Chemistry Test 4 Chapter 11

Front 1

Expand to completely fill their container.

Back 1

Property of Gases

Front 2

Take the shape of their container.

Back 2

Property of Gases

Front 3

Low density.
-Much less than solid or liquid state.

Back 3

Property of Gases

Front 4

Compressible.

Back 4

Property of Gases

Front 5

Mixtures of gases are always homogeneous.

Back 5

Property of Gases

Front 6

Fluid.

Back 6

Property of Gases

Front 7

Gases are composed of particles that are flying around very fast in their container(s).

Back 7

Structure of a Gas

Front 8

They move in straight lines until they encounter either the container wall or another particle, then they bounce off.

Back 8

Structure of a Gas

Front 9

If you were able to take a snapshot of the particles in a gas, you would find that there is a lot of empty space in there.

Back 9

Structure of a Gas

Front 10

The particles of the gas (either atoms or molecules) are constantly moving.

Back 10

Kinetic Molecular Theory

Front 11

The attraction between particles is negligible.

Back 11

Kinetic Molecular Theory

Front 12

When the moving particles hit another particle or the container, they do not stick, but they bounce off and continue moving in another direction.
-Like billiard balls.

Back 12

Kinetic Molecular Theory

Front 13

Pressure = Force/Area

Back 13

Gas Particles Pushing

Front 14

As they move and strike a surface, they exert a force on that surface.

Back 14

Gas Particles Pushing

Front 15

The effect of ___ ___ can cause some amazing and startling effects.

Back 15

The Effect of Gas Pressure

Front 16

Whenever there is a pressure difference, a gas will flow from area of high pressure to low pressure.
The bigger the difference in pressure, the stronger the flow of the gas.

Back 16

The Effect of Gas Pressure

Front 17

If there is something in the gas’ path, the gas will try to push it along as the gas flows.

Back 17

The Effect of Gas Pressure

Front 18

Soda Straws and Gas Pressure - Left Alone
The _______ of the air inside the straw is the same as the ________ of the air outside the straw—so
liquid levels are _____ _____ on both sides.

Back 18

pressure, pressure, the same

Front 19

Soda Straws and Gas Pressure - Sucking
The pressure of the air inside the straw is ______ than the ________ of the air outside the straw—so
liquid is pushed up the straw by the _______ ____.

Back 19

lower, pressure, outside air

Front 20

Gases have taken the shape and volume of their container(s) because the ___ don’t stick together, allowing them to move and fill the container(s) they’re in.

Back 20

particles

Front 21

In _______ and _______, the particles are attracted to each other strongly enough so they stick together.

Back 21

solids, liquids

Front 22

Gases are _______ and have low density because of the large amount of unoccupied space between the particles.

Back 22

compressible

Front 23

Gases are compressible and have ___ _______ because of the large amount of unoccupied space between the particles.

Back 23

low density

Front 24

Gases are compressible and have low density because of the large amount of unoccupied space between the _________.

Back 24

particles

Front 25

If all of the water in a 12-oz (350-mL) can of orange soda were _______ to gaseous steam (at 1 atm pressure and 100 oC), the steam would occupy a ______ equal to 1700 soda cans.

Back 25

converted, volume

Front 26

Because _____ molecules have enough _____ energy to overcome attractions, they keep moving around and spreading out until they fill the container.

Back 26

gas, kinetic

Front 27

Because the gas molecules have enough kinetic energy to overcome attractions, they keep moving around and spreading out until they fill the container. As a result, gases take the _____ and the _____ of the container they are in.

Back 27

shape, volume

Front 28

Because there is a lot of unoccupied space in the structure of a gas, the gas molecules can be ______ closer together.

Back 28

squeezed

Front 29

Because there is a lot of unoccupied space in the structure of a gas, gases do not have a lot of ____ in a given volume, the result is that they have ___ ______.

Back 29

mass, low density

Front 30

_______ is the result of the constant movement of the gas molecules and their collisions with the surfaces around them.

Back 30

Pressure

Front 31

The pressure of a gas depends on several factors:
______ of gas particles in a given volume.
_______ of the container.
Average speed of the gas particles: ________ !

