1 / 20

Chapter 11 – Ideal Gas Law and Gas Stoichiometry

Chapter 11 – Ideal Gas Law and Gas Stoichiometry. H 2. He. O 2. N 2. 11.1- Mass and Volume of Gases. Avogadro’s Principle = Equal volume of gases at same T and P have same numbers of molecules. All of these balloons are the same size (same volume).

galeno
Download Presentation

Chapter 11 – Ideal Gas Law and Gas Stoichiometry

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. Chapter 11 – Ideal Gas Law and Gas Stoichiometry

  2. H2 He O2 N2 11.1- Mass and Volume of Gases Avogadro’s Principle = Equal volume of gases at same T and P have same numbers of molecules All of these balloons are the same size (same volume) All of these balloons are at the same Temperature and Pressure inside All of these balloons would have the same number of MOLECULES These balloons would have DIFFERENT masses! World of Chemistry – The Mole (Stop at 6:14)

  3. 11.1- Mass and Volume of Gases 1 mol of anything = 6.02 x 1023 particles 1 mol of any gas = same number particles = 6.02 x 1023 particles = same volume = different mass Molar Volume = Volume of 1 mole of any gas at STP 22.4 L = 1 mole of gas at STP

  4. 11.1- Mass and Volume of Gases Examples:

  5. 11.1- Mass and Volume of Gases Gas Density -Depends on T and P -We will start by looking at density at STP dSTP = Molar Mass Molar Volume Examples:

  6. 11.1- Mass and Volume of Gases Molar Mass MM = dSTP * Molar Volume (will be given)

  7. 11.2 - Ideal Gas Law Used on ONE gas at ONE set of conditions (will be given to Academic) PV = nRT Temperature Pressure moles Volume Ideal Gas Constant R = 0.08206 L atm /mol K = 62.4 L mmHg / mol K = 8.314 L KPa / mol K

  8. 11.2 - Ideal Gas Law How do you know which R to pick??? R = 0.08206 L atm /mol K = 62.4 L mmHg / mol K = 8.314 L KPa / mol K By thePRESSURE UNIT!! If Pressure is in mmHg… Pick 62.4 L mmHg / mol K If Pressure is in KPa… Pick 8.314 L KPa / mol K

  9. 11.2 - Ideal Gas Law Examples:

  10. 11.2 - Ideal Gas Law Examples:

  11. 11.2 - Ideal Gas Law Examples:

  12. Non-STP Gas Density d = MM * P (will be given) R * T Examples:

  13. Non-STP Molar Mass MM = mass sample * R * T P * V Will be given Examples:

  14. 11.3- Stoichiometry of Gases -NEED BALANCED EQUATION!! -Could include info from Chapter 3, 7,8,9, 10, or 11!!

  15. Ratio from Balanced Equation Molar Mass from Periodic Table Molar Mass from Periodic Table Grams A Moles A Moles B Grams B 11.3- Stoichiometry of Gases Review: NewInformation: With GASES…There are other options: Moles to Volume using 22.4L/mole at STP or PV=nRT Volume to Moles using 22.4L/mole at STP or PV=nRT

  16. Ratio from Balanced Equation Molar Mass from Periodic Table Molar Mass from Periodic Table Grams A Moles A Moles B Grams B 11.3- Stoichiometry of Gases 22.4 L/mol IF at STP OR PV=nRT if NOT STP 22.4 L/mol IF at STP OR PV=nRT if NOT STP Volume A if a GAS Volume B if a GAS

  17. 11.3- Stoichiometry of Gases Examples:

  18. 11.3- Stoichiometry of Gases Examples:

  19. 11.3- Stoichiometry of Gases Examples:

  20. 11.3- Stoichiometry of Gases Examples:

More Related