1. Take out a new sheet of paper and label it: Gas Law Problems #2
1. The pressure of a car tire is at 30 psi early in the morning when it is 0 ° C. In the middle of the day, when it is 30 ° C, you check the tire pressure again. What will it read?
2. The volume of a balloon is 300mL when I inflate the balloon at room temp (about 20 ° C). I take the balloon outside where it is 35 ° C. What will the new volume of the balloon be?
3. This room is at STP and is 10ft by 40ft by 25ft. If I run a vacuum and suck out a bunch air until the pressure drops to 0.8 atm, what volume of air have I taken away?

2. Ideal Gas Law Practice
4. A 7.50 liter sealed jar at 18 °C contains moles of oxygen and moles of nitrogen gas. What is the pressure in the container?
5. At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?
6. At what temperature (in Kelvin) would 4.0 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres

3. 7. How many moles of Oxygen gas do I have in 50 L pressurized container of 300 kPa that is at -700C?
8. 3 x atoms of helium get put into a balloon. The room is about 65 degrees Fahrenheit. The balloon expands to 40 L. What is the pressure inside the balloon?
9. Construct a Highly Accurate and Scaled Phase Diagram of Ammonia: Here is the relevant data:
Triple point= T= 195.4K P= kPA
Critical Point T= 406 K P= 11,300kPA
Boiling point (at 1 atm)= 240K
Melting Point (at 1atm)= 195K
Label the solid, liquid, gas phases