1. Behavior of Gas Molecules
IDEAL GAS LAW AND
GAS STOICHIOMETRY

2. Essential Questions
Since we ignore the volume and mass of gas molecules, can we assume anything about the volume all gases occupy?
Can we apply this information to solve for the three properties of gases: temperature, volume, and pressure?
Can we apply this to solve stoichiometry problems?

3. How can we increase volume
Quick: What are all of the ways you can think of to increase the volume of a balloon?

4. Avogadro’s Principle
Even though particles that make up gases vary greatly in size, KMT tells us to ignore particle size when talking about the volume a gas occupies.
Therefore, we can say 1000 krypton gas particles occupies the same volume as 1000 helium particles!
Avogadro first proposed this idea in 1811

5. Avogadro’s Principal
States that the same number of particles at the same temperature and pressure contain equal volumes of gases!
1 mol contains 6.02 x 1023 particles
STP is Standard Temperature and Pressure
273K and 1.00 atm pressure (STP)
Avogadro’s Law states that one mole of any gas at Standard Temperature and Pressure (STP) occupies 22.4 Liters of volume
Therefore we can use L/mol as a conversion factor

6. Molar Volume Conversions
1. Find the number of moles in a sample of gas that has a volume of 5.32 L at STP?
Use the molar volume to convert from volume to moles
5.32 L X 1 mol = mol
22.4 L

7. Molar Volume Conversions
The main component of natural gas used for home heating and cooking is methane (CH4). Calculate the volume that 2.00kg of methane gas will occupy at STP.
Answer: 2,800 liters

8. Check for Understanding
Try some molar volume problems on your own

9. IDEAL GAS LAW
Now that we know that one mole of all gases occupy the same volume, we have a NEW Gas Law to introduce
While the Combined Gas Law deals with the relationship of gas properties under changing conditions
The Ideal Gas Law uses the basis of that relationship and applies it to a known set of conditions of those properties and the amount of gas that is present using Avogadro’s Law.

10. Ideal vs. Real Gas Ideal Gas Motion is totally random and linear
All gas particle collisions are elastic
Gas particles do not have any intermolecular attraction
Gas particles have no volume
Real Gas
Motion is almost but not quite random
Gas particle collisions are not perfectly elastic
Gas particles experience very small intermolecular attraction
Gas particles do have small amount of volume

11. Ideal Gas Law
Known as the Ideal Gas Law because it works best for gases that obey the assumptions of the kinetic molecular theory!
P V = n R T
We know what these stand for:
P = Pressure
V = Volume
n = Number of moles
T = Temperature (in Kelvin)
But, what is R?
Notice there are no 1’s and 2’s because the conditions are NOT changing!

12. UNIVERSAL GAS CONSTANT - R
By selecting the values for standard conditions, the value of the constant can be determined:
Standard value for Temperature = 273K
Standard value for Pressure = 1 atm
Standard value for the amount of gas = 1 mole
Standard value for volume = 22.4L
Let’s solve for R: 12

13. Ideal Gas Law Practice
1. Calculate the number of moles of ammonia gas (NH3) contained in a 3.0 L vessel at 300K with a pressure of 1.5 atm.

14. Ideal Gas Law
2. What volume will 2.0 moles of nitrogen occupy at 720 torr and 20oC?
remember that 1.0 atm = 760 torr and that temperature must be in Kelvins

15. Ideal Gas Law
Find the number of grams of CO2 that exert pressure of 785 torrs at a volume of 32.5 L and a temperature of 32oC.
STOP: work on completing Chem Worksheet 14-4

16. Ideal Gas Law Demo Glass Florence flask with stopper with glass tube.
Add a small amount of water and bring it to boiling
Invert over an ice bath

17. Demo
As we heat the flask, the temperature increases and the pressure inside the flask increases. Water vapor replaces the air in the flask.
After inverting, the temperature rapidly decreases, converting the water vapor back into liquid water therefore decreasing the volume of the gases.
Water rushes in to try to increase the pressure to make up for the decrease in temperature and volume.

18. Check for understanding
Try some ideal gas law problems

19. BE LAZY And don’t memorize the gas laws! Tyler Dewitt
(7:09)

20. GAS STOICHIOMETRY
Avogadro’s Law allows for the application of volume ratio to replace mole ratio to compare any two gases in stoichiometric calculations.
You will see two different types of problems:
Volume to volume problems
Volume to mass problems

21. GAS STOICHIOMETRY
Volume to Volume: What volume of hydrogen is necessary to react with 5L of nitrogen to produce ammonia?
(assume constant temperature and pressure)
a) balance the equation
b) volume to volume ratio
c) what volume of ammonia is produce?
___N2 + ___H2  NH3

22. ___C3H8 + ___O2  ___CO2 + ___H2O
GAS STOICHIOMETRY
2. Volume to Volume: If 20 liters of oxygen are consumed in the above reaction, how many liters of carbon dioxide are produced?
Balance the equation
volume to volume ratio
___C3H8 + ___O2  ___CO2 + ___H2O

23. ___N2 (g) + ___H2 (g)  ___NH3 (g)
GAS STOICHIOMETRY
3. Volume to mass problems: Ammonia is synthesize from hydrogen and nitrogen. If 5.0 L of nitrogen react completely with hydrogen at a pressure of 3.00 atm and temperature of 298 K, how much ammonia, in grams, is produced?
___N2 (g) + ___H2 (g)  ___NH3 (g)

24. ___Fe (s) + ___O2 (g)  ___Fe2O3 (s)
GAS STOICHIOMETRY
4. Volume to mass problem: When iron rusts, it undergoes a reaction with oxygen to form iron (III) oxide. Calculate the volume of oxygen gas at STP that is required to completely react with 55.9 grams of iron.
___Fe (s) + ___O2 (g)  ___Fe2O3 (s)