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3. Kinetic Molecular Theory Is a theory that demonstrates how gases should behave. It is also called Ideal Gas Laws.

4. Kinetic Molecular Theory Gas 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.

5. Follow the Ideal Gas Law or KMT.

6. Real Gases Deviate From KMT The 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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9. Boyles Law P V Observation:

10. Boyles Law As pressure increases, volume decrease. Formula: P1V1 = P2V2 (Temperature and number of particles are constant)

11. Charles s Law V T Observation:

12. Charles s Law The higher the temperature (Kelvin), the bigger the volume. Formula: V1 = V2 T1( Kelvin ) T2 ( Kelvin ) Pressure is Constant

13. Gay Lussacs Law P T Observation:

14. Gay Lussacs Law The higher the temperature (Kelvin), the higher the pressure. Formula: P1 = P2 T1( Kelvin ) T2 ( Kelvin ) Volume is constant

15. Combined Gas Law Formula: 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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17. Avagadros Hypothesis Equal volumes of all gases under the same conditions of temperature and pressure have equal numbers of molecules. Avagadros Number = 6.02 x 10 23 One liter of hydrogen has the same number of molecules as one liter of oxygen. 1 mole = 6.02 x 10 23 particles/mol 1 mole of a gas occupies 22.4 liters at STP

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