Gases

Introduction to Gases

100

Refers to a gas that exactly obeys the assumptions of the kinetic theory

ideal gas

200

SI unit of pressure

pascal

300

A compact and rugged instrument that senses pressure using a flexible, airtight metal box

aneroid barometer

400

The assumption that the kinetic energy of gas molecules is directly related to temperature best explains why the volume of a gas is affected by temperature is used with this theory

kinetic theory of matter

500

A relation in which the value of one variable depends directly upon the value of another variable

direct proportion

Gas Laws

100

The pressure of a gas at STP

100 kPa

200

This has a value of 8.314 L x kPa / (K x mol)

gas constant R

300

PV = nRT

ideal gas law

400

Gives relationship between volume and pressure at constant temperature

Boyle's Law

500

Gives relationship between volume and temperature at constant pressure

Charles's Law

Miscellaneous

100

The name for the process of mixing molecules of one substance through another substance by random molecular motion

diffusion

200

A relation in which the value of one variable depends on the reciprocal of another variable

inverse proportion

300

This law states that the rate of diffusion is inversely proportional to the square root of molar mass

Graham's law of diffusion

400

This equals the average atmospheric pressure at sea level

standard atmosphere (atm)

500

This law can be used to convert gas volume to moles and vice versa

ideal gas law

Equations

100

P₁V₁ = P₂V₂

Boyle's Law

200

V₁/n₁ = V₂/n₂

Avogadro's Law

300

V₁/T₁ = V₂/T₂

Charles's Law

400

P_total = P₁ + P₂ + P₃ ...

Dalton's law of partial pressures

500

rate₁/rate₂ = (square root) M₂/M₁

Graham's law of diffusion