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Q:
Which of the following pure substances has the highest melting point?
A) CCl4
B) AlCl3
C) NCl3
D) LiCl
E) MgCl2
Q:
Which of the following pure substances has the lowest melting point?
A) Cs2O
B) CsCl
C) CsBr
D) CsI
E) CsF
Q:
Which of the following pure substances has the lowest melting point?
A) LiF
B) RbF
C) CsF
D) KF
E) NaF
Q:
Which of the following pure substances has the highest normal melting point?
A) KF
B) KI
C) NaF
D) NaCl
E) NaI
Q:
Which of the following is a molecular solid?
A) carborundum, SiC
B) quartz
C) glass
D) hydrogen chloride
E) potassium
Q:
Which bonding interaction best describes the strongest intermolecular forces in AlH3?A) dipole-dipole forcesB) metallic bondingC) ionic bondingD) London dispersion forcesE) primarily hydrogen bonding
Q:
Which of the following is an ionic solid?
A) SiO2(s)
B) Ne(s)
C) Na(s)
D) CsF(s)
E) CO2(s)
Q:
Which of the following is a molecular solid?
A) NaCl
B) CH4
C) SiO2
D) C(graphite)
E) C(diamond)
Q:
Which of the following is not a covalent network solid?A) diamondB) silicon carbideC) quartzD) ironE) graphite
Q:
Which of the following best describes calcium hydride (CaH2) at room temperature and pressure?
A) nonpolar molecular gas
B) metallic solid
C) ionic solid
D) polar molecular gas
E) covalent network solid
Q:
Which substance can be described as cations bonded together by mobile electrons?
A) S8(s)
B) Ag(s)
C) HCl(l)
D) KCl(s)
E) Kr(l)
Q:
Van der Waals forces must be broken to melt this type of solid.
A) A covalent network solid.
B) A metallic solid.
C) A molecular solid.
D) An ionic solid.
E) none of the above
Q:
A solid has a very high melting point, is hard, and in the molten state is a non-conductor. The solid is most likely
A) a covalent network solid.
B) a metallic solid.
C) an amorphous solid.
D) a molecular solid.
E) an ionic solid.
Q:
Which of the following is the strongest intermolecular force present in dry ice, CO2(s)?
A) covalent bonding
B) hydrogen bonding
C) ionic bonding
D) London forces
E) metallic bonding
Q:
Which of the following best describes silane (SiH4) at room temperature and pressure?
A) ionic solid
B) covalent network solid
C) nonpolar molecular gas
D) polar molecular gas
E) metallic solid
Q:
The molecules in a sample of solid SO2 are attracted to each other by a combination ofA) H-bonding and ionic bonding.B) covalent bonding and dipole-dipole interactions.C) London forces and H-bonding.D) London forces and dipole-dipole interactions.E) none of these
Q:
The strongest intermolecular forces between molecules of PH3 areA) hydrogen bonds.B) covalent bonds.C) ionic bonds.D) London forces.E) dipole-dipole attractions.
Q:
The strongest intermolecular forces present in a sample of pure I2 areA) London forces.B) dipole-dipole forces.C) metallic bonds.D) covalent network bonds.E) covalent bonds.
Q:
Which of the following pure substances may exhibit hydrogen bonding?
A) CH3Cl
B) CH3OCH3
C) H2CO
D) N(CH3)3
E) H2NNH2
Q:
Which of the following best describes carbon dioxide (CO2) at room temperature and pressure?
A) ionic solid
B) nonpolar molecular gas
C) metallic solid
D) polar molecular gas
E) covalent network solid
Q:
Which of the following substances has the weakest intermolecular forces?
A) I2
B) C8H18
C) SiH4
D) CH3CH2CH2CH2OH
E) SbCl3
Q:
Which pure substance exhibits hydrogen bonding?
A) HNF2
B) B2H6
C) HBr
D) H2S
E) CaH2
Q:
What is the maximum number of hydrogen bonds in which a water molecule could participate?
A) 2
B) 4
C) 3
D) 6
E) 5
Q:
When two water molecule form a hydrogen bond, which atoms are involved in the interaction?
