Explanation Given: The temperature ( T ) is 308 K . First flask: The pressure of N 2 is 1 atm . Second flask: The mass of H 2 O ( m w ) is 2 g . Third flask: The mass of ethanol ( m e ) is 0.50 g . The vapor pressure of water is 42 mmHg . The vapor pressure of ethanol is 102 mmHg . The ideal gas constant ( R ) is 0.0821 L atm / ( mol K) . Explanation: The total pressure of the flask when all stopcocks are open is equal to the individual pressures of nitrogen, water, and ethanol. P total = P N 2 + P H 2 O + P C 2 H 6 O Here, P N 2 is the pressure of nitrogen gas, P H 2 O is the pressure of water, and P C 2 H 6 O is the pressure of ethanol. Calculate the number of moles of water ( n w ) as follows: The molar mass of water ( M w ) is 18.01 g / mol . The number of moles of water is the ratio of the mass of water and its molar mass. n w = m w M w Substitute 18.01 g / mol for M w and 2 g for m w as follows: n w = 2 g 18.01 g / mol = 0.11 mol So, the moles of water is 0.11 mol . The pressure of nitrogen is 1 atm for 1 L . Therefore, calculate the pressure of nitrogen at 3 L as follows. P 1 V 1 = P 2 V 2 Substitute 1 atm for P 1 , 1 L for V 1 , and 3 L for V 2 as follows: 1 × 1 = P 2 × 3 P 2 = 0.33 atm This is equal to the required pressure of the nitrogen in one flask. So, the pressure of nitrogen ( P N 2 ) is 0.33 atm . Now, calculate the pressure of water as follows: P H 2 O V = n w R T Substitute 3 L for V , 308 K for T , 0.0821 L atm / ( mol K) for R , and 0.11 mol for n w : P H 2 O = 0 .11 mol × 0.0821 L atm / ( mol K) × 308 K 3 L = 0.927 atm One mmHg pressure is equal to 0.001316 atm . Convert the vapor pressure of water from mmHg to atmosphere as follows: 42 mmHg = 42 mmHg × 0

Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition

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ISBN: 9780134554259

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 11, Problem 101E

Interpretation Introduction

To determine: The total pressure of the system.

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Chapter 11, Problem 100E

Chapter 11, Problem 102E

Chapter 11 Solutions

Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition

Ch. 11 - Prob. 1SAQ Ch. 11 - Q2. Liquid nitrogen boils at 77 K. The image shown...Ch. 11 - Q3. Based on the expected intermolecular forces,...Ch. 11 - Q4. Which substance experiences dipole–dipole...Ch. 11 - Q5. One of these substances is a liquid at room...Ch. 11 - Prob. 6SAQ Ch. 11 - Q7. Determine the amount of heat (in kJ) required...Ch. 11 - Prob. 8SAQ Ch. 11 - Prob. 9SAQ Ch. 11 - Prob. 10SAQ

