General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
Question
Book Icon
Chapter 13, Problem 13.106SP

(a)

Interpretation Introduction

Interpretation:

Mole fraction of each component present in the given solution has to be calculated.

Concept introduction:

Raoult’s law states that in an ideal mixture of liquid solution, partial pressure of every component is equal to its mole fraction multiplied into vapour pressure of its pure components.

P= χP°

Where,

P- Partial pressure of each component

P°- Partial pressure of its pure components

χ1- Mole fraction of the components

Mole fraction: Concentration of the solution can also expressed by mole fraction. Mole fraction is equal to moles of the component divided by total moles of the mixture.

Mole fraction =moles of a componenttotal moles

(a)

Expert Solution
Check Mark

Answer to Problem 13.106SP

Mole fraction of component A is 0.52

Mole fraction of component B is 0.48

Explanation of Solution

Given data:

Molar mass of liquid A = 100g/mol

Molar mass of liquid B = 110g/mol

Vapour pressure of A = 95mmHg at 55°C

Vapour pressure of B = 42 mmHgat 55°C

Calculate mole fraction of each component:

Assume 1g of each A and B mixed then, the mole fractions are calculated as follows,

1.00g A×1mol A100g A = 0.01molA1.00g B×1mol B110g B= 0.0091molB

The mole fraction of the component is calculated by moles of the component divided by the total number of moles in the mixture.

χA=molAmolA+molB=0.01(0.01+0.0091)= 0.52χB=molBmolA+molB=0.0091(0.01+0.0091)= 0.48

Substituting the values of moles of each component and total moles of the component, the mole fraction of each component has calculated.

(b)

Interpretation Introduction

Interpretation:

The partial pressure of the components over the given solution at 55°C has to be calculated.

Concept introduction:

Raoult’s law states that in an ideal mixture of liquid solution, partial pressure of every component is equal to its mole fraction multiplied into vapour pressure of its pure components.

P= χP°

Where,

P- Partial pressure of each component

P°- Partial pressure of its pure components

χ1- Mole fraction of the components

(b)

Expert Solution
Check Mark

Answer to Problem 13.106SP

Partial pressure of solution A is 50mmHg

Partial pressure of solution B is 20 mmHg

Explanation of Solution

Calculate partial pressure of each component:

At 55°C, PA°= 95mmHg and PB°= 42mmHg

χA= 0.52mmHg and χB= 0.48 mmHg

The formula for partial pressure,

P1= χ1P1°

PA= χAPA°= 0.52 × 95mmHg = 49.4mmHg

PB= χBPB°= 0.48× 42mmHg = 20 mmHg

According to Raoult’s law, the vapour pressure of the solution is sum of the individual partial pressure exerted by the solution and then using partial pressure equation, partial pressure of each component has been calculated.

(c)

Interpretation Introduction

Interpretation:

The mole fraction of each component in the condensed liquid and the vapour pressure of the components above the condensed liquid at 55°C should be calculated.

Concept introduction:

Raoult’s law states that in an ideal mixture of liquid solution, partial pressure of every component is equal to its mole fraction multiplied into vapour pressure of its pure components.

P= χP°

Where,

P- Partial pressure of each component

P°- Partial pressure of its pure components

χ1- Mole fraction of the components

(c)

Expert Solution
Check Mark

Answer to Problem 13.106SP

Mole fraction of component A in condensed liquid is 0.71

Mole fraction of component B in condensed liquid is 0.29

Partial pressure of the component A above condensed liquid at 55°C is 67.45mmHg

Partial pressure of the component B above condensed liquid at 55°C is 12 mmHg

Explanation of Solution

χi=PiPtotal

The mole fraction is equal to partial pressure of the component divided by the total pressure.

Ptotal= 49.4 mmHg + 20mmHg = 69.4mmHg

χA=PAPtotal=49.4mmHg69.4mmHg= 0.71χB=1-0.71= 0.29

Substituting the value of partial pressure of each component and total pressure, the mole fraction of each component at condensed liquid has calculated.

