Deck 6: Gases

Question 1

The SI unit of pressure is atmosphereis defined as exactly 760 mmHg. (atm).

Answer 1

False

Question 2

Avogadro's law states that equal volumes of different gases at the same temperature and pressure contain the same amount of gas.

Answer 2

True

Question 3

Gay-Lussac's law relates volume of a gas with absolute temperature.

Answer 3

False

Question 4

When applying Charles's law, amount of gas and volume are considered to be constants.

Question 5

A sample of a gas has an initial volume of 15.0 L and an initial temperature of 235 K. The temperature of the gas increases to 313 K, if its volume increases to 20.0 L.

Question 6

P₁T₁ = P₂T₂, represents the Charles's law of gases.

Question 7

Real gases are ideal.

Question 8

One torr is an equivalent unit of one millimeter of mercury, the amount of pressure exerted by a column of mercury exactly 1 mm high.

Question 9

According to Gay-Lussac's law, at constant V and n.

Question 10

A 6.00 mol sample of O₂ has a pressure of 0.80 atm and a temperature of 68°C. Its volume is 41.8L.

Question 11

Robert Boyle invented the mercury barometer.

Question 12

The density of O₂ is 1.54 g/L at 30°C and 1.20 atm.

Question 13

If a 2.45 L volume of gas contains 4.5 × 10²¹ gas particles, a 4.9 L volume of gas will contain 4.5 × 10²² gas particles.

Question 14

An ideal gas is a gas that exactly follows the statements of the kinetic theory.

Question 15

Pressure and volume of a gas are inversely related, if other parameters are kept the same.

Question 16

Pascal (Pa) is equal to 1 N/m².

Question 17

A sample of a gas has an initial volume of 16.8 L and an initial temperature of 50°C. The volume of the gas increases to 33.6 L if its temperature is increased to 100° C.

Question 18

The equation, PV = nRT is called the ideal gas law, a gas law that relates all four independent physical properties of a gas under any conditions..

Question 19

According to the kinetic theory of gases, the size of a gas particle is large compared to the distances that separate them.

Question 20

The combined gas law considers the amount of gas as a variable.

Question 21

A gas has an initial pressure of 1.823 atm and an initial volume of 8.026 L. What is its new pressure if volume is changed to 6.323 L? Assume temperature and amount of gas are held constant.

A) 0.9342 atm
B) 1.436 atm
C) 3.105 atm
D) 2.314 atm
E) 27.84 atm

Question 22

What is the Kelvin equivalent of 145°C?

A) 752
B) 293
C) 418
D) 116
E) 292

Question 23

Which of the following laws states for a given amount of a gas, when pressure is constant?

A) Charles's law
B) Boyle's law
C) Avogadro's law
D) Graham's law
E) Gay-Lussac's law

Question 24

is a gas that deviates slightly from agreeing perfectly with the kinetic theory of gases. X is an example of _____ gas.

A) real
B) ideal
C) supreme
D) static
E) sturdy

Question 25

Pressure at a point deep in an ocean is estimated to be 1.074 × 10³ kPa. What is the average atmospheric pressure at that point?

A) 1.074 × 10^-1 atm
B) 1.060 × 10⁶ atm
C) 1.060 x 10¹ atm
D) 1.074 × 10^-4 atm
E) 1.074 × 10³ atm

Question 26

Boyle's law explains the relationship between _____.

A) pressure and temperature
B) volume and temperature
C) the amount of gas and temperature
D) pressure and the amount of gas
E) pressure and volume

Question 27

The vapor pressure of water increases with an increase in its temperature.

Question 28

Which of the following statements is true about the relationship between pressure and volume?

A) Pressure and volume are independent of each other.
B) Pressure and volume decrease with an increase in temperature.
C) Pressure increases as volume decreases.
D) Pressure and volume are not related to temperature.
E) Pressure increases as volume increases.

Question 29

Experiments show that the volume of a gas is related to its temperature in _____.

A) Celsius
B) Fahrenheit
C) Kelvin
D) Joule
E) Newton

Question 30

If mixture of H₂ at 5.00 atm and N₂ at 8.00 atm is stored in a container, the mixture's pressure will be 10.1 atm.

Question 31

A gas has an initial pressure of 1,080 torr and an initial volume of 586 mL. What is its new volume if pressure is changed to 1.30 atm? Assume temperature and amount of gas are held constant.

A) 370 mL
B) 486 L
C) 641 L
D) 487 L
E) 641 mL

Question 32

If a force of 1.50 x10³ N is pressed against an area of 3.00 m², what is the pressure in torr?

A) 3.75
B) 5.65
C) 500
D) 565
E) 3,800

Question 33

A gas that exactly follows the statements of the kinetic theory is called _____.

