We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 1.00 atm to 0.960 atm at 100°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the freezing point of this solution? (Hint: find the molality first, and for water, kf = 1.86 m/°C; freezing point of water: 0.0°C.)
We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 1.00 atm to 0.960 atm at 100°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the freezing point of this solution? (Hint: find the molality first, and for water, kf = 1.86 m/°C; freezing point of water: 0.0°C.)
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.98QE
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We mixed some ethylene glycol with 346 g water to reduce the equilibrium vapor pressure of water from 1.00 atm to 0.960 atm at 100°C. The molar masses of water and ethylene glycol are 18.02 g/mol and 62.07 g/mol, respectively. Assume ideal behavior for the solution. What is the freezing point of this solution? (Hint: find the molality first, and for water, kf = 1.86 m/°C; freezing point of water: 0.0°C.)
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