Back 31

Number, Volume, Temperature

Front 32

In Measuring Air Pressure you use a _______.

Back 32

Barometer

Front 33

Measuring Air Pressure. Column of mercury supported by air pressure. As air pressure increases, mercury moves ______ the column.

Back 33

UP

Front 34

Measuring Air Pressure. Column of mercury supported by air pressure. As air pressure ________, mercury moves DOWN the column.

Back 34

decreases

Front 35

Measuring Air Pressure. Measure pressure by measuring _______ of column.

Back 35

height

Front 36

Average atmospheric pressure at sea level =

Back 36

760 mmHg

Front 37

_________ = 760 mmHg = 760 torr

Back 37

1 atm

Front 38

1 atm = 760 mmHg = ________

Back 38

760 torr

Front 39

1 atm = ___________ = 760 torr

Back 39

760 mmHg

Front 40

Pressure of a gas is inversely proportional to its volume.
--At constant T and amount of gas.
-- V down P up

Back 40

Boyle’s Law

Front 41

Boyle’s Law. Decreasing the volume forces the molecules into a smaller space.

Back 41

volume

Front 42

Boyle’s Law. Decreasing the volume forces the molecules into a smaller space. More molecules will collide with the container at any one instant, increasing the ________.

Back 42

pressure

Front 43

Gas Laws and Temperature
When doing gas problems, always convert your temperatures to ________.

Back 43

kelvins

Front 44

Gas Laws and Temperature
Gases ______ when heated and contract when cooled, so there is a relationship between ______ and temperature.

Back 44

expand, volume

Front 45

Gas Laws and Temperature
Gas molecules move ______ when heated, causing them to strike surfaces with more force, so there is a relationship between _______ and temperature.

Back 45

faster, pressure

Front 46

Gas Laws and Temperature
In order for the relationships to be _________, the temperature must be measured on an absolute (_____) scale.

Back 46

proportional, Kelvin

Front 47

___ = °C + 273

Back 47

K

Front 48

___ = 1.8 °C + 32

Back 48

°F

Front 49

Gas Laws and Temperature
When doing gas problems, always convert your ____________ to kelvins.

Back 49

temperatures

Front 50

°F = ___ + ____

Back 50

1.8 °C + 32

Front 51

K = ____ + ____

Back 51

°C + 273

Front 52

Volume and Temperature
In a rigid container, ______ the temperature increases the pressure.

Back 52

raising

Front 53

Volume and Temperature
For a cylinder with a piston, the pressure outside and inside stay _______.

Back 53

the same

Front 54

Volume and Temperature
To keep the pressure from rising, the piston moves out increasing the ______ of the cylinder.
--As volume increases, pressure decreases.

Back 54

volume

Front 55

As a gas is heated, it expands. This causes the density of the gas to _________.

Back 55

decrease

Front 56

Volume is directly proportional to temperature.
--At constant P and amount of gas.
--T UP V UP

Back 56

Charles’s Law

Front 57

As T increases, V also increases

Back 57

Charles’s Law

Front 58

V = constant x T.
-If T is measured in kelvin

Back 58

Charles’s Law

Front 59

Theoretical temperature at which a gas would have zero volume and no pressure.
--Kelvin calculated by extrapolation (you will do this in lab).

Back 59

Absolute Zero

Front 60

0 K = -273 °C

Back 60

Absolute Zero

Front 61

0 K =

Back 61

-273 °C

Front 62

-273 °C

Back 62

0 K

Front 63

Never attainable.
Though we’ve gotten real close!

Back 63

Absolute Zero

Front 64

All gas law problems use _______________

Back 64

the Kelvin temperature scale.

Front 65

Avogadro’s Law
--- V = _______ x n.
--- At _______ P and T.
--- More gas molecules = larger volume.

Back 65

constant

Front 66

shows the relationship between pressure and volume.
---At constant temperature.

