Chemistry Chapter 11 Gases

Card Set Information

Author:
misol
ID:
301814
Filename:
Chemistry Chapter 11 Gases
Updated:
2015-04-30 00:31:05
Tags:
chemistry sacco wake tech
Folders:

Description:
chemistry sacco wake tech
Show Answers:

Home > Flashcards > Print Preview

The flashcards below were created by user misol on FreezingBlue Flashcards. What would you like to do?


  1. Kinetic Molecular Theory of Gas
    • Particles are separated by large distances
    • They are in random motion 
    • They do not form attractive or repulsion forces on one another 
    • Avg Kinetic Energy α absolute temp 
    • so T ↑, Ek↑
  2. p = force/area
    gas particles colliding with walls of the container
  3. remember this formula
    P1V1/T1 = P2V2/T2

    PV = nRT
  4. Boyle's Law
    relationship b/t P and V

    P1V1 = P2V2

    @ constant T
  5. Charles Law
    • Volume and Temperature @ constant pressure 
    • V1/T1 = V2/T2

    As Temp increases, Volume increases (proportional)

    *Always use kelvin
  6. C to Kelvin
    K = C + 273.15
  7. Avagadros Law
    moles (n) and volume relationship 

    v1/n1 = v2/n2

    so P1V1/n1T1 = P2V2/n2T2
  8. Ideal Gas Equation Law
    PV = nRT

    R is gas constant = .08206 L-atm/molar K
  9. Standard Temp and Pressure (STP)
    1 mol of gas at 0C (273.15K) + 1 atm

    PVnRT (solve for V)

    V = nRT/P
  10. 1 mol gas @ STP
    22.414L
  11. Dalton's Law of Partial Pressure 

    Gas Mixtures
    • Ptotal = ΣPi
    • Ptotal = Pn + Po + Par
  12. Mole Fractions (Xi)
    Tells the relative amounts of a gas mixture 

    • Xi = ni/ntotal         
    • (no units)
  13. Consider the following regarding Mole Fractions
    • 1. Mole fraction of a component is < 1
    • 2. Sum of mole fractions for all components = 1
    • 3. Mole fraction is dimensionless

    Xi = Pi/Ptotal

What would you like to do?

Home > Flashcards > Print Preview