most volatile: v choose one Which liquid is the most volatile? piperidine Which is the least volatile? least volatile: ethylbenzene octane piperidine: °C 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. ethylbenzene: octane: Suppose a beaker of ethylbenzene is put inside a sealed tank containing ethylbenzene gas at 111. degree C and 719. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same more less amount? the same

most volatile: v choose one Which liquid is the most volatile? piperidine Which is the least volatile? least volatile: ethylbenzene octane piperidine: °C 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. ethylbenzene: octane: Suppose a beaker of ethylbenzene is put inside a sealed tank containing ethylbenzene gas at 111. degree C and 719. torr. After ten minutes, will there be more liquid in the beaker, less liquid, or the same more less amount? the same

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter11: Intermolecular Forces And Liquids

Section: Chapter Questions

Problem 33GQ

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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 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?
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?
Two molecules that contain the same number of each kind of atom but [hat have different molecular structures are said to he isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below} have the formula C2H6Oand are isomers; Based on considerations of intermolecular forces. which substance would you expect to be more volatile? Which would you expect 10have the higher boiling point? Explain. methyl ether hyl alcohol msp;CH3OCH3CH3CH2OH
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.
Intermolecular Forces The following picture represents atoms of hypothetical, nonmetallic, monatomic elements A, B, and C in a container at a temperature of 4 K (the piston maintains the pressure at 1 atm). None of these elements reacts with the others. a What is the state (solid, liquid, or gas) of each of the elements represented in the container? b Rank the elements in the container from greatest to least, in terms of intermolecular interactions. Explain your answer. c What type(s) of intermolecular attractions are present in each of these elements? d Explain which element has the greatest atomic mass. e One of the elements in the container has a normal boiling point of 2 K. Which element would that be (A, B, or C)? How do you know? f One of the elements has a melting point of 50 K. Which element would that be (A, B, or C)? Why? g The remaining element (the one you have yet to choose) has a normal boiling point of 25 K. Identify the element. Could this element have a freezing point of 7 K? Explain. h If you started heating the sample to 20 K, explain what you would observe with regard to the container and its contents during the heating. i Describe the container and its contents at 20 K. Describe (include a drawing) how the container and its contents look at 20 K. j Now you increase the temperature of the container to 30 K. Describe (include a drawing) how the container and its contents look at 30 K. Be sure to note any changes in going from 20 K to 30 K. k Finally, you heat the container to 60 K. Describe (include a drawing) how the container and its contents look at this temperature. Be sure to note any changes in going from 30K to 60k