Gas Laws

Boyles Law

P1V1 = P2V2

Charles Law

V1T2 = V2T1

Gay-Lussacs Law

P1T2 = P2T1

Combined Gas law

P1V1/T1 = P2V2/T2

The Ideal Gas Law

PV = nRt

n = ?

Mols

P = ?

Pressure

V = ?

Volume

Volume must be in ?

Liters

T = ?

Temperature

T = ?

Temperature

Temperature must be in ?

Kelvin

R = ?

Universal gas constant

Daltons Law of partial pressures

Ptotal = P1 + P2 + P3

Pressure(gas) = ?

% composition(gas) x total pressure

Mole Fraction (?)

(X)

(X) = ?

Moles of that substance divided by the total number of mols

X(a) = ?

Mol(a) / Mol(total)

Partial pressure of a gas = ?

Total pressure x mole fraction of that gas

P(a) = ?

P(t) times X(a)

STP of Kelvin

273.15K

STP of atm

1 atm

STP of kPa

101.325

STP of mmHg

760

STP of Liters

22.4L

What is the conversion factor for ^oC to K?

^oC + 273.15

how to convert atm into kPa

atm x 101.325

how to convert kPa into mmHg

kPa x 760/101.325

Atm into mmHg

atm x 760

Solid to gas

Sublimation

Line between Solid and liquid in phase diagram

melting curve

line between liquid and gas in phase diagram

boiling point curve

point where solid liquid and gas phases coexist

Triple point

Mols to molecules formula

Mols x 6.02 × 10^23

How to find Moles

Grams/Molar mass

Liquid to solid

Freezing

Solid to Liquid

Melting

Gas to liquid

Condinsation

Liquid to gas

Vaporation

In gas laws temperature should be in …

Kelvin

In which Gas law should the Volume unit match the Specific gas constant?

PV = nRT