1 / 13

Molar Volume, Avogadro's Law and (a little bit about) Dalton’s Law of Partial Pressures

Molar Volume, Avogadro's Law and (a little bit about) Dalton’s Law of Partial Pressures. MOLAR VOLUME. How much space does 1 mole of gas take up?. 1 mole of ANY gas = 22.4 L at STP How many liters does 2.8 moles of Helium take up? 2.8 mol 22.4 L = 62.72 L 1 mol

huela
Download Presentation

Molar Volume, Avogadro's Law and (a little bit about) Dalton’s Law of Partial Pressures

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. Molar Volume, Avogadro's Law and(a little bit about) Dalton’s Law of Partial Pressures

  2. MOLAR VOLUME

  3. How much space does 1 mole of gas take up? • 1 mole of ANY gas = 22.4 L at STP • How many liters does 2.8 moles of Helium take up? 2.8 mol 22.4 L = 62.72 L 1 mol • How many moles are in 137.2 L ? 137.2 L 1 mol = 6.125 moles 22.4 L

  4. How many moles in a given volume? • You have three 1 L flasks. #1 is filled with CO2. #2 is filled with H2 and #3 is filled with C2H6. Which flask has the most number of moles of gas? THEY ARE ALL THE SAME!!!

  5. How many molecules in 0.75 L at STP? Liters  Moles  Molecules Molar Avogadro’s Volume! # 0.75 L 1 mol 6.02 x 1023 molecules = 2.02 x 1022 22.4 L 1 mole molecules

  6. Avogadro’s Law

  7. EQUAL volumes of gas at EQUAL temperatures and pressures have EQUAL numbers of moles/molecules

  8. Avogadro’s Law V1 = V2 n1 n2 • You have gaseous helium in two separate containers at the same temperature and pressure. The volume of container #1 is 3.7 L and has 8.2 moles of the gas. The volume of container #2 is 19.4 L. How many moles are in container #2? 3.7 L = 19.7 L n2 = (19.7 L)(8.2 mol) 8.2 mol n2 (3.7 L) n2 = 43.7 mol

  9. YOU TRY IT… • You have gaseous helium in two separate containers at the same temperature and pressure. The volume of container #1 is 1.8 L and has 7.6 moles of the gas. The volume of container #2 is 3.58 L. How many moles are in container #2? 1.8 L = 3.58 L n2 = (3.58 L)(7.6 mol) 7.6 mol n2 (1.8 L) n2 = 15.1 mol

  10. (a little bit about) Dalton’s Law of Partial Pressure

  11. PARTIAL PRESSURES The total pressure of a gas mixture depends on the total number of gas particles, not on the types of particles. P = 1.00 atm P = 1.00 atm LecturePLUS Timberlake 1 mole H2 0.5 mole O2 + 0.3 mole He + 0.2 mole Ar

  12. DALTON’S LAW OF PARTIAL PRESSURE • In a mixture of gases, the total pressure of the mixture equals the sum of the individual gas pressures Ptotal = Pgas1 + Pgas2 + …. + Pgasn • When a gas is collected over water, you have a mixture of your sample gas as well as water vapor

  13. YOU CAN USE MOLE RATIOS AS IF THEY WERE PARTIAL PRESSURES • A gaseous mixture contains 2 mol Ar and 4.5 mol of CO2. It has a total pressure of 6.8 atm. What is the partial pressure of Ar? ngas = Pgas ntotal Ptotal 2 mol Ar = PAr gas PAr gas = 2.09 atm (2 mol + 4.5 mol) 6.8 atm

More Related