Chemistry Gas And Pressure

Front 1

What are the four states of matter?

Back 1

Gas, solid, liquid, plasma

Front 2

Gases do: (3 things)

Back 2

exert pressure, have mass, can be compressed

Front 3

Kinetic molecular theory

Back 3

gases are small particles with mass and are relatively far apart, in constant rapid and random motion, collide in perfectly elastic conditions, don't exert attractive forces, and the average kinetic energy of a gas depends on the temperature

Front 4

elastic collision

Back 4

energy is the same before and after the collision

Front 5

temperature

Back 5

a measure of the kinetic energy of particles

Front 6

kinetic energy formula

Back 6

Kinetic Energy=1/2 mass (volume squared)

Front 7

diffusion

Back 7

movement of one material through another, the lighter the particle the more quickly it diffuses
-gases diffuse well

Front 8

effusion

Back 8

gas escaped through a tiny hole

Front 9

Graham's Law of Effusion and Difussion

Back 9

gas particles with smaller masses move more rapidly than those with larger particles

Front 10

Pressure

Back 10

force per area
units= torr, mm Hg, atm, Pascal, pounds per square inch

Front 11

barometer

Back 11

determines the atmospheric pressure, the changing Mercury pressure on the reservoir changes the Mercury level in the column. One standard atm is equal to the pressure that supports a column of 760 mm Hg at (0) sea level

Front 12

manometer

Back 12

measures gas pressure, the pressure of the open end is equal to the atmospheric pressure, the gas pressure is the pressure of the closed end, the difference in the Mercury height is the difference in pressure

Front 13

Dalton's Law of Partial Particles

Back 13

the sum of the partial pressures of each gas is equal to the total pressure of the gas mixture

Front 14

Absolute Zero

Back 14

temperature at which a gas wold have no volume or motion, 0 Kelvin and -273 Celsius

Front 15

Boyle's Law

Back 15

pressure and volume of a gas at constant temperature are inversely proportional to each other
P1(V1) = P2(V2)

Front 16

Inversely Proportional

Back 16

as one increases the other decreases

Front 17

(STP)Standard Temperature and Pressure

Back 17

0 degrees Celsius and 273 degrees Kelvin and 1 atm of pressure

Front 18

Charles' Law

Back 18

volume and temperature of a gas at a constant pressure are directly proportional to each other
V1/T1= V2/T2

Front 19

Gas Law Units

Back 19

temperature units must be converted to Kelvin from Celsius by adding 273 degrees and the pressure and volume units must be consistant throughout the problem

Front 20

Gay-Lussac

Back 20

pressure and temperature of a gas at a constant volume are directly proportional to each other
P2/T1= P2/T2

Front 21

Avogadro's Principle

Back 21

equal volumes of gases at the same temperature and pressure contain an equal number of particles

Front 22

Molar volume

Back 22

the volume of mole of gas
22.4 L/mole at STP

Front 23

direct proportion

Back 23

y=kx straight line graph with variables that change in the same direction

Front 24

inverse proportion

Back 24

y-k/x change inversely and the graph is a hyperbole curving downward to the right

Front 25

combined gas law

Back 25

combines Gay-Lussac, Charles' Law, and Boyle's Law; temperature must remain constant {P1(V1)}/T1= {P2(V2)}/T2

Front 26

Ideal gas law

Back 26

adding Avogadro's Principle to the combined gas law; equal volumes of a gas at a constant temperature and pressure have equal number of particles
PV= nRT
{P1(V1)}/{n1(T1)}= {P2(V2)}/{n2(T2)}

real gases behave like ideal gases except in really low temperatures where they have intermolecular attraction and really high pressure where the particle size is a factor

Front 27

Molar mass formula

Back 27

M=DRT/P

Front 28

Density formula

Back 28

d=PM/RT

Front 29

unknown variable formula

Back 29

n=mass/Molar mass

Front 30

The variable that stays the same when you are the combined gas law:

Back 30

temperature

Front 31

The equation for the combined gas law can be used instead of which equation?

Back 31

Boyle's Law

Front 32

relationship between temperature and volume

Back 32

direct

Front 33

relationship between temperature and pressure

Back 33

direct

Front 34

relationship between volume and pressure

Back 34

inverse

Front 35

Avogadro's Constant

Back 35

6.02 x 10 to the 23rd