Behavior of Gases

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Behavior of Gases

• Kinetic Molecular Theory
• (KMT)

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Properties of Gases

• No definite shape they take on the shape of
  their container

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Properties of Gases

• 2) No definite volume they will expand to fill
  their container

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Properties of Gases

• 3) Unlike solids and liquids, they can be easily
  compressed

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Kinetic Molecular Theory (KMT)

• This theory tries to explain why gases behave
  the way they do. It is model of IDEAL gas
  behavior.

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Kinetic Molecular Theory (KMT)

• Idea 1 Gases are made of particles (atoms or
  molecules) that are in constant random
  straight-line motion

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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

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Elastic Collisions
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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.

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Kinetic Molecular Theory (KMT)

• Idea 4 Gas particles are so far apart they do
  not attract each other.

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Pressure and number of gas particles

• More particles higher pressure

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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

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The igloo fiasco
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Temperature and Volume
Volume
Temperature
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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

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Exploding cans.
?

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Temperature and Pressure
Pressure
Temperature
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Pressure and Volume

• Increasing the pressure on a gas in a container
  will decrease the volume

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Pressure and Volume
Volume
Pressure