Deck 11: What If There Were No Intermolecular Forces - the Ideal Gas

Question 1

If the pressure of a gas sample is quadrupled and the absolute temperature is doubled, by what factor does the volume of the sample change?

A) 2
B) 1/2
C) 1/4
D) 1/8

Answer 1

1/2

Question 2

380 mm Hg is equal to ________ atm.

A) 0.50
B) 2.0
C) 5.0
D) 20.0

Answer 2

0.50

Question 3

Assuming that the pressure and quantity of a gas sample remain constant, what will be the final volume of a 4.86 L sample of a gas at 281 °C when it is heated to 300 °C?

A) 5.03 L
B) 3.89 L
C) 2.92 L
D) 2.78 L

Answer 3

5.03 L

Question 4

For an ideal gas, which pairs of the variables below are inversely proportional to each assuming all other variables are kept constant?

A) P and n
B) V and T
C) V and P
D) V and n

Question 5

How many moles of gas are found in a container that occupies a volume of 5.50 L with a pressure of 0.335 atm at 25°C ?

A) 0.0753 moles
B) 0.898 moles
C) 13.3 moles
D) 1.11 moles

Question 6

Calculate the volume occupied by 18.0 g of water vapor at 100 °C and 1.00 atm.

A) 11.2 L
B) 22.4 L
C) 30.6 L
D) 61.2 L

Question 7

A fixed amount of a gas has both its temperature and volume doubled. What happens to its pressure?

A) It doubles.
B) It is halved.
C) It quadruples.
D) It remains the same.

Question 8

For an ideal gas, which pairs of the variables below are directly proportional to each assuming all other variables are kept constant?

A) P and n
B) n and T
C) V and P
D) all of the above

Question 9

1.86 moles of a gas occupy 245 L at 281 °C under a pressure of 0.346 atm. When the pressure is increased to 0.886 atm while keeping the same temperature, the new volume will be ________.

A) 627 L
B) 799 L
C) 95.7 L
D) 47.8 L

Question 10

A pressure of 76.0 cm Hg would be equivalent to what height of a water column? The density of mercury = 13.6 g/mL.

A) 5.59 cm
B) 55.9 cm
C) 0.18 cm
D) 1030 cm

Question 11

855 torr is equal to ________ cm Hg. 1 atm = 760 torr.

A) 1.13
B) 85.5
C) 855
D) 8550

Question 12

Pressure is defined as ________.

A) the amount of force per unit area
B) the amount of force per unit volume
C) the amount of work per unit area
D) the amount of work per unit volume

Question 13

The value of the gas constant R is equal to ________ L∙atm/ K∙mole.

A) 0.0821
B) 8.21
C) 82.1
D) 0.00821

Question 14

1 atm is equal to ________. 1 atm = 760 torr.

A) 760 cm Hg
B) 760 mm Hg
C) 76 torr
D) 76 mm Hg

Question 15

Imagine a balloon that you blow up to a full size. What do you expect to happen if you suspend the balloon over a bunsen burner? Assume that the pressure does not change significantly.

A) increase significantly in size until it bursts
B) decrease significantly in size
C) stay exactly the same size as before
D) One cannot say unless the composition of the gas is known.

Question 16

A gas under an initial pressure of 0.60 atm is compressed at constant temperature from 27 L to 3.0 L. The final pressure becomes ________.

A) 0.060 atm
B) 0.54 atm
C) 5.4 atm
D) 54 atm

Question 17

Imagine a balloon that you blow up to a full size. What do you expect to happen if you pour liquid nitrogen at 77 K over the surface of the balloon? Assume that the pressure does not change significantly.

A) increase slightly in size
B) decrease significantly in size
C) stay exactly the same size as before
D) One cannot say unless the composition of the gas is known.

Question 18

0.15 atm is equal to ________. 1 atm = 760 torr.

A) 11.4 torr
B) 114 torr
C) 1.14 × 10^-5 torr
D) 1.14 × 10^-3 torr

Question 19

Assuming that the pressure and quantity of a gas sample remain constant, what will be the final volume of a 4.86 L sample of a gas at 281 °C which is cooled to 225 °C?

A) 5.19 L
B) 4.37 L
C) 2.92 L
D) 2.78 L

Question 20

The number of moles of hydrogen gas present in a 1,500 mL container at 298 K and 2.0 atm pressure is ________.

A) 0.65 moles
B) 0.12 moles
C) 0.26 moles
D) 0.52 moles

Question 21

The volume of 2.3 g nitrogen gas at STP is ________.

A) 1.8 L
B) 11.2 L
C) 22.4 L
D) 44.8 L

Question 22

If the pressure of a given gas sample doubles, what happens to the volume of gas? The amount of gas and the temperature of the gas stay the same.

