Chapter 9: Gases And Gas Laws

Front 1

Gases are one of...

Back 1

the four phases of matter

Front 2

what are the four phases of matter?

Back 2

solid
liquid
gas
plasma

Front 3

All gases are:

Back 3

homogeneous

Front 4

homogeneous:

Back 4

mixed uniformly(same throughout)

Front 5

compressible:

Back 5

apply pressure to their container, their volume will change

Front 6

pressure:

Back 6

the force exerted over a certain area by the gas against the walls of the container

Front 7

1atm= ____mmHg

Back 7

760mmHg

Front 8

1atm= 760mmHg= ____KPa

Back 8

101.325 KPa

Front 9

Ideal Gases are gases whose...

Back 9

behavior exactly matches these relationships or gas laws in reality, ideal gases don't exist

Front 10

Boyle's Law: at constant temperature the _____ of gas is ________ to pressure

Back 10

volume, inversely proportional

Front 11

equation for Boyle's Law

Back 11

V(proportional to) (1/P) or

P*V=constant

Front 12

Charle's Law: at constant pressure the _____ of gas varies _______________.

Back 12

volume, directly with temperature

Front 13

equation for Charle's Law

Back 13

V(proportional to)T

as T increases V increases

Front 14

Avogadro's Law: At fixed temperature and pressure the _____ of gas varies _________________.

Back 14

volume, directly with the molar quantity

Front 15

equation for Avogadro's law

Back 15

V (proportional to) n

as n increases, V increases

Front 16

Ideal Gas Law

Back 16

PV=nRT

Front 17

P=

Back 17

pressure

Front 18

V=

Back 18

volume

Front 19

n=

Back 19

number of moles

Front 20

R=

Back 20

gas constant (.08206)

Front 21

T=

Back 21

temperature

Front 22

Ideal gas law can be used to __________ if ___, ____, and ___ are known.

Back 22

calculate the # of moles(n), P, V, T

Front 23

Partial Pressure:

Back 23

the pressure of one individual gaseous component of gaseous mixture

Front 24

Dalton's Law of partial pressure

Back 24

the total pressure of a system is equal to the sum of the individual gas pressures.

Front 25

what is the pressure of each gas in our atmosphere?

Back 25

Ptotal= Patm= PN2 + PO2 + PAr + PCO2 + .....

78% N2 * 1.0 atm = .78 atm N2
21% O2 * 1.0 atm = .21 atm O2
----------------
sum=1atm

Front 26

if 2.00g of N2 gas has a volume of .40L and a pressure of 6.0 atm, what is its Kelvin temperature?

Back 26

PV/nR=T

6.0*.40/.0714*.08206 = 409K

Front 27

Used to express the __________ of gases in a _______(x)

Back 27

individual concentration, mixture

Front 28

X= mols of componentA/total mols of mixture(x)

Back 28

nA/nA+nB+nC...

Front 29

what would you get if you multiplied the mole fraction by 100?

Back 29

you would get the percent mol concentration

Front 30

Kinetic Molecular Theory of Gases

Back 30

a theory that explains why gases behave like they do

Front 31

1. Gases are made of _______moving at _______.

Back 31

tiny particles, random

Front 32

2. The volume of the ______ themselves is ______ in comparison to the total volume.

Back 32

particles, small

Front 33

3. Gas particles act ______ of each other.

Back 33

independently

Front 34

4. Collisions of the gas particles with _____ and the ____ of the _____ are ______.

Back 34

each other, walls, container, elastic

Front 35

5. The average Ek of the particles is ________ to ______ in ____.

Back 35

proportional, temp, K

Front 36

Kinetic energy

Back 36

KE=(1/2)mV^2

Front 37

Diffusion:

Back 37

the mixing of gas molecules by random motion

Front 38

Effusion:

Back 38

the escape of gas molecules through a pinhole into a vacuum

Front 39

Graham's Law:

Back 39

the rate of effusion is inverselly proportional to the square root in its mass.

Front 40

rate (proportional to) 1/ square root of mass

Back 40

Graham's Law

Front 41

Kinetic Molecular theory assumes small particle size

Back 41

for real gases at high pressure

Front 42

Kinetic Molecular theory assume no attractive forces between gas particles

Back 42

this is not true at high pressure

Front 43

Van der Waals Equation:

Back 43

[P+(an^2/V^2)]*(V-nb)=nRT