A) real gas
B) kinetic gas
C) dynamic gas
D) ideal gas
E) stationary gas

Question 34

How many atmospheres are there in 2,326 torr?

A) 2.370
B) 23.26
C) 11.63
D) 3.060
E) 1.160

Question 35

A sample of gas has an initial volume of 5.00 L and an initial temperature of 360. K. What is the new volume if the temperature is increased to 900. K? Assume constant pressure and amount for the gas.

A) 2.00 L
B) 3.00 L
C) 8.00 L
D) 12.5 L
E) 5.00 L

Question 36

Which of the following properties of gases must be held constant when applying Boyle's law?

A) Pressure
B) Amount of gas
C) Volume
D) Shape of the container
E) Size of the container

Question 37

Which of the following is the SI approved unit of pressure?

A) Pounds/inch
B) Millimeters of mercury
C) Atmosphere
D) N/cm²
E) Pascal

Question 38

_____ refers to the force of all the gas particle/wall collisions divided by the area of the wall.

A) Temperature
B) Pressure
C) HYPERLINK "http://en.wikipedia.org/wiki/Buoyancy" Buoyancy
D) Density
E) Concentration

Question 39

The mole fraction of He is 0.43 in a mixture containing He at 0.60 atm and Ne at 0.80 atm.

Question 40

Which of the following statements is consistent with the kinetic theory of gases?

A) Gases consist of tiny stationary particles of matter.
B) Gases constantly collide with each other.
C) The size of a gas particle is large when compared to the distances between them.
D) A net loss of energy occurs when particles collide.
E) Strong interactive forces exist between the particles of a gas.

Question 41

A sample of gas reduces its pressure and absolute temperature by 55 percent. What is the percentage change in volume?

A) 0
B) 20
C) 40
D) 50
E) 100

Question 42

Which of the following gas laws relates pressure with absolute temperature?

A) Avogadro's law
B) Graham's law
C) Charles's law
D) Boyle's law
E) Gay-Lussac's law

Question 43

A 1.6608 mol sample of O₂ has a pressure of 0.9561 atm and a temperature of 386 K. What is its volume?

A) 55.0 L
B) 59.0 L
C) 30.2 L
D) 50.6 L
E) 59.8 L

Question 44

Which of the following is considered the standard temperature under STP?

A) 0 K
B) 273 K
C) 160 K
D) 300 K
E) 313 K

Question 45

A sample of gas has an initial volume of 87.01 mL and an initial temperature of 295.5 K. What is the new temperature if the volume is decreased to 50.00 mL? Assume constant pressure and amount for the gas.

A) 169.8 K
B) 514.2 K
C) 158.6 K
D) 530.5 K
E) 14.72 K

Question 46

How many moles of H₂ are present in 69.2 L at STP?

A) 17.3 mol
B) 34.6 mol
C) 3.09 mol
D) 4.00 mol
E) 8.65 mol

Question 47

A sample of gas has a volume of 60. mL and an initial temperature of 380 K. The temperature must be changed to _____ in order to halve the volume. Assume constant pressure and amount for the gas.

A) 273 K
B) 76 K
C) 190 K
D) 760 K
E) 780 K

Question 48

A sample of gas at an initial volume of 65.0 mL, an initial pressure of 866 torr, and an initial temperature of 10.0°C simultaneously changes its temperature to 60.0°C and its volume to 46.0 mL. What is the final pressure of the gas?

A) 154 torr
B) 2,150 torr
C) 6,210 torr
D) 168 torr
E) 1,440 torr

Question 49

Which of the following equations represent the ideal gas law?

A) P₁V₁ = P₂V₂
B)
C)
D)
E) PV = nRT

Question 50

A 5.86 mol sample of Ne has a pressure of 263 torr and a temperature of 54.0°C. What is its volume?

A) 0.598 L
B) 455 L
C) 0.0988 L
D) 460 L
E) 58.6 L

Question 51

Which of the following laws consider amount of gas as a variable?

A) Charles's law
B) Avogadro's law
C) Combined gas law
D) Boyle's law
E) Gay-Lussac's law

Question 52

What is the molar volume of oxygen gas (O₂) at STP?

A) 44.8 L
B) 22.4 L
C) 103.04 L
D) 411.2 L
E) 716.8 L

Question 53

Which of the following statements is true about the ideal gas law?

A) Pressure is considered to be a constant when applying the ideal gas law.
B) The ideal gas law does not require a change in the conditions of a gas sample.
C) Volume is considered to be a constant when applying the ideal gas law.
D) According to ideal gas law, temperature is not an independent property of gases.
E) The ideal gas law is represented by the equation P₁V₁ = P₂V₂.

Question 54

What is the final temperature of a gas whose initial pressure is 455 torr, initial temperature is 105°C, and final pressure is 690 torr? Assume volume and amount of gas are held constant.

