Chemistry: Gasses + Gas Laws

Kinetic Molecular Theory

Gas particles move very fast in straight lines until they collide with each or the container

Pressure of gas

The force the gas exerts on the walls of its container

Standard Unit of Pressure: Atmosphere

1 atm

Standard Unit of Pressure: kilopascals

101.3 kPa

Standard Unit of Pressure: Millimeters mercury

760 mmHg

Standard Units of Pressure: torr

760 torr

Liters to Millimeters

1000mL=1L

Celsius to Kelvin

°C+273=K

Pressure vs Volume

Inversely Proportional; V decreases as P increases

Boyle’s Law

P₁V₁=P₂V₂

Volume vs Temperature

Directly Proportional; as V decreases T also decreases

Charles’s Law

V₁/T₁= V₁/T₂

Pressure vs Temperature

Directly Proportional; as P increases T also increases

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

When are gases most ideal

At high temperatures and low pressures

Ideal Gas Law

PV=nRT

Ideal Gas Constant: kPa

8.314

Ideal Gas Constant: atm

0.08206