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Chem > Ch 10 Section 1 > Flashcards

Ch 10 Section 1 Flashcards

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1
Q

scientists developed the kinetic-molecular theory of matter to account for the

A

behavior of the atoms and molecules that make up matter

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2
Q

the kinetic-molecular theory is based on the idea that particles of matter are

A

always in motion

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3
Q

the kinetic-molecular theory can be used to explain the properties of solids, liquids, and gases in terms of the

A

energy of particles and the forces that act between them

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4
Q

the kinetic-molecular theory can help you understand the behavior of gas

A

molecules and the physical properties of gases

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5
Q

the theory provides a model of what is called an

A

ideal gas

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6
Q

an ideal gas is a hypothetical gas that perfectly fits all the assumptions of the

A

kinetic-molecular theory

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7
Q

(5 assumptions of the kinetic-molecular theory) gases consist of large numbers of tiny particles that are

A

far apart relative to their size

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8
Q

(5 assumptions of the kinetic-molecular theory) these particles, usually molecules or atoms, typically occupy a volume that is about 1000 times greater than the

A

volume occupied by an equal number of particles in the liquid or solid state

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9
Q

(5 assumptions of the kinetic-molecular theory) molecules of gases are much farther apart than molecules of

A

liquids or solids

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10
Q

(5 assumptions of the kinetic-molecular theory) most of the volume occupied by a gas is empty space, which is the reason that gases have a

A

lower density than liquids and solids do (explains that gases are easily compressed)

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11
Q

(5 assumptions of the kinetic-molecular theory) collisions between gas particles and between particles and container walls are

A

elastic collisions

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12
Q

(5 assumptions of the kinetic-molecular theory) an elastic collision is one in which there is no net loss of

A

total kinetic energy

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13
Q

(5 assumptions of the kinetic-molecular theory) kinetic energy is transferred between two particles during

A

collisions

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14
Q

(5 assumptions of the kinetic-molecular theory) however, the total kinetic energy of the two particles remains the same as long as

A

temperature is constant

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15
Q

(5 assumptions of the kinetic-molecular theory) gas particles are in continuous,

A

rapid, random motion

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16
Q

(5 assumptions of the kinetic-molecular theory) since gas particles are in continuous, rapid, random motion they possess

A

kinetic energy, which is energy of motion

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17
Q

(5 assumptions of the kinetic-molecular theory) gas particles move in all

A

directions

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18
Q

(5 assumptions of the kinetic-molecular theory) the kinetic energy of the gas particles overcomes the attractive forces between them, except near the

A

temperature at which the gas condenses and becomes a liquid

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19
Q

(5 assumptions of the kinetic-molecular theory) there are no forces of…..gas particles

A

attraction between

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20
Q

(5 assumptions of the kinetic-molecular theory) the temperature of a gas depends on the average

A

kinetic energy of the particles of the gas

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21
Q

(5 assumptions of the kinetic-molecular theory) the kinetic energy of any moving object, including a particle, is given by the following equation:

A

KE= 1/2 mv²

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22
Q

(5 assumptions of the kinetic-molecular theory) in the equation, m is the

A

mass of the particle and v is its speed

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23
Q

because all the particles of a specific gas have the same mass, their kinetic energies depend only on

A

their speeds

24
Q

the average speeds and kinetic energies of gas particles increase with an increase in …. and decrease with a decrease in….

A

temperature, temperature

25
Q

all gases at the same temperature have the same

A

average kinetic energy

26
Q

at the same temperature, lighter gas particles (like hydrogen molecules) have higher average speeds than do

A

heavier gas particles, such as oxygen molecules

27
Q

although ideal gases do not actually exist, many gases behave nearly ideally if pressure is not very

A

high and temperature is not very low

28
Q

gases do not have a definite

A

shape or a definite volume

29
Q

gases completely fill any container in which they are

A

enclosed, and they take its shape

30
Q

the fact that gases fill any container and take its shape is explained by the assumptions that gas particles move

A

rapidly in all directions without significant attraction between them

31
Q

because the attractive forces between gas particles are insignificant (assumption 4) gas particles glide easily

A

past one another

32
Q

this ability to flow causes gases to behave as

A

liquids do

33
Q

because liquids and gases flow, they are both referred to as

A

fluids

34
Q

the density of a gaseous substance at atmospheric pressure is about ….the density of the same substance in the…

A

1/1000; liquid or solid state

35
Q

the reason that the density of a gas is lower than in the other states is that the particles are so much farther apart in the

A

gaseous state (assumption 1)

36
Q

during compression, the gas particles, which are initially very far apart (assumption 1), are

A

crowded closer together

37
Q

the volume of a given sample of a gas can be greatly

A

decreased

38
Q

steel cylinders containing gases under pressure are widely

A

used in industry

39
Q

when they are full, such cylinders may contain more than 100 times as many particles of gas as

A

nonpressurized containers of the same size could contain

40
Q

gases spread out and mix with one another, even without being

A

stirred

41
Q

diffusion is the spontaneous mixing of the …. of two substances caused by their

A

particles; random motion

42
Q

gases diffuse readily into one another and mix together due to the rapid motion of the molecules and the

A

empty space between the molecules

43
Q

effusion is a process by which gas particles pass through a

A

tiny opening

44
Q

the rates of effusion of different gases are directly proportional to the

A

velocities of their particles

45
Q

because of this proportionality, molecules of low mass effuse…than molecules of high mass

A

faster

46
Q

because particles of gases occupy space and exert attractive forces on each other, all real gases deviate to some degree from

A

ideal gas behavior

47
Q

a real gas is a gas that does not behave completely, according to the

A

assumptions of the kinetic-molecular theory

48
Q

at very high pressures and low temperatures, the gas particles will be closer together and their kinetic energy will be insufficient to

A

overcome completely the attractive forces

49
Q

at such conditions, the gas is most likely to behave like a

A

non-ideal gas

50
Q

the kinetic-molecular theory is more likely to hold true for gases whose particles have little

A

attraction for each other

51
Q

the noble gases show essentially ideal gas behavior over a wide range of

A

temperatures and pressures

52
Q

the particles of noble gases are monatomic and thus

A

nonpolar

53
Q

the particles of gases, such as nitrogen and hydrogen, are nonpolar

A

diatomic molecules

54
Q

the behavior of these molecules (diatomic) most closely approximates that of the

A

ideal gas under certain conditions

55
Q

the more polar the molecules of a gas are, the greater the attractive forces between them and the more the gas will

A

deviate from ideal gas behavior

56
Q

highly polar gases deviate from ideal behavior to a larger degree than

A

nonpolar gases

Chem (54 decks)

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