1. Chapter 13 and 14

2. Essential Question: What are three units for pressure and how do you convert units? Warm-Up: What are the three states of matter? List one thing you know about each one.

3. How do solids, liquids and gases compare? Solids: Hold their shape, the particles are tightly packed, they are not easily compressed, and they do not flow

4. Liquids: Take the shape of their container, the particles are loosely packed, they are not easily compressed and they flow easily

5. Gases: Fill their container, the particles are far apart, are easily compressed and flow easily

6. What are the units for pressure and how to you convert between units of pressure? 1. Pascal (1000 Pa = 1kPa) 2. ATM (1 ATM = 101.3 kPa=760 mmHg) 3. mmHg 4. Bar 5. Torr 6. Psi

7. 1 ATM = 760 mmHg = 101.3 kPa 7. How many ATM are equivalent to 450 kPa?

8. Check-Out: 1. What are three units for pressure and how do you convert units? 2. How many ATM are equal to 1999 mmHg? (show your work)

9. Essential Question: What are the triple point and critical point of a substance? Warm-Up: 1. How many ATM in 893 mmHg? 2. How many kPa?

10. How is vaporization different from evaporation? 1. Vaporization- when the particles in a liquid have enough kinetic energy to escape the liquid and become a vapor/gas 2. Evaporation- when the particles at the surface become vapor because they have more kinetic energy than the others; occurs faster in hot liquids 3. Evaporation is a cooling process because it lowers the temperature of the liquid

11. What is the relationship between rate of evaporation and the rate of condensation? 1. Relates to liquids in a closed container 2. Particles evaporate and then condense and become a liquid again 3. In a system at constant vapor pressure the rate of evaporation equals the rate of condensation; vapor pressure is constant

12. What is the relationship between boiling point and temperature and boiling point and pressure? 1. When a liquid is heated to a temperature at which particles throughout the liquid have enough energy to vaporize the liquid begins to boil 2. Liquids do not boil at the same temperature 3. A liquid boils when its vapor pressure is equal to the external pressure; liquids at lower atmospheric pressure boil at a lower temperature 4. In a pressure cooker the vapor pressure increases, the water boils at a higher temperature (more than 100 C) and the food cooks faster

13. What are the various phase changes substance can undergo?

14. What does a phase change diagram represent? 1. The conditions of pressure and temperature at which two phases exist in equilibrium 2.

16. Check-Out: What are the triple point and critical point of a substance?

17. What are some properties of gases? 1. The particles of a gas are small, hard spheres with insignificant volume. 2. Their motion is rapid, constant and random. 3. Collisions are elastic.

18. What are the factors that affect gas pressure? 1. Amount of gas 2. Volume 3. Temperature

19. What are some common gases found in the Earth’s atmosphere? 1. Nitrogen 2. Argon 3. Carbon Dioxide 4. Oxygen

20. What happens to the volume of a gas as the pressure increases at a constant temperature? What is the equation that represents Boyle’s Law? If Volume increases, pressure decreases; if volume decreases, pressure increases Boyle’s Law is an inverse relationship V 1 P 1 = V 2 P 2

21. What happens to the volume of a gas as the temperature increases at constant pressure? What is the equation that represents Charles’s Law? If the temperature increases the volume will increase; if the temperature decreases the volume will decrease It is a direct relationship V1 = V2 T1 T2

22. What happens to temperature of a gas as the pressure increases if the volume stays the same? What is the formula used for represent Gay-Lussac’s Law? If the temperature increases the pressure will increase; if the temperature decreases the pressure will decrease It is a direct relationship T1 = T2 P1 P2

23. What is the equation for the ideal gas law? Real gases differ most from an ideal gas at low temperatures and high pressures; no gas is ideal PV= nRT P= pressure (ATM) V= volume (liters) T= Temperature (Kelvin) * 273 + C n = number of moles R=.0821 Liters x ATM/mol x K

24. What is Dalton’s Law? The sum of the individual pressures of all the gases that make up a mixture is equal to the total pressure P total= P1+P2+P3

25. How does diffusion differ from effusion? Diffusion is the movement of a gas from an area of high concentration to low concentration Effusion is when a gas escapes through a small hole in the container Gases of lower mass diffuse and effuse faster than gases of higher mass

26. How can effusion be compared?