Name _

EVALUATION

,---". LIQUIDS

Date Class

CHAPTER 17

Write the letter of the term or phrase that completes the statement or answers the question.

___ 1. When the particles of a solid gain enough kinetic energy to break their ordered arrangement andslip past one another, the solid __ .a. vaporizes b. melts c. decomposes d. freezes

___ 2. The term used for the gaseous state of substances that are solids or liquids at room temperature is

a. plasma b. mist c. vapor d. fog

d. acetone

___ 3. A condition in which no net change occurs to the components of a system is called __ .a. equilibrium b. symmetry c. normal d. permanent

___ 4. The gaseous phase of a system is saturated with vapor when the rate of evaporation of the liquid

a. is less than the rate of condensationb. is greater than the rate of condensationc. is equal to the rate of condensationd. produces boiling throughout the liquid

___ 5. A certain liquid is in equilibrium with its vapor. If the volume of the vapor is doubled, which ofthe following will occur as equilibrium is again established?a. The concentration of the vapor molecules increases.b. The vapor pressure doubles.c. The vapor pressure is halved.

"'--./ d. The number of vapor particles increases.

___ 6. The vapor pressure of an unknown liquid is measured and found to be very high. Which of thefollowing is the best inference about this unknown?a. It is composed of molecules with asymmetrical polar covalent bonds.b. It has a high degree of hydrogen bonding.c. It is composed of molecules with nonpolar covalent bonds.d. It is composed of atoms with high electronegativity differences.

___ 7. The temperature at which the vapor pressure of a liquid is equal to standard atmospheric pres­sure is its __ .a. normal melting point c. triple pointb. normal boiling point d. critical temperature

8. Which of the following describes a change from the solid to the gaseous state without passingthrough the liquid state?a. liquefaction b. sublimation c. saturation d. aeration

9. Which of the following is an example of a nonvolatile liquid?a. glycerol b. alcohol c. ether

o 20 40 60 80 100

Temperature (OC)

__ 10. (ij'~ 1101.3 kPa

-; 100:; 80~ 60~ 40o 200.eo.>

What is the boiling point of CCl4 if the pressure on the sur­face of the liquid is 65 kPa?a. 100°Cb. 80°C

CHAPTER 17

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Users of Chemistry: A Modern Course have the publisher's permission to reproduce this page. 405

___ 11. The condensation of substances which are normally gases is called __ .a. sublimation b. freezing c. liquefaction d. fusion

___ 12. The temperature and pressure at which the solid, liquid, and gaseous phases of a substance arein equilibrium is the __ .a. critical temperature b. normal boiling point c. triple point d. melting point

___ 13. The point above which no amount of pressure will result in liquefying the gas is the __ .a. critical temperature b. critical pressure c. triple point d. equilibrium point

c. O°Cd. 31°C

__ 14.7390

-;;;Q.~ 518.0

'" ~ 101.3~ '"cl:

Temperature

What is the temperature for the triple point of carbon diox­ide?a. -78°Cb. -57°C

___ 15. From the phase diagram above what is the minimum pressure required for carbon dioxide to. exist as a liquid?a. 101 kPa b. 320 kPa c. 518 kPa d. 7400 kPa

___ 16. During condensation the particles of a substance undergo a __ .a. loss of potential energy c. loss of kinetic energyb. gain of potential energy d. gain of kinetic energy

___ 17. The energy required to change one gram of a solid to a liquid at its melting point is the __ .a. specific heat c. enthalpy of fusionb. heat of formation d. enthalpy of vaporization

___ 18. You have 200.0 cm3 of a soft drink at 25.0°C (treat the soft drink as though it were pure water). Ifyou want to cool the drink to O°C, how many grams of ice at O.O°C will be required?a. 14.9 g b. 25.0 g c. 62.6 g d. 200 g

___ 19. Hydrogen bondipg is stronger than other dipole attractions because __ .a. of unequal sharing of the electron pairb. of symmetrical sharing of the electron pairc. it is a polar bondd. of the high concentration of positive charge at hydrogen

___ 20. Hydrogen bonding causes all of the following to be higher than normal except the __ .a. melting point b. viscosity c. boiling point d. vapor pressure

___ 21. In a comparison of a series of substances, as the critical temperatures of the substances increase,the strength of the attractive forces among component particles __ .a. increases b. decreases c. remains the same d. varies at random

___ 22. Particles at the surface of a liquid may experience unbalanced forces of attraction. This idea isused to explain all of the following except __ .a. surface tension c. spherical shape of liquid dropsb. viscosity d. capillary rise

___ 23. The best conditions for the liquefaction of a gas are __ .a. high temperature and high pressure c. high temperature and low pressureb. low temperature and high pressure d. low temperature and low pressure

___ 24. In a comparison of a series of substances, as the attractive forces among component particlesincrease, the vapor pressure __ .a. increases b. decreases c. remains the same d. varies at random

___ 25. Which of the following would be used to predict the effect of a stress applied to a system inequilibrium? ~a. Boltzmann's distribution c. Le Chatelier's principleb. Faraday's law d. De Broglie's hypothesis

I

I

406Merrill Publishing Company, © 1990, 1987

Users of Chemistry: A Modern Course have the publisher's permission to reproduce this page.

CHAPTER 17

EVALUATION MASTER