05 CTR ch14 7/12/04 8:13 AM Page 347 THE PROPERTIES OF ...hs.pequannock.org/ourpages/auto/2014/9/2/36294835/Chapter 14 Student Worksheets.pdf• Relate the total pressure of a mixture

Chapter 14 The Behavior of Gases 347

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THE PROPERTIES OF GASES14.1

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Section ReviewObjectives• Explain why gases are easier to compress than solids or liquids are

• Describe the three factors that affect gas pressure

Vocabulary

Part A CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.

Gases are easily , or squeezed into a smaller volume 1.

because of the between particles in a gas. The four variables 2.

used to describe a gas are pressure, (P), (V ), (T ), 3.

and number of (n). 4.

You can use theory to predict and explain how gases 5.

will respond to a change in conditions. Doubling the amount of 6.

gas in a rigid container the pressure. You can raise the 7.

pressure exerted by a contained gas by its volume. As the 8.

temperature of an enclosed gas decreases, the pressure . 9.

Part B True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 10. According to kinetic theory, the volume of the particles in a gas issmall compared to the total volume of the gas.

________ 11. Air will rush into a sealed container when the container is opened.

________ 12. Gas flows from a region of lower pressure to a region of higherpressure.

________ 13. Adding air to an object will cause the object to inflate.

________ 14. Four variables are used to describe a gas, P, V, T, and n, where n � number of moles.

9

8

7

6

5

43

2

1

• compressibility

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348 Core Teaching Resources

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Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.

Part C MatchingMatch each description in Column B to the correct term in Column A.

Part D Questions and ProblemsAnswer the following in the space provided.

20. Explain each assumption of the kinetic theory of gases in your own words.

Column B

a. used to compress a gas in a cylinder

b. the SI unit of pressure

c. result in pressure exerted by a gas

d. distance between particles in an enclosed gas atroom temperature

e. a measure of how much the volume of matterdecreases under pressure

Column A

________ 15. collisions of particles

________ 16. 10 times the diameter ofa particle

________ 17. compressibility

________ 18. piston

________ 19. kilopascals

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THE GAS LAWS14.2

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Section Review

Objectives• Describe the relationship among the temperature, volume, and pressure of a gas

• Use the combined gas law to solve problems

Vocabulary

Key Equations


The pressure and volume of a fixed mass of gas are 1.

related. If one decreases, the other . This relationship is 2.

known as law. The volume of a fixed of a gas is 3.

directly proportional to its temperature. This relationship 4.

is known as law. law states that the pressure of a 5.

gas is proportional to the Kelvin temperature if the 6.

volume remains constant. 7.

These three separate gas laws can be written as a single 8.

expression called the gas law. It can be used in situations 9.

in which only the of gas is constant. 10.10

9

8

76

5

43

2

1

• Boyle’s law: P1 � V1 � P2 � V2

• Charles’s law: �VT1

1� � �VT2

2�

• Gay-Lussac’s law: �PT1

1� � �PT2

2�

• combined gas law: �P1

T�

1

V1� � �P2

T�

2

V2�

• Boyle’s law

• Charles’s law

• Gay-Lussac’s law

• combined gas law

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________ 11. According to Charles’s law, T2 � .

________ 12. According to Boyle’s law, when the volume of a gas at constanttemperature increases, the pressure decreases.

________ 13. A balloon with a volume of 60 L at 100 kPa pressure will expand to avolume of 120 L at a pressure of 50 kPa.

________ 14. In an inverse relationship, the ratio of two variable quantities is constant.

________ 15. When using the combined gas law, pressure must always be inkilopascals but temperature can be in kelvins or degrees Celsius.

________ 16. When 20.0 L of O2 is warmed from �30.0�C to 85.0�C at constantpressure, the new volume is 29.5 L.



22. A rigid container holds a gas at a pressure of 55 kPa and a temperature of �100.0�C. What will the pressure be when the temperature is increased to 200.0�C?

