What mass of ethylene glycol (C2H6O2), molar mass 62.1 g/mol), the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car’s radiator that freezes at 10.0OF (23.3C)? Assume the density of water is exactly 1 g/mL.A solution is prepared by mixing 5.81 g acetone (C3H6O, molar mass 58.1 g/mol) and 11.9 g chloroform (CHCl3) , molar mass 119.4 g/mol). At 35OC, this solution has a total vapor pressure of 260. torr. Is this an ideal solution? The vapor pressures of pure acetone and pure chloroform at 35C are 345 and 293 torr, respectively.

the freezing point of the solution = 10.0 °F = (10°F − 32) × 5/9 = -12.22°C Depression in freezing…

Answered: What mass of ethylene glycol (C2H6O2),…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 73QAP: Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol,...

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What mass of ethylene glycol (C₂H₆O₂), molar mass 62.1 g/mol), the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car’s radiator that freezes at 10.0^OF (23.3C)? Assume the density of water is exactly 1 g/mL.
A solution is prepared by mixing 5.81 g acetone (C₃H₆O, molar mass 58.1 g/mol) and 11.9 g chloroform (CHCl₃) , molar mass 119.4 g/mol). At 35^OC, this solution has a total vapor pressure of 260. torr. Is this an ideal solution? The vapor pressures of pure acetone and pure chloroform at 35C are 345 and 293 torr, respectively.

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