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Gas Laws

This resource provides a comprehensive overview of the gas laws and the behavior of ideal gases. Students will learn how to apply the gas laws to analyze the relationships between pressure, temperature, and volume of any amount of gas or gas mixture. The resource also discusses the assumptions of ideal gases and the deviations from ideal behavior in real gases.

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Gas Laws

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  1. Gas Laws

  2. CA Standards Students know how to apply the gas laws to relations between the pressure, temperature, and volume of any amount of an ideal gas or any mixture of ideal gases.

  3. Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory. • Gases consist of tiny particles that are far apart relative to their size. • Collisions between gas particles and between particles and the walls of the container are elastic collisions • No kinetic energy is lost in elastic collisions

  4. Ideal Gases (continued) • Gas particles are in constant, rapid motion. They therefore possess kinetic energy, the energy of motion • There are no forces of attraction between gas particles • The average kinetic energy of gas particles depends on temperature, not on the identity of the particle.

  5. Real Gases Do Not Behave Ideally Real gases DO experience inter-molecular attractions Real gases DO have volume Real gases DO NOT have elastic collisions

  6. Deviations from Ideal Behavior

  7. The Combined Gas Law The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas.

  8. Boyle’s Law Pressure is inversely proportional to volume when temperature is held constant.

  9. A Graph of Boyle’s Law

  10. The volume of a gas is directly proportional to temperature, and extrapolates to zero at zero Kelvin. (P = constant) Charles’s Law Temperature MUST be in KELVINS!

  11. A Graph of Charles’ Law

  12. Gay Lussac’s Law The pressure and temperature of a gas are directly related, provided that the volume remains constant. Temperature MUST be in KELVINS!

  13. A Graph of Gay-Lussac’s Law

  14. For a mixture of gases in a container, PTotal = P1 + P2 + P3 + . . . Dalton’s Law of Partial Pressures This is particularly useful in calculating the pressure of gases collected over water.

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