Kinetic Molecular Theory
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13 Terms
An ideal gas consists of…
Tiny spherical particles that are far apart relative to their size.
An ideal gas’s particles are in…
constant rapid, random motion
Collisions between gas particles are:
Elastic collisions (kinetic energy may be transferred between particles, but not lost)
T or F: there can be forces of attraction or repulsion between ideal gas particles
FALSE- no forces of attraction or repulsion, no condensation, all motion must be completely independent
As number of moles of gas increases…
Pressure increases (direct correlation)
As volume decreases…
Pressure increases (inverse correlation)
As temperature increases…
Pressure increases (direct correlation)
Pressure =
force / area
R=
PV/nT
PV=
nTR
Why does P increase as the number of particles (n) increases?
More particles means more collisions.
Why does P increase as temperature (T) increases?
Collisions are harder as particles move faster
Why does P increase as volume (V) decreases?
As the container becomes smaller, collisions become more frequent as particles travel less distance to reach the walls
Note 
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