23. What is the volume of a sample of CO2 at STP that has a volume of 75.0 mL at30.0�C and 91 kPa?

Column B

a. The volume of a fixed mass of gas is directly proportionalto its Kelvin temperature if the pressure is kept constant

b. �P1

T�

1

V1� � �P2

T�

2

V2�

c. For a fixed mass of gas at constant temperature, thevolume of gas varies inversely with pressure.

d. The pressure of a gas is directly proportional to theKelvin temperature if the volume remains constant.

e. �273.15�C

Column A

________ 17. Boyle’s law

________ 18. combined gas law

________ 19. absolute zero

________ 20. Charles’s law

________ 21. Gay-Lussac’s law

V1 � V2�T2

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IDEAL GASES14.3

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Section Review

Objectives• Compute the value of an unknown using the ideal gas law

• Compare and contrast real and ideal gases

Vocabulary• ideal gas constant (R)

• ideal gas law

Key Equation• Ideal gas law: P � V � n � R � T or PV � nRT


The ideal gas law permits you to solve for the of a 1.

contained gas when the pressure, volume, and temperature are 2.

known. The ideal gas law is described by the formula 3.

where the variable represents the number of moles of 4.

gas and the letter R is the . R is equal to . 5.

A gas that conforms to the gas laws at all conditions of 6.

temperature and pressure is an gas. No gas 7.

behaves ideally at all temperatures and pressures. Deviations 8.

from ideal behavior at high pressures can be explained by the 9.

intermolecular between particles in a gas and the actual

of the particles.9

8

76

54

3

2

1

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________ 10. The ideal gas law allows you to solve for the number of moles of acontained gas when pressure, volume, and temperature are known.

________ 11. The ratio (P � V)/(R � T) is equal to 1 for real gases.

________ 12. The behavior of a gas is most likely to approach ideal behavior at a highpressure and a low temperature.

________ 13. For an ideal gas, pressure and volume are directly proportional to eachother when all other factors remain constant.

________ 14. The number of moles of gas is directly proportional to the number ofparticles.



19. Calculate the number of moles of oxygen in a 12.5-L tank if the pressure is 25,325 kPa and the temperature is 22�C.

20. Calculate the mass of nitrogen dioxide present in a 275-mL container if thepressure is 240.0 kPa and the temperature is 28�C.

Column B

a. 8.31 �

b. a gas that follows the gas laws at all conditions ofpressure and temperature

c. a gas that can be liquefied by applying pressure

d. PV � nRT

Column A

________ 15. ideal gas law

________ 16. real gas

________ 17. ideal gas

________ 18. ideal gas constant (R)

LpkPa�Kpmol

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GASES: MIXTURES AND MOVEMENTS14.4

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Section Review

Objectives• Relate the total pressure of a mixture of gases to the partial

pressures of the component gases

• Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses

Vocabulary

Key Equations• Dalton’s law of partial pressures: Ptotal � P1 � P2 � P3 � . . .

• Graham’s law of effusion: � ��Part A CompletionUse this completion exercise to check your understanding of the concepts and termsthat are introduced in this section. Each blank can be completed with a term, shortphrase, or number.

According to Dalton’s law of partial pressures, at constant 1.

volume and temperature, the pressure exerted by a 2.

mixture of gases is equal to the of the partial pressures 3.

of the component gases. 4.

Molecules tend to move to areas of concentration 5.

until the concentration is . This process is called 6.

. During a gas escapes through a tiny 7.

in its container. 8.

The rate of effusion of a gas is proportional to the 9.

square root of the gas’s . This relationship is described 10.

by of effusion.10

9

8

765

4

3

2

1

molar massB��molar massA

RateA�RateB

• partial pressure

• Dalton’s law of partial pressures

• diffusion

• effusion

• Graham’s law of effusion

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________ 11. The fraction of the pressure exerted by a gas in a mixture does notchange as the temperature, pressure, or volume changes.

________ 12. The rate of diffusion of a gas is not influenced by its molar mass.

________ 13. Two objects with the same mass move at the same velocity.

________ 14. Diffusion is the tendency of molecules to move towards areas of lowerconcentration until the concentration is uniform throughout.



18. Explain, using kinetic theory, why molecules of low molar diffuse more rapidlythan molecules with a higher molar mass.

Column B

a. the pressure exerted by each gas in a gaseous mixture

b. the escape of a gas through a tiny hole in its container

c. The rate of effusion of a gas is inversely proportionalto the square root of its formula mass.

Column A

________ 15. partial pressure

________ 16. effusion

________ 17. Graham’s law of effusion

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THE BEHAVIOR OF GASES14

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Practice ProblemsIn your notebook, solve the following problems.

SECTION 14.1 THE PROPERTIES OF GASES1. Using kinetic theory, explain why a tire is more likely to blow out during a

trip in the summer than during one in the winter.

2. Use kinetic theory to explain why on a cold autumn morning a camper’s airmattress may appear to be somewhat flatter than when it was blown up theafternoon before. Assume no leaks.

SECTION 14.2 THE GAS LAWS1. The volume of a gas at 155.0 kPa changes from 22.0 L to 10.0 L. What is the

new pressure if the temperature remains constant?

2. Is it possible for a balloon with an initial pressure of 200.0 kPa to naturallyexpand to four times its initial volume when the temperature remainsconstant and atmospheric pressure is 101.3 kPa?

3. Exactly 10.0 L of O2 at �25�C is heated to 100.0�C. What is the new volume ifthe pressure is kept constant?

4. A gas at a pressure of 501 kPa and a temperature of 25�C occupies a volumeof 5.2 L. When the gas is heated to 100.0�C the volume increases to 7.00 L.What is the new pressure?

5. A sample of O2 with an initial temperature of 50.0�C and a volume of 105 L is cooled to �25�C. The new pressure is 105.4 kPa and the new volume is 55.0 L. What was the initial pressure of the sample?

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SECTION 14.3 IDEAL GASES1. A sample of argon gas is at a pressure of 1.24 � 104 kPa and a temperature of

24�C in a rigid 25-L tank. How many moles of argon does this tank contain?

2. A 35.0-L tank contains 7.00 mol of compressed air. If the pressure inside thetank is 500.0 kPa, what is the temperature of the compressed gas?

3. How many grams of helium does a 25.0-L balloon contain at 102.0 kPa and 24�C?

4. Calculate the volume that 2.25 mol of O2(g) will occupy at STP.

5. A sample of water vapor occupies a volume of 10.5 L at 200�C and 100.0 kPa.What volume will the water vapor occupy when it is cooled to 27�C if thepressure remains constant?

6. What is the volume occupied by 0.355 mole of nitrogen gas at STP?

7. What is the volume of a container that holds 25.0 g of carbon dioxide gas at STP?

SECTION 14.4 GAS MOLECULES: MIXTURES AND MOVEMENTS1. A gaseous mixture consisting of nitrogen, argon, and oxygen is in a 3.5-L vessel

at 25�C. Determine the number of moles of oxygen if the total pressure is 98.5kPa and the partial pressures of nitrogen and argon are 22.0 kPa and 50.0 kPa,respectively.

2. Compare the effusion rates of O2 (molar mass, 32.0 g/mol) and N2 (molar mass,28.0 g/mol).

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INTERPRETING GRAPHICSUse with Section 14.3

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Determination of the Molar Mass of a Volatile Liquid

You can use the ideal gas law to determine the molar mass of a liquid. Using the setupshown, a student added a small volume of an unknown liquid to a round-bottom flask,which can hold 267 mL of water. The flask was then submerged in a hot-water bath tocompletely vaporize all of the liquid. As the vapor forms, any excess vapor escapesthrough the top of the flask. Next, the flask was cooled to condense the vapor in the flask.Then the mass of the flask and condensed vapor was determined. Use the data in thetable to answer the following questions.

1. What is the mass of the condensed vapor?

a. Trial 1

b. Trial 2

Vapor

Boiling water

Trial 1 Trial 2

Mass of flask � stopper 83.32 g 83.39 g

Mass of flask � stopper � condensed vapor 83.73 g 83.82 g

Temperature of boiling water 99.0�C 99.0�C

Barometric Pressure 773.5 mm Hg 812.0 mm Hg

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2. What is the volume of the vapor in each trial?

3. What is the temperature of the vapor in kelvins?

a. Trial 1

b. Trial 2

4. What is the pressure of the vapor in kPa?

a. Trial 1

b. Trial 2

5. Calculate the number of moles of condensed vapor.

a. Trial 1

b. Trial 2

6. Calculate the molar mass of the volatile liquid.

a. Trial 1

b. Trial 2

7. Average the two molar masses.

8. If the unknown liquid is composed of carbon, hydrogen, and oxygen, write onepossible molecular formula for this substance.

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Vocabulary ReviewMatch the correct vocabulary term to each numbered statement. Write the letter of thecorrect term on the line.

Column B

a. combined gas law

b. ideal gas constant (R)

c. diffusion

d. compressibility

e. Boyle’s law

f. partial pressure

g. Dalton’s law of partialpressures

h. effusion

i. Charles’s law

j. Graham’s law of effusion

Column A

At constant volume and temperature, the totalpressure exerted by a mixture of gases is equal to thesum of the partial pressures of the component gases.

The volume of a fixed mass of gas is directlyproportional to its Kelvin temperature if thepressure is kept constant.

The rate of effusion of a gas is inversely proportionalto the square root of its molar mass.

the contribution each gas in a mixture makes to thetotal pressure of that mixture

a measure of how much the volume of matterdecreases under pressure

For a given mass of gas at constant temperature, thevolume of the gas varies inversely with pressure.

the tendency of molecules to move toward areas oflower concentration until the concentration isuniform throughout

�P1

T�

1

V1� � �P2

T�

2

V2�

the escape of a gas through a tiny hole in acontainer of gas

8.31 (LpkPa)/(Kpmol)

________ 1.

________ 2.

________ 3.

________ 4.

________ 5.

________ 6.

________ 7.

________ 8.

________ 9.

________ 10.

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© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.

Chapter QuizFill in the word(s) that will make each statement true.

1. Adding more gas to a closed container increases the number 1.of of particles with the walls of the container.

2. Doubling the number of particles of a gas in a container 2.the pressure, assuming that the temperature is constant.

3. According to kinetic theory, the particles of a gas have a 3.volume that is compared to the total volume of the gas.

4. One difference between real gases and ideal gases is that 4.gases may be liquefied when they are cooled and

pressure is applied to them.

5. The tendency of a gas to move toward areas of lower 5.concentrations until the concentration is uniform throughoutis .

Solve the following problems in the space provided.

6. A rigid container of O2 has a pressure of 388 kPa at a temperature of 713 K. 14.2What is the pressure at 273 K?

7. A flexible gas storage container has a volume of 3.5 � 105 m3 when the 14.2temperature is 27�C and the pressure is 115 kPa. What is the new volume of the container if the temperature drops to �10�C and the pressure drops to 99 kPa?

8. A mixture of gases at a total pressure of 145.0 kPa contains N2, CO2, and O2. 14.4The partial pressure of the N2 is 28.5 kPa, and the partial pressure of the CO2

is 76.0 kPa. What is the partial pressure of the O2?

5

14.4

4

14.3

3

14.1

14.12

1

14.1

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Chapter Test AA. MatchingMatch each description in Column B with the correct term in Column A. Write theletter of the correct description on the line.

B. Multiple ChoiceChoose the best answer and write its letter on the line.

________ 9. As the temperature of a fixed volume of gas increases, the pressure will a. vary inversely. c. be unchanged.b. decrease. d. increase.

________ 10. A breathing mixture used by deep-sea divers contains helium,oxygen, and carbon dioxide. What is the partial pressure of oxygenat 101.3 kPa total pressure if PHe � 84.0 kPa and PCO2

� 0.10 kPa?a. 10.3 kPa c. 34.4 kPab. 17.2 kPa d. 185.4 kPa

Column B

a. The volume of a fixed mass of gas is directly proportionalto the Kelvin temperature if the volume is kept constant.

b. At constant volume and temperature, the total pressureexerted by a mixture of gases is equal to the sum of thepartial pressures of the component gases.

c.

d. the contribution each gas in a mixture makes to the total pressure

e. A gas tends to move to an area of lower concentrationuntil the concentration is uniform throughout.

f. �P1

T�

1

V1� � �P2

T�

2

V2�

g. P � V � n � R � T

h. For a given mass of gas at constant temperature, thevolume of gas varies inversely with the pressure.

Column A

ideal gas constant (R)

Boyle’s law

Dalton’s law of partialpressures

ideal gas law

combined gas law

Charles’s law

diffusion

partial pressure

________ 1.

________ 2.

________ 3.

________ 4.

________ 5.

________ 6.

________ 7.

________ 8.

8.31 LpkPa�Kpmol

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________ 11. Increasing the volume of a given amount of gas at constanttemperature causes the pressure to decrease becausea. the molecules are striking a larger area with the same force.b. there are fewer molecules.c. the molecules are moving more slowly.d. there are more molecules.

________ 12. When a container is filled with 3.00 mol of H2, 2.00 mol of O2, and 1.00 mol of N2, the pressure in the container is 465 kPa. The partialpressure of O2 isa. 78 kPa. c. 155 kPa.b. 116 kPa. d. 212 kPa.

________ 13. A box with a volume of 22.4 L contains 1.0 mol of nitrogen and 2.0 molof hydrogen at 0�C. Which of the following statements is true?a. The total pressure in the box is 202.6 kPa.b. The partial pressure of N2 and H2 are equal.c. The total pressure is 101.3 kPa.d. The partial pressure of N2 is 101.3 kPa.

________ 14. The volume of a gas is doubled while the temperature is held constant.The pressure of the gasa. remains unchanged. c. is doubled.b. is reduced by one half. d. depends on the kind of gas.

________ 15. As the temperature of the gas in a balloon decreasesa. the volume increases.b. the pressure increases.c. the average kinetic energy of the gas particles decreases.d. All of the above are true.

________ 16. The volume of a gas is increased from 0.5 L to 4.0 L while thetemperature is held constant. The pressure of the gasa. increases by a factor of four. c. increases by a factor of eight.b. decreases by a factor of eight. d. increases by a factor of two.

________ 17. A gas occupies 40.0 mL at �123�C. What volume does it occupy at 27�C, assuming pressure is constant?a. 182 mL c. 80.0 mLb. 8.80 mL d. 20.0 mL

________ 18. A gas occupies a volume of 0.2 L at 25 kPa. What volume will the gasoccupy at 2.5 kPa?a. 4 L c. 2 Lb. 20 L d. 0.02 L

________ 19. Which of these changes would not cause an increase in the pressure ofa contained gas?a. Another gas is added to the container.b. Additional amounts of the same gas are added to the container.c. The temperature is increased.d. The gas is moved to a larger container.

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________ 20. If a balloon containing 1000 L of gas at 50�C and 101.3 kPa rises to an altitude where the pressure is 27.5 kPa and the temperature is 10�C, its volume there is

a. 1000 L � �12071.5.3

kkPPaa

� c. 1000 L � �12071.5.3

kkPPaa

� � �32

28

33

KK

�

b. 1000 L � �23

82

33

KK

� � �12071..53

kkPPaa

� d. 1000 L � �51

00

�

�

CC

� � �12071..53

kkPPaa

�

C. ProblemsSolve the following problems in the space provided. Show your work.

21. A gas has a pressure of 655 kPa at 227�C. What will its pressure be at 27�C if thevolume does not change?

22. A 10-g mass of krypton occupies 15.0 L at a pressure of 156 kPa. Find thevolume of the krypton when the pressure is increased to 215 kPa at the sametemperature.

23. A gas occupies a volume of 180 mL at 35.0�C and 95.9 kPa. What is the volume ofthe gas at conditions of STP?

24. A gas has a volume of 550 mL at a temperature of �55.0�C. What volume will thegas occupy at 30.0�C, assuming constant pressure?

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D. EssayWrite a short essay for the following.

25. What are some of the differences between a real gas and an ideal gas?

E. True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 26. Two small bicycle pumps are filled with different gases; one containsHe, the other Ar. Using the same pressure, it will take longer to forceout the He than the Ar.

________ 27. Theoretically, an ideal gas will contract in volume with increasingpressure and reduced temperature until absolute zero is reached.

________ 28. To obtain a value for the number of moles using the ideal gas law, oneuses the conditions of STP.

________ 29. The kinetic energy of a moving body is directly proportional to thesquare of its velocity.

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F. Additional ProblemsSolve the following problems in the space provided. Show your work.

30. The gaseous product of a reaction is collected in a 25.0-L container at 27�C. The pressure in the container is 216 kPa, and the gas has a mass of 96.0 g. Whatis the molar mass of the gas?

31. The separation of uranium-235 from uranium-238 has been carried out usinggaseous diffusion. Calculate the relative rates of diffusion of gaseous UF6

containing these isotopes.

Molar mass of UF6 containing uranium-235 � 349.0 amu.Molar mass of UF6 containing uranium-238 � 352.0 amu.

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© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.

Chapter Test B

A. MatchingMatch each term in Column B with the correct description in Column A. Write theletter of the correct term on the line.

B. Multiple ChoiceChoose the best answer and write its letter on the line.

________ 11. Reducing the volume of a contained gas by one third, while holdingtemperature constant, causes pressure toa. be decreased by two thirds.b. be increased by two thirds.c. be decreased by one third.d. be increased by one third.

Column B

a. combined gas law

b. ideal gas constant (R)

c. diffusion

d. compressibility

e. Boyle’s law

f. partial pressure

g. Dalton’s law of partialpressures

h. effusion

i. Charles’s law

j. Graham’s law of effusion

Column A

At constant volume and temperature, the totalpressure exerted by a mixture of gases is equal to thesum of the partial pressures of the component gases.

The volume of a fixed mass of gas is directlyproportional to its Kelvin temperature if the pressureis kept constant.

The rate of effusion of a gas is inversely proportionalto the square root of its molar mass.

the contribution each gas in a mixture makes to thetotal pressure of that mixture

a measure of how much the volume of matterdecreases under pressure

For a given mass of gas at constant temperature, thevolume of the gas varies inversely with pressure.

the tendency of particles to move toward areas oflower concentration until the concentration isuniform throughout

�P1

T�

1

V1� � �P2

T�

2

V2�

the escape of a gas through a tiny hole in a containerof gas

8.31 (LpkPa)/(Kpmol)

________ 1.

________ 2.

________ 3.

________ 4.

________ 5.

________ 6.

________ 7.

________ 8.

________ 9.

________ 10.

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________ 12. Which of the following would double the pressure on a contained gasat constant temperature?a. doubling the volume of the containerb. halving the number of particles in the containerc. doubling the number of particles in the containerd. none of the above

________ 13. A gas occupies a volume of 2.50 L at a pressure of 350.0 kPa. If thetemperature remains constant, what volume would the gas occupy at1750 kPa?a. 5.00 L c. 12.5 Lb. 0.500 L d. 1.40 � 102 L

________ 14. If the temperature of a gas in a closed container increasesa. the pressure of the gas decreases.b. the average kinetic energy of the molecules decreases.c. the molecules collide with the walls of the container less frequently.d. the pressure of the gas increases.

________ 15. Absolute zero isa. �273.15�C.b. the lowest possible temperature.c. the temperature at which the average kinetic energy of particles

would theoretically be zero.d. all of the above

________ 16. The graph of several pressure-volume readings on a contained gas atconstant temperature would bea. a straight line. c. a horizontal line.b. a curved line. d. a vertical line.

________ 17. At constant pressure, the volume of a fixed mass of gas and its Kelvintemperature are said to bea. directly related. c. unrelated.b. inversely related. d. constant.

