This graph shows how the vapor pressure of three liquids varies with temperature: vapor pressure, torr 900- 800 700+ 600+ 500 400. 300 200 100 0+ 100 110 130 temperature, °C Use the graph to answer the following questions: Which liquid is the most volatile? Which is the least volatile? 120 What is the normal boiling point of each liquid? Note: your answer must be within 1°C of the exact answer to be graded correct. Suppose a beaker of toluene is put inside a sealed tank containing toluene gas at 103. degree C and 845. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same amount? acetylacetone toluene octane most volatile: least volatile: 140 acetylacetone: toluene: octane: more less the same choose one choose one пос °C °C

This graph shows how the vapor pressure of three liquids varies with temperature: vapor pressure, torr 900- 800 700+ 600+ 500 400. 300 200 100 0+ 100 110 130 temperature, °C Use the graph to answer the following questions: Which liquid is the most volatile? Which is the least volatile? 120 What is the normal boiling point of each liquid? Note: your answer must be within 1°C of the exact answer to be graded correct. Suppose a beaker of toluene is put inside a sealed tank containing toluene gas at 103. degree C and 845. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same amount? acetylacetone toluene octane most volatile: least volatile: 140 acetylacetone: toluene: octane: more less the same choose one choose one пос °C °C

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 24QAP

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Similar questions

Suppose that three unknown pure substances are liquids at room temperature. You make vapor pressure measurements and find that substance Q has a pressure of torr, substance R has a pressure of 42 torr, and substance S has a pressure of 330 torr. If you slowly increase the temperature, which substance will boil first and which will boil last?
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.
A fluorocarbon, CF4, has a critical temperature of 45.7 C and a critical pressure of 37 atm. Are there any conditions under which this compound can be a liquid at room temperature? Explain briefly.
A liquid has a vapH of 38.7 kJ/mol and a boiling point of 110 C at 1 atm pressure. Calculate the vapor pressure of the liquid at 97 C.
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?
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?
What are intermolecular forces? How do they differ from intramolecular forces? What are dipole-dipole forces? How do typical dipole-dipole forces differ from hydrogen bonding interactions? In what ways are they similar? What are London dispersion forces? How do typical London dispersion forces differ from dipole-dipole forces? In what ways are they similar? Describe the relationship between molecular size and strength of London dispersion forces. Place the major types of intermolecular forces in order of increasing strength. Is there some overlap? That is, can the strongest London dispersion forces be greater than some dipole-dipole forces? Give an example of such an instance.