Test Review Chapters 10-12(Phases of Matter & Kinetic Theory)

The first page of the test will be matching. Any or all definitions given in the notes or book are fair game. Any of the questions or type of problems from the home work or book are also fair game for the test.

For sure you should be able to :1. Be able to list the three assumption of Kinetic Theory

1. Matter is composed of tiny particles.2. Particles of matter are in continual motion.3. Total kinetic energy of colliding particles remains constant.

2. Convert temperatures

3. Be able to explain kinetic theory and its relations with the phases

4. Be able to explain the Kinetic Theory of Pressure and the relationship between temperature, pressure, and volume. [W.S. 10-1]

5. Describe the nature of each phase of matter (solid, liquid, & gas)

6. Be able to work any type of problem concerning pressure, volume, and temperature. [W.S. 10-2, 10-3,10-4]

7. Know the Boiling point and freezing point of Water in all three temperature scales.

Freezing point 32o F 0o C 273 K

Boiling point 212o F 100oC372 K

8. Be familiar with STP:Standard temperature and pressure 273 K 760 mm or 1 atm

9. Relate kinetic theory to a real life.

9. Be able to answer any questions from the rest of this review.

Chapter 10

Multiple ChoiceIdentify the letter of the choice that best completes the statement or answers the question.

____ 1. According to the kinetic-molecular theory, particles of mattera. are in constant motion. c. have different colors.b. have different shapes. d. are always fluid.

____ 2. The kinetic-molecular theory explains the behavior ofa. gases only. c. liquids and gases.b. solids and liquids. d. solids, liquids, and gases.

____ 3. According to the kinetic-molecular theory, which substances are made of particles?a. ideal gases only c. all matterb. all gases d. all matter except solids

____ 4. Which is an example of gas diffusion?a. inflating a flat tireb. the odor of perfume spreading throughout a roomc. a cylinder of oxygen stored under high pressured. All of the above

____ 5. By which process do gases take the shape of their container?a. evaporation c. adhesionb. expansion d. diffusion

____ 6. If a gas with an odor is released in a room, it quickly can be detected across the room because ita. diffuses. c. is compressed.b. is dense. d. condenses.

____ 7. According to the kinetic-molecular theory, how does a gas expand?a. Its particles become larger.b. Collisions between particles become elastic.c. Its temperature rises.d. Its particles move greater distances.

____ 8. Which is an example of effusion?a. air slowly escaping from a pinhole in a tireb. the aroma of a cooling pie spreading across a roomc. helium dispersing into a room after a balloon popsd. oxygen and gasoline fumes mixing in an automobile carburetor

____ 9. What happens to the volume of a gas during compression?a. The volume increases.b. The volume decreases.c. The volume remains constant.d. It is impossible to tell because all gases are different.

____ 10. Pressure is the force per unita. volume. c. length.b. surface area. d. depth.

2

____ 11. What does the constant bombardment of gas molecules against the inside walls of a container produce?a. temperature c. pressureb. density d. diffusion

____ 12. Why does a can collapse when a vacuum pump removes air from the can?a. The inside and outside forces balance out and crush the can.b. The unbalanced outside force from atmospheric pressure crushes the

can.c. The atmosphere exerts pressure on the inside of the can and crushes it.d. The vacuum pump creates a force that crushes the can.

____ 13. Standard temperature is exactlya. 100ºC. c. 0ºC.b. 273ºC. d. 0 K.

____ 14. Standard pressure is the pressure exerted by a column of mercury exactlya. 273 mm high. c. 760 cm high.b. 760 mm high. d. 1.00 m high.

____ 15. Standard pressure is exactlya. 1 atm. c. 101.325 atm.b. 760 atm. d. 101 atm.

____ 16. If the temperature of a fixed quantity and volume of gas changes, what also changes?a. pressure c. massb. density d. formula

____ 17. To study the relationship between the temperature and volume of a gas, which factor must be held constant?a. elasticity c. kinetic energyb. fluidity d. pressure

____ 18. Why does the air pressure inside the tires of a car increase when the car is driven?a. Some of the air has leaked out.b. The air particles collide with the tire after the car is in motion.c. The air particles inside the tire increase their speed because their

temperature rises.d. The atmosphere compresses the tire.

