11 Gas Laws Kinetic Molecular Theory

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Gas Laws

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​Class Announcements:

• Mini Test Friday

• 16 days to makeup or retake exams!
  

School Announcements:

• May 15th Early Release

• Boyle's Law

• Charles’s Law

• Avogadro’s Law

• Ideal Gas Law

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Behavior of Gasses

Gas Particles are:

Gas molecules fill the entire container they occupy.

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• ​In constant random motion

• There are no forces of attraction or repulsion between the gas particles

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Kinetic Molecular Theory

Kinetic Energy - the energy of an object in motion

Pressure is a result of the kinetic energy of gasses as they collide with each other and the walls of the container they occupy

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• ​Gas molecules are in constant motion = kinetic energy

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Kinetic Molecular Theory

Pressure and Volume are an inverse relationship

Boyle's Law

P₁V₁=P₂V₂

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• Increase in pressure results in a decrease in volume

• Decrease in pressure results in an increase in volume

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​Volume Units

Kilo Liters KL 0.01 L
Liters L 1 L
milliliters mL 1000 L







Cubic meter m³ 1 KL
Cubic centimeters cm³ 1 mL​

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Kinetic Molecular Theory

The temperature of a substance is related to the average kinetic energy of its particles

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• Increasing the temperature releases "stored" potential energy

• An Increase in temperature result in an increases kinetic energy

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Kinetic Molecular Theory

The temperature of a substance is related to the average kinetic energy of its particles

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• Lower temperatures less kinetic energy

• Higher temperatures more kinetic energy

​More kinetic energy more collisions increase and an increase in volume

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Kinetic Molecular Theory

The temperature and volume are directly proportional

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• An Increase in temperature results in an increase in volume

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Kinetic Molecular Theory

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• Gas particles move in constant random motion

• Gas particles collisions determine pressure

  • The more gas particles the increase in collisions

  • The higher the temperature the increases collisions

  • Volume and pressure are inversely related