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The Kinetic Theoryof Matter

Class Date

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DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that bestcompletes the statement.

1. An important idea in kinetic theory is that particles of matter (a) are in constant m'otion;(b) have different shapes; (c) have different colors; (d) are always fluid.

2. The kinetic theory can explain the behavior of (a) gases only; (b) solids and liquids; (c) liquidsand gases; (d) solids, liquids, and gases.

3. The kinetic theory explains the properties of solids, liquids, and gases in terms of the energypossessed by the particles and (a) gravitational forces; (b) the forces that act between theparticles; (c) diffusion; (d) the mass of the particles.

4. If two steel balls collide, they will bounce back at the same speed as the starting rate. This isan example of (a) Boyle's law; (b) the law of gravity; (c) elastic collision; (d) Boyle's law andCharles' law.

5. According to the kinetic theory, the most significant difference between gases and liquids is(a) the shapes of the particles; (b) the mass of each particle; (c) the distance between theparticles; (d) the fact that only the collisions in liquids are elastic.

6. An ideal gas is an imaginary gas that (a) is not made of particles; (b) conforms to all of theassumptions of the kinetic theory; (c) has particles of zero mass; (d) is made of motionlessparticles.

7. One difference between a real gas and an ideal gas is that in a real gas (a) all particles move inthe same direction; (b) the particles all have the same kinetic energy; (c) diffusion cannotoccur; (d) the particles exert attractive forces on each other.

8. The observation that gases can take the shape of any container is an example of (a) density;(b) expansion; (c) adhesion; (d) evaporation.

9. If a gas with an odor is released in a room, it soon can be detected across the room because(a) the gas can diffuse; (b) the gas is dense; (c) the gas is compressed; (d) the gas condenses.

10. The density of a substance undergoes the greatest change when (a) a liquid changes to a gas;(b) a liquid changes to a solid; (c) a solid changes to a liquid; (d) a gas cools but does notchange to a liquid.

11. According to the kinetic theory, a gas expands because (a) the particles become larger in size;(b) collisions between particles become elastic; (c) particles collide more often; (d) particlesmove farther apart.

12. The conditions under which real gases most resemble ideal gases are (a) low pressure and lowtemperature; (b) low pressure and high temperature; (c) high pressure and high temperature;(d) high pressure and low temperature.

13. The cases in which the kinetic theory does not hold true for gases can be explained by

(a) forces between molecules; (b) differences in the kinetic energies of the molecules; (c) largespaces between the molecules; (d) the small size of real molecules.

14. A gas at low temperature does not behave like an ideal gas because (a) there is too muchspace between the particles; (b) the attractive forces are too weak; (c) the kinetic energy of theparticles is too low; (d) the particles undergo chemical reactions.

15. Which of the following types of gases will behave most like an ideal gas? (a) gases made ofhighly polar molecules; (b) gases made of monatomic, nonpolar molecules; (c) gases made ofdiatomic, polar molecules; (d) gases near their condensation temperatures.

The Kinetic Theory of MatterHRW material copyrighted under notice appearing earlier in this work

Section 11.1 37

Name _

Qualitative Descriptionof Gases

Class Date· _

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DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that bestcompletes the statement.

1. The constant bombardment of the walls of a container by the moving molecules of a gasproduces the characteristic called (a) temperature; (b) density; (c) pressure; (d) diffusion.

2. To fully describe the condition of a gas, one must use all of the following except (a) volume;(b) pressure; (c) temperature; (d) chemical formula.

3. As the temperature of a gas increases, the particles of the gas (a) increase in speed;(b) increase in mass; (c) lose kinetic energy; (d) collide less frequently.

4. A 5-liter bottle of gas on a laboratory shelf (a) contains the same number of gas particles asall other 5-liter bottles of gas; (b) contains an unknown quantity of gas; (c) has more gas particles nearthe top than at the bottom; (d) is at absolute zero.

5. If you know the volume, pressure, and quantity of a gas, you can calculate its (a) yield;(b) formula; (c) temperature; (d) fluidity.

6. To study the relationship between the pressure and volume of a gas, a factor that must be heldconstant is the (a) density; (b) fluidity; (c) temperature; (d) collision rate.

7. If one holds a gas at a fixed pressure and quantity, one can investigate the effect oftemperature on the gas's (a) volume; (b) kinetic energy; (c) mass; (d) flammability.

8. If the quantity and volume of a gas remain unchanged, a change in pressure will cause achange in (a) density; (b) expansion; (c) weight; (d) temperature.

9. To study how a gas's pressure varies with the quantity of the gas, the factors that must be keptconstant are (a) mass and volume; (b) mass and temperature; (c) temperature and volume;(d) mass and weight.

