An antifreeze solution is prepared by mixing 1.00 L of water and 946 mL of ethylene glycol, C¿H6O2 (molar mass = 62.07 g/mol). Calculate: (a) the mass percent of ethylene glycol in the mixture; (b) the mole fraction of ethylene glycol in the solution, and (c) the molality of ethylene glycol in the solution.

An antifreeze solution is prepared by mixing 1.00 L of water and 946 mL of ethylene glycol, C¿H6O2 (molar mass = 62.07 g/mol). Calculate: (a) the mass percent of ethylene glycol in the mixture; (b) the mole fraction of ethylene glycol in the solution, and (c) the molality of ethylene glycol in the solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

An antifreeze solution is prepared by mixing 1.00 L of water and 946 mL of ethylene glycol, C,H,O2
(molar mass = 62.07 g/mol). Calculate: (a) the mass percent of ethylene glycol in the mixture; (b) the
mole fraction of ethylene glycol in the solution, and (c) the molality of ethylene glycol in the solution.
(d) Determine the freezing point and boiling point of the solution.
(Assume density of water = 1.00 g/mL; Kf= 1.86°C/m; K = 0.512°C/m; density of EG = 1.114 g/mL)

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