A) increase by a factor of 2
B) decrease by a factor of 2
C) stay exactly the same

Question 23

A 4.23 L sample of a gas is originally at 747 mm Hg at 297 K. The volume occupied by the same quantity of gas under the same temperature and 700. torr is ________. 1 atm = 760 torr.

A) 3.96 L
B) 4.51 L
C) 1.88 L
D) 1.68 L

Question 24

Which of the following gases will have the same density at STP?

A) oxygen and methane
B) hydrogen and helium
C) carbon monoxide and nitrogen
D) hydrogen chloride and fluorine

Question 25

A gas occupies a volume of 480 mL at 127 °C and 140 mm Hg. What mathematical expression will yield the correct volume at 177 °C and 400 mm Hg?

A) 480 × (140/400) × (450/400)
B) 480 × (400/140) × (450/400)
C) 480 × (140/400) × (400/450)
D) 480 × (400/140) × (400/450)

Question 26

A gas occupies 2.00 L at 298 K and 2.10 atm. The volume of this gas at STP is ________.

A) 22.4 L
B) 2.24 L
C) 3.84 L
D) 2.00 L

Question 27

If the volume of a given gas sample doubles, what happens to the temperature of the gas? The amount of gas and the pressure of the gas stay the same.

A) increase by a factor of 2
B) decrease by a factor of 2
C) stay exactly the same

Question 28

The density of carbon dioxide as STP is ________.

A) 0.46 g/ L
B) 1.97 g/ L
C) 3.94 g/ L
D) 5.62 g/ L

Question 29

A gas sample occupies a volume of 8 L at 20 °C. What is the temperature at which the gas would double its volume?

A) 40 °C
B) 10 °C
C) 273 K
D) 586 K

Question 30

0.249 g of a diatomic element occupies a volume of 125. mL at 120. °C and 2.00 atm. This element is ________.

A) nitrogen
B) oxygen
C) chlorine
D) bromine

Question 31

Which of the following gases occupy the smallest volume at STP?

A) 4.032 g H₂
B) 1.000 mol of carbon dioxide
C) 35.45 g CL₂
D) 6.022 × 10²³ molecules of O₂

Question 32

Which statement is true for an ideal gas?

A) The pressure of a gas increases when its volume decreases.
B) The pressure of a gas increases when its temperature increases.
C) The pressure of a gas increases when the number of gas moles increases.
D) All of the above statements are correct.

Question 33

0.024 moles of nitrogen gas occupy 4.0 L at 0.90 atm pressure. What will be the final volume if the container is allowed to expand and the pressure is reduced to 0.30 atm while the temperature is kept constant?

A) 1.33 L
B) 3.6 L
C) 6.0 L
D) 12 L

Question 34

What weight of nitrogen gas will occupy a volume of 1.25 L at a pressure of 1.0 atm and a temperature of 200.°C?

A) 0.45 g
B) 0.90 g
C) 1.80 g
D) 3.60 g

Question 35

Which of the following gases occupy the largest volume at STP?

A) 12.00 g He
B) 2 mol of water
C) 38.00 g F₂
D) 6.022 × 10²³ molecules of ammonia

Question 36

A gas occupies 340 mL at 273 K and 610 torr. What is the final temperature when the pressure is increased to 1 atm, and the volume being held constant? 1 atm = 760 torr.

A) 67 °C
B) 267 °C
C) 340 °C
D) 613 °C

Question 37

A gas occupies a volume of 0.500 L at 125 °C and 0.443 atm. What mathematical expression will yield the correct temperature at 0.750 L and 0.689 atm?

A) (0.689 × 0.750 × 125)/(0.443 × 0.500)
B) (0.443 × 0.500 × 398)/(0.689 × 0.750)
C) (0.443 × 0.500)/(0.689 × 0.750 × 398)
D) (0.689 × 0.750 × 398)/(0.443 × 0.500)

Question 38

The volume occupied by 4.00 g oxygen gas at STP is ________.

A) 22.4 L
B) 11.2 L
C) 5.60 L
D) 2.80 L

Question 39

Assume that the temperature and quantity of a gas sample remain constant. A 1.6 L sample of a gas is originally at 330 K and 4.84 atm. Calculate the final pressure when the volume is reduced to 840 mL.

A) 9.22 atm
B) 4.61 atm
C) 18.44 atm
D) 3.66 atm

Question 40

STP conditions stand for ________.

A) 0 K, 1 atm
B) 0 °C, 760 cm Hg
C) 0 °C, 760 mm Hg
D) 0 K, 76 cm Hg

Question 41

The atmospheric pressure increases as an airplane increases in altitude.

Question 42

Which statement is not true about an ideal gas?

A) Ideal gas molecules travel in a straight line.
B) Molecular collisions are elastic.
C) The intermolecular forces in gas molecules are very weak except when they collide.
D) Higher temperatures slow down the speed of the molecules.

Question 43

88.0 g of carbon dioxide gas will occupy ________ at STP.

