Studied by 15 people
gas law formulas, and their scientists
pressure
force per area, p=f/a
Things that do affect pressure…
Mass/ size of particles
things that do not affect pressure…
# of particles
Units of pressure
kPA, Atm, torr, mmHg
conversion factors for pressure
760 torr= 760 mmHG= 1 atm= 101.325 kPa
Charles law
when pressure is constant, volume and temp are directly related
when one goes up/down so does the other
Charles law formula
V1/T1= V2/T2
Boyle’s law
when temp is constant pressure and volume are inversely related ( when one goes up the other goes down)
Boyles formula
P1•V1=P2•V2
Gay-Lussacs law
when V is constant pressure and Temp are directly related
Gay-Lussacs law formula
P1/t1=p2/t2
avagadros law
volumes of gas at same temp/pressure have = # of particles
Avagadros formula
V1/n1=V2/n2 ( directly realated)
what does the temperature always have to be in?
KELVIN!
How to convert Celcius to kelvin
C°+ 273= K
celsius to fahrenheit
F°= 1.8 C° +32
Fahrenheit to celsius
C°= F°-32/1.8
Daltons law
Partial=pressure if each gas in a mixture
ptotal= p1+p2+p3…
combined law
p1 v1/T1= p2 v2/T1
ideal gas
an imaginary gas that perfectly fits all assumptions of kinetic molecular theory
PV=nRT
kinetic molecular theory
Gas particles in constant rapid motion
The temperature depends on kinetic energy
STP
temp- 0 C° or 293.15 K
Pressure- 1 Atm
Real gas
take up space have attraction
does not fit with kinetic theory
change more at high pressure and low temp
closest gas
when do gases act most ideal
at high temps and low pressures
what is attraction like in ideal gases
there is no attractive or repulsive forces
how does energy behave in ideal gases
no energy is lost in collisions
how does a barometer work
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.
