This graph shows how the vapor pressure of three liquids varies with temperature: 900 800 700 600 500 400 300 cyclohexanol - cyclohexanone dimethyl sulfoxide 200 100 0 150 160 170 180 190 temperature, °C Use the graph to answer the following questions: Which liquid is the most volatile? most volatile: choose one Which is the least volatile? least volatile: choose one cyclohexanol: What is the normal boiling point of each liquid? Note: your answer must be within 1°C of the exact answer to be graded correct. cyclohexanone: dimethyl sulfoxide: °C Suppose a beaker of cyclohexanone is put inside a sealed tank containing cyclohexanone gas at 153. degree C and 880. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same more less amount? O the same vapor pressure, torr

This graph shows how the vapor pressure of three liquids varies with temperature: 900 800 700 600 500 400 300 cyclohexanol - cyclohexanone dimethyl sulfoxide 200 100 0 150 160 170 180 190 temperature, °C Use the graph to answer the following questions: Which liquid is the most volatile? most volatile: choose one Which is the least volatile? least volatile: choose one cyclohexanol: What is the normal boiling point of each liquid? Note: your answer must be within 1°C of the exact answer to be graded correct. cyclohexanone: dimethyl sulfoxide: °C Suppose a beaker of cyclohexanone is put inside a sealed tank containing cyclohexanone gas at 153. degree C and 880. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same more less amount? O the same vapor pressure, torr

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem ISP

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A 1.50-g sample of methanol (CH3OH) is placed in an evacuated 1.00-L container at 30 C. (a) Calculate the pressure in the container if all of the methanol is vaporized. (Assume the ideal gas law, PV = nRT.) (b) The vapor pressure of methanol at 30 C is 158 torr. What mass of methanol actually evaporates? Is liquid in equilibrium with vapor in the vessel?
Suppose that three unknown pure substances are liquids at room temperature. You make vapor pressure measurements and find that substance Q has a pressure of torr, substance R has a pressure of 42 torr, and substance S has a pressure of 330 torr. If you slowly increase the temperature, which substance will boil first and which will boil last?
Diethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6C, diethyl ether has a vapor pressure of 760. torr, and at 17.9C, it has a vapor pressure of 400. torr. What is the H of vaporization for diethyl ether?
The molecular mass of butanol, C4H9OH, is 74.14; that of ethylene glycol, CH2(OH)CH2OH, is 62.08, yet their boiling points are 117.2 C and 174 C, respectively. Explain the reason for the difference.
Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?
What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.
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Of the four general types of solids, which one(s) (a) are generally insoluble in water? (b) have very high melting points? (c) conduct electricity as solids?
Two molecules that contain the same number of each kind of atom but [hat have different molecular structures are said to he isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below} have the formula C2H6Oand are isomers; Based on considerations of intermolecular forces. which substance would you expect to be more volatile? Which would you expect 10have the higher boiling point? Explain. methyl ether hyl alcohol msp;CH3OCH3CH3CH2OH
Methane (CH4) cannot be liquefied at room temperature, no matter how high the pressure. Propane (C3H8), another simple hydrocarbon, has a critical pressure of 42 atm and a critical temperature of 96.7 C. Can this compound be liquefied at room temperature?