Please correct answer and don't use hand raiting What is the effect of an external applied pressure on vapor pressure? Is the vapor pressure ofice in T14, Figure 2 at -10°C the same as that in T14, Figure 3 at the same temperature? Hint:Proceed as in CA T13 CTQ 8,9 but recognize that T is constant.

Effect of External Pressure on Vapor PressureVapor pressure is the pressure exerted by a vapor in…

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Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter11: Intermolecular Forces And Liquids

Section: Chapter Questions

Problem 39IL

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The following data are the equilibrium vapor pressure of limonene, C10H16, at various temperatures. (Limonene is used as a scent in commercial products.) (a) Plot these data as ln P versus 1/T so that you have a graph resembling the one in Figure 11.13. (b) At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is it 650 mm Hg? (c) What is the normal boiling point of limonene? (d) Calculate the molar enthalpy of vaporization for limonene using the Clausius-Clapeyron equation.
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.
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?
The vapor pressure of I2(s) at 30C is 0.466 mm Hg. (a) How many milligrams of iodine will sublime into an evacuated 750.0-mL flask? (b) If 3.00 mg of I2 are used, what will the final pressure in the flask be? (c) If 7.85 mg of I2 are used, what will the final pressure in the flask be?
p-Dichlorobenzene, C6H4Cl2, can be one of the ingredients in mothballs. Its vapor pressure at 20C is 0.40 mm Hg. (a) How many milligrams of C6H4Cl2 will sublime into an evacuated 750-mL flask at 20C? (b) If 5.0 mg of p-dichlorobenzene were put into an evacuated 750-mL flask, how many milligrams would remain in the solid phase? (c) What is the final pressure in an evacuated 500-mL flask at 20C that contains 2.00 mg of p-dichlorobenzene? Will there be any solid in the flask?
The vapor pressure of ethanol, C2H5OH, at 50.0 C is 233 mmHg, and its normal boiling point at 1 atm is 78.3 C. Calculate the vapH of ethanol.
8.89 The following data show the vapor pressure of liquid propane as a function of temperature (a) Plot a vapor pressure curve for propane and use it to estimate the normal boiling point. (b) Use your curve to estimate the pressure (in atm) in the propane rank supplying fuel for a gas barbecue grill on a hot summer day when the temperature is 95°F (c) What implications might your answer to part (b) have for an engineer designing propane storage tanks? T (°C) -100 -80 -60 -40 -20 0 20 P (torr) 22.4 100.6 328.8 856.9 1888.6 3665.6 6445.9
Dichloromethane, CH2Cl2,is widely used as a degreaser and paint stripper. Its vapor pressure is 381.0 mm Hg at 21.9C and 465.8 mm Hg at 26.90C. Estimate (a) its heat of vaporization (Hvap). (b) its normal boiling point.
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?
Given the following data about CO2: â€¢ triple point: -57C, 5.11 atm â€¢ critical point: 31C, 73 atm â€¢ sublimes at -78.5C, 1 atm â€¢ The solid is the denser phase. (a) Construct a simplified (not to scale) phase diagram for CO2. (b) Estimate the vapor pressure of CO2 at 0C. (c) At 10 atm pressure and -50C, is CO2 a liquid?
Chloroform, CHCl3, has a normal boiling point of 61C. Its vapor pressure at 43C is 0.526 atm. What is the concentration (in g/L) of CHCl3 when it saturates the air at 27C?

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What is the effect of an external applied pressure on vapor pressure? Is the vapor pressure of ice in T14, Figure 2 at -10°C the same as that in T14, Figure 3 at the same temperature? Hint: Proceed as in CA T13 CTQ 8,9 but recognize that T is constant.