A) 11.2 L
B) 22.4 L
C) 44.8 L
D) 67.2 L

Question 44

Which gas has a density equal to 1.43 g/L at STP?

A) nitrogen
B) oxygen
C) helium
D) carbon monoxide

Question 45

The molar volume of an ideal gas is ________.

A) always equal to 22.4 L at room temperature
B) proportional to the molecular weight of the gas
C) always equal to 22.4 L at STP
D) inversely proportional to the molecular weight of the gas

Question 46

Find the number of liters occupied by 3.0 g of nitrogen gas at STP.

A) 67 L
B) 7.5 L
C) 2.4 L
D) 0.13 L

Question 47

The density of hydrogen gas at STP is ________ the density of oxygen under identical conditions.

A) four times larger than
B) eight times larger than
C) sixteen times smaller than
D) equal to, since both densities are taken under the same conditions

Question 48

The number of moles of oxygen that are present in a 15-L container at STP is ________.

A) 0.1
B) 0.67
C) 0.89
D) 336

Question 49

At sea level, if a low pressure system comes through then the atmospheric pressure is below 760 mm Hg.

Question 50

0.123 g of a gas occupy a volume of 124 mL at 120. °C and 760. torr. The possible formula of the gas is ________.

A) CH₄
B) CO₂
C) CL₂
D) O₂

Question 51

An unknown gaseous substance has a density of 1.06 g/L at 31 °C and 371 torr. Its molecular weight is ________.

A) 27 g/mol
B) 54 g/mol
C) 81 g/mol
D) 108 g/mol

Question 52

An unknown gaseous substance has a density of 1.06 g/L at 31 °C and 371 torr. If the substance has the following percent composition: 88.8% C and 11.2% H, its molecular formula is ________.

A) CH₃
B) C₂H₃
C) C₄H₆
D) C₂H₅

Question 53

0.123 g of a gas occupy a volume of 124 mL at 120. °C and 760. torr. Its molar mass is ________ g/mol.

A) 22.4
B) 28.1
C) 71.1
D) 32.0

Question 54

The density of sulfur vapor at 1273 K and 740 mm Hg is 0.5977 g/L. Its molar mass is ________.

A) 32
B) 64
C) 96
D) 128

Question 55

The density of sulfur vapor at 1273 K and 740 mm Hg is 0.5977 g/L. Sulfur at that temperature will be ________.

A) monoatomic
B) diatomic
C) triatomic
D) tetraatomic

Question 56

The density of hydrogen gas at STP is ________.

A) 0.045 g/L
B) 0.090 g/L
C) 0.180 g/L
D) 0.360 g/mL

Question 57

3.01 × 10²³ molecules of methane gas will occupy ________ at STP.

A) 11.2 L
B) 22.4 L
C) 44.8 L
D) 67.2 L

Question 58

The density of carbon tetrachloride at 0.94 atm and 398 K is ________.

A) 1.11 g/L
B) 2.21 g/L
C) 4.43 g/L
D) 8.86 g/L

Question 59

14.0 g of nitrogen gas will occupy ________ at STP.

A) 1.12 L
B) 2.24 L
C) 11.2 L
D) 22.4 L

Question 60

Find the number of liters occupied by 3.0 moles of nitrogen gas at STP.

A) 67 L
B) 7.5 L
C) 4.8 L
D) 0.13 L

Question 61

The term elastic indicates that no kinetic energy is transferred during a collision.

Question 62

As temperature increases the volume of a gas increases, even if the pressure is not kept constant.

Question 63

30.19 inches of Hg is equal to 1.009 atm.

Question 64

The molar volume of any gas is equal to 22.4 L at any temperature.

Question 65

The pressure of 2.00 atm is equal to 152 cm Hg.

Question 66

1 torr is equal to 1 cm Hg. 1 atm = 760 torr.

Question 67

Ideal gas molecules undergo non-elastic collisions.

Question 68

The molar volume of any gas whether diatomic or monatomic is 22.4 L at STP.

Question 69

947 mbar is equal to 0.933 atm. 1 atm= 1.015 bar.

Question 70

One of the assumptions taken when dealing with ideal gas law is that most volume occupied by a gas is actually empty space.

Question 71

0.0309 atm is equal to 23.5 cm Hg.

Question 72

The pressure of 0.500 atm is equal to 0.500 mm Hg.

Question 73

124 cm Hg is equal to 1.63 atm.

Question 74

In the Ideal gas law, temperature is measured in K.

Question 75

As the volume of a gas is allowed to double, its pressure is halved as long as the temperature is kept constant.

Question 76

Increasing the temperature of a gas from 100 °C to 200 °C will cause the volume to double.

Question 77

The typical units for the density of gases are g/L.

Question 78

As the temperature of a gas increases, its pressure increases as long as the volume is kept constant.

Question 79

Increasing the temperature of a gas from 100 K to 200 K will cause the volume to double.

Question 80

76 cm Hg is equal to 1 atm.