Transcript Chapter 8

Chapter 3
States of Matter
Solid
Liquid
Gas
Plasma
States of Matter
Imagine that you have a baseball and
a small packet of ketchup.
1. If you squeeze the ketchup packet,
how would it change?
2. If you squeeze the baseball, how
would it change?
3. What would these results tell you
about the properties of solids and
liquids?
Homework
Find the definitions and write
into your notebook.
Solid
Liquid
Gas
Kinetic
Energy
Solids
Definite volume and shape.
Liquids
Definite volume but no definate shape.
Gases
No definite volume or shape.
Plasma
High energy, electrically
charged particles.
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Kinetic Theory of Matter
All matter is made up of tiny
particles.
These particles are in constant
motion.
Kinetic Theory of Matter
 Solids - particles move back and
forth but do not change position.
Kinetic Theory of Matter
 Liquids - particles stay close
together but can change position.
Kinetic Theory of Matter
Gases - particles have so much
energy that the force between
them can be ignored. These
particles move freely, in straight
lines, through its container.
Kinetic Theory of Matter
Crystals
Solids where particles are arranged
in repeating patterns. Leaves a
flat surface when broken.




Salt
Sugar
Diamond
Snow Flake
Amorphous Solids
Solids that have a less regular pattern.
( Noncrystalline )
Glass
• Wax
•
Thermal Expansion
When you heat or do work
on matter, its thermal energy
increases. The kinetic and
potential energy of its
particles increases.
Thermal Expansion
As a result of the increase in
kinetic energy the particles
move faster and collide with
other particles more
violently.
Thermal Expansion
Thus, the particles move
farther apart, and the volume
of the material increases.
Homework 3-1
3.1 Assessment
Worksheet
Due: 10/7/08
Behavior of Gases
Pressure
The total force divded by the
area of the surface.
Force
Pressure =
Area
Pressure
Blaise Pascal
 Pascal
 Pa
is the unit for Pressure
is the abbreviation for the Pascal
P = F
A
Pascal =
Newton
Square Meter
Pa =
N
m²
The combined effect of a very large
number of particles constantly
bouncing off the surface causes the
pressure of the gas.
Factors that Affect Air Pressure
Temperature
 Raising
Temperature increases
Pressure
Particles are moving faster!!!
Factors that Affect Air Pressure
Volume
 Reducing
Volume increases
Pressure
Particles in a smaller volume!!!
Factors that Affect Air Pressure
Number
of Particles
 Increasing
the Number of Particles
increases Pressure
More Particles hitting the walls!!
Charles’ Law
If a sample of gas is kept at a
Constant Pressure
and the
Temperature Increases
the
Volume of the gas will Increase.
T2
T1
V1
V2
Pressure is Constant
T2 is Greater than T1
V2 is Greater than V1
Charles's Law Equation
V2
V1
=
T2
T1
T must be Kelvin!!!
°C + 273 = K
Charles's Law
Boyle’s Law
If a sample of gas is kept at a
constant Temperature,
decreasing the Volume
of the gas will
increase the Pressure
Robert Boyle
the gas exerts.
P1
V1
P2
V2
Temperature is Constant
V1 is Greater than V2
P2 is Greater than P1
Boyle’s Law Equation
V1P 1 =
V2 P2
Ideal Gas Law Equation
P2 V2
P1 V1
=
T2
T1
Example
A cylinder that contains air at a
pressure of 100 kPa has a volume
of 0.75 L. The pressure is
increased to 300 kPa. The
temperature does not change.
Find the new volume of air.
P2
P1
V1
V1 = 0.75L
P1 = 100 kPa
V2
V2 = ?
P2 = 300 kPa
Temperature is the same!!
Given:  V1 = 0.75L


P1 = 100 kPa
P2 = 300 kPa
Equation:
Solve:
Find:  V2 = ?
V1 P1 = V2 P2
V1 P 1
= V2
P2
(.75L)(100kPa)
300kPa
= V2
Calculations
0.25L= V2
Bose–Einstein
Condensate
State of matter that exists at very low
temperature, almost at absolute zero.
Albert
Einstein
Satyendra Nath Bose
At a temperature of 200K , a closed
cylinder contains gas at a pressure
of 400 kPa . If the temperature
increases to 280K , what is the new
pressure.
Given:  T1 = 200K


Find:  P2 = ?
P1 = 400 kPa
T2 = 280K
Volume is constant.
Equation:
P1 V1
T1
=
P2 V2
T2
Volume is constant.
P1
T1
=
P2
T2
We are looking for P2.
P1T2
T1
=
P2
P1T2
T1
Solve:
=
P2
(400kPa)(280K)
= P2
200K
560kPa = P2
At 10°C, the gas in a cylinder has a
volume of 0.250 L. The gas is
allowed to expand to 0.285 L. What
must the final temperature be for the
pressure to remain constant
Homework 3-2 (Math Excercises)
Finish Worksheet
Book: Page 80
Math Practice: 1-2
Due: 10/9/08
Homework 8-4
Finish Worksheet
3-2 Assessment
Page:81
Due: 10/13/06
Changes in State
(Phase Changes)
Solid
Liquid
Liquid
Gas
Vaporization
Solid
Gas
Sublimation
Melting
Changes in State
( Phase Changes )
Liquid
Solid
Gas
Liquid Condensation
Gas
Solid
Freezing
Deposition
E
D
Temperature (°C)
100
80
60
C
40
20
B
0
-20 A
10 20 30 40 50 60 70 80 90
Heat (kJ)
A: Ice, Temperature Increases
B: Ice & Water, No Change in
Temperature
C: Water, Temperature Increases
D: Water & Steam, No Change in
Temperature
E: Steam, Temperature Increases
Energy and Phase Change
Phase Change:
 Energy
is added or released
but there is no change in
Temperature
 Energy is used to break the
forces holding the particles
together.
Heat and State Changes
Solid
Liquid
Melting
Heat of Fusion( H2O = 334 kJ/kg )
Liquid
Gas
Heat of Vaporization
( H2O = 2261 kJ/kg )
Boiling
Heat of Fusion
 Energy
needed to go from a
solid to a liquid.
 Water: 334 joules for 1 gram
of ice.
Heat of Vaporization
 Energy
needed to go from a
liquid to a gas.
 Water: 2261 joules for 1 gram
of liquid water.
Sublimation
Phase change
from a solid
to a gas.
Deposition
Phase change
from a gas to
a solid.
Endothermic
Phase change
from a gas to
a solid.
Exothermic
Phase change
from a gas to
a solid.
Homework 3-2
Finish Worksheet
3-3 Assessment
Word Wise/Math
Due: 10/15/08