Chemistry- gas laws

force per area, p=f/a

Mass/ size of particles

# of particles

kPA, Atm, torr, mmHg

760 torr= 760 mmHG= 1 atm= 101.325 kPa

when pressure is constant, volume and temp are directly related

when one goes up/down so does the other

V1/T1= V2/T2

when temp is constant pressure and volume are inversely related ( when one goes up the other goes down)

P1•V1=P2•V2

when V is constant pressure and Temp are directly related

P1/t1=p2/t2

volumes of gas at same temp/pressure have = # of particles

V1/n1=V2/n2 ( directly realated)

KELVIN!

C°+ 273= K

F°= 1.8 C° +32

C°= F°-32/1.8

Partial=pressure if each gas in a mixture

ptotal= p1+p2+p3…

p1 v1/T1= p2 v2/T1

an imaginary gas that perfectly fits all assumptions of kinetic molecular theory

PV=nRT

• Gas particles in constant rapid motion

• The temperature depends on kinetic energy

temp- 0 C° or 293.15 K

Pressure- 1 Atm

take up space have attraction

does not fit with kinetic theory

change more at high pressure and low temp

closest gas

at high temps and low pressures

there is no attractive or repulsive forces

no energy is lost in collisions

The mercury sits in a circular, shallow dish surrounding the tube. The mercury in the tube will adjust itself to match the atmospheric pressure above the dish. As the pressure increases, it forces the mercury up the tube.