2. Properties of Gases (Review)
Properties of Gases (Review)
No definite shape
No definite shape
No definite
No definite
volume
volume
compressible
compressible
4. Basic Kinetic Theory of Gases
Basic Kinetic Theory of Gases
1.
1. Composed of particles like atoms
Composed of particles like atoms
(ex: He) or molecules like (O
(ex: He) or molecules like (O2
2 and
and
CO
CO2
2)
)
There are no attractive/repulsive
There are no attractive/repulsive
forces.
forces.
Lots of empty space!!
Lots of empty space!!
5. Basic Kinetic Theory of Gases
Basic Kinetic Theory of Gases
2. Particles move in
2. Particles move in
random, constant,
random, constant,
straight-line motion.
straight-line motion.
Move independently
Move independently
of each other.
of each other.
6. Basic Kinetic Theory of Gases
Basic Kinetic Theory of Gases
3. All collisions are elastic meaning
3. All collisions are elastic meaning
that KE is transferred without loss of
that KE is transferred without loss of
energy.
energy.
No change in kinetic energy.
No change in kinetic energy.
Gases tend to diffuse towards areas of
Gases tend to diffuse towards areas of
lower concentration
lower concentration.
.
7. Gas Pressure
Gas Pressure
Pressure
Pressure- force exerted on container
- force exerted on container
walls by particles in a gas
walls by particles in a gas
Units used-
Units used- kPa, atm, Torr, mmHg
kPa, atm, Torr, mmHg
STP (Standard Temperature and
STP (Standard Temperature and
Pressure) Table A
Pressure) Table A
273 K or 0°C and
273 K or 0°C and
101.3 kPa = 1 atm = 760 Torr (mmHg)
101.3 kPa = 1 atm = 760 Torr (mmHg)
8. Factors Affecting Pressure
Factors Affecting Pressure
Amount of
Amount of
Gas (number
Gas (number
of moles)
of moles)
Increasing amount
Increasing amount
will increase P
will increase P
(and vice versa)
(and vice versa)
Ex: bicycle tires,
Ex: bicycle tires,
car tires
car tires
Temperature
Temperature Increasing temp.
Increasing temp.
will increase P
will increase P
(and vice versa)
(and vice versa)
Ex: Tires deflate
Ex: Tires deflate
in winter
in winter
Volume
Volume Decreasing
Decreasing
volume will
volume will
increase P,
increase P,
increasing volume
increasing volume
decreases P
decreases P
Ex: press down
Ex: press down
on a balloon and
on a balloon and
it pops
it pops
9.
Pressure
Pressure and
and volume
volume have an inverse
have an inverse
relationship, if temperature remains
relationship, if temperature remains
constant.
constant.
If
If volume
volume is increased,
is increased, pressure
pressure is
is
decreased by the same factor.
decreased by the same factor.
10. Mathematically, the product of PV is constant or PV = k
Mathematically, the product of PV is constant or PV = k
(where k is some constant).
(where k is some constant).
Boyle’ Law
P1 V1 = P2 V2 = P3
V3…
12.
Volume
Volume and
and temperature
temperature have a
have a
direct relationship, if pressure is held
direct relationship, if pressure is held
constant.
constant.
If
If temperature (K)
temperature (K) is increased,
is increased,
volume
volume is increased by the same
is increased by the same
factor.
factor.
13. Mathematically, the relationship of volume divided by Kelvin
Mathematically, the relationship of volume divided by Kelvin
temperature is constant or V/T = k.
temperature is constant or V/T = k.
Charles’ Law
V1 /T1 = V2 /T2 = V3 /T3 …
15.
Pressure
Pressure and
and temperature
temperature have a
have a
direct relationship, if volume remains
direct relationship, if volume remains
constant.
constant.
If
If temperature (K)
temperature (K) is increased,
is increased,
pressure
pressure will be increased by the
will be increased by the
same factor.
same factor.
16. Mathematically, the relationship of volume divided by Kelvin
Mathematically, the relationship of volume divided by Kelvin
temperature is constant or P/T = k.
temperature is constant or P/T = k.
P
r
e
s
s
u
r
e
Gay-Lussac’s Law
P1 /T1 = P2 /T2 = P3 /T3 …
18. Combined Gas Law Equation
Combined Gas Law Equation
P
P1
1 V
V1
1 =
= P
P2
2 V
V2
2
T
T1
1 T
T2
2
19. Combined Gas Law Equation
Combined Gas Law Equation
Steps:
Steps:
Determine which variable (if any) is kept
Determine which variable (if any) is kept
constant.
constant.
