The Kinetic Molecular Theory and
Gasses (2023 Update)
According to the Kinetic Molecular Theory, ideal gases should: - - contain particles that
are
... [Show More] in random, constant straight-line motion
- be so small that compared to the volume of space that they occupy, their volume is
insignificant (zero)
- be separated by great differences relative to their particle size
- NOT have attractive forces between the particles
- when gas particles collide, there can be a transfer of energy between particles but the
total energy of the system must remain constant
In reality, Real Gases: - - DO have mass and volume and take up space
- DO have attractive forces between particles
The most ideal gasses would be: - H2 (Hydrogen) and He (Helium)
To make a real gas behave like an Ideal Gas the particles must: - - spread out as much
as possible in the given container
- This can only be done under conditions of high temperature and low pressure on a gas
(increase in volume)
Avagadro's Hypothesis - when the VOLUME, TEMPERATURE and PRESSURE of two
or more DIFFERENT GASSES are the SAME, they will also then contain the SAME
NUMBER of MOLECULES
Temperature vs Pressure (Guy Lussac's Law) - - as the temperature of a gas increases,
there is an increase in movement and in the number of collisions between gas particles
and the walls of the containers
- the increase in the number of collisions then causes an increase in gas pressure
Temperature vs Volume (Charles' Law) - - as the temperature of a gas increases, there
is an increase in the movement and the number of collisions between gas particles and
the walls of the containers
- the increase in the number of collisions causes gas particles to spread out more,
therefore increase the volume of a gas
Volume - space occupied
Temperature - movement
Volume vs. Pressure (Boyle's Law) - - as the volume of a space a gas occupies
increases there is a decrease in the number of collisions between gas particles and the
walls of the containers
- the decrease in the number of collisions causes the pressure to decrease
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