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Understanding Gas Behavior: Pressure, Boyle's Law, and Charles's Law Explained

This chapter explores the behavior of gases focusing on pressure, Boyle's Law, and Charles's Law. Gas particles are in constant motion, leading to pressure measured in pascals (Pa). The text explains how decreasing container size increases pressure due to more frequent particle collisions, and how heating gas increases its volume, illustrated with practical examples like weather balloons and spray canisters. Utilizing equations, it highlights the relationships between pressure, volume, and temperature in gas behavior.

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Understanding Gas Behavior: Pressure, Boyle's Law, and Charles's Law Explained

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Presentation Transcript

  1. Chapter 16 Section 3 Behavior of Gases

  2. Pressure • Gas particles are constantly moving and colliding, which results in pressure (Force/area) • Containers (balloons, tires) remain inflated because particles collide with the walls of the container • If more particles of gas are pumped into the container, there will be more collisions and the walls will be pushed further outward

  3. Pascal • Pressure is measured in pascals (Pa) • 1 Pa = 1 N/1m2 • 1000 Pa = 1 kPa • At Earth’s surface, the atmosperic pressure = 101.3 kPa • 101,300 N per square meter

  4. Boyle’s Law • What happens to gas pressure if you decrease the size of the container? • Particles will strike each other and the walls more often, increasing pressure • If you give the gas particles more space, they will hit the walls less often, pressure will decrease • Weather balloons

  5. Boyle’s Law in Action (Volume-Pressure Equation) • A balloon has a volume of 10.0 L at a pressure of 101 kPa. What will be the new volume when the pressure drops to 43.0 kPa? • P1V1 = P2V2 • 101 x 10.0 = 43.0 x V2 • 1010 = 43.0 x V2 43.0 43.0 • 23.5 L = V2

  6. The Pressure-Temperature Relationship • Why do you need to keep pressurized spray canisters away from heat? • Hotter temp. = faster moving particles (more collisions with the walls) • Volume can’t be increased (rigid canister) • Pressure increases • Canister will explode

  7. Charles’s Law • Gases expand when they are heated (hot air balloons) • Hot air is less dense than cool air • The volume of gas increases with increasing temp. (also, the volume of gas decreases with decreasing temp) • Gas is heated  particles move faster  particles strike the walls of their container more often and with more force  Larger volume

  8. Using Charles’s Law • Temperature must be in Kelvin • V1 = V2 T1 T2 • What would be the resulting volume of a 2.0 L balloon at 25 C that was placed in a container with ice water at 3 C ? • T1 = 25 C + 273 = 298 K • T2 = 3 C + 273 = 276 K • 2 = V2 298 276 • 2 x 276 = 298 x V2 • 552 = 298 x V2 • 1.9 L = V2

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