Using a phase diagram to predict phase at a given temperature... Study t..uilowing phase diagram of Substance X. 1.6- 0.8 solid liquid gas 0. 200 400 temperature (K) Use this diagram to answer the following questions. Suppose a small sample of pure X is held at –9. °C and 1.0 atm. What will be the state of the sample? (choose one) 8 Suppose the temperature is held constant at -9. °C but the pressure is decreased by 0.5 atm. What will happen to the sample? v (choose one) Nothing. It will melt. Suppose, on the other hand, the pressure is held constant at 1.0 atm It will freeze. but the temperature is decreased by 109. °C. What will happen to the It will boil. sample? It will condense. It will sublime. It will deposit. Explanation Check pressure (atm) ||

Using a phase diagram to predict phase at a given temperature... Study t..uilowing phase diagram of Substance X. 1.6- 0.8 solid liquid gas 0. 200 400 temperature (K) Use this diagram to answer the following questions. Suppose a small sample of pure X is held at –9. °C and 1.0 atm. What will be the state of the sample? (choose one) 8 Suppose the temperature is held constant at -9. °C but the pressure is decreased by 0.5 atm. What will happen to the sample? v (choose one) Nothing. It will melt. Suppose, on the other hand, the pressure is held constant at 1.0 atm It will freeze. but the temperature is decreased by 109. °C. What will happen to the It will boil. sample? It will condense. It will sublime. It will deposit. Explanation Check pressure (atm) ||

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter10: Solids, Liquids, And Phase Transitions

Section: Chapter Questions

Problem 69AP

See similar textbooks

Similar questions

Given the following data about xenon, normalboilingpoint=108Cnormalmeltingpoint=112Ctriplepoint=121Cat281mmHgcriticalpoint=16.6Cat58atm (a) Construct an approximate phase diagram for xenon. (b) Estimate the vapor pressure of xenon at -115C. (c) Is the density of solid Xe larger than that for liquid Xe?
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.
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?
Use the phase diagram of water in Figure 6.6 and count the total number of phase transitions that are represented.
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.
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?
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.
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?