1. Quick Write p126: What happens to a plastic bottle placed in the freezer overnight?

2.  Honor time limits  Actively participate (Have S.W.A.G.)  Listen respectfully to your colleagues  Place cell phones on vibrate or silent mode  Participants may write burning questions on a sticky note and place on the parking lot  BE PRESENT (Developing H.O.T.S. for Science)

3. Burning Issues Questions Comments Ideas to Share

4. Charles’ Law The Temperature-Volume Relationship

5. Charles’ Law French chemist J JJ Jacques Charles discovered that the volume of a gas at constant pressure changes with temperature. As the temperature of the gas increases, so does its volume, and as its temperature decreases, so does its volume.

6. C h a r l e s ’ L a w V= Volume k= Charles’ Law constant of Proportionality T= Temperature in Kelvin

7. Explanation Raising the temperature of a gas causes the gas to fill a greater volume as long as pressure remains constant. Gases expand at a constant rate as temperature increases, and the rate of expansion is similar for all gases.

8. Example If the temperature of a given amount of gas is doubled, for example, its volume will also double (as long as pressure remains unchanged). 2V = 2kT

9. Charles’ Law Charles’ Law can be modified to a convenient form by solving for k.

10. Charles’ Law In a sample with volume V 1 & temperature T 1, changing either volume or temperature converts these variables to V 2 & T 2.

11. Demonstration of Charles’ Law

12. Charles’s law states that when a gas is kept at constant pressure, the volume of the gas will change with temperature. In this experiment, balloons keep a small amount of gas (air) at an approximately constant pressure.

13. As the balloons are dipped into a beaker of liquid nitrogen (- 196°C; -320°F), the air inside them quickly cools. The volume of the air inside the balloons decreases as the temperature of the balloons decreases.

17. Relationship of Boyle’s Law and Charles’ Law

18. Temperature in kelvins Pressuree in kilograms per square centimeter

19. Practical Applications

20. Hot AIR Balloon The hot air that gives the hot-air balloon its name is commonly created by a propane gas burner that sends powerful jets of flame into the colorful rip-stop nylon envelope. Once the balloon is aloft, its height is maintained by opening and closing the blast valve, which controls the flow of the gas to the burner.

21. Charles’ Law Calculations

22. 1.Calculate the decrease in temperature when 2.00 L at 20.0 °C is compressed to 1.00 L. 2. 600.0 mL of air is at 20.0 °C. What is the volume at 60.0 °C? 3. A gas occupies 900.0 mL at a temperature of 27.0 °C. What is the volume at 132.0 °C? 4. What change in volume results if 60.0 mL of gas is cooled from 33.0 °C to 5.00 °C? 5. Given 300.0 mL of a gas at 17.0 °C. What is its volume at 10.0 °C? 6. A gas occupies 1.00 L at standard temperature. What is the volume at 333.0 °C? 7. At 27.00 °C a gas has a volume of 6.00 L. What will the volume be at 150.0 °C? 8. At 225.0 °C a gas has a volume of 400.0 mL. What is the volume of this gas at 127.0 °C? Abbreviations atm – atmosphere mm Hg - millimeters of mercury torr - another name for mm Hg Pa - Pascal (kPa = kilo Pascal) K - Kelvin °C - degrees Celsius Conversions K = °C + 273 1 cm 3 (cubic centimeter) = 1 mL (milliliter) 1 dm 3 (cubic decimeter) = 1 L (liter) = 1000 mL Standard Conditions 0.00 °C = 273 K 1.00 atm = 760.0 mm Hg = 101.325 kPa = 101,325 Pa

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