1. Gas PropertiesGas Properties Chemistry: Gas Laws Review Learning Goals: Design experiments to measure the relationships between pressure, volume, and temperature. Create graphs based on predictions and observations. Make qualitative statements about the relationships between pressure, volume and temperature using molecular models. Previous knowledge: Students are able to describe a molecular model of gas pressure.

2. 1.P 1 /T 1 = P 2 /T 2 2. 1.As pressure increases, volume decreases 2.Direct relationship between volume and temperature 3.PV = nRT 4.Law that allows for respiration! 5.Law involving the direct relationship between moles and pressure/volume Warm up Number 1-7: Name the law… 1.Gay-Lussac 2.Combined Gas Law 3.Boyles 4.Charles 5.Ideal gas law 6.Boyles 7.Ideal

3. 8. Whose Law? Gay Lussac Law

4. 9. Whose law? BOYLE P 1 (V 1 ) = P 2 (V 2 ) 11. This is a direct relationship. True or False? F

5. 10. Whose Law? Charles’ Law V 1 / T 1 = V 2 / T 2 11. This is a direct relationship. True or False? T

6. 11. Name the law… Boyle’s Law Allows for respiration!

7. 12. What does this graph indicate?

8. 13. What variables were held constant? A.Pressure and Volume B.Pressure, number of particles, and Volume C.Number of particles and temperature D.Volume, number of particles and temperature

9. 14. What does this graph indicate?

10. 15. Which explanation could be used to explain the relationship between temperature and pressure for gases? A.Pressure depends on the number of collisions and if the temperature increases, the molecules increase speed, so they would hit the sides more and the pressure would go up. B.Pressure depends on the energy of collisions and if the temperature increases, the molecules increase speed, so they would hit the sides with more energy and the pressure would go up. C.Both help explain D.Neither help explain

11. 16. What are the properties of gas? (#1 on study guide) 17. What units are used to measure pressure and what factors affects pressure? 1.Expansion: 2.Fluidity: 3.Low density: 4.Compressibility: 5.Diffusion and effusion: Atm, kPa, mmHg, torr Affected by: Kinetic theory (collisions) Pressure Volume Temperature

12. Absolute zero https://www.youtube.com/watch?v=f1eAO ygDP5shttps://www.youtube.com/watch?v=f1eAO ygDP5s https://www.youtube.com/watch?v=g97Mz BArEkMhttps://www.youtube.com/watch?v=g97Mz BArEkM

13. Math problems! Work on the gas law problems in your study guide, #23-34 –Solve on a separate sheet of paper (show work) and attach to study guide

14. List the things that affect gas pressure and draw graphs and equations that shows the correct relationships.

15. Gas Laws with just 2 variables P 1 V 1 = P 2 V 2 Remember that the other variables must be held constant

16. 6. You are flying from Denver (high altitude) to Boston (low altitude), and you bring along a ½ full bottle of shampoo that was well sealed before you left Denver. You land in Boston and proceed to your hotel. The number of air molecules within the shampoo bottle: A. has decreased B. has stayed the same C. has increased

17. 7. If the walls of the shampoo bottle are strong and rigid so that the bottle has the same shape as before you left Boston (low altitude), how does the pressure of the air inside the bottle compare to the pressure of the air in Denver (higher altitude)? A.less than B.equal to C.greater than

18. 8. How does the pressure inside the bottle compare to the pressure of the air in Boston? A.less than B.equal to C.greater than

19. 9. If you had a water bottle with very soft sides. When you open your suitcase in Boston (lower altitude), the bottle would look A.squished B.same size C.puffed out

20. People who climb the tallest mountains in the world often use oxygen tanks to help them breathe. If a mountain climber asked you to explain the physics behind the “thin air”, what would you say to him?

21. Which is most likely oxygen gas? ABCABC

22. How could material be the same temperature and yet have different Phase? Different pressures Neon Liquid-Gas Like water- water vapor in a water bottle