
5 properties of gasas
 Gases have an indefinite shape
 Gases can expand
 Gases can compress
 Gases have low densities
 Gases diffuse uniformly throughout their containers

All temp. calculations must be in?

The result of constantly moving molecules striking the inside wall of the container
Gas pressure

collide with wall less frequently and less energy, results in a lower pressure
molecules that move more slowly

collide more often, so the gas pressure increases
Molecules move more rapidly

Measured by an instrument called a barometer
Atmospheric pressure

Standard pressure of Atmosphere?
1 ATM

Standard pressure of millimeters of Hg?
760 mm Hg

Standard pressure of torr
760 torr (exactly)

Equal standard pressure?
1 ATM= 760 mHg= 760 torr

Volume and pressure are?
inversely proportional. as pressure goes up, volume goes down.

Boyle's law is written?
P1V1=P2V2

As pressure goes up, temp?
Goes up!

Charles Law is written?
V1/T1 = V2/T2

n (mol) and P (pressure): As one goes up, ?
so does the other

At constant pressure, the volume, V, occupied by a gas sample is directly proportional to ?

At constant vlume, the pressure, P, exerted by a gas sample is directly proportional to ?

3 gas laws can be combined to represent the relationship between the three variables when they all change simultaneously
The combined gas law

molecules of water in constant motion
some strike the surface with enough energy to escape the gas phase
when in a closed container, the vapor is collected in the space above the liquid
Vapor pressure

vapor pressure of water is dependent on?
 the temp but not the volume of water.
 increases as temp increases

Ptotal = P1+P2+P3+.......
 Daltons Law of partial pressures
 (587torr N + 158torr O + 7 torr Ar = 752 torr)

a gas that always behaves in a predictable and consistent manner
an Ideal gas

behave very much like the ideal gas model except at low T and high P
Real gases

Always use what Conversions for..
P (pressure)=
V (volume)=
N (mole)=
T (temp)=
 P= ATM
 V= Liter
 N= mol
 T= Kelvin

demonstrate rapid motion, move in straight lines, and travel in random directions
gas molecules

the average kinetic energy of gas particles is proportional to the ?
Kelvin temp

have no attraction for one another. After colliding they simply bounce away in a different direction
Gas molecules

An ideal gas at absolute zero has?
No kinetic energy and therefore no motion

in a collision between gas particles, there is no net loss of kinetic energy
elastic collisions

referred to as the Ideal Gas constant, R
.0821 L atm/mol K

PV = nRT
Ideal gas constant, R