A) Two hydrogens from one molecule and one hydrogen from the other molecule
B) An oxygen from one molecule and an oxygen from the other molecule
C) Two hydrogens from one molecule and one oxygen from the other molecule
D) A hydrogen from one molecule and a hydrogen from the other molecule
E) A hydrogen from one molecule and an oxygen from the other molecule
Q:
In an experiment, 40.0 mmol of helium gas is collected over water. The total volume of gas collected is 0.224 L. Under similar conditions, the gas is collected over two other liquids, A and B. The total volume of gas collected over A and B are 0.222 L and 0.227 L, respectively. Which of the following statements is false?
A) Liquid B boils at a higher temperature than water
B) Liquid A boils at a higher temperature than water
C) The vapor pressure of B is higher than that of A
D) The vapor pressure of B is higher than that of water
E) Liquid A boils at a temperature higher than B
Q:
Which of the following concerning intermolecular forces is/are correct?
1) Intermolecular forces depend in part on the shape of a molecule.
2) London forces contribute to the net forces of attraction found in all molecular solids and liquids.
3) Hydrogen bonding is a special category of dipole-dipole attractions.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
Rank the following in order of increasing normal boiling point: N2, O2, Br2, Xe.
A) N2 < O2< Xe < Br2
B) O2 < N2< Xe < Br2
C) Br2 < Xe < N2< O2
D) N2 < O2< Br2< Xe
E) Xe < Br2 < N2 < O2
Q:
Rank the following molecules in order of increasing normal boiling point: CH3CH2OH, CH3CH2CH2OH, CH3CH2OCH3.
A) lowest CH3CH2CH2OH, CH3CH2OCH3, CH3CH2OH highest.
B) lowest CH3CH2OH, CH3CH2OCH3, CH3CH2CH2OH highest.
C) lowest CH3CH2CH2OH, CH3CH2OH, CH3CH2OCH3highest.
D) lowest CH3CH2OCH3, CH3CH2OH, CH3CH2CH2OH highest.
E) lowest CH3CH2OCH3, CH3CH2CH2OH, CH3CH2OH highest.
Q:
Which of the following pure substances has an unusually high normal boiling point?
A) CH3OCH3
B) CH3SH
C) HCl
D) CH3NH2
E) CH3Cl
Q:
At 25C, the vapor pressure of diethyl ether, (CH3CH2)2O, is higher than the vapor pressure of its isomer n-butanol, CH3CH2CH2CH2OH, because
A) diethyl ether has a higher density than n-butanol.
B) diethyl ether has weaker intermolecular forces than n-butanol.
C) diethyl ether has a lower critical temperature than n-butanol.
D) diethyl ether has a higher surface tension than n-butanol.
E) diethyl ether has weaker intramolecular forces than n-butanol.
Q:
Which of the following pure substances has the highest standard enthalpy of vaporization at 25ºC?A) H2OB) NH3C) PH3D) AsH3E) SbH3
Q:
Which of the following pure substances has the highest vapor pressure at room temperature?
A) Si3H8
B) Si2H6
C) Si2Cl6
D) Si4H10
E) SiH4
Q:
Which of the following pure substances has the lowest vapor pressure at 25ºC?A) SbH3B) NH3C) PH3D) AsH3E) H2O
Q:
Why does hydrogen fluoride have an unusually high normal boiling point compared to the other hydrogen halides?
A) The H-F bond in hydrogen fluoride is very strong.
B) Hydrogen fluoride has very strong London dispersion forces.
C) Hydrogen fluoride is capable of forming hydrogen bonds.
D) Hydrogen fluoride is ionic.
E) Hydrogen fluoride is covalent.
Q:
Which of the following pure substances has the highest normal boiling point?
A) HI
B) HCl
C) HF
D) H2S
E) HBr
Q:
Which of the following compounds is expected to have the lowest vapor pressure?
A) CH3OCH3
B) CH3CH2F
C) CH3CH2OH
D) CH3CH2CH2CH3
E) CH3CH2CH3
Q:
Which of the following compounds has the lowest normal boiling point?
