Chapter 12: Gaseous State Of Matter

Front 1

Why does melting occur

Back 1

the molecules or ions have absorbed enough energy to break out the rigid structure of the solid

Front 2

Robert Boyle

Back 2

Formed a general theory called the kinetic molecular theory that explained the behavior and properties of gases.

Front 3

Kinetic Molecular Theory

Back 3

It is based on the motion of particles , particularly gas molecules.

Front 4

Ideal Gas

Back 4

a gas that behaves exactly as outlined in the KMT.

Front 5

When does real gases deviate greatly from ideal behavior?

Back 5

very high pressure and low temperatures

Front 6

What are the Principal assumptions of the kinetic molecular theory?

Back 6

1) gases consist of tiny particles
2) the distance between particles is large compared with the size of the particles themselves.The volume occupied by a gas consist mostly of empty space.
3) gas particles have no attraction for one another
4)gas particles move in straight lines in all directionss, colliding frequently with one another and with the walls of the container.
5) no energy is lost by the collision of a gas particle with another gas particle or with the walls of the container. All collisions are perfectly elastic.
6) the average kinetic energy for particles is the same for all gases at the same temperature, and its value is is directly proportional to the kelvin temperature.

Front 7

The kinetic energy (KE) of a particle is expressed by the equation?

Back 7

KE=.... 2
...½ mv

Front 8

In the KE formula the m stands for what?

Back 8

mass

Front 9

In the KE formula the v stands for what?

Back 9

velocity of the particle

Front 10

All gases have the same what at room temperature

Back 10

kinetic energy

Front 11

Diffusion

Back 11

the ability of two or more gases to mix spontaneously until they form a uniform mixture.

Front 12

Effusion

Back 12

process by which gas molecules pass through a very small opening from a container at higher pressure to one at lower pressure.

Front 13

Thomas Graham

Back 13

a scottish chemist.He observed that the rate of effusion was dependent on the density of a gas.

Front 14

Grahams law of effusion

Back 14

Graham found experimentally that the rate of effusion of a gas is inversely proportional to the square root of the mass of its particles.

Front 15

Pressure

Back 15

force per unit area

Front 16

Gases in the Atmosphere

Back 16

nitrogen=78%
oxygen=21%
Argon=0.93%
Carbon Dioxide=0.033%

Front 17

Atmospheric Pressure

Back 17

exerted by the gases in the atmosphere.

Front 18

the pressure exerted by a gas depends on what?

Back 18

1)number of molecules of gas present
2)temperature
3)volume in which the gas is confined

Front 19

what holds the atmosphere relativly close to the earth and prevents air molecules from flying off into space?

Back 19

gravitational forces

Front 20

the atmospheric pressure at any point is due to what?

Back 20

to the mass of the atmosphere pressing downward at that point

Front 21

barometer measures what

Back 21

the pressures of the gases in the atmosphere

Front 22

atmospheric pressure varies with what

Back 22

altitude

Front 23

when the temperature and mass are kept constant the pressure is directly proportional to what

Back 23

to the number of moles or molecules of gas present

Front 24

the pressure of a gas in a fixed volume varies with what

Back 24

temperature

Front 25

Boyles Law

Back 25

at a constant temperature, the volume of a fixed mass of a gas is inversely proportional to the pressure .

Front 26

when the pressure on a gas is increased, its volume will do what

Back 26

decrease

Front 27

when boyle doubled the pressure on a specific quantity of gas, keeping the temperature constant, what happened to the volume

Back 27

it was reduced to one half the original volume

Front 28

Charle's Law

Back 28

french physicist.he found that at constant pressure the volume of a fixed mass of any gas is directly proportional to the absolute temperature

Front 29

if the absolute temperature of a gas is doubled what else will double

Back 29

volume

Front 30

Gay Lussac's Law

Back 30

the pressure of a fixed mass of a gas, at constant volume is directly proportional to the kelvin temperature.

Front 31

What is STP used for

Back 31

to compare volumes of gases, common references points of temperature and pressure.

Front 32

when the temperature and pressure change at the same time, the new volume may be calculated how

Back 32

by multiplying the initial volume by the correct ratios of both pressure and temperature

Front 33

daltons law of partial pressures

Back 33

the total pressure of a mixure of gases is the sum of the partial pressures exerted by each of the gases in the mixures.

Front 34

partial pressures

Back 34

each gas in the mixure exerts a pressure that is independent of the other gases present

Front 35

gay lussacs law of combining volumes

Back 35

when measured at the same temperature and pressure the ratio of the volumes of reacting gases are small whole numbers

Front 36

avogadros law

Back 36

equal volumesof different gases at the same temperature and pressure contain the same number of molecules

Front 37

molar volume

Back 37

22.4 L

Front 38

what is the ideal gas law equation

Back 38

PV=nRT

Front 39

what is an allotrope

Back 39

different molecular forms of an element

Front 40

concentrations of ozone greater then 0.1 parts per million of air cause what

Back 40

coughing,choking,headache, fatigue and less resistance to respiratory problems

Front 41

concentrations between what of ozone are deadly to humans

Back 41

10 to 20 ppm