Gases + Gas Laws

Standard Units of Pressure

• 1 atmosphere (atm)

• 101.3 kilopascals (kPa)

• 760 millimeter mercury (mmHg)

• 760 torr

Standard Units of Temperature

• 0º C

• 273 ºK

Celsius to Kelvin

ºC + 273= K

Pressure vs Volume

A volume decreases, pressure increases (Inversely proportional)

Boyle’s Law

P₁V₁ = P₂V₂

Volume vs Temperature

As volume increases, temperature increases (directly proportional)

Charles’ Law

V₁/T₁ = V₂/T₂

Pressure vs Temperature

As temperature increase, pressure increases (directly proportional)

Gay-Lussac’s Law

P₁/ T₁ = P₂/T₂

Combined Gas Law

(P₁)(V₁)/ (T₁) = (P₂)(V₂)/(T₂)

Ideal Gases

Gases that follow closely to the kinetic molecular theory. Behave most ideal at high temperatures and low pressures

Ideal Gas Law

PV=nRT

Ideal Gas Law Standard

P= Pressure in kPa (or atm)

V=Volume in L

n= Moles of gas

R= Ideal Gas Constant

T= Temperature in K

Ideal Gas Constant R

kPa= 8.314

atm=0.08206

Diffusion

Movement of a gas molecules from an area of high concentration to low concentration

Effusion

Diffusion of gas through a small hole

Graham’s Law