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Kinetic Molecular Theory

Is a theory that demonstrates how gases “should” behave.

It is also called “Ideal Gas Laws”.

Kinetic Molecular TheoryGas particles are in random, constant, straight-

line motion. Gas particles are separated by great distances

relative to their size; the volume of the gas particles is considered negligible.

Gas particles have no attractive forces between them.

Gas particles have collisions that may result in a transfer of energy between gas particles, but the total energy of the system remains constant.

Follow the Ideal Gas Law or KMT.

Real Gases Deviate From KMTThe volume of gas

particles is significant. Gas particles DO have volume.

Gas particles DO have a force of attraction.

The two deviations are significant under high pressure and low temperature (molecule are closer together).

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Boyle’s Law

P

VObservation:

Boyle’s LawAs pressure increases, volume decrease.

Formula: P1V1 = P2V2

(Temperature and number of particles are constant)

Charles’ s Law

V

T

Observation:

Charles’ s LawThe higher the temperature (Kelvin), the

bigger the volume.

Formula: V1 = V2 T1(Kelvin) T2 (Kelvin)

Pressure is Constant

Gay Lussac’s Law

P

T

Observation:

Gay Lussac’s LawThe higher the temperature (Kelvin), the

higher the pressure.

Formula: P1 = P2 T1(Kelvin) T2 (Kelvin)

Volume is constant

Combined Gas LawFormula: P1V1 = P2V2

(Table T) T1(Kelvin) T2 (Kelvin)

Table A - STP

May be used to solve any of the previous gas law problems.

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Avagadro’s HypothesisEqual volumes of all gases under the same

conditions of temperature and pressure have equal numbers of molecules.

Avagadro’s Number = 6.02 x 1023

One liter of hydrogen has the same number of molecules as one liter of oxygen.

1 mole = 6.02 x 1023 particles/mol

1 mole of a gas occupies 22.4 liters at STP

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