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Chemistry (1)
Properties of gases
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Leah Murphy
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Cards (19)
Diffusion
High
concentration
to
low
concentration
Properties
of Gases
Temperature
in Kelvin (K)
Pressure
in Pa
Volume
in m³
0°C =
273K
Experiment to measure pressure
Barometer
Boyle's Law
At constant
temp
, vol of fixed mass of gas is
inversely
proportional to its
pressure
Charles' Law
Fixed mass of gas at
constant
pressure is directly proportional to the
temp
Brownian movement
Constant, random, straight line of particles
Avogadro's
Law
Same no. of
particles
in 1L of any gas at STP (
22.4L
)
1L of gas at RTP =
24.4L
Ideal Gas Equation
PV
=
nRT
Real
Gases
Differ from ideal gases due to
contradictions
Most like ideal at
high temp
and
pressure
Assumptions
of Kinetic Theory of Gases
Continuous
rapid random
movement
No
attractive
or
repulsive
forces
Volume is
negligible
Collisions are
perfectly
elastic
No
such
gas
exists that obeys all assumptions of
kinetic
theory
Ideal Gas
Obeys
all assumptions of
kinetic
theory under all
temp
and
pressure
General Gas Law
PV/T
=
constant
Gay-Lussac's Law
of
Combining Volumes
Ratio
of
small whole numbers
If you know the
mass
of a thing, you can find the
moles
of anything
Contradictions
: There may be
attractive
forces when particles move
close
together
Inversely proportional: as one
increases
the other
decreases.