1. Chapter 14 The Behavior of Gases

2. Section 14.1 The Properties of Gases
OBJECTIVES:
Explain why gases are easier to compress than solids or liquids are.
Describe the three factors that affect gas pressure
Describe the relationships among the temperature, pressure, and volume of a gas.
Use the combined gas law to solve problems.

3. Compressibility
Gases can expand to fill its container, unlike solids or liquids
The reverse is also true: They are easily compressed, or squeezed into a smaller volume
Compressibility is a measure of how much the volume matter decreases under pressure

4. Gas Particle Compression in an Air Bag
This is the idea behind placing “air bags” in automobiles
Particles of gas (in the airbag) compress more than particles of solid (in the steering wheel or dash board)
The impact forces the gas particles closer together, because there
is a lot of empty space
between them

5. Variables that describe a Gas
The four variables and their common units:
1. Pressure (P) in kilopascals
2. Volume (V) in Liters
3. Temperature (T) in Kelvin
4. Amount (n) in number of particles
The amount of gas, volume, and temperature are factors that affect gas pressure.

6. Amount of Gas
When we add air to a bicycle tire, we are adding gas molecules.
More gas particles means more collisions
thus, the pressure increases
This is why the tire feels harder after pumping it up
Relationship:
# gas particles __, Pressure ___
Before pumping
After pumping

7. Pressure Gradient Gas particles naturally move from areas of
high pressure  low pressure
Example – whipped cream, hair spray, spray paint
Stored with air under high pressure
When you press the nozzle, the gas is free to move – and it move out of the can because atmospheric pressure is lower than the pressure inside the can.

8. Pressure Gradient
Why do the instructions on an aerosol can say to hold the can upright while spraying?
Compressed air is less dense than product, so air moves up…
Air enters the tube instead of product

9. Volume of Gas
In a smaller container, the molecules have less room to move.
The particles hit the sides of the container more often.
As volume decreases, pressure increases

10. Temperature of Gas Raising the temperature of a gas increases
the pressure, if the volume is held constant.
Remember, temperature is a measure of energy…
Gases at higher temp. have more kinetic energy:
The molecules hit the walls harder, and more frequently
What would happen if you threw an aerosol can into a fire?
What happens to a helium filled balloon on a cold day?
When should your car tire pressure be checked?
Heat from fire adds energy, as energy , temp.  and pressure .
When can can’t withstand pressure, it explodes.

11. Section 14.2 The Gas Laws Objectives
Describe the relationships among the temperature, pressure, and volume of a gas
Use the combined gas law to solve problems

12. The Gas Laws V, P T , V T, P
The relationships we talked about in section 1 are described by three gas laws:
Boyle’s Law – Pressure and Volume
If temperature is constant, as the volume of a gas is decreased, the pressure increases.
Charles’s Law – Temperature and Volume
If pressure is constant, as temperature of an enclosed gas increases, the volume increases
Gay-Lussac’s Law – Pressure and Temperature
If volume is constant, as temperature of an enclosed gas increases, the pressure increases
V, P
T , V
T, P

13. The Gas Laws GREAT NEWS! There is a catch…
All three laws can be combined into one called … the combined gas law!
Described the relationship among pressure, temperature and volume of an enclosed gas
Allows us to do calculations for situations in which only the amount of gas is constant
There is a catch…
All temperature measurements MUST be in Kelvin
Remember K = oC + 273

14. The Combined Gas Law
The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas.
“PLEASE VOMIT OVER TOILET”

15. Using the Combined Gas Law with
constant Temperature
If the temperature remains constant... P1 x V1 P2 x V2 = T1 T2

16. Using the combined gas law with constant Pressure
If the pressure remains constant... P1 x V1 P2 x V2 = T1 T2

17. Using the Combined Gas Law with constant Volume
If the volume remains constant... P1 x V1 P2 x V2 = T1 T2

18. Section 14.3 – Ideal Gases Objectives
Compare and contrast real and ideal gases

19. Ideal Gases
An ideal gas is a gas that obeys the gas laws under ALL conditions of temperature and pressure.
It does this because:
The particles themselves have no volume
There are no attractive forces between the particles
However… An ideal gas does not really exist!

20. Ideal Gases don’t exist, because:
Gas particles do take up space
- In other words, they do have volume
There are attractive forces between particles
- otherwise there would be no liquids formed

21. However, Real Gases behave like Ideal Gases ...
When the particles are very far apart and do not take up as big a % of the space
We can ignore the particle volume.
This happens at low pressure

22. Real Gases behave like Ideal Gases…
When particles are moving fast
This is at high temperature
Collisions are harder and faster.
Particles are not next to each other very long.
Attractive forces can not play a role.

23. Why we work with Ideal Gases
Although ideal gases do not really exist, real gases can behave like ideal gases at low pressure and high temperature, and so…
If we ASSUME a gas is ideal:
it is much easier to predict how it will behave,
the math is much easier
and in reality it is a very close approximation for how the real gas will behave.

24. Section 14.4 Gases: Mixtures and Movements
OBJECTIVES:
Relate the total pressure of a mixture of gases to the partial pressures of the component gases.

25. Dalton’s Law of Partial Pressures
Dalton’s Law of partial pressure states that at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
Let’s see what that looks like…

26. If the first three containers are all put into the 4th, we can find the pressure in the 4th container by adding up the pressure in the first 3:
= 6 atm
2 atm
+ 1 atm
+ 3 atm 1 2 4 3

27. Dalton’s Law of Partial Pressures
For a mixture of gases in a container,
PTotal = P1 + P2 + P
P1 represents the partial pressure of gas in container 1 (or the contribution that the gas in container 1 made to the total pressure)