1. Unit 6 Test NEXT CLASS Practice and Review Today

2. Review and Practice Make tables into groups. For each question, work with your group to find a solution or answer. Every member be prepared for discussion/explanation of each question. Make note of the types of questions being asked  TEST MATERIAL!

3. Chapter 13 Kinetic Theory for Solids, Liquids, and Gases Properties and Behaviors of Solids, Liquids, and Gases Allotropes Phase Changes Phase Diagrams Unit Conversions (Temperature and Pressure) Notes E and F

4. Q1 Review the kinetic theory, then… Use kinetic theory to explain what causes gas pressure.

5. Q2 Convert the following pressures to kilopascals. 0.95 atm 45 mm Hg

6. Q3 In terms of kinetic energy, explain how a molecule in a liquid evaporates.

7. Q4 How are particles arranged in solids? How do allotropes of an element differ?

8. Q5 Which has a higher melting point? An ionic compound or a molecular compound? Why?

9. Q6 When discussing phases changes, what is happening when he following occur? Sublimation Condensation Vaporization Deposition Melting Freezing

10. Q7 What is a phase diagram? Describe in no more than two sentences.

11. Q8 What does the triple point on the phase diagram describe?

12. Q9 According to the phase diagram, at what temperature and pressure does the triple point occur? Include units!!!!!!

13. Q10 How many boiling points does water have? How many melting points? Careful! Trick Question

14. Q11 According to the phase diagram, estimate the boiling point of water at 50 kPa.

15. Q12 What happens to the average kinetic energy of your body when you have a fever? What happens to the temperature of a substance when the average kinetic energy decreases?

16. Q13 Predict the physical state (solid, liquid, or gas) of each substance at the indicated temperature. Use the data below to help. Ammonia -25 Degrees Celsius Phenol at 99 Degrees Celsius Methanol at -100 Degree Celsius Methanol in an ice water bath SubstanceMelting Point (Degree Celsius) Boiling Point (Degrees Celsius) ammonia-77.7-33.4 methanol-97.764.7 phenol40.9181.9

17. Chapter 14 Properties of Gases: Compressibility Factors Affecting Gas Pressure The Gas Laws: Boyles, Charles, Gay-Lussac Direct and Inverse Proportions and what their graphs look like Combined Gas Law Ideal Gas Law Gas Mixtures and Movement: – Dalton’s Law, Grahams Law, Diffusion, and Effusion Notes G and H

18. Q1 Why is a gas easy to compress?

19. Q2 List three factors that can affect gas pressure. Are they inversely or directly proportional?

20. Q3 What are the three Gas Laws and their mathematical expressions? Identify if they represent direct or inverse relationships.

21. Q4 Illustrate each gas law by sketching a graph for each gas law. (Use their inverse/ direct relationship)

22. Q5 What is the mathematical expression for the combined gas law? Why do we use the combined gas law?

23. Q6 He gas in a closed container is 300 kPa at 303K. What will he pressure be if the temperature is lowered to 101K?

24. Q7 Calculate the volume of a gas at a pressure of 100 kPa if its volume at 120 kPa is 0.150L.

25. Q8 Show how Gay-Lussac’s law can be derived from the combined gas law.

26. Q9 A gas at 155 kPa and 25 degrees Celsius has an intial volume of 1.00L. The pressure of the gas increases to 605 kPa as the temperature is raised to 125 degrees Celsius. What is the new volume?

27. Q10 How do ideal gases differ from real gases? What is the ideal gas law equation?

28. Q11 What pressure is exerted by 0.450 mol pf a gas at 25 degrees Celsius if the gas is in a 0.650L container?

29. Q12 A child’s lungs can hold 2.20L. How many moles of air do her lungs hold at a pressure of 102 kPa and a body temperature of 37 degrees Celsius?

30. Q13 In a mixture of gases, how is he total pressure determined? What law is this?

31. Q14 A gas mixture containing oxygen, nitrogen, and carbon dioxide has a total pressure of 32.9 kPa. If P O2 = 6.6 kPa and P N2 = 23.0 kPa, what is P CO2 ?

32. Q15 What distinguishes effusion from diffusion? How are these similar?

33. Q16 What is the mathematical expression for Graham’s Law of Effusion?

34. Q17 What is the effect of molar mass on rates of diffusion and effusion?

35. Q18 Calculate the ratio of helium atoms to the velocity of Neon molecules at the same temperature.

36. BONUS Convert the following into Kelvin: – 25 Degrees Celsius – 100 Degrees Celsius