Gas Laws/KMT/Gas properties

pressure types

1 atm= 101.3 kPa= 760 mmHg= 760 Torr

465 Torr —> ___ atm

0.612atm

1.26atm —> ____mmHg

958mmHg

2.79atm—> ___kPa

283 kPa

167 kPa—> ___mmHg

1253

Temp

must be in Kevin (273+C)

Standard temp and pressure (STP)

1.00 atm and 0C or 273K

Boyle’s law

deals with volume and pressure while temp is held constant

PV=PV

graph: gradual slope down

Charle’s law

deals with temp and volume while pressure if held constant

V/T=V/T

graph: middle slope up

Gay-Lussac’s law

deals with temp and pressure while volume is held constant

P/T=P/T

graph: faster slope up

Avogadro’s Law

deals with volume adn moles while temp/pressure is held constant

v/n=v/n

graph: up

combined gas law

combines all laws

temp=K

PV/T=PV/T

KMT (1)

Gases are made up of tiny particles that are spaced far apart from 1 another

KMT (2)

Gases move in a constant/ random motion

KMT (3)

Since gases are so far apart, it’s assumed that they don’t exert many attractive or repulsive forces on each other

KMT (4)

Collisions of gas particles with the container are perceived as “pressure”. Collisions between gas particles are elastic, which means no energy is lost/ transferred

KMT (5)

The 2 factors that determine the energy of a gas are mass and velocity. The amount of kinetic energy a gas has can be measured by the temperature in K.

Gas properties (1)

gases expand to fill their containers

Gas properties (2)

since there is a lot of space between gas particles, gases tend to have a low density

Gas properties (3)

the space between gas particles also allows gases to be easily compressed

Gas properties (4)

gases are fluid b/c they flow from 1 place to another, such as through a pipe

ideal gas laws

PV=nRT

p=atm

Dalton’s law of partial pressures

the total pressure of all gases in a container is equal to the sum of all partial pressures in the mixture

P(total)= p1 +p2 +p3 …