1. Topic 4
Topic 4-Phases of Matter
Phases of Matter

2. Topic 4-Phases of Matter
Phases of Matter Gas Laws
a. Solid a. Boyle’s Law
b. Liquid b. Charles’ Law
c. Gas c. Gay-Lussac’s Law
Heating/Cooling Curves d. Combined Gas Law
a. Potential energy Use Table T
b. Kinetic energy
c. Sublimation and Deposition 7. Kinetic-Molecular Theory
Temperature Scales (KMT)
a. Kelvin
b. Celsius Ideal Gas vs. Real Gas
c. Use Formula on Table T
Heat vs. Temperature 9. Filtration
*know the difference
Measuring Heat Energy Distillation
a. Heat of Fusion-Table B
b. Heat of Vaporization-Table B 11. Chromatography
c. Specific Heat of Water-Table B
d. Use Formulas on Table T

3. Properties of Solids
1. Definite shape
6. Particles are packed tightly
together, often in an orderly
arrangement
2. Definite volume
3. Incompressible
4. Expand only slightly when heated
5. Particles vibrate around a fixed point

4. Properties of Liquids
Indefinite shape-take shape of
container
2. Definite volume
3. Arrangement of particles is not
orderly or rigid
4. Almost incompressible.
5. Expand slightly when heated
6. Particles are free to flow

5. Properties of Gases
1. Indefinite shape
2. Indefinite volume
3. Expands to fill the entire container
4. Easily compressible
5. Particles are far apart from each other

6. 3 Phases of Matter
Some people claim there is a 4th phase of matter called:
Plasma
The three normal phases of matter have been known for many years. In recent times, we have begun to study matter at the very high temperatures and pressures which typically occur on the Sun, or during re-entry from space. Under these conditions, the atoms themselves begin to break down; electrons are stripped from their orbit around the nucleus leaving a positively charged ion behind. The resulting mixture of neutral atoms, free electrons, and charged ions is called a plasma.

7. A term used for substances, like oxygen, that exist
Gas vs. Vapor
What is the difference?
Gas-
A term used for substances, like oxygen, that exist
in the gaseous state at room temperature
Vapor-
Describes the gaseous state of a substance that
is generally a liquid or solid at room temperature
Water in the gaseous state is a vapor because at room
temperature, it is a liquid
Oxygen in the gaseous state is a gas because at room
temperature, it is a gas

10. The phase changes from: S  L  g  plasma
Are all endothermic
Endothermic-describes a physical change or chemical reaction that absorbs heat energy

11. Most substances go through all three phase changes:
Exothermic: g  L  s (heat/energy released) Or
Endothermic: S  L  g (heat/energy absorbed)
BUT:
Some substances like to skip a phase

12. Sublimation-
The process in which a solid changes
to a gas or vapor without passing
through the liquid state
The process in which a gas or vapor
changes to a solid without passing
through the liquid state
Deposition-
Two substances which these terms apply to are:
1. Dry ice (carbon dioxide)-CO2
2. Iodine (I2)

13. Temperature-the property or condition of a body that
determines the direction of heat flow
between it and another body.
It is a measure of the
AVERAGE KINETIC ENERGY (KE)
of the molecules
As temperature increases, so does average KE
As temperature decreases, so does average KE
If temperature remains the same (RTS) so does average KE

14. The energy stored in a bond
Potential Energy
the energy of a body or a system with respect to the arrangement of the particles of the system
The energy stored in a bond
As temperature increases = PE remains the same
As temperature decreases = PE remains the same

15. Calorimetry-
Precise measurement of the heat flow into or
out of a system for chemical and physical
processes
Even though there are five areas on a cooling or
heating curve, there are only three equations:
1. Q = mc T-when temperature changes
2. Q = mHf-when substance melts or freezes
3. Q = mHv-when substance boils or condenses

16. How much energy is needed to raise the temperature of 500 g of water at 30 C to 70 C?
Notice: no phase change just temperature change
Only need Q = mc T
Q = (500)(4.18)(40)
Q = joules

17. How much energy is needed to melt 60 g of ice at 0 C?
Just a phase change: melting/fusion
no temperature change
Only need one equation:
Q = mHf
Q = (60)(334)
20040 joules

18. How much energy is needed to raise the temperature of
10 g of ice at -23 C to water at 50 C?
Notice: temperature change & phase change
Q = mc T
Raise the temperature from -23 to 0 C
Q = (10)(2.09)(23)
= joules
Now make the phase change
Q = mHf
Q = (10)(334)
= 3340 joules
Now raise the temperature from 0 to 50 C
Q = mc T
Q = (10)(4.18)(50)
= 2090 joules
Add the 3 numbers: = joules

19. How much energy is needed to raise 50g of water at 50 C
to steam at 115 C?
There is a phase change and a temperature change
1. Raise temperature from 50 to 100 C
Q = mc T
Q = (50)(4.18)(50)
= joules
2. Vaporize the water
Q = mHv
Q = (50)(2260)
= joules
3. Raise the temperature from 100 to 115
Q = mc T
Q = (50)(2.09)(15)
= joules
Add them up: joules

20. Temperature
Temperature-
AVERAGE KINETIC ENERGY
Is a measure of how hot or cold something is.
An object’s temperature determines the direction of heat transfer.
Heat ALWAYS moves from an area of high temperature to low temperature

21. Scientists commonly use two equivalent units of temperature, the degree Celsius and the kelvin
Anders Celsius ( )
freezing point of water = 0 C
boiling point of water = 100 C
The distance between these two fixed points is
divided into 100 equal intervals
Lord Kelvin ( )
freezing point of water = 273 K
boiling point of water = 373 K
The distance between these two fixed points is
divided into 100 equal intervals

22. A change of one degree on the Celsius scale is equivalent to one kelvin on the Kelvin Scale
To convert between the scales,
use Table T
K = C + 273
C = K - 273 or

23. Notice that for ANY temperature scale, there are two fixed points:
Freezing point and boiling point
Also:
The freezing point = melting point of any substance
Water freezes at 0 C and melts at 0 C
So if you know the melting point of a substance, you also know the freezing point
Table S lists the melting point of all the elements so you
also know the freezing point of all the elements

24. The zero point on the Kelvin temperature
0 K = absolute zero
Absolute zero-
The zero point on the Kelvin temperature
scale, equivalent to C
At absolute zero, all molecular motion stops

25. A measure of the force exerted by a gas above a liquid
Vapor Pressure
A measure of the force exerted by a gas above a liquid
in a sealed container; a dynamic equilibrium exists
between the vapor and the liquid
Temperature has nothing to do with boiling.
Pressure determines when a substance boils

26. The temperature at which the vapor
Boiling point-
The temperature at which the vapor
pressure of a liquid is equal to the
atmospheric pressure on the liquid
Normal boiling point-
Boiling point of a liquid at a pressure
of kPa (standard pressure)

28. Low bp = high vapor pressure
High bp = low vapor pressure
Low bp = weak intermolecular forces (IMFs)
High bp = strong intermolecular forces (IMFs)
Low bp = high vp = weak IMFs
High bp = low vp = strong IMFs

29. Energy that transfers from one object to another
Heat
Energy that transfers from one object to another
because of a temperature difference between
the objects
Law of Conservation of Energy
The heat released by the system is equal to the heat
absorbed by the surroundings. Conversely, the heat
absorbed by a system is equal to the heat released
by its surroundings.

30. 3 Factors that Affect the Behavior of Gases
1. temperature
2. pressure
3. volume
A small change in any of these factors causes a huge
change in the behavior of the gas.
3 scientists studied the behavior of gases by holding one of the variables constant and adjusting the other two variables.