A) CH3CH2CH2NH2
B) CH3CH2CH2F
C) CH3CH2CH2OH
D) CH3CH2COOH
E) CH3CH(OH)CH3
Q:
Which of the following indicates the existence of strong intermolecular forces of attraction in a liquid?
A) a very low critical temperature
B) a very low boiling point
C) a very low vapor pressure
D) a very low viscosity
E) a very low enthalpy of vaporization
Q:
Which compound has the lowest standard enthalpy of vaporization at 25ºC?A) C6H14B) C8H16C) C5H12D) C8H18E) C7H16
Q:
Methane (CH4) is able to be liquefied at low temperatures due to which intermolecular force?A) ionic bondingB) covalent bondingC) hydrogen bondingD) dipole-dipoleE) London dispersion
Q:
Which of the following pure substances has the lowest normal boiling point?
A) H2S
B) NH3
C) H2O
D) H2Te
E) H2Se
Q:
Which of the following compounds has the highest vapor pressure at 25ºC?A) CH3CH2OHB) CH3CH2CH2CH3C) CH3OCH3D) CH3CH2CH3E) CH3CH2CH2Cl
Q:
Which of the following compounds has the highest normal boiling point?
A) CH3CH2CH2CH3
B) CH3Cl
C) CH3CH2OH
D) CH3OCH3
E) CH3CH2CH3
Q:
Which one of the following decreases as the strength of the attractive intermolecular forces increases?
A) The normal boiling temperature.
B) The vapor pressure of a liquid.
C) The extent of deviations from the ideal gas law.
D) The heat of vaporization.
E) The sublimation temperature of a solid.
Q:
In which of the following substances are intermolecular forces of attraction absent?
A) HF(l)
B) CCl4(l)
C) NaCl(l)
D) H2O(l)
E) N2(l)
Q:
The measure of the resistance to flow of a liquid is
A) London forces.
B) van der Waals forces.
C) viscosity.
D) vapor pressure.
E) surface tension.
Q:
Which of the following concerning surface tension and viscosity is/are correct?
1) A molecule at the surface of a liquid experiences a net attractive force toward the interior of the liquid.
2) The surface tension of a liquid is unaffected by substances dissolved in the liquid.
3) The viscosity of a liquid is determined in part by the strength of intermolecular forces.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1 and 3
Q:
Which of the following forces is/are responsible for capillary action, a property of liquids?
1) attractive forces between the liquid and the capillary material
2) surface tension of the liquid
3) viscosity of the liquid
A) 1
B) 2
C) 3
D) 1 and 2
E) 1, 2, and 3
Q:
Which is the best reason for why water in a glass capillary has a concave meniscus, while mercury in a glass capillary has a convex meniscus?
A) Mercury has a greater dispersion force than water.
B) The water is attracted more strongly to the glass than the mercury is attracted to the glass.
C) The mercury is attracted more strongly to the glass than the water is attracted to the glass.
D) Water is a molecular compound while mercury is a metallic element.
E) Water has a greater dispersion force than mercury.
Q:
If the diameter of a spherical water droplet is 100.0 m, how much energy is required to increase the diameter of the water droplet by 3.0 m? The surface tension of water is 1.0x10-3J/m2.A) 3.1 x10-11JB) 1.9 x10-12JC) 2.8 x10-14JD) 7.7 x10-12JE) 3.3 x10-11J
Q:
Which explanation best describes surface tension?
A) Molecules at the surface of a liquid experience a net force towards the liquid's interior.
B) Molecules at the edges of a liquid adhere to the surface of the liquid's container.
C) Molecules of a liquid tend to form a concave meniscus.
D) Molecules of a liquid tend to resist flow.
E) Molecules of a liquid have a very low vapor pressure.
Q:
Below is a phase diagram for a substance. What is the name for point Z on the diagram?
A) normal boiling point.
B) critical point.
C) melting point.
D) boiling point.
E) triple point.
Q:
If the liquid of a pure substance has a lower density than the solid, what is the effect on the pressure-temperature phase diagram?
