The document discusses the properties and behavior of gases, including the kinetic molecular theory, gas laws, and differences between ideal and real gases. Key concepts include the relationships between pressure, volume, and temperature, as outlined in Boyle's, Charles', and Gay-Lussac's laws. Additionally, it addresses vapor pressure, evaporation, and boiling points, emphasizing the influence of intermolecular forces on boiling temperatures.

1. The Behavior of Gases
The Behavior of Gases
Science 10
Science 10

2. Properties of Gases (Review)
Properties of Gases (Review)

No definite shape
No definite shape

No definite volume
No definite volume

Compressible
Compressible

3. Examples of Gases (Review)
Examples of Gases (Review)

Air
Air

Helium
Helium

Ozone
Ozone

Carbon dioxide
Carbon dioxide

Water vapor
Water vapor

5. Kinetic Molecular Theory
Kinetic Molecular Theory
moving molecules well supported ideas

6. Examples of KMT:
Examples of KMT:
1.
1. Ice melts when you remove it from the
Ice melts when you remove it from the
freezer.
freezer.
2.
2. A balloon bursts on a warm day.
A balloon bursts on a warm day.
3.
3. Dry ice disappears without being noticed.
Dry ice disappears without being noticed.
4.
4. Mist
Mist appears on the surface of your
appears on the surface of your
eyeglasses after you come out of a
eyeglasses after you come out of a
cold room.
cold room.
5.
5. You
You feel a cool sensation after you get
feel a cool sensation after you get
out of a pool.
out of a pool.

7. Basic Kinetic Theory of Gases
Basic Kinetic Theory of Gases
1.
1. Composed of particles like
Composed of particles like
atoms (ex: He) or molecules like
atoms (ex: He) or molecules like
(O
(O2
2 and CO
and CO2
2)
)
There are no attractive/repulsive
There are no attractive/repulsive
forces.
forces.
Lots of empty space.
Lots of empty space.

8. 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.

9. 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
Gases tend to diffuse towards areas
of
of lower concentration
lower concentration.
.

10. 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)
Pressure)

Temperature: 273.15 K or 0°C
Temperature: 273.15 K or 0°C

Pressure: 1 atm = 760 mmHg
Pressure: 1 atm = 760 mmHg
= 760 torr
= 760 torr
= 101.325 kPa
= 101.325 kPa

11. 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 (and
will increase P (and
vice versa)
vice versa)
Ex: bicycle tires,
Ex: bicycle tires,
car tires
car tires
Temperature
Temperature Increasing temp.
Increasing temp.
will increase P (and
will increase P (and
vice versa)
vice versa)
Ex: Tires deflate
Ex: Tires deflate
in winter
in winter
Volume
Volume Decreasing volume
Decreasing volume
will increase P,
will 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

12. 
Pressure
Pressure and
and volume
volume have an inverse
have an inverse
relationship, if
relationship, if temperature remains
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.

13. Mathematically, the product of PV is constant or
Mathematically, the product of PV is constant or
PV = k (where k is some constant).
PV = k (where k is some constant).
Boyle’ Law
P1 V1 = P2 V2 = P3 V3…

14. Summary
Summary

15. 
Volume
Volume and
and temperature
temperature have a
have a
direct relationship, if
direct relationship, if pressure is held
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.

16. Mathematically, the relationship of volume divided
Mathematically, the relationship of volume divided
by Kelvin temperature is constant or V/T = k.
by Kelvin temperature is constant or V/T = k.
Charles’ Law
V1 /T1 = V2 /T2 = V3 /T3 …

17. Summary
Summary

18. 
Pressure
Pressure and
and temperature
temperature have a
have a
direct relationship, if
direct relationship, if volume remains
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.

19. Mathematically, the relationship of volume divided
Mathematically, the relationship of volume divided
by Kelvin temperature is constant or P/T = k.
by Kelvin 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 …

21. 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

22. 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.

23. 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).

24. 
“
“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).

25. 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.
.

26. 
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).

27. 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).

29. 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)

30. 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

31. 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.
.

32. 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.
.

33. Table H
Table H
Notice, increasing
temperature increases
vapor pressure.
Line drawn at 101.3 kPa
corresponds to normal
boiling point.