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The Gas Laws

Learn about the kinetic molecular theory of gases and the properties of gases such as expansion, fluidity, low density, compressibility, and effusion/diffusion. Understand the abbreviations used and the units of pressure and temperature. Explore Boyle's Law, Charles' Law, Gay-Lussac's Law, and Avogadro's Law.

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The Gas Laws

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  1. The Gas Laws A Tutorial on the Behavior of Gases. Presented by: Mr. Forte Chemistry Atascadero High School

  2. Kinetic Molecular Theory of Gases • Gases consist of small particles in constant motion. • The individual particles occupy a very tiny volume. • Collisions with walls of container are elastic and exert pressure. • Particles do not interact with one another. • Average kinetic energy is directly proportional to the Kelvin temperature.

  3. Properties of Gases • Gases expand to fill their containers • No definite shape or volume • Gases are fluid – they flow • Gases have low density • 1/1000 the density of the equivalent liquid or solid • Gases are compressible • Gases effuse and diffuse

  4. Abbreviations P – Pressure V – Volume n – Number of particles, in moles R – Universal Gas Constant T – Temperature, in Kelvin

  5. Units of Pressure atm - atmospheres mm Hg - millimeters of mercury torr – same as mm Hg Pa – Pascal (SI (metric) standard) kPa - kiloPascal

  6. Units of Temperature K - Kelvin °C - degrees Celsius °F - degrees Fahrenheit

  7. Standard Conditions STP: Standard Temperature and Pressure Temperature: 273 K = 0.0 °C Pressure: 1.00 atm = 760 mm Hg (torr)

  8. Robert Boyle (1627-1691) Boyle’s Law: the volume of a fixed mass of gas varies inversely with the pressure at constant temperature. P1V1 = P2V2 1 = original; 2 = new

  9. Sample Boyle’s Law Problem A gas occupies 12.3 liters at a pressure of 400 mm Hg. What is the volume when the pressure is increased to 600 mm Hg and the temperature remains constant? P1V1/P2 = V2 (400 torr)(12.3 L)/(600 torr) = 8.2 L

  10. Jacques Charles (1746-1823) Charles’ Law: The volume of a fixed mass of gas varies directly with the Kelvin temperature at constant pressure. V1/T1 = V2/T2

  11. Sample Charles’ Law Problem Calculate the new temperature of a gas when 2.50 L at 293 K is compressed to 1.00 L at constant pressure. V2T1/V1 = T2 (1.0 L)(293 K)/(2.5 L) = 117 K

  12. Joseph Gay-Lussac (1778-1850) Gay-Lussac’s Law: The pressure of a fixed mass of gas varies directly with the Kelvin temperature at constant volume. P1/T1 = P2/T2

  13. Sample Gay-Lussac’ Law Problem Calculate the new pressure of a gas when a sample at 1.25 atm and 300 K is cooled to 210 K assuming constant volume. P1T2/T1 = P2 (1.25 atm)(210 K)/(300 K) = 0.875 atm

  14. Amedeo Avogadro (1776-1856) Avogadro’s Law: for a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas V1/n1 = V2/n2

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