Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chemistry > unit 7 > Flashcards

unit 7 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

kinetic molecular theory (kmt)

A

describes the behavior of matter in terms of particles in potion, it makes assumptions about the size, motion, and energy of gas particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

kmt - particle size and attractive forces

A

small particles, little to no attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

kmt - particle motion

A

constant and random motion in a straight line

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

kinetic energy of a particle

A

1/2 mv^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

how does kmt explain gas expanding or contracting

A

when the volume of a container increases, particles fill that space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

diffusion

A

the movement of one material through another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

kmt diffusion

A

particles can easily flow because there is no attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

effusion

A

diffusion through a tiny opening

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

what effuses faster

A

lighter gasses effuse faster

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

grahams law of effusion

A

rate of effusion is inversely proportional to the square root of its molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

pressure

A

when particles collide with the walls of their containers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

used to measure atmospheric pressure

A

barometer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

used to measure pressure of a gas

A

manometer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ideal gas

A

a gas where its particles take up no space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

ideal gas properties

A

-no imf attraction forces
-not attracted to or repelled by the walls of the container
-constant random motion in straight lines
-perfectly elastic
-follows gas laws

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

when do real gasses act most like ideal gasses

A

at high temps and low pressures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what types of gas particles deviate most from ideal gas behavior

A

large gas particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

intramolecular forces

A

forces inside a molecule

19
Q

intermolecular forces

A

forces between molecules

20
Q

solid to liquid

A

melting, energy and distance up, imfs down

21
Q

liquid to solid

A

freezing, energy and distance down, imfs up

22
Q

liquid to gas

A

boiling / vaporation, energy and distance up, imfs down

23
Q

gas to liquid

A

condensation, energy and distance down, imfs up

24
Q

solid to gas

A

sublimation, energy and distance up, imfs down

25
Q

gas to solid

A

deposition, energy and distance down, imfs up

26
Q

volatile liquids

A

evaporate easy, low imfs - gasoline, perfume - high pressure

27
Q

non volatile liquids

A

do not evaporate easy, high imfs - water - strong imfs have a lower equilibrium vapor pressure because when imfs are strong its difficult for molecules to enter a gas phase, so there are fewer molecules of gas and less pressure

28
Q

relationship of imfs and pressure

A

imfs are strong so it is difficult for it to enter gas phase and so there are fewer molecules of gas which is a lower pressure

29
Q

boiling point and pressure

A

lower the atmospheric pressure, lower the boiling point

30
Q

critical point

A

the temperature above which gas cannot be liquified no matter the pressure

31
Q

triple point

A

condition where all three phases can be present

32
Q

boyles law

A

p and v are inversely proportional

33
Q

charles law

A

v and t are directly proportional

34
Q

gay-lussacs law

A

p and t are directly proportional

35
Q

equilibrium

A

a dynamic condition in which opposing changes are occurring at the same rate in a closed system

36
Q

equilibrium vapor pressure of a liquid

A

the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature,,, pressure of a gas above its liquid

37
Q

increase in temperature ___ equilibrium pressure,, why?

A

increases, because increasing temp increases KE and so more molecules change from liquid to gas, so there are more molecules which means more pressure

38
Q

boiling or evaporation

A

boiling happens within the liquid while evaporation is just at the surface

39
Q

boiling point

A

the temperature where the equilibrium vapor pressure equals the surrounding atmospheric pressure

40
Q

what happens to temp when a liquid boils

A

it stays constant

41
Q

volatile is __ vapor pressure

A

high vapor pressure == volatile

42
Q

why does increasing atmospheric pressure increase boiling point

A

more energy is required to boil

43
Q

how can gas pressure be increased

A

decrease volume, increase temperature, increase amt of gas

chemistry (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions