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Atmospheric Chemistry

Gas Laws

Avogadro’s law

Volume

Number of particles

P1/n1=P2/n2

Boyle’s Law

Pressure

Volume

Inverse operation

P1xV1=P2xV2

Gay Lussac’s Law

Pressure

Temperature

P1/T1=P2/T2

Charle’s Law

Volume

Temperature

V1/T1=V2/T2

Ideal Gas Law

Hypothetical gas properties

PV=nRT

Quantitative relationships

Gas variables

Physical property

Gasses

Standard conditions

Fixed variables

Temperature and pressure

Compare different sets of experiments

Physical constant

Molar gas constant

Pressure

Force exerted

Gas particles

Surface

KiloPascals

Temperature

Speed of motion

Gas particles

Kelvin

Volume

Container

Litres

Number of moles

Gas particles

Large quantities

Atoms or molecules

Combined Gas Law

Hypothetical gas properties

P1 x V1 / T1 = P2 x V2 /T2

Number of moles

Constant

Kinetic Molecular theory

Brownian motion discovery

Particle collisions

Gas behaviours

Molecular motion

Kinetic energy

Temperature

Container

Small gas particles

Large number of particles

Particles

Elastic collisions

Kinetic energy

Conserved

All particles

Ideal gas behaviour

Not true

Partial Pressures

Specific pressure of gas

Ideal gas mixture

Atmosphere

Nitrogen, oxygen, argon

Dalton’s Law of partial pressures

Total pressure

Container

The sum of each individual gas pressures

Ptotal = P1 + P2 + P3….

Pgas = proportion x ptotal

States of matter

Dalton’s particle model

Idea of atoms

The properties

The states of matter

Solid

Fixed shape, volume, position

Strong attraction

Particles

Liquid

Fixed volume

Can flow to different places

Somewhat strong attraction

Particles

Gas

Shape of container

Lots of space

Little attraction

Particles