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Chemistry > Ch 14: The Behavior of Gases > Flashcards

Ch 14: The Behavior of Gases Flashcards

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1
Q

What are three factors that determine the volume of a gas?

A

Temperature
Pressure
Amount of gas

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2
Q

Type of relationship: P ∝ 1/V

A

Inverse

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3
Q

Type of relationship: T ∝ V

A

Direct

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4
Q

Type of relationship: n ∝ V

A

Direct

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5
Q

Type of relationship: quantity A goes up, then quantity B goes up.

A

Direct relationship

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6
Q

Type of relationship: quantity A goes up, then quantity B goes down (and vice-versa).

A

Inverse relationship

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7
Q

How do we purify mixtures?

A

With a physical change (boiling, filter, magnet, diffusion, distillation, chromatography).

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8
Q

How do we break apart compounds?

A

With a chemical change (heat and properties change).

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9
Q

How do we break down elements (into other elements)?

A

With nuclear change (fission, fusion).

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10
Q

Kind of atoms they hold together: covalent bonds

A

Nonmetal atoms

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11
Q

Kind of atoms they hold together: ionic bonds

A

A nonmetal and a metal

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12
Q

Kind of atoms they hold together: metallic bonds

A

Metal atoms or positively charged ions

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13
Q

How/why do they hold atoms together: covalent bonds

A

Both holding on to electrons in the covalent bond.

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14
Q

How/why do they hold atoms together: ionic bonds

A

Attraction between opposite charges.

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15
Q

How/why do they hold atoms together: metallic bonds

A

Opposite charges between positive metal cation and negative anion electrons.

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16
Q

What is not shared evenly or uneven sharing classified as?

A

Polar

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17
Q

What is even sharing classified as?

A

Nonpolar

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18
Q

What are oppositely charged sides of neighboring polar molecules attract each other?

A

Dipole-dipole

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19
Q

What type of forces are dipole-dipoles?

A

Intermolecular forces; between molecule

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20
Q

What is an especially strong attraction between neighboring molecules that contain an O-H bond, or an N-H bond, or an H-F bond?

A

Hydrogen bonding

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21
Q

Because O, N, and F are very electronegative, what is left?

A

An unprotected proton.

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22
Q

What does salt do to Hydrogen bonds?

A

Enhances the effect.

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23
Q

What is an electron cloud of a negative molecule that shifts about randomly?

A

London dispersion forces (van der Waals forces)

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24
Q

When van der Waals forces shift about randomly, an non polar molecule becomes a temporary ______.

A

dipole

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25
Q

The London dispersion forces shift induces a neighboring molecule to shift its electrons and these charge interactions do what?

A

Hod the particles together.

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26
Q

Kind of atoms they hold together: dipole-dipole

A

Polar molecules

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27
Q

Kind of atoms they hold together: London dispersion forces (van der Waals)

A

Non-polar molecules

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28
Q

Kind of atoms they hold together: Hydrogen bonds

A

Molecules that contain O-H, N-H, H-F bond.

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29
Q

What is the strongest bond?

A

Covalent bond

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30
Q

What is the second-strongest bond?

A

Ionic bond

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31
Q

What is the third-strongest bond?

A

Metallic bond

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32
Q

What is the fourth-strongest bond?

A

Hydrogen bond

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33
Q

What is the fifth-strongest force?

A

Dipole-dipole forces

34
Q

What is the sixth-strongest force?

A

London dispersion forces

35
Q

Why are gases easily compressed?

A

Because of the space between the particles in a gas.

36
Q

What is pressure a measure of?

A

How concentrated a particular force is.

37
Q

________ = force/area

A

Pressure

38
Q

What is the tool used for measuring atmospheric pressure?

A

Barometer

39
Q

What is the tool for measuring the pressure of a contained gas?

A

Manometer

40
Q

What is an “ocean of air?”

A

Atmosphere

41
Q

What has mass and is bearing down us due to accelerations?

A

Atmosphere

42
Q

Why is there less atmospheric pressure at higher altitudes?

A

Because there is less air mass above.

43
Q

Standard pressure: atmospheres

A

1 atm

44
Q

Standard pressure: pascals

A

101,325 Pa

45
Q

Standard pressure: kilopascals

A

101.3 kPa

46
Q

Standard pressure: millimeters of Mercury

A

760 mm Hg

47
Q

Standard pressure: torr

A

760 torr Hg

48
Q

Standard pressure: pounds per square inch

A

14.7 psi

49
Q

Standard pressure: inches of Mercury

A

29.9 in

50
Q

What all affect gas pressure?

A

Amount of gas
volume
temperature

51
Q

Why does the pressure increase when more gas is added to a container without changing the volume of the container?

A

There are more collisions when more gas is added.

52
Q

What happens when more gas is added to a container without changing the volume of the container?

A

The pressure increases.

53
Q

When you increase the temperature of a gas, what does the pressure do?

A

The pressure increases.

54
Q

Why does the pressure increase when you increase the temperature of a gas?

A

The warm temperatures heat the particles and collisions happen more forcefully.

55
Q

If the temperature is constant, as the pressure of a gas increases, the volume _________.

A

decreases

56
Q

If the temperature is ________, as the pressure of a gas increases, the volume decreases.

A

constant

57
Q

How does the pressure relate to the volume, of a fixed amount of gas at a constant temperature?

A

Inversely

58
Q

What are the manipulated variables in Boyle’s law?

A

Pressure and volume.

59
Q

What are the constant variables in Boyle’s law?

A

Temperature and amount of gas.

60
Q

P1 X V1 = P2 X V2

A

Boyle’s law

61
Q

If the pressure is constant, what happens to the volume as the temperature of an enclosed gas increases?

A

The volume increases.

62
Q

What are the manipulated variables in Charles’s law?

A

Volume and temperature.

63
Q

What are the constant variables in Charles’s law?

A

Amount of gas and pressure.

64
Q

What is the variable relationship in Charles’s law?

A

Direct

65
Q

V1 / T1 = V2 / T2

A

Charles’s law

66
Q

According to Gay-Lussac’s law, as the temperature of an enclose gas increases, the pressure _________, is the volume is constant.

A

increases

67
Q

What are the manipulated variables in Gay-Lussac’s law?

A

Pressure and temperature.

68
Q

What are the constant variables in Gay-Lussac’s law?

A

Volume and amount of gas.

69
Q

What is the variable relationship in Gay-Lussac’s law?

A

Direct

70
Q

P1 / T1 = P2 / T2

A

Gay-Lussac’s law

71
Q

What type of calculations does the combined gas law allow you to do?

A

Calculations for situations in which only the amount of gas is constant.

72
Q

P1 X V1 / T1 = P2 X V2 / T2

A

Combined gas law

73
Q

What states at constant temperature and pressure, the volume of gas is directly related to the number of gas particles?

A

Avogadro’s law

74
Q

What are the manipulated variables in Avogadro’s law?

A

Volume and number of gas particles.

75
Q

What are the constant variables in Avogadro’s law?

A

Pressure and temperature.

76
Q

What is the variable relationship in Avogadro’s law?

A

Direct

77
Q

N1 / V1 = N2 / V2

A

Avogadro’s law

78
Q

What is required to calculate the number of moles of a contained gas?

A

An expression that contains the variable n.

79
Q

When do real gases differ most from an ideal gas?

A

At low temperatures and high pressures.

80
Q

In a mixture of gases, the total pressure is the ___ of the partial pressures of the gases.

A

Sum

81
Q

P = P1 + P2 + P3 + …

A

Total pressure is the sum of the partial pressures of the gases.

Chemistry (19 decks)

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