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Behavior of Gases

Behavior of Gases. Kinetic Molecular Theory (KMT). Properties of Gases. No definite shape: they take on the shape of their container. Properties of Gases. 2) No definite volume: they will expand to fill their container. Properties of Gases.

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Behavior of Gases

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  1. Behavior of Gases Kinetic Molecular Theory (KMT)

  2. Properties of Gases No definite shape: they take on the shape of their container

  3. Properties of Gases 2) No definite volume: they will expand to fill their container

  4. Properties of Gases 3) Unlike solids and liquids, they can be easily compressed

  5. Kinetic Molecular Theory (KMT) This theory tries to explain why gases behave the way they do. It is model of IDEAL gas behavior.

  6. Kinetic Molecular Theory (KMT) Idea # 1: Gases are made of particles (atoms or molecules) that are in constant random straight-line motion

  7. Kinetic Molecular Theory (KMT) Idea # 2: Gases particles collide with each other and the walls of their container. These collisions are elastic, meaning no energy is lost during the collision, only transferred. These collisions are measured as pressure of the container walls

  8. Elastic Collisions

  9. Kinetic Molecular Theory (KMT) Idea # 3: Gas particles are separated by great distances. Therefore the volume of the individual gas particles is negligible compared the volume of the container.

  10. Kinetic Molecular Theory (KMT) Idea # 4: Gas particles are so far apart they do not attract each other.

  11. Pressure and number of gas particles More particles = higher pressure

  12. Temperature and volume • Higher Temperature = bigger volume (if the container has expandable walls so that pressure does not change) • WHY? • Remember temp = ave kinetic energy • Higher temp means the gas particles move faster, hitting the walls of the container harder and pushing it outward

  13. The igloo fiasco

  14. Temperature and Volume Volume Temperature

  15. Temperature and pressure • Higher temperature = higher pressure (if walls of container are not exandable) • WHY? • temp = ave kinetic energy • Higher temp means the gas particles are moving faster, hitting the walls of the container harder. • This results in more pressure measured on the container walls

  16. Exploding cans…. = ? +

  17. Temperature and Pressure Pressure Temperature

  18. Pressure and Volume • Increasing the pressure on a gas in a container will decrease the volume

  19. Pressure and Volume Volume Pressure

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