Discovery 2-1: Energy & Motion A. States of Matter Part 1: Properties of the States of Matter 1. Watch the three short Eureka videos (solids-16, liquids-17, gases-18) and read your textbook on the states of matter. Write down key points about each phase of matter at the particle level. Part 2: Diffusion of Gases 2. Briefly describe (or draw) the set-up. Record your observations. 3. Prepare a storyboard showing how the arrangement of particles changed over the time from when the bottle was opened until the odor had permeated the room. 4. What must matter be like at its simplest level to explain your observations? Part 3: Diffusion of Liquids in Hot and Cold Liquids 5. Briefly describe (or draw) the set-up. Record your observations. 6. Prepare a storyboard showing how the arrangement of particles changed over the time in both the cold water and the hot water. 7. Relate the impact of energy on matter to explain your observations. Part 4: Thermal Expansion of Liquids 8. Briefly describe (or draw) the set-up. Record your observations. 9. Draw a storyboard explaining your observations at the particulate level for the red liquid (alcohol) and the blue liquid (water). Why did the liquid in one tube rise higher than the other? 10. What property of matter best describes the way a typical alcohol thermometer works? Explain (in terms of energy transfer) why the alcohol level in the thermometer rises (or falls) when you place the thermometer in contact with warmer (or colder) objects. B. Kinetic Molecular Theory (KMT) & Pressure The Kinetic Molecular Theory (KMT) is a model used to describe the forces between molecules and the energy that they possess. We will be focusing on how the KMT applies to gases and their behavior. Read Chapter 11.1-11.3 in your textbook. Answer the following questions. 1. List the key points of the KMT. Leave space between each for additional notes. 2. How does the KMT explain gas pressure? 3. Convert pressure measurements from one system of units to another in the following problems. 1 atm = 760 mmHg = 760 torr = 101.3 kPa = 14.7 psi (pounds per square inch) = 29.92 inHg a. 320 mmHg to atm. b. 30.0 psi to mmHg c. 90.5 kPa to atm d. 28.9 inHg to atm For Problems #4-5, calculate the pressure of the gas in the flask connected to the manometer.

6. Observe and explain the pressure activities (Pop Can & Index Card/Glass). C. Behavior of Gases In this discovery, we will be exploring the relationships between pressure, volume, temperature, and amount of gas. We will collect data using a LabQuest, pressure sensors and temperature sensors. Part 1: Pressure vs. Volume Relationship We will change the volume of the gas in a syringe and measure the effect on the pressure of the gas. The temperature and the amount of gas in the syringe remain constant. 1. Draw a picture of the graph. Label the axes. 2. When the volume decreases, the pressure . This is a (direct/inverse) relationship. Write a mathematical description of the relationship. 3. Pick three points (label them 1, 2, 3) on your graph. Draw a particle diagram (label them 1, 2, 3) for each point on the graph. Then, write a verbal explanation for why this relationship occurs (think particles and collisions). Part 2: Pressure vs. Number of Particles Relationship We will change the number of gas particles in a syringe and measure the effect on the pressure of the gas. The temperature and volume of gas in the syringe remain constant. 4. Draw a picture of the graph. Label the axes. 5. When the number of particles increases, the pressure . This is a (direct/inverse) relationship. Write a mathematical description of the relationship. 6. Pick three points (label them 1, 2, 3) on your graph. Draw a particle diagram (label them 1, 2, 3) for each point on the graph. Then, write a verbal explanation for why this relationship occurs (think particles and collisions). Part 3: Pressure vs. Temperature Relationship We will change the temperature of the gas in a syringe and measure the effect on the pressure of the gas. The volume and the amount of gas in the syringe remain constant. 7. Draw a picture of the graph. Label the axes. 8. When the temperature increases, the pressure . This is a (direct/inverse) relationship. Write a mathematical description of the relationship. 9. Pick three points (label them 1, 2, 3) on your graph. Draw a particle diagram (label them 1, 2, 3) for each point on the graph. Then, write a verbal explanation for why this relationship occurs (think particles and collisions). D. Gas Law Problems For each problem: a. Make a PVnT table. Fill in the given initial and final values for P, V, n, or T. b. Make a decision as to how a change in P, V, n, or T will affect (Increase or Decrease) the starting quantity. c. Multiply by the appropriate factor to get the final value. Show your work below or next to the table. d. Draw particle diagrams of the initial and final conditions.

1. What would be the new pressure if 250 cm3 of gas at standard pressure is compressed to a volume of 150cm3? 2. A closed flask of air (0.250L) contains 5.0 “puffs” of particles. The pressure probe on the flask reads 93 kPa.

A student uses a syringe to add an additional 3.0 “puffs” of air through the stopper. Find the new pressure inside the flask. 3. The pressure in a bicycle tire is 105 psi at 25˚C. You take the bicycle up a mountain, where the temperature is – 5˚C. What is the pressure in the tire? 4. A sample of gas occupies 150 mL at 25˚C. What is its volume when the temperature is increased to 50˚C? (P and n = constant) 5. Sam’s bike tire contains 15 units of air particles and has a volume of 160mL. Under these conditions the pressure reads 13 psi. The tire develops a leak. Now it contains 10 units of air and has contracted to a volume of 150mL. What would the tire pressure be now? 6. What would be the new volume if 250 cm3 of gas at 25˚C and 730 mm pressure were changed to standard conditions of temperature and pressure? 7. A 350 mL sample of gas has a temperature of 30˚C and a pressure of 1.20 atm. What temperature would needed for the same amount of gas to fit into a 250 mL flask at standard pressure?