- Units
- Pressure (what it is and units)
- Temperature (Use Kelvin Scale, 273.15)
- Volume
- Standard Temperature and Pressure (STP)
- 1 bar (10
^{5}Pa), previously 1 atm - 0 °C

Pa | (N/m^{2}) | 101325 Pa = 1 atm |

bar | (10^{5} Pa) | 1.01325 bar = 1 atm |

torr and mmHg | (133.322 Pa) | 760 torr = 1 atm |

atmosphere | (101325 Pa) | |

PSI | (6894.76 Pa) | 14.7 PSI = 1 atm |

Unit | Conversion to Liter | Conversion to m^{3} |

m^{3} |
10^{3} liter |
1 m^{3} |

cm3 (ml) | 10^{-3} liter |
10^{-6} m^{3} |

liter (dm^{3}) |
1 liter | 10^{-3} m^{3} |

ft^{3} |
35.323 liter | 0.03532 m^{3} |

in^{3} |
0.01639 liter | 1.639x10^{-5} m^{3} |

- Introduce concept of an ideal gas
- No volume
- No interaction
- Discuss behavior of ideal gas
- Ideal Gas Behaviors. Gas Law Spreadsheet (123, Excel)
- Boyle's Law (PV = C
_{B}) - Derive relationship from ideal gas "concept with picture on board
- Animation from ( Internet© Saunders, 1997)
- Graph relationship
- Write equation for graph
- Work a problem.
- P/T = C
- Derive relationship from ideal gas "concept with picture on board
- Animation from ( Internet© Saunders, 1997)
- Graph relationship
- Write equation for graph
- Work a problem.
- Charles Law (V/T = C
_{C}) - Derive relationship from ideal gas "concept with picture on board
- Graph relationship
- Write equation for graph
- Work a problem.
- Combine above equations to get (PV)/T = C
- Practice Problems.

- Boyle's Law (PV = C
- P/n = C
- Derive relationship from ideal gas "concept with picture on board
- Animation from ( Internet© Saunders, 1997)
- Graph relationship
- Write equation for graph
- Work a problem.

- Gas data for 1 gram at STP. Calculate the molar volume
- H
_{2}11.1 L - He 5.57 L
- N
_{2}0.800 L - Cl
_{2}0.316 L - Relate molar volume to combined gas law and derive ideal gas law
- PV = nRT
- Units for R
- Calculate R from above data
- Convert R to SI units (Note: Pa = N/m
^{2}and J = Nm) - How many moles of gas in the sampling balloon above?
- Work a problem.

- Dalton's Law of Partial pressure
- P
_{total}= P_{1}+ P_{2}+ P_{3}+ ... - P
_{total}V = (n_{1}+ n_{2}+ n_{3}+ ...) RT - Problem

- What is an ideal gas
- elastic collisions
- Boltzman Plots (
Internet© Saunders, 1997)
- KE
_{avg}proportional to T - KE = 1/2 mv
^{2} - For two different gases

- Non Ideal Behaviors
- Volume of gas particles (Overhead)
- Interaction of gas molecules (overhead)

- Derive van der walls equation
- Start with the ideal gas law where Pi and Vi are the "ideal" pressure and volume:
- The "real" volume (V
_{r}) is the ideal volume plus the volume of the gas molecules (n*b), where n is the number of moles and b is the volume of one mole of gas molecules. That is the molecules, not the space that contains the molecules. - The "real" pressure (P
_{r}) is the ideal pressure minus a term that describes how the gas molecules stick together. This sticking together reduces the apparent pressure. It is possible to develop this equiation from "first principles", but we will leave that exercise for when you take physical chemistry. - Now these new expressions for the ideal pressure and the ideal volume may be substituted into the ideal gas law to give:
- Which is the Van der Walls equation.

- Start with the ideal gas law where Pi and Vi are the "ideal" pressure and volume:
- Work an problem.
- Comparison of ideal gas and Van der Walls gas from Mathcad
- Helium at 25 C (pressure vs volume)
- CO
_{2}at 25 C - CO
_{2}at 100 C

This page is maintained by

Scott Van Bramer

Department of Chemistry

Widener University

Chester, PA 19013

Please send any comments, corrections, or suggestions to svanbram@science.widener.edu.

This page has been accessed
times since 5/30/97.

Last Updated Friday, May 25, 2001 1:59:43 PM