1 / 25

The Gas Laws

The Gas Laws. And what they can do for me! =D. Put Simply. The gas laws are a series of rules and equations used to determine how a gas will react to various changes in its established situation. Put simply-er. These are the rules used to tell what will happen to a gas when stuff happens.

lovey
Télécharger la présentation

The Gas Laws

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. The Gas Laws And what they can do for me! =D

  2. Put Simply. The gas laws are a series of rules and equations used to determine how a gas will react to various changes in its established situation.

  3. Put simply-er These are the rules used to tell what will happen to a gas when stuff happens.

  4. Here is what will be covered… • Boyle’s law for pressure. • Charle’s law for temperature. • Gay Lussac’s law of temperature. • Combined gas law. • Ideal gas law. • Avogadro’s hypothesis. • Dalton’s law of partial pressure. • Graham’s law of effusion.

  5. Boyle’s law for pressure • For a given mass of gas at a constant temperature the volume varies inversely with pressure • P1 x V1 = P2 x V2

  6. Boyle’s law for pressure Pressure=200kPa Volume=0.5 L Pressure=100kPa Volume=1.0 L Pressure=50kPa Volume= 2.0 L

  7. Boyle’s law for pressure

  8. According to Boyle’s law… • If pressure doubles volume will do what? • If volume quadruples then pressure is divided by? Volume will be divided in half. 4

  9. Charles’ law for Temperature • The Volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant. • V1 / T1 = V2 / T2

  10. Charles’ law for Temperature Pressure=100 kPa Volume=20 L Temperature=200 K Pressure=100 kPa Volume=5 L Temperature=50 K Pressure=100 kPa Volume=10 L Temperature=100 K

  11. Charles’ law for Temperature

  12. According to Charles’ law • If temperature is doubled then volume does what? • If Volume triples then pressure does what? Volume doubles PSYCH! Nothing.

  13. Gay-Lussac’s law of temperature • The pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant. • P1 / T1 = P2 / T2

  14. Gay-Lussac’s law of temperature Pressure=200 kPa Pressure=50 Pressure=100 kPa Volume=10 L Volume=10 L Volume=10 L Temperature=400 K Temperature=100 K Temperature=200 K

  15. According to Gay Lussac’s law… • If pressure triples then temperature does what? • If the temperature stays constant can the pressure go up? Temperature triples Hell naw it can’t

  16. Combined gas law • A combination of Gay-Lussac’s law, Charles’ law & Boyle’s law. • No need to remember all 3 separately. • (P1 x V1)/T1 = (P2 x V2)/T2 • Any part can be canceled out to make the other laws

  17. Ideal gas law. • Adds fourth variable to Combined gas law. • Moles (n), take in to account the size of gas particles. • (P1 x V1)/(T1 x n1) = (P2 x V2 )/(T2 x n2)

  18. Ideal gas law questions • !Double worth! • Show how you can make the ideal gas law equation turn in to any of the preceding equations.

  19. Avogadro’s Hypothesis • Equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

  20. Avogadro’s Hypothesis Pressure, temperature, and volume is same for both.

  21. Avogadro’s hypotheses questions • What is Avogadro’s hypothesis? • How many particles were shown on the last fame? Equal volumes of gases at the same temperature and pressure contain equal numbers of particles. 32

  22. Graham’s law of effusion • The rate of effusion for a gas is inversely proportionate to the square root of the gases molar mass. • Diffusion= the tendency of molecules to move towards areas of lower concentration until equilibrium is reached. • Effusion= gas escaping through a tiny hole. • Rate A = sqr root of molar mass B Rate Bsqr root of molar mass A

  23. Diffusion Effusion

  24. Graham’s law questions • What is diffusion? • What is effusion • A gas’s rate of effusion is ________ proportionate to its __________. the tendency of molecules to move towards areas of lower concentration until equilibrium is reached. gas escaping through a tiny hole. Inversely Molar mass

  25. K.THNX.CLAP.

More Related