressure of pure ethanol at 35?Cis 1.00

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.

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Calculate the mass of ethylene glycol (C2H6O2) that must beadded to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressureby 9.00torr at 35âC. The vapor pressure of pure ethanol at 35âC is1.00Ã102 torr.

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Calculate the mass of ethylene glycol (C2H6O2) that must beadded to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressureby 9.00torr at 35âC. The vapor pressure of pure ethanol at 35âC is1.00Ã102 torr.

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Chemistry: A Molecular Approach

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Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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Weekly leaderboard

Calculate the mass of ethylene glycol (C2H6O2) that must beadded to 1.00 kg of ethanol (C2H5OH) to reduce its vapor pressureby 9.00torr at 35âC. The vapor pressure of pure ethanol at 35âC is1.00Ã102 torr.