1 / 24

Understanding Gas Laws and Pressure: Key Concepts in Chemistry

This guide explores fundamental concepts related to pressure and gas laws in chemistry. It discusses pressure units, Boyle's Law, Charles's Law, and the Combined Gas Law with graphical representations. Additionally, it covers the Ideal Gas Law, Dalton's Law of Partial Pressures, and the significance of STP. The definitions of density and Avogadro's number are also included, along with the molecular mass calculations and when real gases differ from ideal gases. A thorough understanding of these principles is essential for mastering gas behavior in various conditions.

imala
Télécharger la présentation

Understanding Gas Laws and Pressure: Key Concepts in Chemistry

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. What is pressure? What are the units of pressure? Do 32

  2. What is Boyles law? • Graph it

  3. What is Charles Law?Special units to keep in mind? Graph it

  4. What is the combined gas law?Special units to keep in mind?

  5. What is Amedo Avogadro’s #? • What is the volume of one mole of any gas at STP? Do the evens 34 – 48

  6. What does STP stand for and what are the values you should know?

  7. What is the ideal gas law? • Special units to keep in mind?

  8. What are the 4 (3) different values of R WITH units?

  9. Do evens 50 – 56

  10. What is the formula for density? • Where does density tie into Mole Town? • Do evens 58 – 62

  11. How would you use density to find MM? • Do 64

  12. What to do if conditions are not at STP? • Use ideal gas law to get moles and then do stoich • Use stoich to get moles and the ideal gas law to get pressure or volume

  13. Do evens 68 – 74

  14. Explain Dalton’s law of partial pressure • Do 76

  15. Ideal gas law to get pressure and then Dalton’s law of pp • Do 78

  16. May not be given pressures • Use % to find pp • Use mole fraction to get pp • Do 80

  17. Why should we care if the gas was collected over water? • Do 82

  18. List the 4 points of the Kinetic Theory.

  19. Root-means-square what’s that? • Do evens 84 – 88

  20. Why could G smell the H2S (rotten gases) within 3 seconds?

  21. Why do balloons deflate over time? • Formula(s)?

  22. Do evens 90 – 94

  23. When do real gases differ from ideal? • 2 reasons

  24. What is van der Waals equation? • You do not need to have this one memorized; however, you need to know why there are additions to van der Waals equation in comparison with the ideal gas law. • Do evens 96 – 98

More Related