- Pressure and volume; Boyle's Law. Given an initial volume of 350 in
^{3}and a compression ratio of 10:1, what is the final volume? Solution. - Pressure and temperature. A pressure cooker starts out at 25 C and 1 atm pressure. What is the pressure at 200 C? Solution
- Volume and temperature; Charles' Law: 1 m
^{3}of steam is heated from 100 C to 500 C at constant pressure. What is the final volume? Solution - Combined Gas Law; A stratospheric sampling balloon starts at sea level, 760 torr and 20 C with
a volume of 1000 m
^{3}. The balloon rises to a pressure altitude of 1000 Pa (appx 40 km) where the temperature is -40 C. What is the volume of the balloon at this altitude? Solution

- 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
Solution - A stratospheric sampling balloon starts at sea level, 760 torr and 20 C with a volume of 1000 m
^{3}. The balloon rises to a pressure altitude of 1000 Pa (appx 40 km) where the temperature is -40 C. What is the volume of the balloon at this altitude? How many moles of He are in the balloon, what is the mass of the He in the balloon. Solution

- A 250 mL Erlenmyer Flask is weighed on an analytical balance; mass = 158.2376 g
- The flask is filled with water at 20 oC and weighed on an analytical balance; mass = 420.9165 g
- The flask is emptied and throughly dried.
- Next 10.0 mL of a liquid is added to the flask, the mouth of the flask is covered with foil and a pin hole made in the foil.
- The flask is placed in a water bath and heated to 95 oC for 20 minutes until no liquid is observed in the flask.
- The flask is cooled to room temperature, vapor is observed to consdense in the flask, the temperature is measured T = 20 oC
- The flask is weighed on an analytical balance; mass = 158.8714 g

- Given 100 g of NaN
_{3}, what is the final volume of the air bag at 783 torr and 15 C? The air bag is show in this video; ( Internet© Saunders, 1997) The reaction for an air bag is:2NaN Solution_{3}(s) --> 2Na(s) + 3 N_{2}(g)

- Calculate the pressure for 0.01, 0.1, 1.0, 10, 100 moles of an ideal gas in a 1 liter container at 273.15 K. Also calculate the pressure of He and CO
_{2}using the Van der Walls Equation to account for non-ideal behavior. - Calculate the pressure for 0.1 moles of an ideal gas in a 1 liter container at 100, 200, 400 and 800 K. Also calculate the pressure of He and CO
_{2}using the Van der Walls Equation to account for non-ideal behavior.

Van der Waals Constants (From Zumdahl, 4th ed) | ||
---|---|---|

Gas | a (atm*L^{2} * mol^{-2}) |
b (L mol^{-1}) |

He | 0.0341 | 0.0237 |

Ne | 0.211 | 0.0171 |

Kr | 2.32 | 0.0398 |

N_{2} |
1.39 | 0.0391 |

CO_{2} |
3.59 | 0.0427 |

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Scott Van Bramer

Department of Chemistry

Widener University

Chester, PA 19013

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Last Updated Friday, May 25, 2001 2:10:36 PM