Match the process that eventually happens with the change in conditions according to this phase diagram. Scroll to see all of the possible answers. All or nothing points. • B A • • C Starting at Cwe decrease the temperature at constant pressure. deposition Starting at B we lower the pressure at constant temperature. vaporization melting Starting at A we increase the temperature at constant pressure. Next

Match the process that eventually happens with the change in conditions according to this phase diagram. Scroll to see all of the possible answers. All or nothing points. • B A • • C Starting at Cwe decrease the temperature at constant pressure. deposition Starting at B we lower the pressure at constant temperature. vaporization melting Starting at A we increase the temperature at constant pressure. Next

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter86: Sublimation

Section: Chapter Questions

Problem 4P

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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.
Consider the following data for xenon: Triple point: 121C, 280 torr Normal melting point: 112C Normal boiling point: 107C Which is more dense, Xe(s) or Xe(l)? How do the melting point and boiling point of xenon depend on pressure?
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?
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.
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.
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?
If you've ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed container above a liquid. What processes in the container give rise to this phenomenon?
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?
8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
A pure substance X has the following properties: Mp=90C, increasing slightly as pressure increases; normal bp=120C; liquid vp=65mm Hg at 100C, 20 mm Hg at the triple point. (a) Draw a phase diagram for X. (b) Label solid, liquid, and vapor regions of the diagram. (c) What changes occur if, at a constant pressure of 100 mm Hg, the temperature is raised from 100C to 150C?