1. Mixed Gas Law Calculations

2. Common Core Connection
Objectives:
Today I will be able to:
Apply Boyle, Charles, Gay-Lussac, Combined, Ideal, and Dalton’s gas law to solving problems
Informal assessment – monitoring student interactions and questions as they complete the practice problems
Formal assessment – analyzing student responses to the practice problems and exit ticket
Common Core Connection
Make sense of problems and persevere in solving them
Reason abstractly and quantitatively

3. Lesson Sequence Evaluate: Warm – Up Explain: Dalton’s Law
Elaborate: Dalton’s Law Practice
Elaborate: Mixed Gas Law Problems
Evaluate: Exit Ticket

4. Warm - Up
Carbon dioxide gas occupies a volume of 200 ml at STP. What is the density of the gas?
How do I know when to use the combined gas law, ideal gas law and graham’s law to solve problems?

5. Objectives Today I will be able to:
Apply Boyle, Charles, Gay-Lussac, Combined, Ideal and Dalton’s gas law to solving problems

6. Homework
Finish practice problems

7. Agenda Warm Up Mixed Homework Review Ideal Gas Law
Ideal Gas Law Practice
Dalton’s Law Notes
Dalton’s Law Practice
Exit Ticket

8. Lets look over the homework together!
Mixed Gas Law Homework
Lets look over the homework together!

9. Kinetic Molecular Theory, Ideal Gas Law

10. Kinetic Molecular Theory of Gases
Gases consist of small particles, either atoms or molecules, that have mass
Gas particles must be separated from each other by relatively large distances
- While gases do have volume, that volume is considered to be zero, which is why we say the volume of a gases’ container is the volume of the gas

11. Kinetic Molecular Theory of Gases
Gas particles must be in constant, straight-line, rapid motion
- Explains why when you spray a bottle of perfume at one end of the room, the people at the other end are able to smell it right away
- Gases diffuse rapidly

12. Kinetic Molecular Theory of Gases
Gases exert pressure because their particles collide with the walls of the container
-Think about blowing up a balloon – the balloon blows up evenly because gas particles are hitting all points of the inside walls the same

13. Kinetic Molecular Theory of Gases
Gas particles exert no force on one another – they neither attract or repel
- It is true enough for our class

14. Kinetic Molecular Theory of Gases
Gas particles may collide with each other, but these collisions are assumed to be elastic
- Think about playing pool – you transfer kinetic energy from your stick to the cue ball to make it move

15. Kinetic Molecular Theory of Gases
The average kinetic energy of the gas particles depends on the temperature of the gas
- Gas particles do not all have the same kinetic energy – some move slowly and some move very fast, but most are in between

16. Elastic

17. Inelastic

18. Kinetic Molecular Theory of Gases
A gas that obeys all these “rules” is called an Ideal Gas
No gas will obey all the “rules,” but some are close enough
Nonpolar gases at high temperatures and low pressure are very close

19. Ideal Gas Law PV = nRT P = pressure V = volume (use only L)
n = number of moles of gas
R = constant (.0821 atm-L/mol-K or 62.4 mmHg- L/mol-K)
T = temperature in Kelvin

20. Complete the practice at your desk!
Ideal Gas Law Practice
Complete the practice at your desk!

21. Dalton’s Law

22. Dalton’s Law of Partial Pressures
The sum of the pressures of all gases present in a system equals the total pressure of the system
P1 + P2 + P3 + … = Pt

23. Dalton’s Law Practice
Complete the practice at your desk. If you have questions, please ask Mr. Klotz. We will review selected problems

24. Exit Ticket Which problem was most challenging on the worksheet
What strategies did you use to determine which gas law you needed to use to solve the problem?