Gasses and atmospheric chemistry

KMT (kinetic molecular theory)

1. Gasses are made up of very small particles

2. Gaseous particles always move straight, but different directions

3. Gaseous particles undergo elastic collisions

4. Gaseous particles exert no force of attraction

Ideal Gas

a theoretical gas composed of randomly moving point particles that do not interact with each other except through perfectly elastic collisions.

Pressure

force per unit area, which is resulted by one object hitting another object

High pressure → Low pressure

Gas pressure

force caused by constant collisions

1. Number of gas particles

• The more # of particles = the more collisions = higher pressure

2. Temperature

• Higher temperature = Increased speed of particles = Increased force of collisions = increased pressure

Boyle’s Law

compares the relationship between pressure and volume of gas

Volume is inversely proportional to pressure

Equation: P1V1 = P2V2

Absolute zero

Absolute zero is at -273, its also the most lowest a temperature can go to

Kevin scale

• No negative values

• Kelvin = Celcius + 273

Gas laws key factores

1. Temperature:

   • As temperature increase, molecules gain kinetic energy and occupy more space

2. Pressure:

   • As pressure increases, molecules become more compressed (takes up less space)

3. Amount of gas

   • More gas = More space

Charles’ Law

• Compares the relationship between volume and temperature of a gas

• As temperature increases, volume increases (if factors kept constant)

T1/T2 = V1/V2

Gay Lussac’s Law

• Compares the relationship between volume and temperature of a gas

• As temperature increases, pressure increases

P1/P2 = T1/T2

Combined gas law

Compares relationship between volume, pressure and temperature of a fixed amount of gas

P1V1/ T1 = P2V2/T2 (all three laws combined)

Partial Pressure

Pressure of gas in a gas mixture that it would exert if it were the only gas present in the same volume

Dalton’s Law

Total pressure of mixture = sum of partial pressures

PT = P1 + P2…