SOLID 1. Make sure your state of matter is set on solid. Write your observations below:

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1 Chemistry Ms. Ye Name Date Block Properties of Matter: Particle Movement Part 1: Follow the instructions below to complete the activity. Click on the link to open the simulation for this activity: you will need to download the file and then open the simulation. Java needs to be up to date. SOLID 1. Make sure your state of matter is set on solid. Write your observations below: 2. Move the temperature bar down to cool the solid to 0K and make your observations below: 3. Move the temperature bar up to heat the solid to 30K and make your observations below:

2 LIQUID 1. Make sure your state of matter is set on liquid. Write your observations below: 2. Move the temperature bar down to cool the liquid from 26 K to 13 K and make your observations below: 3. Move the temperature bar up to heat the liquid from 26 K to 35 K and make your observations below: GAS 1. Make sure your state of matter is set on gas. Write your observations below: 2. Move the temperature bar down to cool the gas from 55 K to 35 K and make your observations below: 3. Move the temperature bar up to heat the gas from 55 K to 95 K and make your observations below: FINAL SUMMARY: Temperature is a form of energy. When you cool down the system, you are removing the energy from the system. When you heat up the system, you are adding energy to the system. Write an explanation of particle movement when energy is removed and added to the system. Use evidence to support your claim

3 Kinetic Molecular Theory (KMT) of Gases Go to: Run the java application. Our fundamental understanding of ideal gases makes the following 4 assumptions. Play with the simulation and describe/draw how each of these assumptions is represented in the simulation. Assumption of KMT Representation in Simulation 1. Gas particles are small and separated by relatively large distances. 2. Gas molecules are constantly in random motion and undergo elastic collisions with each other and the walls of the container. (elastic collisions mean the particles don t lose energy after a collision) 3. Gas molecules are not attracted or repulsed by each other. 4. The average kinetic energy of gas molecules in a sample is proportional to temperature (in K).

4 Kinetic Molecular Theory States that particles of matter are always in Explains properties of gases, liquids, and solids in terms of energy using an ideal gas Ideal Gas an which fits all the assumptions of kinetic molecular theory ***Note: An IDEAL GAS is THEORETICAL and is used to PREDICT the behavior of REAL GASES (O2, H2, He, etc.). The ASSUMPTIONS above are not true of REAL GASES. Problems with KMT: 1. Gas atoms/molecules 2. exist between gas molecules 3. Small volume containers result in between gas molecules Conditions in which a REAL GAS behaves MOST like an IDEAL GAS: (fast moving) (more space to move, less likely to collide) Physical Characteristics of Gases:

5 Variables that Define Gases - how much space a gas takes up; may be expressed in liters, milliliters, cm 3, dm 3. Always expressed in Kelvin!!!! to convert between C and Kelvin, you can use the following formula (yes you must know it!): Temperature Conversion Examples: 1. The temperature of the room was measured to be 25 C. What is this temperature in Kelvin? 2. If the boiling point of a substance was measured to be 300K, what is this temperature in C? - how many particles are present in the sample of gas -the force per unit area on a surface o Exerted by all gases on any surface they collide with o cause pressure! o Units of Pressure: Pascal = Pa (SI unit of pressure); Millimeter of mercury = mmhg (used in a barometer); Torr = torr; Atmosphere = atm (pressure of the atmosphere at sea level=1atm) 1 atm = Pressure Conversion Examples: 1. What is the pressure in torr of 345mmHg? 2. What is the pressure in atm of 123 kpa?

6 Barometer o used to measure o The higher the altitude the the atmospheric (air) pressure and the the height of the mercury in the thermometer Manometero measures the pressure of an enclosed sample o Can be open or closed Gas pressure is than atmospheric (air) pressure when the height of the liquid in the manometer is higher on the. Therefore you will the height and the atmospheric pressure. Gas pressure is than atmospheric (air) pressure when the height of the liquid in the manometer is higher on the. Therefore you will the height and the atmospheric pressure. Examples: If the atmospheric (air) pressure is 757.8mmHg, what is the pressure of the gas in each of the following manometers?

7 PRACTICE: Convert the following temperatures. 1. Convert 32 C to Kelvin 2. Convert 12 C to Kelvin 3. Convert 450 K to C Convert the following pressures. 1. What is pressure of 1.45 atm in torr? 3. What is the pressure of 645 mmhg in kpa? 2. What is the pressure of 890 torr in Pa? Calculate the pressure for each gas in the following open manometers

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