Gas Laws

Boyles

$P1V1=P2V2$

Pressure and volume have an inverse relationship (when one doubles, the other halves)

Charles

$\frac{V1}{T1}=\frac{V2}{T2}$

Volume and temperature have a direct relationship; when you heat a gas, it expands (cool gas = contracts)

Gay Lussac

$\frac{P1}{T1}=\frac{P2}{T2}$

Pressure and Temperature have a direct relationship; when you increase one, the other also increases (increase the pressure and the temperature will rise)

Combined

$\frac{P1V1}{T1}=\frac{P2V2}{T2}$

A combination of all laws above. With five known variables, it is possible to fine the missing one.

Ideal gas law

$PV=nRT$

R is a constant being 8.314$\frac{LkPa}{Kmol}$

Using three given variables, it is possible to find the fourth.

Avogadro’s

$V_{m}=\frac{V}{n}$

at a specific pressure and temperature, the same amount of moles will always be in the same amount of liters

Law of combining volumes

Gases will always react with each other to form whole number ratios

Ex.

2H₂ + (1)O₂ → 2H₂O

2mol H₂ + 1mol O₂ → 2mol H₂O

2mL H₂ + 1mL O₂ → 2mL H₂O

2 : 1 : 2

You can multiply the ratios:

4ml H₂ + 2mL O₂ → 4mol H₂O [this was x2]

Therefore: the coefficients of an equation can be used to find the ratios of moles or liters.