Back 66

Boyle’s law

Front 67

shows the relationship between volume and absolute temperature.
---at constant pressure.

Back 67

Charles’ law

Front 68

Volume is directly proportional to the number of gas molecules.
--- V = constant x n.
--- At constant P and T.
--- More gas molecules = larger volume.

Back 68

Avogadro’s Law

Front 69

Boyle’s law and Charles’ law can be combined together.
---As long as the amount of gas stays constant.

Back 69

The Combined Gas Law

Front 70

Avogadro’s Law
Count number of gas molecules ________.

Back 70

by moles, n

Front 71

By combining the gas laws, we can write a general equation.

Back 71

Ideal Gas Law

Front 72

R is called the ___ ________.

Back 72

Gas Constant. (Ideal Gas Law)

Front 73

___ is called the Gas Constant.

Back 73

R (Ideal Gas Law)

Front 74

The value of R depends on the units of __ and ___.

Back 74

P, V (Ideal Gas Law)

Front 75

According to __________, the particles in a gas behave independently.

Back 75

Kinetic Molecular Theory (Mixtures of Gases)

Front 76

Air is a _______, yet we can treat it as a single gas

Back 76

mixture (Mixtures of Gases)

Front 77

Also, we can think of each gas in a mixture __________ of the other gases
---though all gases in the mixture have the same volume and ___________
>all gases completely occupy the container, so all gases in the mixture have the _________ of the container

Back 77

independent, temperature, volume(Mixtures of Gases)

Front 78

According to Kinetic Molecular Theory, the particles in a gas behave __________.

Back 78

independently (Mixtures of Gases)

Front 79

the pressure of a component gas in a mixture is called a

Back 79

Partial Pressure

Front 80

each gas in the mixture _____ a pressure independent of the other gases in the mixture

the pressure of an component gas in a mixture is called a partial pressure

Back 80

exerts

Front 81

the _____ of the partial pressures of all the gases in a ______ equals the total pressure

Back 81

sum, mixture

Front 82

the sum of the _______ of all the gases in a mixture equals the __________

Back 82

partial pressures, total pressure

Front 83

P(total) = P(gas) A + P(gas) B + P(gas) C +...

Back 83

Dalton’s Law of Partial Pressures

Front 84

to find the partial pressure of a gas, multiply the ________ of the mixture by the ____________ of the gas

Back 84

total pressure, fractional composition

Front 85

Common reference points for comparing gases.

Back 85

Standard Conditions, STP

Front 86

Standard pressure =

Back 86

1.00 atm

Front 87

1.00 atm =

Back 87

Standard pressure

Front 88

Standard temperature =

Back 88

0 °C (273 K)

Front 89

0 °C (273 K) =

Back 89

Standard temperature

Front 90

Standard Conditions are abbreviated as

Back 90

STP

Front 91

1 mole of any gas at STP will occupy 22.4 L.

Back 91

Molar Volume at STP

Front 92

1 ____ of any gas at STP will occupy 22.4 L.

Back 92

mole

Front 93

1 mole of any gas at STP will occupy _____.

Back 93

22.4 L.

Front 94

1 mole of any gas at STP will occupy 22.4 L.
This volume is called the _________and can be used as a conversion factor.
(As long as you work at STP).

Back 94

molar volume

Front 95

1 mol ///

Back 95

22.4 L

Front 96

PV = ____
Molar Volume at STP.

Back 96

nRT

Front 97

___ =nRT

Back 97

PV

Front 98

1 mole of ______ at STP will occupy 22.4 L.

Back 98

any gas

Front 99

Volume is directly proportional to the number of gas molecules.
V = constant x n.
At constant P and T.
More gas molecules = larger Volume is directly proportional to the number of gas molecules.
__ = constant x n.
At constant P and T.
More gas molecules = larger ______

Back 99

V, volume

Front 100

Volume is directly proportional to the number of gas molecules.
-V = constant x n.
-At constant P and T.
-More ______ = larger volume.

Back 100

gas molecules