1. Chapter 3
States of Matter

2. 5 States of matter
Solid
Liquid
Gas
Plasma
Bose-Einstein condensate

3. Solids What makes a solid a solid? Definite shape and volume
The atoms are packed close together
They have an orderly arrangement
Particles vibrate but don’t move

4. Liquids What makes a liquid a liquid? Definite volume
Takes the shape of container
Flows easily
Loosely held together
Arrangement more random

5. Gases What makes a gas a gas? Not definite shape nor volume
No pattern to them
Lots of space between, no bonds
Can be compressed (aerosol cans)

6. Plasmas Exists at extremely high temperatures
Very similar to gases but the atoms have lost electrons, we call them free electrons
Most common state in the universe

7. Bose-Einstein condensate
Exists at extremely low temperatures
Named after the two scientists S. Bose and A. Einstein
Near -273 oC groups of atoms behave as one

8. Kinetic Energy Kinetic energy is the energy of movement
The faster an object moves, the more Kinetic Energy it has
Even though we may not see it, all particles are constantly moving. This is the Kinetic Theory of matter.

9. How the Different Particles Move
Gas: Particles are always bouncing around, colliding into each other
They move in a straight line. If they collide one atom may slow down and the other may speed up.
The particles in a gas have weak attractions and don’t have an affect on movement.

10. Kinetic Theory of Gases
The constant motion of particles in a gas allows a gas to fill a container of any shape or size
We just looked at the 3 main points of this theory on the previous slide

11. Behavior of liquids
Has a definite volume because it is heavier and their attraction to each other.
Liquids are closely packed like a hallway
Particles in a liquid can flow to new locations because the attraction keeps the particles close together

12. Behavior of Solids
Particles have a fixed locations and volume doesn’t change
They vibrate but never leave their location

13. Phase Changes
The reversible physical change that occurs when substance changes from one state of matter to another.
The temperature during a phase change stays the same.
Energy is either absorbed or released during a phase change

14. Exothermic vs. Endothermic
Endothermic: Absorbs energy from its surroundings
Types: Melting, Vaporization, Sublimation
Exothermic: Releases energy to its surroundings
Types: Freezing, Condensation, Deposition

15. The Cycle

16. pressure Pressure is the result of a force distributed over an area.
SI unit for Pressure based on Force and area
Force is measure in newtons (N)
Area is measure in meters2
Pressure is N/m2
Can be expressed as a Pascal (Pa): SI Unit

17. Gas Pressure
Collisions between particles and the walls cause the pressure in a close container.
Factors that affect gas Pressure
Temperature: High Temp=High KE=More collisions=Greater pressure
Volume: Reducing Volume=Greater pressure
Number of Particles: Increase #= Greater pressure

18. Gas Laws
Formulas that explain the behaviors of gases at different temperatures, pressures, and volumes.

19. Charles’s Law
States that the volume of a gas is directly proportional to its temperature in Kelvins if the pressure and the number of particles of the gas are constant.
What that means: If you increase the temperature you increase the volume

20. Charles’s Law Formula
V1 = V2
T T2
Example Problems

21. Boyle’s Law Shows relationship between pressure and volume of a gas
It can be described as an inverse relationship
As pressure increases, volume would decrease and vice-versa

22. Boyle’s Law Formula
P1V1 = P2V2
Example Problems

23. Combined Gas Law
Shows the total relationship between temperature (in Kelvins), volume, and pressure of a gas when particles are constant.
P1V1 = P2V2
T1 T2
Example Problems

24. Charles’ Law Examples
What volume will a sample of hydrogen occupy at 28.0 oC if the gas occupies a volume of 2.23 L at a temperature of 0.0 oC?   Assume that the pressure remains constant.

25. If a gas occupies 733 mL at 10.0 oC, at what temperature will it occupy 950 mL?  Assume that pressure remains constant.

26. A gas occupies 560 mL at 285 K.  To what temperature must the gas be lowered to, if it is to occupy 25.0 mL?  Assume a constant pressure.

27. What volume would a sample of helium occupy at standard temperature, if it occupies 250 cm3 at 185 K?  Assume constant pressure.

28. A sample of oxygen gas has a volume of 2. 73 L at 21. 0 oC
A sample of oxygen gas has a volume of 2.73 L at 21.0 oC.  At what temperature would the gas have a volume of 4.00 L?

29. Boyle’s Law
The volume of the lungs is measured by the volume of air inhaled or exhaled.  If the volume of the lungs is L during exhalation and the pressure is kPa, and the pressure during inhalation is kPa, what is the volume of the lungs during inhalation? 

30. It is hard to begin inflating a balloon. A pressure of 800
It is hard to begin inflating a balloon.  A pressure of kPa is required to initially inflate the balloon mL.  What is the final pressure when the balloon has reached it's capacity of 1.2 L?

31. If a gas at 25. 0 °C occupies 3. 60 liters at a pressure of 1
If a gas at 25.0 °C occupies 3.60 liters at a pressure of 1.00 atm, what will be its volume at a pressure of 2.50 atm?

32. A gas occupies 12. 3 liters at a pressure of 40. 0 mm Hg
A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg?

33. A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure becomes 3.00 atm?

34. Combined Gas Law Examples
500.0 liters of a gas are prepared at 10 atm and °C. The gas is placed into a tank under high pressure. When the tank cools to 20.0 °C, the pressure of the gas is 30.0 atm. What is the volume of the gas?

35. What is the volume of gas at 2. 00 atm and 200
What is the volume of gas at 2.00 atm and K if its original volume was L at atm and K?

36. A gas balloon has a volume of 106. 0 liters when the temperature is 45
A gas balloon has a volume of liters when the temperature is 45.0 °C and the pressure is mm of mercury. What will its volume be at 20.0 °C and mm of mercury pressure?

37. A gas is heated from K to K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?

38. 73. 0 mL of nitrogen at STP is heated to 80
73.0 mL of nitrogen at STP is heated to 80.0 °C and the volume increase to 4530 mL. What is the new pressure?