Chemistry- gas laws

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

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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

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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.