31. Standard Temperature & Pressure (STP)
0 C
273 K
Pressure
1 atm
101.3 kPa
760 torr
760 mm Hg
These can be found on Table A

32. Boyle’s Law
Robert Boyle
Held temperature constant
Varied pressure & volume
volume
Pressure =
Pressure =
volume
Indirect/inverse relationship

33. Boyle’s Law

34. A balloon contains 30 L of helium gas at 103 kPa.
Boyle’s Law Equation
V1P1 = V2P2
You can use any units of volume and pressure as long as they are the same on both sides
A balloon contains 30 L of helium gas at 103 kPa.
What is the volume of the helium when the balloon rises
to an altitude where the pressure is only 25 kPa
Temperature is not mentioned so we know it is constant
V1P1 = V2P2
(30)(103) = (x)(25)
X = L

35. Charles’ Law
Jacques Charles
Held pressure constant
Temp =
volume
Temp =
volume
Direct Relationship

36. Charles’ Law

37. What temperature in Celsius is need to change 50 mL of
Charles’ Law Equation
V1 = V2
T1 T2
*temperature MUST be in Kelvin
What temperature in Celsius is need to change 50 mL of
a gas at 37 C to 200 mL?
50 mL = 200 mL
310 K x
X = 1240 K
Which equals 967 C

38. Gay-Lussac’s Law
Joseph Louis Gay-Lussac
Held volume constant
Temp =
pressure
Temp =
pressure
Direct Relationship

39. Gay-Lussac’s Law

40. If a gas at a temp of 30 C and a pressure of 2 atm is
Gay-Lussac Problem
If a gas at a temp of 30 C and a pressure of 2 atm is
raised to 500 K, what is the new pressure?
P1 = P2
T T2
*temp must be in Kelvin
*Be careful…notice one temperature is in Celsius and the other is in Kelvin. Just change the Celsius temperature to Kelvin
2 atm = x atm
303 K K
X = 3.30 atm

41. It is extremely difficult to hold any of these variables
COMBINED GAS LAW
(Table T)
It is extremely difficult to hold any of these variables
(temperature, pressure or volume) constant. Usually,
all three change.
If all three change, use the combined gas law.
V1P1 = V2P2
T T2

42. Combined Gas Law Problem
If 100 mL of a gas at STP is raised to a temperature
of 500 C and a pressure of 300 kPa, what will be the
new volume?
*STP give you the conditions for temperature and
pressure. You must use Table A if you don’t remember!
V1P1 = V2P2
T T2
(100 mL)(101.3kPa) = (x mL)(300 kPa)
273 K K
X = mL

43. Avogadro’s Hypothesis
Equal volumes of gases at the same temperature and
pressure contain equal number of particles
3 liters of H2O (g) and 3 liters of Ne (g) have equal number
of particles but their mass is very different from each other

44. Kinetic Molecular Theory (KMT) of an Ideal Gas
The particles of a gas in constant, random,
straight-line motion.
Collisions are elastic-KE is transferred without
loss from one particle to another. Total KE RTS.
3. There is a great distance between gas molecules
4. There is no attraction between gas molecules
5. A gas has no volume.

45. Yet, a real gas does have attractive forces and does have a volume…so numbers 4 & 5 do not hold for a real gas. The KMT is still sound so we still use it even though some aspects of it are incorrect.
So…there is no ideal gas…it only exists in theory
Under what conditions will a real gas behave most ideally?
Low pressure and high temperature
Remember: P L I G H T
pressure
low
ideal
gas
high
temperature

46. What type of gases behave most ideally?
The lighter the gas, the more ideally it behaves.
Therefore, H2 and He are the two gases that behave most
Ideally.
Question: Which of the following gases behaves
most ideally?
A. O2
32 g
C. NH3
17 g
64 g
D. SO2
B. CO2
44g
Therefore it is NH3 because it is the lightest!

47. Physical Means of Separating Mixtures
Filtering-a process in which an insoluble solid is recovered
from a mixture
The solid remains on the filter paper and anything
dissolved in the water, passes through the filter paper.
Ex. Sand, salt and water. Sand would remain on filter
paper because it does not dissolve in water but the filtrate
would have water and dissolved salt in it. To recover the
salt, evaporate the water and the salt will remain.

48. Chromotagraphy-
is an analytical technique for separating and identifying mixtures that are or can be colored, especially pigments

49. Separation of a mixture based on differences in boiling points
Fractional Distillation/Distillation-
A process used to separate
dissolved solids from a
liquid, which is boiled to
produce a vapor that is then
condensed into a liquid
Separation of a mixture based on differences in boiling points