Ozone is a simple molecule made up of three Oxygen molecules linked together by very unstable bonds (O3). This makes ozone a very reactive gas. It is also a gas that blocks ultraviolet (UV) radiation from the sun. Read all about some of the good and bad sides of ozone at the following link:
NASA. (2004). The good, the bad and the ozone. Retrieved fromhttps://www.nasa.gov/missions/earth/f-ozone.html
Too much ozone could give you asthma and send you to the hospital, while not enough ozone is blamed for increasing UV-B exposure, which is linked to skin cancer. How can ozone be both bad and good at the same time?
After reading up on ozone, do some research on your own. Be sure to use academic sources for your research. The Kaplan Library is a great place to start.
Then, during this unit, discuss the following with your classmates:
• What are some of the causes and implications of the ozone hole in the atmosphere?
• How are scientists addressing ozone depletion and how successful are these efforts?
• Why do people need to be concerned about ozone levels in the air?
• What are some of the challenges in getting people to reduce their production of ozone on the ground?
• What things can you personally do to address the ground ozone problem, as well as the atmospheric ozone problem?
Assignment:
Gases
Before you come to Seminar, prepare the answers to the following problems. Your instructor will work through these problems step-by-step with you during the Seminar, but be sure to work them through first so that you can identify where you might be making errors. Your instructor will also go over various gas laws - including Boyle's Law, Charles's Law, and the Ideal Gas Law - along with tips and tricks to use when working through gas law calculations.
1. Determine the volume of CO2 in a gas cylinder given the following conditions:
Original Conditions
Volume = 15.2 liters
Pressure = 1.35 atm
Temperature = 33° C
New Conditions
Pressure = 3.50 atm
Temperature = 35° C
2. Calculate the pressure of O2 (in atm) when 0.100 mole of O2 gas is kept in a 2.00 liter gas cylinder at 75.0° C.
3. One mole of CH4 gas occupies 20.0 liters at 1.00 atm pressure. What is the temperature of the gas in Kelvin?
4. A steel tank is filled with nitrogen gas at a pressure of 6.50 atm. What is this pressure in torr?
5. How many moles of Neon are present in a 2.0 liter flask that has a pressure of 850 torr at a temperature of 35°C? What is the mass of this Neon?