The substance methane has the following properties: normal melting point: 90.7 K normal boiling point: 109.1 K triple point: 9.2x102 atm, 90.6 K critical point: 45.7 atm, 190.7 K At temperatures above 190.7 K and pressures above 45.7 atm, CH, is a supercritical fluid CH, does not exist as a liquid at pressures below 9.2x10^-2 atm. |at 44.0 atm and 83.7 K. at 9.20x10 atm and 116.0 K. v at 1.00 atm and 102.0 K. CH4 is a gas CH4 is a CH4 is a

The substance methane has the following properties: normal melting point: 90.7 K normal boiling point: 109.1 K triple point: 9.2x102 atm, 90.6 K critical point: 45.7 atm, 190.7 K At temperatures above 190.7 K and pressures above 45.7 atm, CH, is a supercritical fluid CH, does not exist as a liquid at pressures below 9.2x10^-2 atm. |at 44.0 atm and 83.7 K. at 9.20x10 atm and 116.0 K. v at 1.00 atm and 102.0 K. CH4 is a gas CH4 is a CH4 is a

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 16Q: Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is...

See similar textbooks

Similar questions

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.
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?
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?
At a resort in Sante Fe, New Mexico, the barometric pressure is 625 mm Hg. Water boils in an open pot at 94.5C. A pressure cooker is set for 1.75 atm. (a) At what temperature will water boil in that pressure cooker? (For water, Hvap=40.7kJ/mol.) (b) What is the difference between the boiling point in the open pot and in the pressure cooker?
Classify each of the following statements as true or false. a Intermolecular attractions are stronger in liquids than in gases. b Substances with weak intermolecular attractions generally have low vapor pressures. c Liquids with high molar heats of vaporization usually are more viscous than liquids with low molar heats of vaporization. d A substance with a relatively high surface tension usually has a very low boiling point. e All other things being equal, hydrogen bonds are weaker than induced dipole or dipole forces. f Induced dipole forces become very strong between large molecules. g Other things being equal, nonpolar molecules have stronger intermolecular attractions than polar molecules. h The essential feature of a dynamic equilibrium is that the rates of opposing changes are equal. i Equilibrium vapor pressure depends on the concentration of a vapor above its own liquid. j The heat of vaporization is equal to the heat of fusion, but with opposite sign. k The boiling point of a liquid is a fixed property of the liquid. l If you break shatter an amorphous solid, it will break in straight lines, but if you break a crystalline solid, it will break in curved lines. m Ionic crystals are seldom soluble in water. n Molecular crystals are nearly always soluble in water. o The numerical value of heat of vaporization is always larger than the numerical value of heat of condensation. p The units of heat of fusion are kJ/gC. q The temperature of water drops while it is freezing. r Specific heat is conerned with a change in temperature.
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?
Methane (CH4) cannot be liquefied at room temperature, no matter how high the pressure. Propane (C3H8), another simple hydrocarbon, has a critical pressure of 42 atm and a critical temperature of 96.7 C. Can this compound be liquefied at room temperature?
The heats of vaporization of liquid O2, liquid Ne, and liquid methanol, CH3OH, are 6.8 kJ/moL 1.8 kJ/mol, and 34.5 kJ/mol, respectively. Are the relative values as you would expect? Explain.
Chloroform, CHCl3, a volatile liquid, was once used as an anesthetic but has been replaced by safer compounds. Chloroform boils at 61.7C and has a heat of vaporization of 31.4 kJ/mol. What is its vapor pressure at 37.2C?
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?