(2) Sublimation. Figures below represent the phase diagrams for water and carbon dioxide. (a) Describe the difference in sublimation behavior under the pressure and temperature conditions prevailing on Earth. (b) How would you explain the sublimation of the polar ice caps on Mars during the Martian Summer? 217.7 METING FREZING Normal melting point Solid - Normal boiling point Liquid VAPQURISON DENSATION Gas 0.006 SUBLIMATION DEPOSITION 100 374.4 Temperature (C) Pressure (atm)

(2) Sublimation. Figures below represent the phase diagrams for water and carbon dioxide. (a) Describe the difference in sublimation behavior under the pressure and temperature conditions prevailing on Earth. (b) How would you explain the sublimation of the polar ice caps on Mars during the Martian Summer? 217.7 METING FREZING Normal melting point Solid - Normal boiling point Liquid VAPQURISON DENSATION Gas 0.006 SUBLIMATION DEPOSITION 100 374.4 Temperature (C) Pressure (atm)

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

Section9.4: Solids And Changes Of Phase

Problem 9.7CE: Sublimation is an excellent means of purification for compounds that will readily sublime. Explain...

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Similar questions

8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
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?
Referring to Figure 9.7, state what phase(s) is (are) present at (a) 1 atm, 10C. (b) 3 mm Hg, 20C. (c) 1000 mm Hg, 75C.
What feature characterizes the dynamic equilibrium between a liquid and its vapor in a closed container?
The phase diagram for water over a relative narrow pressure and temperature range is given in Figure 9.19. A phase diagram over a considerably wider range of temperature and pressure (kbar) is given nearby. This phase diagram illustrates the polymorphism of ice, the existence of a solid in more than one form. In this case, Roman numerals are used to designate each polymorphic form. For example, Ice I, ordinary ice, is the form that exists under ordinary pressures. The other forms exist only at higher pressures, in some cases extremely high pressure such as Ice VII and Ice VIII. Using the phase diagram, give the approximate P and T conditions at the triple point for Ice III, Ice V, and liquid water. Determine the approximate temperature and pressure for the triple point for Ices VI, VII, and VIII. What is anomalously different about the fusion curves for Ice VI and Ice VII compared to that of Ice I? What phases exist at 8 kbar and 20 °C? At a constant temperature of −10 °C, start at 3 kbar and increase the pressure to 7 kbar. Identify all the phase changes that occur sequentially as these conditions change. Explain why there is no triple point for the combination of Ice VII, Ice VIII, and liquid water.
The normal boiling point of SO2 is 263.1 K and that of NH3 is 239.7 K. At −40 °C, would you predict that ammonia has a vapor pressure greater than, less than, or equal to that of sulfur dioxide? Explain.
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.
Sublimation is an excellent means of purification for compounds that will readily sublime. Explain how purification by sublimation works at the nanoscale.