10. If the pressure and temperature of a gas are held constant, one can observe the effect of achanging quantity of gas on the gas's (a) kinetic energy; (b) volume; (c) elasticity; (d) fluidity.

11. Suppose the temperature of the air in a balloon is raised. If the pressure remains constant,what quantity must change? (a) volume (b) number of molecules (c) compressibility (d) adhesion

12. After an automobile has been driven for several miles, the air pressure inside the tiresincreases. The best explanation for this is that (a) some of the air has leaked out; (b) the airparticles inside begin colliding with the tire; (c) the air particles inside the tire increase theirspeed; (d) the atmosphere compresses the tire.

13. The gas pressure inside a container decreases when (a) the number of gas molecules isincreased; (b) the number of gas molecules is decreased; (c) the temperature is increased;(d) the number of molecules is increased and the temperature is increased.

14. If both the temperature and volume of a gas remains constant, then (a) the pressure of the gaswill remain constant; (b) the pressure change cannot be predicted; (c) the pressure willincrease; (d) the pressure will decrease.

15. If the volume of a mole of gas remains constant and the pressure increases, it must be becauseof (a) a temperature decrease; (b) a kinetic energy decrease; (c) condensation of the gas;(d) a temperature increase.

38 Section 11.2 Qualitative Description of GasesHRW material copyrighted under notice appearing earlier in this work.

Name _

Quantitative Descriptionof Gases

Class Date

Sect!on 113ReVIew •

DIRECTIONS: Write on the line at the right of each statement the letter preceding the word or expression that best

completes the statement.

1. Standard temperature is exactly (a) 100°C; (b) 273°C; (c) O°C; (d) OK.

2.. Pressure is defined as the force per unit of (a) volume; (b) surface area; (c) length; (d) depth.

3. Pressure and volume changes at constant temperature can be calculated using the lawdeveloped by (a) Boyle; (b) Charles; (c) Kelvin; (d) Dalton.

4. Absolute zero is equal to (a) - 760°C; (b) - 273°F; (c) O.Ol°C; (d) - 273°C.

5. It is believed that absolute zero is the coldest possible temperature because at that

temperature (a) the volume of any gas should become zero; (b) the kinetic energy of themolecules is very large; (c) all gases diffuse; (d) the mass of the molecules becomes zero.

6. If a gas at ooe were warmed to 1°C and the pressure did not change, then the volume would(a) increase by 1/273; (b) decrease by 1/273; (c) become very large; (d) be impossible topredict.

7. Where V is the original volume, V' the new volume, T the original Kelvin temperature, and T'the new Kelvin temperature, Charles' law may be expressed mathematically as (a) V' = VT'IT;(b) V = V'T'IT; (c) V' = V - T'IT; (d) V' = VIT' + T.

8. A sample of gas at a constant volume experiences a drop in pressure of 75 mm Hg. The mostlikely explanation is that (a) the container exploded; (b) the temperature increased; (c) thetemperature decreased; (d) fewer particles are present.

9. If V,P, and T represent, respectively, the original volume, pressure, and temperature in thecorrect units, and V', P' , and T' represent the new conditions, the gas-law formula for thissituation is (a) PVIT' = P' V'IT; (b) PV'IT = P' VIT'; (c) P' VIT = PV' IT'; (d) PVIT =P'V'IT'.

10. The idea that the total pressure of a mixture of gases is the sum of their partial pressures iscredited to (a) Charles; (b) Boyle; (c) Kelvin; (d) Dalton.

11. To correct for the partial pressure of water vapor, the vapor pressure of H20 at the collecting

temperature is (a) divided by 22.4; (b) multiplied by 22.4; (c) subtracted from the gas pressure;(d) added to the gas pressure.

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DIRECTIONS: Write the answer to questions 12-15 on the line to the right, and show your work in the space

provided.

12. A 360-mL sample of hydrogen is collected when the pressure is 800 mm Hg. What isthe volume that the gas will occupy when the pressure is 720 mm Hg?

13. On a cold winter morning when the temperature is -13°C, the air pressure in anautomobile tire is 1.5 atm. If the volume does not change, what will be the pressure afterthe tire has warmed to 13°C?

14. A gas collected when the temperature is 11°C and the pressure is 710 mm Hg measures14.8 mL. Calculate the volume of the gas at 20.0°C and 740 mm Hg.

15. A sample of hydrogen with a volume of 800 mL exerts a pressure of 620 mm Hg at 5°C.Approximately what volume will it occupy at standard temperature and pressure?

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Quantitative Description of GasesHRW material copyrighted under notice appearing earlier in this work.

Section 11.3 39