Calculation of partial pressure of each component

The mole fraction of each component in condensed liquid is,

χA= 0.71 and  χB= 0.29

PA= χAPA°= 0.71 × 95mmHg = 67.45mmHg

PB= χBPB°= 0.29× 42mmHg = 12 mmHg

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 13 Solutions

General Chemistry

Ch. 13.6 - Prob. 2PECh. 13.6 - Prob. 2RCCh. 13.6 - Prob. 3PECh. 13.6 - Prob. 4PECh. 13.6 - Prob. 3RCCh. 13.6 - Prob. 5PECh. 13.6 - Prob. 4RCCh. 13 - Prob. 13.1QPCh. 13 - Prob. 13.2QPCh. 13 - Prob. 13.3QPCh. 13 - 13.4 As you know, some solution processes are...Ch. 13 - Prob. 13.5QPCh. 13 - Prob. 13.6QPCh. 13 - Prob. 13.7QPCh. 13 - Prob. 13.8QPCh. 13 - 13.9 Arrange these compounds in order of...Ch. 13 - Prob. 13.10QPCh. 13 - Prob. 13.11QPCh. 13 - Prob. 13.12QPCh. 13 - Prob. 13.13QPCh. 13 - 13.14 Calculate the amount of water (in grams)...Ch. 13 - Prob. 13.15QPCh. 13 - Prob. 13.16QPCh. 13 - Prob. 13.17QPCh. 13 - 12.20 For dilute aqueous solutions in which the...Ch. 13 - Prob. 13.19QPCh. 13 - 13.20 The concentrated sulfuric acid we use in the...Ch. 13 - 13.21 Calculate the molarity and the molality of...Ch. 13 - 13.22 The density of an aqueous solution...Ch. 13 - Prob. 13.23QPCh. 13 - Prob. 13.25QPCh. 13 - 13.26 The solubility of KNO3 is 155 g per 100 g of...Ch. 13 - Prob. 13.27QPCh. 13 - Prob. 13.28QPCh. 13 - Prob. 13.29QPCh. 13 - Prob. 13.30QPCh. 13 - Prob. 13.31QPCh. 13 - 13.32 A man bought a goldfish in a pet shop. Upon...Ch. 13 - Prob. 13.33QPCh. 13 - 13.34 A miner working 260 m below sea level opened...Ch. 13 - Prob. 13.35QPCh. 13 - 13.36 The solubility of N2 in blood at 37°C and at...Ch. 13 - Prob. 13.37QPCh. 13 - Prob. 13.38QPCh. 13 - Prob. 13.39QPCh. 13 - 13.40 How is the lowering in vapor pressure...Ch. 13 - Prob. 13.41QPCh. 13 - Prob. 13.42QPCh. 13 - Prob. 13.43QPCh. 13 - Prob. 13.44QPCh. 13 - Prob. 13.45QPCh. 13 - Prob. 13.46QPCh. 13 - Prob. 13.47QPCh. 13 - 13.48 How many grams of sucrose (C12H22O11) must...Ch. 13 - Prob. 13.49QPCh. 13 - 13.50 The vapor pressures of ethanol (C2H5OH) and...Ch. 13 - Prob. 13.51QPCh. 13 - Prob. 13.52QPCh. 13 - 13.53 What are the boiling point and freezing...Ch. 13 - 13.54 An aqueous solution contains the amino acid...Ch. 13 - 13.55 Pheromones are compounds secreted by the...Ch. 13 - 12.58 The elemental analysis of an organic solid...Ch. 13 - Prob. 13.57QPCh. 13 - 13.58 A solution is prepared by condensing 4.00 L...Ch. 13 - Prob. 13.59QPCh. 13 - 13.60 A solution of 2.50 g of a compound of...Ch. 13 - Prob. 13.61QPCh. 13 - 13.62 A solution containing 0.8330 g of a protein...Ch. 13 - Prob. 13.63QPCh. 13 - 13.64 A solution of 6.85 g of a carbohydrate in...Ch. 13 - 13.65 Define ion pairs. What effect does ion-pair...Ch. 13 - Prob. 13.66QPCh. 13 - Prob. 13.67QPCh. 13 - Prob. 13.68QPCh. 13 - Prob. 13.69QPCh. 13 - Prob. 13.70QPCh. 13 - Prob. 13.71QPCh. 13 - 13.72 At 25°C the vapor pressure of pure water is...Ch. 13 - 13.73 Both NaCl and CaCl2 are used to melt ice on...Ch. 13 - Prob. 13.74QPCh. 13 - Prob. 13.75QPCh. 13 - Prob. 13.76QPCh. 13 - Prob. 13.77QPCh. 13 - Prob. 13.78QPCh. 13 - Prob. 13.79QPCh. 13 - Prob. 13.80QPCh. 13 - Prob. 13.81QPCh. 13 - Prob. 13.82QPCh. 13 - Prob. 13.83QPCh. 13 - Prob. 13.84QPCh. 13 - Prob. 13.85QPCh. 13 - Prob. 13.86QPCh. 13 - Prob. 13.87QPCh. 13 - Prob. 13.88QPCh. 13 - Prob. 13.89QPCh. 13 - Prob. 13.90QPCh. 13 - 13.91 Hydrogen peroxide with a concentration of...Ch. 13 - 13.92 Before a carbonated beverage bottle is...Ch. 13 - Prob. 13.93QPCh. 13 - 13.94 Explain each of these statements: (a) The...Ch. 13 - Prob. 13.95QPCh. 13 - Prob. 13.96QPCh. 13 - Prob. 13.97QPCh. 13 - Prob. 13.98QPCh. 13 - Prob. 13.99QPCh. 13 - Prob. 13.100QPCh. 13 - Prob. 13.101QPCh. 13 - Prob. 13.102QPCh. 13 - Prob. 13.103QPCh. 13 - Prob. 13.104QPCh. 13 - Prob. 13.105SPCh. 13 - Prob. 13.106SPCh. 13 - Prob. 13.107SPCh. 13 - Prob. 13.108SPCh. 13 - Prob. 13.109SPCh. 13 - Prob. 13.110SPCh. 13 - 13.111 A student carried out the following...Ch. 13 - Prob. 13.112SPCh. 13 - Prob. 13.113SPCh. 13 - Prob. 13.114SP
Knowledge Booster
Background pattern image
Recommended textbooks for you
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY