Deck 8: Gases

Question 1

Which of the following is NOT part of the kinetic theory of gases?

A)A gas is composed of very small particles.
B)There is very little empty space in a gas.
C)Gas particles move rapidly.
D)Gas particles do not attract or repel one another.
E)Gas particles move faster when the temperature increases.

Answer 1

There is very little empty space in a gas.

Question 2

According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because

A)a gas is composed of very small particles.
B)the particles of a gas are very far apart.
C)gas particles move rapidly.
D)gas particles do not attract or repel one another.
E)gas particles move faster when the temperature increases.

Answer 2

the particles of a gas are very far apart.

Question 3

A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?

A)1.50 mmHg
B)507 mmHg
C)760 mmHg
D)1140 mmHg
E)7.5 mmHg

Answer 3

1140 mmHg

Question 4

In a gas, the distance between the particles is

A)very close relative to the size of the molecules.
B)close relative to the size of the molecules.
C)fixed relative to the size of the molecules.
D)small relative to the size of the molecules.
E)very large relative to the size of the molecules.

Question 5

Which of the following correctly describes the process of inspiration (air entering the lungs)?

A)The lungs expand, causing their internal pressure to decrease.
B)The lungs expand, causing their internal pressure to increase.
C)The lungs contract, causing their internal pressure to decrease.
D)The lungs contract, causing their internal pressure to increase.
E)There is no change in the internal pressure in the lungs.

Question 6

The volume of a gas with an initial pressure of 380 mmHg atm increases from 5.0 L to 8.0 L. What is the final pressure of the gas,in atm, assuming no change in moles or temperature?

A)238 atm
B)2.4 atm
C)0.31 atm
D)0.80 atm
E)8.0 atm

Question 7

At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 L to 3.00 L, with no change in moles or temperature. What was the new pressure exerted by the helium on its container?

A)800. torr
B)2280 torr
C)15.0 torr
D)3800 torr
E)1270 torr

Question 8

The air pressure on a rainy day is usually ________ air pressure on a sunny day.

A)higher than
B)lower than
C)the same as

Question 9

Which measurement describes the pressure of a gas?

A)315 K
B)1.2 g/L
C)2.5 L
D)725 mmHg
E)0.45 moles

Question 10

In the kinetic molecular theory of gas behavior, particles of a gas tend to move ________ and collisions between them are ________.

A)rapidly; rare
B)slowly; rare
C)rapidly; elastic
D)slowly; elastic
E)slowly; unusual

Question 11

A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in torr?

A)1.50 torr
B)507 torr
C)760 torr
D)1140 torr
E)7.5 torr

Question 12

The volume of a gas with a pressure of 1.2 atm increases from 1.0 L to 4.0 L. What is the final pressure of the gas, assuming no change in moles or temperature?

A)1.2 atm
B)0.30 atm
C)3.3 atm
D)4.8 atm
E)1.0 atm

Question 13

The force of gas particles against the walls of a container is called

A)pressure.
B)volume.
C)temperature.
D)quantity of gas.
E)density.

Question 14

The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming no change in moles or temperature?

A)4100 L
B)5.0 L
C)0.0060 L
D)5.4 L
E)4.6 L

Question 15

As you rise higher in Earth's atmosphere, the atmospheric pressure

A)increases.
B)decreases.
C)remains the same.

Question 16

According to the kinetic theory of gases, particles of a gas

A)are very large.
B)are very far apart.
C)lose their valence electrons.
D)move slowly.
E)decrease kinetic energy as temperature increases.

Question 17

According to Boyle's Law, the pressure of a gas increases as the volume decreases because

A)the gas particles get bigger.
B)the kinetic energy of the gas particles increases.
C)the temperature of the gas increases.
D)the gas particles strike the walls of the container with more force.
E)the gas particles strike the walls of the container more often.

Question 18

The atmospheric pressure in Denver, CO is 633 mmHg. What is this pressure in atm?

A)1.20 atm
B)633 atm
C)0.833 atm
D)1.00 atm
E)127 atm

Question 19

In the kinetic molecular theory of gas behavior, the assumption is made that gas molecules

A)move rapidly in random directions.
B)are attracted to each other by strong forces.
C)are close together in their container.
D)move with a kinetic energy equal to their centigrade temperature.
E)occasionally come to rest.

Question 20

The unit of 1 atmosphere used to describe the pressure of a gas is equal to

A)1 mmHg .
B)100 mmHg.
C)200 mmHg.
D)600 mmHg.
E)760 mmHg.

Question 21

What unit of temperature is used in gas law calculations?

A)degrees Fahrenheit
B)degrees Celsius
C)Kelvin
D)either degrees Celsius or degrees Fahrenheit
E)either degrees Celsius or Kelvin

Question 22

An autoclave is used to sterilize surgical equipment because

A)it allows water to boil at temperatures less than 100 °C.
B)it allows water to boil at 100 °C at pressures less than 1 atm.
C)it allows water to boil at 100 °C at pressures greater than 1 atm.
D)it allows water to boil at temperatures above 100 °C.
E)it provides very high temperatures and very low pressures.

Question 23

The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

A)210. mL
B)1170 mL
C)0.0095 mL
D)0.0470 mL
E)110. mL

Question 24

Vapor pressure can be described as

A)the temperature at which bubbles of vapor appear in a liquid.
B)the pressure exerted on the Earth by the particles in the air.
C)the temperature at which the vapor pressure of a liquid equals atmospheric pressure.
D)the pressure exerted by a gas above the surface of its liquid.
E)the pressure within the lungs during inhalation.

Question 25

When the combined gas law is rearranged to solve for V₂, the following is the correct expression: V₂ =

A)T₂T₁V₁/P₂P₁.
B)P₁V1T₂/P₂T₁.
C)P₁V1T₁/P₂T₂.
D)P₂T₂/P₁V1T₁.
E)P1V1/T1 - P₂/T2.

Question 26

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions.
The balloon is put into a chamber whose pressure is less than the atmospheric pressure and at atmospheric temperature.

A)A
B)B
C)C
D)A and B
E)B and C

Question 27

The boiling point of water at sea level is 100 °C. At higher altitudes, the boiling point of water will be

A)lower, because temperatures are lower.
B)lower, because the atmospheric pressure is lower.
C)higher, because the altitude is greater.
D)higher, because there are fewer water molecules in the air.
E)the same, because water always boils at 100 °C.

Question 28

A balloon is filled with helium gas. For the question(s) that follow, select the letter of the balloon diagram that corresponds to the given change in conditions.
The temperature is changed from 50 °C to -150 °C at constant pressure.

A)A
B)B
C)C
D)A and B
E)B and C

Question 29

In Gay-Lussac's Law, the pressure of a gas increases due to an increase in temperature because

A)the molecules strike the walls of the container less often.
B)the molecules strike the walls of the container more often.
C)the molecules get bigger.
D)there is a decrease in the volume of the container.
E)there is an increase in the number of gas particles.

Question 30

A sample of helium gas at 27.0 °C and 3.60 atm pressure is cooled in the same container to a temperature of -73.0 °C. What is the new pressure?

A)3.12 atm
B)2.40 atm
C)5.40 atm
D)2.38 atm
E)4.15 atm

Question 31

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C, at constant moles and pressure. What was its new volume?

A)4.84 L
B)5.17 L
C)7.00 L
D)3.57 L
E)4380 L

Question 32

A sample of argon gas at 300. °C and 50.0 atm pressure is cooled in the same container to a temperature of 0.00 °C. What is the new pressure?

A)105 atm
B)45.5 atm
C)54.9 atm
D)23.8 atm
E)42.7 atm

Question 33

As the temperature of a gas increases, the density of the gas will

A)increase.
B)decrease.
C)remain constant.

Question 34

The temperature of a 350. mL sample of gas increases from 27 °C . to 227 °C . What is the final volume of the sample of gas, if the pressure and moles in the container is kept constant?

A)583 mL
B)210. mL
C)2940 mL
D)41.6 mL
E)110. mL

Question 35

Complete the following statement: In Charles's Law, the volume of a gas ________ when the ________ decreases.

A)increases; temperature
B)increases; quantity of gas
C)increases; pressure
D)decreases; temperature
E)decreases; pressure

Question 36

At 570. mm Hg and 25 °C, a gas sample has a volume of 2270 mL. What is the final pressure (in mmHg) at a volume of 1250 mL and a temperature of 175 °C, if the moles are constant?

A)1560 mmHg
B)210. mmHg
C)700. mmHg
D)690. mmHg
E)470. mmHg

Question 37

The volume of a sample of gas, initially at 25 °C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant?

A)8.8 °C
B)71 °C
C)105 °C
D)-168 °C
E)576 °C

Question 38

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. What is the volume of the bubble when it reaches the surface where the pressure is 1.0 atm and the temperature is 27 °C, if the moles are constant?

A)580 mL
B)630 mL
C)100 mL
D)110 mL
E)1100 mL

Question 39

A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank then?

A)0.625 atm
B)4.44 atm
C)5.63 atm
D)40.0 atm
E)69.5 atm

Question 40

A gas contained in a steel tank has a pressure of 1.5 atm at a temperature of 320 K. What will be the gas pressure when the temperature changes to 450 K, at constant moles and volume?

A)1.5 atm
B)0.94 atm
C)0.47 atm
D)2.1 atm
E)1.1 atm

Question 41

At STP, what is the mass of 11.2 liters of O₂ gas?

A)16.0 g
B)32.0 g
C)64.0 g
D)128 g
E)8.00 g

Question 42

The mathematical expression of the ideal gas law is

A)P₁V₁ = P₂V₂.
B) =
C) =
D)PV = nRT.
E)PT = P₁ + P₂ + P₃.

Question 43

At STP, what is the volume of 1.00 mole of carbon dioxide?

A)1.00 L
B)44.0 L
C)273 L
D)22.4 L
E)12.2 L

Question 44

At STP conditions, 11 g of SO₂ has a volume of

A)250 L.
B)3.8 L.
C)22 L.
D)0.0076 L.
E)130 L.

Question 45

What volume would a 0.250 mole sample of H₂ gas occupy, if it had a which has a pressure of 1.70 atm, and a temperature of 35 °C?

A)0.269 L
B)0.423 L
C)1.25 L
D)3.72 L
E)283 L

Question 46

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr, if the moles are constant?

A)530 mL
B)450 mL
C)970 mL
D)240 mL
E)400 mL

Question 47

According to Avogadro's law

A)the volume of a gas is inversely related to the number of moles at constant temperature and pressure.
B)the volume of a gas is inversely related to the number of moles at standard temperature and pressure.
C)the volume of a gas depends only on the temperature and pressure.
D)the volume of a gas depends only on the number of moles in the sample.
E)the volume of a gas is directly related to the number of moles at constant temperature and pressure.

Question 48

A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 330 mmHg and the partial pressure of the oxygen is 1.0 atm, what is the total pressure of the mixture in torr?

A)330 torr
B)430 torr
C)760 torr
D)1.4 torr
E)1100 torr

Question 49

Zn(s) + 2HCl(aq) → H₂(g) + ZnCl₂(aq) When 25.0 g of Zn reacts, how many L of H₂ gas are formed at STP?

A)4.28 L
B)0.0171 L
C)8.56 L
D)22.4 L
E)0.382 L

Question 50

The pressure exerted by a gas on its container is directly proportional to

A)the volume of the container.
B)the mass of the individual gas molecules.
C)the centigrade temperature of the gas.
D)the number of moles of gas in the sample.
E)the Fahrenheit temperature of the gas.

Question 51

Zn(s) + 2 HCl(aq) → H2(g) + ZnCl₂(aq) When 25.0 g of Zn reacts, how many L of H₂ gas are formed at 25 °C and a pressure of 854 mmHg?

A)8.56 L
B)0.120 L
C)8.32 L
D)22.4 L
E)0.382 L

Question 52

What is the mass of neon that exerts a pressure of 720. mmHg,with a temperature of -15.0 °C , when the volume of the container is 760. mL?

A)0.0340 g
B)0.686 g
C)0.615 g
D)517 g
E)25.8 g

Question 53

What is the mass of a sample of O₂ gas, which has a pressure of 740.mmHg, at a temperature of 25 °C, in a volume of 250. mL?

A)0.318 g
B)3.82 g
C)201 g
D)292 g
E)320. g

Question 54

At STP, what is the volume of 4.50 moles of nitrogen gas?

A)167 L
B)3420 L
C)101 L
D)60.7 L
E)1230 L

Question 55

What is the pressure, in mmHg, of a 4.00 g sample of O₂ gas, which has a temperature of 30.0 °C, and a volume of 3000 mL?

A)0.788 mmHg
B)1.04 mmHg
C)78.0 mmHg
D)7880 mmHg
E)788 mmHg

Question 56

How many moles of neon occupy a volume of 14.3 L at STP?

A)36.7 moles
B)32.0 moles
C)6.45 moles
D)0.638 moles
E)1.57 moles

Question 57

At STP, temperature and pressure have the values of

A)0 K and 1 atm.
B)273 K and 1 mmHg.
C)273 K and 760 mmHg.
D)0 K and 760 mmHg.
E)760 K and 273 atm.

Question 58

Which of the following is NOT a potential use for a hyperbaric chamber?

A)treatment for burns and infections
B)counteracting carbon monoxide poisoning
C)increasing the rate at which a broken bone heals
D)treating a diver with the bends
E)treating some cancers

Question 59

The total pressure in a mixture of gases is equal to the partial pressure(s) of

A)the gas with the greatest number of moles.
B)the gas with the smallest number of moles.
C)the gas with the highest molecular weight.
D)the gas that occupies the largest volume.
E)all the gases added together.

Question 60

At STP, how many moles of helium gas would occupy 1.00 L?

A)2.24 moles
B)224 moles
C)22.4 moles
D)0.446 moles
E)0.0446 moles

Question 61

At STP, the molar volume of a gas is ________.

Question 62

Boyle's Law is usually written as ________.

Question 63

The pressure unit 1 mmHg is the same pressure unit as the pressure unit ________.

Question 64

Gay-Lussac's Law is usually written as ________.

Question 65

A gas sample contains 4.0 g of CH₄ and 2.0 g of He. What is the volume of the sample at STP?

A)130 L
B)11 L
C)17 L
D)30. L
E)5.6 L

Question 66

Which of the following correctly describes the partial pressures of gases in the body?

A)high O₂, low CO₂, oxygenated blood
B)high O₂, low CO₂, deoxygenated blood
C)high O₂, high CO₂, oxygenated blood
D)high O₂, high CO₂, tissue
E)low O₂, low CO₂, deoxygenated blood

Question 67

A barometer is usually filled with ________.

Question 68

The relationship P₁/T₁ = P₂/T₂ is called ________.

A)Boyle's Law
B)Charles's Law
C)Gay-Lussac's Law
D)The Combined Gas Law
E)Avogadro's Law

Question 69

The relationship V₁/n₁ = V₂/n₂ is called ________.

A)Boyle's Law
B)Charles's Law
C)Gay-Lussac's Law
D)The Combined Gas Law
E)Avogadro's Law

Question 70

A tank contains a mixture of helium, neon, and argon gases. If the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 215 mmHg and 102 mmHg, respectively, what is the partial pressure of neon?

A)0.228 mmHg
B)603 mmHg
C)377 mmHg
D)807 mmHg
E)173 mmHg

Question 71

If atmospheric pressure on a certain day is 749 mmHg, what is the partial pressure of nitrogen, given that nitrogen is about 78% of the atmosphere?

A)170 mmHg
B)580 mmHg
C)600 mmHg
D)750 mmHg
E)760 mmHg

Question 72

Nitrogen makes up about ________ percent of the atmosphere.

Question 73

Avogadro's Law is usually written as ________.

Question 74

Oxygen makes up about ________ percent of the atmosphere.

Question 75

A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?

A)2.1 atm
B)0.55 atm
C)1.0 × 10³ atm
D)1.5 atm
E)1600 atm

Question 76

One atmosphere is the same as ________ mmHg.

Question 77

In the kinetic molecular theory of gas behavior, the distance between gas molecules is assumed to be ________ the diameter of the gas molecules.

A)22.4 times
B)small relative to
C)dependent on
D)approximately the same as
E)large relative to

Question 78

The relationship P₁V₁ = P₂V₂ is called ________.

A)Boyle's Law
B)Charles's Law
C)Gay-Lussac's Law
D)The Combined Gas Law
E)Avogadro's Law

Question 79

A barometer is a device for measuring ________.

A)atmospheric pressure
B)blood pressure
C)gas pressure in a container
D)gas pressure in the lung
E)vapor pressure

Question 80

The pressure exerted by the particles of vapor above a liquid is called the ________.

A)vapor pressure
B)barometric pressure
C)standard pressure
D)molar pressure
E)atmospheric pressure