____ 19. Pressure and volume changes at a constant temperature can be calculated usinga. Boyle's law. c. Kelvin's law.b. Charles's law. d. Dalton's law.

____ 20. Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?a. Charles c. Kelvinb. Boyle d. Dalton

Short Answer

21. Why are gases described as fluid?

22. What are standard temperature and pressure? Why was a standard needed?

3

Multiple ChoiceIdentify the letter of the choice that best completes the statement or question.____ 1. Compared with the particles in a gas, the particles in a liquid

a. have more energy. c. move around less.b. are larger. d. are farther apart.

____ 2. The compressibility of a liquid is generallya. less than that of a gas. c. equal to that of a gas.b. more than that of a gas. d. zero.

____ 3. The attractive forces in a liquid area. strong enough to prevent the particles from changing positions.b. too weak to hold the particles in fixed positions.c. more effective than those in a solid.d. too weak to limit the movements of the particles.

____ 4. The particles in a liquid are usuallya. closer together and lower in energy than those in a solid.b. farther apart and higher in energy than those in a gas.c. closer together and lower in energy than those in a gas.d. farther apart and lower in energy than those in a solid.

____ 5. Which term best describes the process by which particles escape from the surface of a nonboiling liquid and enter the gas state?a. vaporization c. surface tensionb. evaporation d. aeration

____ 6. What is the physical change of a liquid to a solid by the removal of heat?a. solidification c. freezingb. particle arrangement d. both a and c

____ 7. Particles within a solida. do not move. c. vibrate energetically.b. vibrate weakly about fixed

positions.d. exchange positions easily.

____ 8. Forces holding particles together are strongest in aa. solid. c. gas.b. liquid. d. vapor.

____ 9. The energy level of the particles in a solid isa. higher than the energy of the particles in a gas.b. high enough to allow the particles to interchange with other particles.c. higher than the energy of the particles in a liquid.d. lower than the energy of the particles in liquids and gases.

____ 10. Compared with the particles in a liquid, the particles in a solid usually area. higher in energy. c. more massive.b. closer together. d. more fluid.

____ 11. The compressibility of solids is generallya. lower than the compressibility of liquids and gases.b. higher than the compressibility of liquids.c. about equal to the compressibility of liquids.d. zero.

____ 12. Solids have a definite volume becausea. the particles do not have a tendency to change positions.b. the particles are far apart.c. they can be easily compressed.

4

d. the energy of the particles is high.____ 13. In general, most substances are

a. least dense in the liquid state. c. less dense as solids than as liquids.

b. more dense as gases than as solids.

d. most dense in the solid state.

____ 14. The rate of diffusion in solids is very low because thea. particles are not free to move

about.c. attractive forces are weak.

b. surfaces of solids usually contact gases.

d. melting points are high.

____ 15. Compared with gases, solids area. more easily compressed. c. lower in density.b. more likely to diffuse. d. incompressible.

____ 16. Which of the following properties do solids share with liquids?a. fluidity c. definite volumeb. definite shape d. slow rate of diffusion

____ 17. What causes the high density of solids?a. The particles are more massive than those in liquids.b. The intermolecular forces between particles are weak.c. The particles are packed closely together.d. The energy of the particles is very high.

____ 18. Compared with a crystalline solid, the particles in an amorphous solida. occur in a random pattern.b. occur in a definite, three-dimensional arrangement.c. consist of molecular sheets.d. have a more complex unit cell.

____ 19. As the atmospheric pressure on the surface of a liquid decreases, its boiling pointa. decreases. c. remains unchanged.b. increases. d. shows no correlation.

____ 20. Why are water molecules polar?a. They contain two kinds of atoms.b. The electrons in the covalent bonds spend more time closer to the

oxygen nucleus.c. The hydrogen bonds are weak.d. They have covalent bonds.

____ 21. What is the freezing point of water at standard pressure?a. –10ºC c. 4ºCb. 0ºC d. 32ºC

____ 22. Why doesn't water in lakes and ponds of temperate climates freeze solid during the winter and kill nearly all the living things it contains?a. Water is colorless.b. Ice floats.c. The molar heat of fusion of ice is relatively low.d. Water contracts as it freezes.

Short Answer

23. How are vaporization and evaporation related?

5

6