A) The vapor-pressure curve arches upward.
B) The normal melting point is above room temperature.
C) The melting-point curve has a negative slope.
D) The vapor-pressure curve arches downward.
E) The melting-point curve has a positive slope.
Q:
Below is a phase diagram for a substance. Which line represents the vapor-pressure curve of the substance?
A) S-Z
B) X-Z
C) S-X
D) M-N
E) R-X
Q:
Below is a phase diagram for a substance. Which line represents the melting-point curve of the substance?
A) R-X
B) S-X
C) X-Z
D) S-Z
E) M-N
Q:
Below is a phase diagram for a substance. What is the name for point X on the diagram?
A) boiling point
B) normal boiling point
C) triple point
D) melting point
E) critical point
Q:
The critical point of CCl4is 283ºC and 45 atm pressure. Liquid CCl4has a vapor pressure of 10.0 atm at 178ºC. Which of the following statements must be true?A) Vapor and liquid can only be in equilibrium at one temperaturethe normal boiling point.B) Liquid CCl4can exist at temperatures greater than 283ºC if the pressure is greater than 45 atm.C) Liquid and solid can only be in equilibrium at one temperaturethe freezing point.D) The triple point of CCl4must be less than 178ºC.E) The normal boiling point of CCl4must be greater than 178ºC.
Q:
The triple point of iodine is at 90 torr and 115ºC. This means that liquid I2A) cannot have a vapor pressure less than 90 torr.B) is more dense than I2(s).C) cannot exist at 1 atmosphere pressure.D) cannot exist above 115ºC.E) can exist at pressure of 10 torr.
Q:
From a consideration of the phase diagram below, a change from point M to point N corresponds to A) sublimation.
B) liquefaction.
C) evaporation.
D) condensation.
E) freezing.
Q:
Choose the correct statement about the diagram below. A) The diagram shows the triple point above 1 atm pressure.
B) The diagram is qualitatively correct for water.
C) The diagram shows that the melting point of the solid increases with increasing pressure.
D) The diagram could represent the phase diagram of CO2.
E) None of the above statements is correct.
Q:
Given the accompanying phase diagram, under what conditions will liquid be found in equilibrium with either solid or gas? A) Anywhere along curve AB.
B) Anywhere along curve AC.
C) Anywhere along curve AD.
D) Anywhere along curve AB and AC.
E) Anywhere along curve AB and AD.
Q:
Which of the following statements concerning the accompanying phase diagram is false? A) The solid is more dense than the liquid.
B) Point C is the critical point of the substance.
C) Point A is the triple point of the substance.
D) The normal boiling point is above the triple point.
E) The curve AD divides the solid region from the gas region.
Q:
In the accompanying phase diagram, a liquid can be present at combinations of temperature and pressure corresponding to points A) A, C, G, and D.
B) A, C, D, and F.
C) A, B, C, and G.
D) A and C only.
E) G, C, D, and E.
Q:
What is the enthalpy of vaporization of a compound that has a vapor pressure of 131 mmHg at 211 K and 2.23 mmHg at 177 K? (R= 8.31 J/(K mol))A) 996 kJ/molB) 1.15 kJ/molC) 3.31 kJ/molD) 37.2 kJ/molE) 368 kJ/mol
Q:
Knowing that Hvap for water is 40.7 kJ/mol, calculate Pvapof water at 37ºC.A) 52.7 torrB) 25.4 torrC) 18.7 torrD) 12.4 torrE) 6.90 torr
Q:
For a particular liquid, raising its temperature from 319 K to 337 K causes its vapor pressure to double. What is the enthalpy of vaporization of this liquid? (R=8.31J/(K mol))A) 34.4 kJ/molB) 320 kJ/molC) 2.01 kJ/molD) 228 kJ/molE) 104 kJ/mol
Q:
In a certain mountain range, water boils at 94ºC. What is the atmospheric pressure under these conditions? The enthalpy of vaporization of water at 100ºC is 40.7 kJ/mol. (R=8.31J/(K mol))A) 1760 mmHgB) 324 mmHgC) 613 mmHgD) 942 mmHgE) 329 mmHg
Q:
A liquid has an enthalpy of vaporization of 30.8 kJ/mol. At 275 K it has a vapor pressure of 117 mmHg. What is the normal boiling point of this liquid? (R= 8.31 J/(K mol))A) 293 KB) 319 KC) 275 KD) 259 KE) 241 K
Q:
A particular compound has an enthalpy of vaporization of 28300 J/mol. At 281 K it has a vapor pressure of 101 mmHg. What is its vapor pressure at 301 K? (R= 8.31 J/(K mol))A) 98.8 mmHgB) 123 mmHgC) 45.2 mmHgD) 226 mmHgE) 103 mmHg
Q:
The vapor pressure of a given liquid will increase if
A) the liquid is moved to a container in which its surface is very much larger.
