Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Chapter 13, Problem 77QRT

(a)

Interpretation Introduction

Interpretation:

The mass of the glycol that have been added has to be determined.

Concept introduction

Freezing point is the temperature at which liquid turns into solid.

The Freezing point depression (ΔTf) is indicated as ΔTf= Kfmsoluteisolute.

Where,

ΔTf Change in freezing point.

Kf Molal freezing point constant.

m Molality of the solution.

isolute- van’t Hoff factor.

(a)

Expert Solution
Check Mark

Answer to Problem 77QRT

The mass of the glycol that have been added is 2500g C2H6O2.

Explanation of Solution

Using Freezing point of the solution:

    ΔT=T°(solution)-T(solvent)= -15.0C+(-0.0C)= -15.0C.

Given data is as follows:

Using the formula as shown below,

  ΔT= KfmC2H6O2iC2H6O2mC2H6O2=ΔT Kf=-15.0oC(-1.86oC.kg.mol-1)=8.06mol/kg.

Mass of the glycol:

  5.0kgwater×8.06molC2H6O21kgwater×62.07molC2H6O21molC2H6O2=2500g C2H6O2.

Therefore, the mass of the glycol that have been added is 2500g C2H6O2.

(b)

Interpretation Introduction

Interpretation:

The boiling point of the coolant mixture has to be calculated.

Concept introduction

Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is 100°C. That is water changes from liquid phase to gas phase at temperature 100oC.

  ΔTb= Tb- Tb°

Where,

  ΔTb Change in boiling point.

  Tb Boiling point of the solution.

  Tb° Boiling point of pure solvent.

The Boiling point elevation(ΔTb) is indicated as ΔTb= Kbm.

Where,

  ΔTb Change in boiling point.

  Kb Molal boiling point constant.

  m Molality of the solution.

(b)

Expert Solution
Check Mark

Answer to Problem 77QRT

Boiling point of the solution is 104.12oC.

Explanation of Solution

Given data as follows: Mass of ethylene glycol from part (a) =2500 g.

Mass of water is 100 g.

Value of Kb (water)=0.512oC kg/mol

Calculate mole of solute (urea):

  Molesofsubstance GivenmassofsubstanceMolecularmass=2500g62.07g/mol= 40.3mol[ethylene glycolMolecularmass=62.07 g/mol].

Substituting the values of ethylene glycol mass and its molecular mass into the moles–mass conversion formula, the moles of the substance was obtained.

Calculate molality of the solution:

  molality =40.3mol5.0 kg water=8.06m.

Substituting in the value of moles of the solute and mass of solvent in kilogram; molality of the solution was obtained.

Calculate Boiling point of the solution:

Using the boiling point formula as follows,

  ΔT= Kbmsolute= (0.512°C/m)(8.06m.) = 4.12CΔTb= Tb- Tb°

  Tb=ΔTb+Tb°=100C+ 4.12C=104.12oC.

Substituting the values of molality, the boiling point was calculated.

Therefore, the Boiling point of the solution is 104.12oC.

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Chapter 13 Solutions

Chemistry: The Molecular Science

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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY