Deck 7: Gases

Question 1

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.

Answer 1

pressure.

Question 2

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.

Answer 2

The lungs expand, causing their internal pressure to decrease.

Question 3

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.

Answer 3

the gas particles strike the walls of the container more often.

Question 4

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 5

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

Question 6

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 constant temperature?

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

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 9

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 constant temperature?

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

Question 10

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 11

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.

Question 12

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 13

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

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

Question 14

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 15

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 16

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 17

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.

Question 18

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 19

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 20

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 21

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 22

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 23

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 24

A sample of argon 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 25

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

A) increase
B) decrease
C) remain constant

Question 26

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

A) T₂ T₁ V₁/P₂P₁
B) P₁V1T₂/P₂T1
C) P₁V1T1/P₂T₂
D) P₂T₂/P₂V1T₁
E) P₁V₁/T₁ - P₂/T₂

Question 27

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?

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

Question 28

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 29

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?

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

Question 30

A gas sample in a closed, expandable container of initial volume 5.00 L was allowed to warm from 25 °C to 35 °C. 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 31

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 32

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?

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

Question 33

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 34

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 35

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 36

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 37

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 38

At STP, how many moles of helium 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 39

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 in the container is kept constant?

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

Question 40

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?

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

Question 41

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 42

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 43

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 44

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 45

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 46

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 47

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 48

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 49

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 50

1 mole of a gas occupies 22.4 L at

A) 0 °C and 0.50 atm.
B) 0 °C and 760 mmHg.
C) 100 °C and 1 atm.
D) 100 °C and 10 atm.
E) 0 K and 1 atm.

Question 51

As the reaction of carbon with oxygen to produce carbon monoxide proceeds in a sealed container at a constant temperature of 600 K, the pressure in the container will __________. 2C(s) + O₂(g) → 2CO(g)

A) increase
B) decrease
C) remain constant
D) depend on whether a catalyst is present

Question 52

A diver exhales a bubble with a volume of 250 mL at a pressure of 2.4 atm and a temperature of 15 °C. How many gas particles are in this bubble?

A) 1.5 × 10²² gas particles
B) 0.25 gas particles
C) 6.02 × 10²³ gas particles
D) 490 gas particles
E) 2.9 × 10²⁶ gas particles

Question 53

The mathematical expression of the ideal gas law is

A) P₁V₁ = P₂V₂
B) $\frac { P _ { 1 } } { T _ { 1 } }$ = $\frac { P _ { 2 } } { T _ { 2 } }$
C) $\frac { P _ { 1 } } { V _ { 1 } }$ = $\frac { P _ { 2 } } { V _ { 2 } }$
D) PV = nRT
E) PT = P₁ + P₂ + P₃

Question 54

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 55

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 56

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

A) 2.21 × 10²⁵ atoms
B) 1.92 × 10²⁵ atoms
C) 3.88 × 10²⁴ atoms
D) 3.84 × 10²³ atoms
E) 9.45 × 10²³ atoms

Question 57

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 58

4Na(s) + O₂(g ) → 2Na₂O(s) How many L of O₂ gas at STP, are needed to react with 15.0 g of Na?

A) 3.65 L
B) 14.6 L
C) 7.30 L
D) 22.4 L
E) 32.0 L

Question 59

A 1.20-L container contains 1.10 g of an unknown gas at STP. What is the molecular weight of the unknown gas?

A) 1.32 g/mole
B) 0.917 g/mole
C) 22.4 g/mole
D) 20.5 g/mole
E) 1.10 g/mole

Question 60

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 61

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 62

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 63

The pressure exerted by a gas on its container is inversely related to its Kelvin temperature.

Question 64

The kinetic energy of a gas sample is directly proportional to the Kelvin temperature of the gas.

Question 65

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

Question 66

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 67

Oxygen makes up about __________ percent of the atmosphere.

Question 68

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 69

A barometer is usually filled with __________.

Question 70

One atmosphere is the same as __________ mmHg.

Question 71

According to Boyle's, when volume increases, pressure decreases.

Question 72

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

Question 73

Nitrogen makes up about __________ percent of the atmosphere.

Question 74

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 75

Gas law calculations normally require the use of the Kelvin temperature scale.

Question 76

The use of high-pressure chambers to control disease processes is known as __________.

Question 77

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) 165 mm Hg
B) 584 mm Hg
C) 600 mm Hg
D) 749 mm Hg
E) 760 mm Hg

Question 78

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 79

In the combined gas law, temperatures are given in °C.

Question 80

1 mmHg is the same as 760 atm.