1 / 29

Chem 300 Thermo/Kinetics

Chem 300 Thermo/Kinetics. www.amey.oxy.edu/chem300. Information Card. Last, First Name (Nickname?) Class yr Phone # e-mail Mail Box # Major? Home City, State, Country? Math Courses Completed Completed Chem 305?. Refer to Manual for:.

dandre
Download Presentation

Chem 300 Thermo/Kinetics

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. Chem 300Thermo/Kinetics www.amey.oxy.edu/chem300

  2. Information Card Last, First Name (Nickname?) Class yr Phone # e-mail Mail Box # Major? Home City, State, Country? Math Courses Completed Completed Chem 305?

  3. Refer to Manual for: • Syllabus • Homework assignments • Exam dates • Hints for successful studying • Performance Objectives • Chapter hints • and much, much more...

  4. Ch 1/#1Today’s To Do List • Fill out info card • Review P, V, T • Review Ideal Gas Law • The Compressibility Factor • “Real” Equations of State

  5. Concepts of P, V, T • Molecular • Mechanical

  6. Mechanical Equilibrium

  7. Volume • DUH!! • Measure containment dimensions

  8. Thermal Equilibrium

  9. Zeroth Law of Thermo

  10. Zeroth Law of Thermo • When 2 bodies, in intimate contact, no longer show change in their physico-mechanical properties, they are in thermal equilibrium (TE). • When bodies A & B are in TE, and A & C are also in TE, then B & C are in TE.

  11. Properties of simple gases

  12. Boyle’s Law: P = m/V (const T)

  13. Charles’ Law: V = mT (const P)

  14. P = mT (const V)

  15. f = (P,V,T)

  16. Ideal Gas Law • PV = nRT • n = number of mols of gas • R = gas constant • = 0.082058 L-atm/mol-K • = 8.3145 J/mol-K • = V/n = molar volume = Vm • P = RT

  17. IG Assumptions • Point masses • No Attractive forces • Elastic collisions

  18. Examining Reality • Define Compressibility Factor (Z): • Z = PV/nRT = P /RT • For Ideal Gas: Z = 1 • For Nonideal Gases: Z  or  1

  19. Compressibility Factor: Z=PV/nRT

  20. Temperature Dependence of Z • For Ideal Gas: Z(T) = constant • For NonIdeal Gases: • Z(T) is very T-dependent

  21. The Boyle Temperature

  22. Real Gases

  23. Real (Nonideal) Gases

  24. The Critical Point

  25. How do we show this? • Devise a better equation of state by: • Correcting for IG deficiencies. • Curve-fitting experimental data.

  26. Next Time • Equationsof State catchup • More about the Critical State • Law of Corresponding States • Virial Equations • Intermolecular Potentials(Intro)

More Related