Ch. 11 - Prob. 1E Ch. 11 - 2. Why are intermolecular forces important? Ch. 11 - 3. What are the main properties of liquids (in...Ch. 11 - 4. What are the main properties of solids (in...Ch. 11 - Prob. 5E Ch. 11 - Prob. 6E Ch. 11 - Prob. 7E Ch. 11 - Prob. 8E Ch. 11 - Prob. 9E Ch. 11 - Prob. 10E Ch. 11 - Prob. 11E Ch. 11 - Prob. 12E Ch. 11 - 13. What is hydrogen bonding? How can you predict...Ch. 11 - Prob. 14E Ch. 11 - Prob. 15E Ch. 11 - Prob. 16E Ch. 11 - Prob. 17E Ch. 11 - Prob. 18E Ch. 11 - 19. Why is vaporization endothermic? Why is...Ch. 11 - 20. How is the volatility of a substance related...Ch. 11 - 21. What is the heat of vaporization for a liquid...Ch. 11 - 22. Explain the process of dynamic equilibrium....Ch. 11 - Prob. 23E Ch. 11 - Prob. 24E Ch. 11 - Prob. 25E Ch. 11 - 26. What is the Clausius–Clapeyron equation and...Ch. 11 - Prob. 27E Ch. 11 - Prob. 28E Ch. 11 - Prob. 29E Ch. 11 - Prob. 30E Ch. 11 - 31. Examine the heating curve for water in Section...Ch. 11 - Prob. 32E Ch. 11 - Prob. 33E Ch. 11 - Prob. 34E Ch. 11 - Prob. 35E Ch. 11 - Prob. 36E Ch. 11 - Prob. 37E Ch. 11 - Prob. 38E Ch. 11 - 39. Arrange these compounds in order of increasing...Ch. 11 - Prob. 40E Ch. 11 - Prob. 41E Ch. 11 - Prob. 42E Ch. 11 - Prob. 43E Ch. 11 - Prob. 44E Ch. 11 - Prob. 45E Ch. 11 - Prob. 46E Ch. 11 - Prob. 47E Ch. 11 - Prob. 48E Ch. 11 - Prob. 49E Ch. 11 - 50. Explain why the viscosity of multigrade motor...Ch. 11 - 51. Water in a glass tube that contains grease or...Ch. 11 - Prob. 52E Ch. 11 - Prob. 53E Ch. 11 - Prob. 54E Ch. 11 - Prob. 55E Ch. 11 - Prob. 56E Ch. 11 - 57. The human body obtains 915 kJ of energy from a...Ch. 11 - Prob. 58E Ch. 11 - Prob. 59E Ch. 11 - Prob. 60E Ch. 11 - Prob. 61E Ch. 11 - Prob. 62E Ch. 11 - Prob. 63E Ch. 11 - Prob. 64E Ch. 11 - Prob. 65E Ch. 11 - Prob. 66E Ch. 11 - Prob. 67E Ch. 11 - Prob. 68E Ch. 11 - Prob. 69E Ch. 11 - Prob. 70E Ch. 11 - Prob. 71E Ch. 11 - 72. How much heat (in kJ) is evolved in converting...Ch. 11 - Prob. 73E Ch. 11 - 74. Consider the phase diagram for iodine shown...Ch. 11 - Prob. 75E Ch. 11 - Prob. 76E Ch. 11 - Prob. 77E Ch. 11 - Prob. 78E Ch. 11 - Prob. 79E Ch. 11 - Prob. 80E Ch. 11 - Prob. 81E Ch. 11 - 82. How is the density of solid water compared to...Ch. 11 - Prob. 83E Ch. 11 - Prob. 84E Ch. 11 - Prob. 85E Ch. 11 - Prob. 86E Ch. 11 - Prob. 87E Ch. 11 - Prob. 88E Ch. 11 - Prob. 89E Ch. 11 - 90. A sample of steam with a mass of 0.552 g and...Ch. 11 - Prob. 91E Ch. 11 - Prob. 92E Ch. 11 - Prob. 93E Ch. 11 - 94. A sealed flask contains 0.55 g of water at 28...Ch. 11 - Prob. 95E Ch. 11 - 96. Consider a planet where the pressure of the...Ch. 11 - Prob. 97E Ch. 11 - 98. Given that the heat of fusion of water is...Ch. 11 - 99. The heat of combustion of CH4 is 890.4 kJ/mol,...Ch. 11 - Prob. 100E Ch. 11 - Prob. 101E Ch. 11 - 102. Butane (C4H10) has a heat of vaporization of...Ch. 11 - Prob. 103E Ch. 11 - 104. One prediction of global warming is the...Ch. 11 - Prob. 105E Ch. 11 - Prob. 106E Ch. 11 - Prob. 107E Ch. 11 - Prob. 108E Ch. 11 - Prob. 109E Ch. 11 - Prob. 110E Ch. 11 - Prob. 111E Ch. 11 - Prob. 112E Ch. 11 - Prob. 113QGW Ch. 11 - Prob. 114QGW Ch. 11 - Prob. 115QGW Ch. 11 - Prob. 116QGW Ch. 11 - 117. Students in a chemistry laboratory course are...

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