   # The vapor pressure of a solution containing 53.6 g glycerin (C 3 H 8 O 3 ) in 133.7 g ethanol (C 2 H 5 OH) is 113 torr at 40°C. Calculate the vapor pressure of pure ethanol at 40°C assuming that glycerin is a nonvolatile, nonelectrolyte solute in ethanol. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 10, Problem 52E
Textbook Problem
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## The vapor pressure of a solution containing 53.6 g glycerin (C3H8O3) in 133.7 g ethanol (C2H5OH) is 113 torr at 40°C. Calculate the vapor pressure of pure ethanol at 40°C assuming that glycerin is a nonvolatile, nonelectrolyte solute in ethanol.

Interpretation Introduction

Interpretation: The vapour pressure of given solvent has to be calculated.

Concept Introduction: "At a constant temperature, the quantity of a known gas that dissolves in a given type and quantity of liquid is directly proportional to the partial pressure of that gas in equilibrium with so as to liquid."

### Explanation of Solution

Record the given data from question

Weight of Glycerine =53.6g

Molecular weight of Glycerine =92.09g/mole

To find the moles of Glycerine.

MoleC3H8O3=53.6g×1mole92.09g=0.582moleC3H8O3

The moles of Glycerin were calculated by substituting the values of the weight of Glycerine and molecular weight of Glycerine. Hence the moles of Glycerin is 0.582mole.

To find the moles of Ethanol.

133.7gC2H5OH×1moleC2H5OH46.07g=2

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