Use the vapor-pressure curve in Figure 11.22 to estimate the external pressure under which ethyl alcohol will boil at 30°C.. torr What is the normal boiling point of diethly ether? Centegrade Vapor pressure (torr) 600 400 200 0 34.6°C Diethyl ether 20 78.3°C 100°C Ethyl alcohol (ethanol) 40 60 Temperature (°C) Figure 11.22. Water Ethylene glycol 80 100

Use the vapor-pressure curve in Figure 11.22 to estimate the external pressure under which ethyl alcohol will boil at 30°C.. torr What is the normal boiling point of diethly ether? Centegrade Vapor pressure (torr) 600 400 200 0 34.6°C Diethyl ether 20 78.3°C 100°C Ethyl alcohol (ethanol) 40 60 Temperature (°C) Figure 11.22. Water Ethylene glycol 80 100

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter10: Liquids And Solids

Section: Chapter Questions

Problem 91E: In Breckenridge, Colorado, the typical atmospheric pressure is 520. torr. What is the boiling point...

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8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?
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?
Equilibrium vapor pressures of benzene, C6H6, at various temperatures are given in the table. (a) What is the normal boiling point of benzene? (b) Plot these data so that you have a graph resembling the one in Figure 11.12. At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is the vapor pressure 650 mm Hg? (c) Calculate the molar enthalpy of vaporization for benzene using the ClausiusClapeyron equation.
Answer the following questions using Figure 11.12: (a) What is the equilibrium vapor pressure of diethyl ether at room temperature (approximately 20 C)? (b) Place the three compounds in Figure 11.12 in order of increasing intermolecular forces. (c) If the pressure in a flask is 400 mm Hg and if the temperature is 40 C, which of the three compounds (diethyl ether, ethanol, and water) are liquids, and which are gases? Figure 11.12 Vapor pressure curves for diethyl ether [(C2H3)2O], ethanol (C2H5OH), and water. Each curve represents conditions of T and P of which the two phases, liquid and vapor, are in equilibrium. These compounds exist as liquids for temperatures and pressures to the left of the curve and as gases under conditions to the right of the curve. (See Appendix G for vapor pressures for water of various temperatures.)
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.
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?
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?