A) 300.°C
B) 69°C
C) 159°C
D) -23.7°C
E) 186°C

Question 55

What is the final pressure of a gas whose initial pressure is 590 torr, initial temperature is 308 K, and final temperature is 286 K? Assume volume and amount of gas are held constant.

A) 585 torr
B) 386 torr
C) 150 torr
D) 550 torr
E) 631 torr

Question 56

A gas has an initial volume of 65.08 mL and an initial temperature of 577°C. What is its new volume if temperature is changed to 417°C? Assume pressure and amount of gas are held constant.

A) 56.2 mL
B) 47.0 mL
C) 80.2 mL
D) 90.1 mL
E) 52.8 mL

Question 57

Which of the following is a constant when applying the combined gas law?

A) Pressure
B) Volume
C) Amount of gas
D) Temperature
E) Density

Question 58

For a 0.0962 mol sample of O₂, V = 58 L and T = 456 K. What is its pressure?

A) 0.61 atm
B) 0.021 atm
C) 0.21 atm
D) 0.047 atm
E) 0.062 atm

Question 59

A 3.8 mL volume of gas contains 5.6 × 10²² gas particles. How many gas particles are there in 15 mL if the gas is at the same pressure and temperature?

A) 3.8 × 10²²
B) 1.5 × 10²³
C) 2.2 × 10²³
D) 1.5 × 10²²
E) 5.4 × 10²²

Question 60

Which of the following laws proposes a relationship between pressure, temperature, and volume of a gas when the amount of gas is a constant?

A) Gay-Lussac's law
B) Boyle's law
C) Combined gas law
D) Charles's law
E) Avogadro's law

Question 61

What is Avogadro's law? Explain.

Question 62

What is pressure? How is it calculated?

Question 63

Explain the concept of ideal gas law.

Question 64

A container has a mixture of H₂ at 1.2 atm and O₂ at 1.6 atm. What is the mole fraction of H₂?

A) 0.55
B) 0.45
C) 0.57
D) 0.40
E) 0.43

Question 65

Which of the following statements is consistent with the Dalton's law of partial pressures?

A) The total pressure of a mixture of gases is less than the sum of the partial pressures of individual gases.
B) The total pressure of a gas mixture is equal to the sum of the partial pressures of the components.
C) The total pressure of a gas mixture is calculated by assessing the weighted average of the molecular pressures of the components.
D) The total pressure of a gas mixture is independent of the partial pressures of the components.
E) The total pressure of a mixture of gases is more than the sum of the partial pressures of individual gases.

Question 66

Briefly explain Dalton's law of partial pressures.

Question 67

What are the postulates of the kinetic theory of gases?

Question 68

What is molar volume? What is the molar volume of gases at STP

Question 69

Briefly explain Boyle's law.

Question 70

What is the combined gas law?

Question 71

Briefly describe Gay-Lussac's law. Highlight the difference between Gay-Lussac's and Charles's law.

Question 72

A mixture of helium at 1.600 atm and neon at 900.0 torr is in a container. What is the total pressure in the container?

A) 1,008 torr
B) 901.6 torr
C) 450.8 torr
D) 2,116 torr
E) 598 torr

Question 73

What are ideal gases? Can real world gases be called ideal gases?

Question 74

Briefly explain Charles's law.

Question 75

Explain the concept of standard temperature and pressure.

Question 76

Explain the significance and use of the ideal gas law.

Question 77

H₂ stored in a 50.0 L container has a pressure of 500.0 torr. O₂ stored in a 25.0 L container has a pressure of 800.0 torr. If both these gases are released together to be stored in a 100.0 L container, what is the total pressure in the 100.0 L container?

A) 800 torr
B) 500 torr
C) 450 torr
D) 650 torr
E) 1,300 torr

Question 78

CO₂ generated by the decomposition of ZnCO₃, is collected in a 5.6 L container over water. If the temperature is 40.0°C and the total pressure inside the container is 580 torr, how many moles of CO₂ were generated?

A) 0.09 mol
B) 0.74 mol
C) 0.18 mol
D) 0.15 mol
E) 0.86 mol

Question 79

What are the various units of pressure? Show how to convert one pressure unit into another using dimensional analysis.
The formal, SI-approved unit of pressure is the pascal (Pa), which is defined as 1 N/m². A common unit of pressure is the atmosphere (atm), which was originally defined as the average atmospheric pressure at sea level. A more reliable and common unit is millimeters of mercury (mmHg), which is the amount of pressure exerted by a column of mercury exactly 1 mm high. An equivalent unit is the torr, which equals 1 mmHg. 1.00 atm

Question 80

A mixture of H₂ at 566 torr and O₂ at 600 torr is in a container. What is the total pressure in the container?

A) 3,396 torr
B) 566 torr
C) 600 torr
D) 1,166 torr
E) 3,000 torr