1. Ideal Gas Law

2. Kinetic Molecular Theory
We will use pressure instead of force to describe gases. This is because of the nature of gases which is described by the Kinetic Molecular Theory.
1. Gases are made of tiny particles.
2. These particles are always in high speed random motion.

3. Kinetic Molecular Theory
Image by Becarlson
3. The particles of gas collide with the wall of their container without losing any momentum. The force of the gas that is exerted over the surface of the container is what we measure as pressure.

4. NO! Some molecules will travel faster than others.
4. The speed of these particles is related to the temperature of the system.
Temperature is the measure of the average kinetic energy of the particles in a system.
Since temperature is an average, will all of the molecules be going at the same speed?
NO! Some molecules will travel faster than others.

5. Boyle’s Law
Robert Boyle published his findings on the relationship between the pressure and volume of a gas in He determined that they were inversely proportional and behaved according to the equation found on your reference sheet.

6. Charles’ Law
Jacques Charles discovered the relationship between the volume and temperature of a gas during the 1780s. He determined that they were directly proportional and behaved according to the equation found on your reference sheet.

7. Avogadro’s Law
1 mole
2 mole
Amedeo Avogadro hypothesized the relationship between the volume and number of moles of a gas in He determined that they were directly proportional and behaved according to the equation found on your reference sheet.

8. This is Dalton’s Law of Partial Pressures
Sometimes more than one type of gas will be inside a container. Each one of these gases exerts part of the total pressure. If you add up each of the gases individual pressures, you will get the total pressure inside of a container.
This is Dalton’s Law of Partial Pressures 8

9. Partial Pressures PTotal = 450 kPa + 220 kPa + 100 kPa
What is the pressure inside a container if it contains neon gas at a pressure of 450 kPa, helium gas at a pressure of 220 kPa and nitrogen gas at a pressure of 100 kPa?
PTotal = 450 kPa kPa kPa
PTotal = 770 kPa

10. Partial Pressures 10 atm = 3 atm + 2 atm + PNe
A container holding argon, neon and nitrogen gas has a total pressure of 10 atm. What is the partial pressure being exerted by neon if the argon gas exerts a pressure of 3 atm and the nitrogen gas exerts a pressure of 2 atm?
10 atm = 3 atm + 2 atm + PNe
10 atm – 3 atm – 2 atm = PNe
PNe = 5 atm 10

11. Complete the questions on your notes using Dalton’s Law of Partial Pressures.
720 kPa
3.7 atm

12. 3. millimeters of mercury (mm Hg)
Measuring
Pressure
There are 3 units of pressure that we will focus on in this class:
1. atmospheres (atm)
2. kilopascals (kPa)
3. millimeters of mercury (mm Hg)

13. Converting Between Temperature Scales
Absolute Zero
0 K = -273 oC
Kelvin = oC + 273
oC = K - 273
Important Fact: In order for our gas law equations to work correctly, temperatures must ALWAYS be in Kelvin!

14. Ideal Gas
Both the Combined Gas Law and the Ideal Gas Law is based on the idea of an ideal gas. An ideal gas is a gas that:
(1) does not take up any space
(2) its particles do not interact with each other.
While there is no such thing as an ideal gas, most gases behave very closely to ideal when they are at low pressures and low temperatures. This allows us to make predictions that are very close to the truth. 14

15. This number (R) is known as the
The Ideal Gas Constant
The reason that the combined gas law allows us to predict how changing the pressure, volume, temperature or amount of gas will affect the system is because (PV)/(nT) always equals the same number.
P1V1 P2V2
n1T1 n2T2 =
P1V1
n1T1 = R
This number (R) is known as the
ideal gas constant, and it can be easily calculated from a set of known information. 15

16. Standard Temperature and Pressure
Standard Temperature and Pressure (STP) is an agreed up set of variables that all scientists can use to study gases and describe their properties.
The volume of 1 mole of ideal gas at STP is 22.4 liters. This information is also found on your formula chart.
We will use this information to calculate the value of R. 16

17. Convert Celsius into Kelvin:
The Ideal Gas Constant
Convert Celsius into Kelvin:
0oC = 273 K
P V
n T = R
(1 atm)(22.4 L) = R
(1 mol)(273 K)
R = L·atm/mol·K 17

18. The Ideal Gas Constant P V n T = R = R P V n T = R = R
We also need to calculate what R would be if either of the other units of pressure are used.
P V
n T = R
(760 mm Hg)(22.4 L) = R
(1 mol)(273 K)
R = 62.4 L·mm Hg/mol·K
P V
n T = R
(101.3 kPa)(22.4 L) = R
(1 mol)(273 K)
R = 8.31 L·kPa/mol·K

19. The Ideal Gas Constant How will you know which one to use?
These values can all be found on your
Chemistry STAAR Reference Sheet.
How will you know which one to use?
You will always use the value of R that matches the units of pressure used in the problem.

20. The Ideal Gas Constant PV = nRT PV nT = R nT × × nT
We can now rearrange this equation into what we call the Ideal Gas law. PV nT = R
nT ×
× nT
PV = nRT 20

21. The Ideal Gas Law
While the Combined Gas Law allows us to predict how changing one variable will affect the others, the Ideal Gas Law allows us to completely define a single set of variables for a system.
The Ideal Gas Law can be used to determine the number of moles in a system, or it can be used to predict the pressure or volume a certain amount of gas will have at a given temperature.

22. The Ideal Gas Law PV = nRT
How many moles of an ideal gas are present in a 2.00 L container at 20.0oC if the gas is exerting a pressure of kPa?
Which R value do you use?
Convert Celsius into Kelvin:
20oC = 293 K
PV = nRT
(200.0 kPa)(2.00 L) = n (8.31 L·kPa/mol·K)(293 K)
n = (200.0 kPa)(2.00 L)
(8.31 L·kPa/mol·K)(293 K)
n = moles

23. The Ideal Gas Law PV = nRT Which R value do you use?
How large should a container be if it will not need to sustain a pressure greater than 10.0 atmospheres, it will contain no more than moles of gas and will be kept at a temperature of 25.0oC?
Which R value do you use?
Convert Celsius into Kelvin:
25oC = 298 K
PV = nRT
(10.0 atm) V = (100.0 mol)( L·atm/mol·K)(298 K)
V = (100.0 mol)( L·atm/mol·K)(298 K)
(10.0 atm)
V = 245 liters

24. Complete Ideal Gas Law problems at the end of your notes.24