________ 18. The temperature of 6.24 L of a gas is increased from 25.0�C to 55.0�C atconstant pressure. The new volume of the gas isa. 13.7 L. c. 6.87 L.b. 5.67 L. d. 2.84 L.

________ 19. A temperature of �25�C is equivalent to:a. 248 K. c. �25 K.b. 25 K. d. 298 K.

________ 20. A sample of chlorine gas has a pressure of 7.25 kPa at 20.0�C. What willits pressure be at 60.0�C if its volume remains constant?a. 2.42 kPa c. 21.8 kPab. 8.24 kPa d. 6.38 kPa

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________ 21. If a sample of oxygen occupies a volume of 2.15 L at a pressure of 58.0 kPa and a temperature of 25�C, what volume would this sampleoccupy at 101.3 kPa and 0�C?a. 1.35 L c. 4.10 Lb. 1.13 L d. 3.44 L

________ 22. The volume (in L) that would be occupied by 5.00 mol of O2 at STP isa. 0.411 L. c. 41.6 L.b. 22.4 L. d. 112 L.

________ 23. How many moles of H2 would be contained in 4.0 L of the gas at 202.6 kPa and 127�C?a. 89.6 mol c. 0.24 molb. 6.38 mol d. 0.77 mol

________ 24. A sample of H2 is collected over water such that the combinedhydrogen–water vapor sample is held at a pressure of 1 standardatmosphere. What is the partial pressure of the H2 if that of the watervapor is 2.5 kPa?a. 103.8 kPa c. 2.5 kPab. 98.8 kPa d. 101.3 kPa

_________25. What is the mass, in grams, of 0.125 L of CO2 at STP?a. 0.246 g c. 181 gb. 2.80 g d. 4.11 g

________ 26. Among the gases listed, which would have the fastest rate of effusion?a. NH3 c. SO2

b. CH4 d. NO2

C. ProblemsSolve the following problems in the space provided. Show your work.

27. A sample of hydrogen occupies a volume of 1.20 L at a pressure of 425 kPa. Ifthe temperature of the gas is kept constant, what would the new volume of thegas be at 615 kPa?

28. A sample of nitrogen occupies a volume of 0.650 L at 20.0�C. What volumewould the gas occupy at 40.0�C if the pressure remains constant?

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29. The temperature of a sample of helium at 85.0 kPa is 37�C. If the volume of thegas remains constant, at what temperature (in �C) would the pressure of the gasbe at 98.0 kPa?

30. If a sample of oxygen gas occupies a volume of 3.50 L at 57�C and 80.0 kPa, whatvolume would the gas occupy at STP?

31. How many grams of CO2 would be contained in 8.0 L at 152 kPa and 27�C?

D. EssayWrite a short essay for the following.

32. If all gases behaved as ideal gases under all conditions of temperature and pressure, no solid orliquid forms of these substances could exist. Explain.

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E. True-FalseClassify each of these statements as always true, AT; sometimes true, ST; or never true, NT.

________ 33. Doubling the number of particles of gas in an inflated tire doubles thepressure of the gas in the tire.

________ 34. Halving the Kelvin temperature of a gas in a rigid container decreases thegas pressure by one half.

________ 35. The graph of a relationship between variables that is directlyproportional is a straight line.

________ 36. At constant volume, if the Kelvin temperature of a gas is doubled, thepressure of the gas is halved.

F. Additional ProblemsSolve the following problems in the space provided. Show your work.

37. A sample of oxygen gas occupies a volume of 1.25 L at �23�C. If the pressureremains constant, what is the new Celsius temperature of the gas if its volumedecreases to 0.925 L?

38. How many moles of N2 would be contained in a 10.0-L balloon at 50.6 kPa and �73�C?

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05 CTR ch14 7/12/04 8:13 AM Page 347 THE PROPERTIES OF ...hs.pequannock.org/ourpages/auto/2014/9/2/36294835/Chapter 14 Student Worksheets.pdf• Relate the total pressure of a mixture