1 / 11

Gas Laws

Gas Laws. Chemistry Mrs. Coyle. Factors Affecting Gas Pressure. Number of Moles (Amount of gas) As the number of particles increases, the number of collisions with the container wall increases. Volume The smaller the volume, the greater the pressure exerted on the container. Temperature

zulema
Download Presentation

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. Gas Laws ChemistryMrs. Coyle

  2. Factors Affecting Gas Pressure • Number of Moles (Amount of gas) • As the number of particles increases, the number of collisions with the container wall increases. • Volume • The smaller the volume, the greater the pressure exerted on the container. • Temperature • As temperature increases, kinetic energy increases, increasing the frequency of collision. Thus pressure increase.

  3. If Mass and Temp are Constant

  4. If Mass and Pressure are Constant

  5. Boyle’s Law P1V1=P2V2 T constant # moles constant P vs V hyperbola Isotherm High Temp P V

  6. Charles Law V1 =V2 P constant T1 T2 # Moles constant Isobar V T (K)

  7. Guy-Lussac P1 = P2 V constant T1 T2 # moles Constant isochoric P T

  8. Combined Gas Law P1V1 = P2V2_ T1 T2

  9. Ideal Gas Law: P V = n R T P = pressure Pa = N/m2 V = volume measured in m3 n =# of moles T = temperature K R=Universal gas constant =8.314 kPa L / (mol K) =0.0821 L atm/(mol K) =62.3 mmHg L/(mol K)

  10. Dalton’s Law of Partial Pressures • Ptot=P1+P2+…. • Total pressure of a mixture of gases in a container is the sum of the individual pressures (partial pressures) of each gas, as if each took up the total space alone. • http://www.wwnorton.com/college/chemistry/gilbert/tutorials/interface.asp?chapter=chapter_08&folder=daltons_law

  11. Ideal Gas Laws mostly hold at: • Low pressure • High temperature

More Related