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; Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition (4th Edition)

4th Edition

ISBN: 9780134568188

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

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Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. N₂H₅ClO₄

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Chemistry: A Molecular Approach; Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition (4th 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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