Atmospheric Chemistry

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Atmospheric Chemistry

States of matter

Gas

Shape of container

Lots of space

Little attraction

Liquid

Fixed volume

Can flow to different places

Somewhat strong attraction

Solid

Fixed shape, volume, position

Strong attraction

Dalton’s particle model

Idea of atoms

The properties

The states of matter

Partial Pressures

Dalton’s Law of partial pressures

Total pressure

The sum of each individual gas pressures

Ptotal = P1 + P2 + P3….

Pgas = proportion x ptotal

Atmosphere

Nitrogen, oxygen, argon

Specific pressure of gas

Ideal gas mixture

Kinetic Molecular theory

All particles

Ideal gas behaviour

Not true

Particles

Elastic collisions

Conserved

Small gas particles

Large number of particles

Kinetic energy

Gas behaviours

Molecular motion

Brownian motion discovery

Particle collisions

Gas Laws

Combined Gas Law

P1 x V1 / T1 = P2 x V2 /T2

Constant

Number of moles

Large quantities

Atoms or molecules

Container

Litres

Speed of motion

Kelvin

Force exerted

Gas particles

Surface

KiloPascals

Physical constant

Molar gas constant

Standard conditions

Fixed variables

Temperature and pressure

Compare different sets of experiments

Quantitative relationships

Gas variables

Physical property

Gasses

Ideal Gas Law

Hypothetical gas properties

PV=nRT

Charle’s Law

V1/T1=V2/T2

Gay Lussac’s Law

Temperature

P1/T1=P2/T2

Boyle’s Law

Pressure

Inverse operation

P1xV1=P2xV2

Avogadro’s law

Volume

Number of particles

P1/n1=P2/n2