Study Guide Chapter 5 - Gases
1. Definition of pressure
2. Units of pressure
3. Conversion of pressure units
4. Temperature
5. What is absolute zero and what does it mean
6. Conversion between C and K
7. Gas Laws - problems dealing with all of the below
Boyle PV=PV
Charles V/T=V/T
Avogadro V=an
Put it all together you get PV=nRT
R=0.08206 L atm/K mol
8. What is STP? 273, 1 atm
9. What is volume of gas at STP (22.42 L)
10.Combine stoichiometery and gas laws to calculate volume of gas evolved in a reaction
11.Tie between gas density and Molecular mass
Molar mass = density RT/P Be able to use equation to go from density to molar
mass
12. Partial pressures
A. What is the law of partial pressure
B. Can you handle mixtures of gases in calculations
C. What is the mole fraction and how do you calculate it
D. Why do you have to be careful about volumes of gases made in the lab using
water?
13. KMT Theory
A. What does KMT mean?
B. Explain any of the basic gas laws using KMT theory and a diagram
C. How is Kinetic Energy related to temperature
D.Calculate root mean square velocity of a gas molecule
urms =
3RT
Molar Mass
Note in above equation need to use R=8.314 J/K mol and answer is in m/s
14. What is effusion, diffusion (but no calculations)
15. Why would a gas behave in a non-ideal manner?
16. Given the proper equation(page 223) and constants a and b, calculate P for a real gas