Cancel those terms and remove them from
Cancel those terms and remove them from
the equation (Ex: If the question says that
the equation (Ex: If the question says that
temperature remains constant the new
temperature remains constant the new
equation becomes P
equation becomes P1
1V
V1
1 = P
= P2
2V
V2
2).
).
Plug in values that are given.
Plug in values that are given.
Solve for the unknown.
Solve for the unknown.
Be sure to always use temperature in
Be sure to always use temperature in
Kelvins.
Kelvins.
20. Ideal Gases vs. Real Gases
Ideal Gases vs. Real Gases
“
“Ideal gases”
Ideal gases” behave as predicted
behave as predicted
by
by Kinetic Molecular Theory.
Kinetic Molecular Theory.
Examples:
Examples: H
H2
2 and
and He
He
Gases are most ideal at
Gases are most ideal at high
high
temperature
temperature and
and low pressure
low pressure (also
(also
have low mass and low polarity).
have low mass and low polarity).
21.
“
“Real gases”
Real gases” deviate from ideal
deviate from ideal
behavior.
behavior.
Why?
Why?
At low temps, gas particles
At low temps, gas particles
become
become attracted to each other
attracted to each other
(KMT says they are not).
(KMT says they are not).
Under high pressure, gases
Under high pressure, gases occupy
occupy
a specific volume
a specific volume (KMT says they
(KMT says they
don’t).
don’t).
22. Avogadro’s Law
Avogadro’s Law
Avogadro’s number: 6.02 x 10
Avogadro’s number: 6.02 x 1023
23
Simply refers to the quantity of particles
Simply refers to the quantity of particles
found in a
found in a mole
mole.
.
At STP, 6.02 x 10
At STP, 6.02 x 1023
23
particles of a gas
particles of a gas
occupies
occupies 22.4 L
22.4 L.
.
At STP, 3.01 x 10
At STP, 3.01 x 1023
23
particles of a gas
particles of a gas
occupies
occupies 11.2 L
11.2 L.
.
23.
Avogadro also
Avogadro also
hypothesized that
hypothesized that
equal volumes
equal volumes of
of
different gases at the
different gases at the
same temperature
same temperature
and pressure
and pressure contain
contain
equal number of
equal number of
particles
particles (or equal
(or equal
moles).
moles).
24. Vapor Pressure
Vapor Pressure
In a sealed container,
In a sealed container, vapor pressure
vapor pressure
can be measured above a liquid.
can be measured above a liquid.
Evaporation occurs when
Evaporation occurs when some
some
particles from the surface of a liquid
particles from the surface of a liquid
escape
escape causing pressure to build up
causing pressure to build up
above the liquid (not to be confused
above the liquid (not to be confused
with boiling).
with boiling).
26. Factors that Increase the Rate of
Factors that Increase the Rate of
Evaporation
Evaporation
Heating a liquid (not to
Heating a liquid (not to
boiling point)
boiling point)
Increasing surface area
Increasing surface area
Create air currents
Create air currents
(blow across the surface)
(blow across the surface)
27. Liquid-Vapor Equilibrium
Liquid-Vapor Equilibrium
Some of the gas particles condense
Some of the gas particles condense
and then we find
and then we find both evaporating
both evaporating
and condensing occurs at the same
and condensing occurs at the same
rate.
rate.
Rate of Evaporation = Rate of Condensation
Rate of Evaporation = Rate of Condensation
28. Related to Boiling
Related to Boiling
Boiling occurs when the
Boiling occurs when the vapor
vapor
pressure
pressure becomes equal to the
becomes equal to the
external pressure
external pressure.
.
At normal atmospheric pressure, we
At normal atmospheric pressure, we
call this
call this normal boiling point
normal boiling point.
.
29. Boiling and Attractive
Boiling and Attractive
(Intermolecular Forces)
(Intermolecular Forces)
Boiling occurs when
Boiling occurs when heat energy
heat energy
overcomes attractive forces between
overcomes attractive forces between
molecules.
molecules.
The stronger the
The stronger the intermolecular forces
intermolecular forces, the
, the
higher the
higher the boiling point
boiling point.
.
The weaker the
The weaker the intermolecular forces
intermolecular forces, the
, the
lower the
lower the boiling point
boiling point.
.
30. Table H
Table H
Notice, increasing
temperature increases
vapor pressure.
Line drawn at 101.3 kPa
corresponds to normal
boiling point.