B) the volume of the liquid is increased.
C) the temperature is increased.
D) the volume of the vapor phase is increased.
E) a more volatile liquid is added to the given liquid.
Q:
The vapor pressure of a liquid increases with increasing temperature. Which of the following statements best explains this relationship?
A) All the molecules have greater kinetic energies.
B) The number of gaseous molecules above the liquid remains constant, but these molecules have greater average kinetic energy.
C) The faster-moving molecules in the liquid exert a greater pressure.
D) The intermolecular forces between the molecules decrease at higher temperatures.
E) The average kinetic energy of molecules is greater; thus more molecules can enter the gaseous state.
Q:
What is the value of qwhen 8.21 g of water vaporizes at 373 K? The enthalpy of condensation of water at 373 K is -40.7 kJ/mol.A) -334 kJB) -18.5 kJC) 18.5 kJD) 334 kJE) 0.202 kJ
Q:
How much heat is released at constant pressure if a 14.0-L tank containing 56.0 atm of hydrogen sulfide gas condenses at its boiling point of -60.0oC? The enthalpy of vaporization of hydrogen sulfide is 18.7 kJ/mol at -60.0oC. (R= 0.0821 L atm/(K mol))A) 1.17 x102JB) 2.98 x106JC) 4.17 x102JD) 1.87 x104JE) 8.38 x105J
Q:
Assume 12,500 J of energy is added to 2.0 moles (36 grams) of H2O as an ice sample at 0ºC. The molar heat of fusion is 6.02 kJ/mol. The specific heat of liquid water is 4.18 J/g·ºC. The molar heat of vaporization is 40.6 kJ/mol. The resulting sample contains which of the following?A) water and water vaporB) ice and waterC) only waterD) only water vaporE) only ice
Q:
The enthalpy of fusion of sodium is 2.60 kJ/mol. How many grams of sodium can be melted by adding 81.7 kJ of energy to the metal at its melting point?
A) g
B) 9.24 g
C) 3.55 g
D) 31.4 g
E) g
Q:
Which of the following phase changes are endothermic?
A) vaporization
B) freezing
C) liquifaction
D) crystallization
E) condensation
Q:
In which of the following processes will energy be evolved as heat?
A) crystallization
B) melting
C) sublimation
D) vaporization
E) none of these
Q:
Which one of the following liquids would you expect to have the highest vapor pressure at room temperature? (all boiling points are normal boiling points)A) n-pentane, b.p. = 36.1ºCB) methanol, b.p. = 65.0ºCC) carbon tetrachloride, b.p. = 76.7ºCD) acetic acid, b.p. = 118ºCE) mercury, b.p. = 357ºC
Q:
The boiling point of a liquid is
A) always the temperature at which the vapor pressure equals 760 mmHg (1 atm).
B) always the temperature at which the liquid phase of a substance is in equilibrium with the vapor phase.
C) always the temperature at which the vapor pressure equals the pressure exerted on the liquid.
D) always equal to the vapor pressure of the liquid at a given temperature.
E) independent of the pressure exerted on the liquid.
Q:
Which of the following involves a change in temperature during the phase transition?
A) condensation of water
B) fusion of ethanol
C) vaporization of water
D) all of the above
E) none of the above