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

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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.

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Follow the Ideal Gas Law or KMT.

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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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Boyles Law P V Observation:

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

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Charles s Law V T Observation:

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

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Gay Lussacs Law P T Observation:

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

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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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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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The Gas Laws Chapter 14 Chemistry.

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