1. Convert 800C into Kelvin.

2. Solve Charles' Law for V2.

2a. What are the values for STP?

3. If in a system a vessel with constant pressure is cooled from 80C to 40C and the initial volume was 300mL what will the final volume be?

4. Solve the combined gas law for T2.

5. A 300 mL sample is heated and pressured from STP to 200C and 14atm. What will the new volume be?

6. If you double the number of molecules present what will happen to the volume in a system with constant pressure and temperature?

7. A gas sample has a mass of 48g. What is the molar mass of the compound if it takes up 80.0L at STP?

8. If pressure and temperature are held constant what will happen to the volume of a gas if the number of moles doubles?

9. A chemist forgot to write down the temperature of a reaction that he ran. He took the following measurements though. The volume was 32mL, the pressure was 4.2 atmospheres, and he knew there were 1.32 moles in the reaction. What was the temperature?

10. Write down the three gas laws that have proper names and label them.

11. Write down the combined gas law, Dalton's law of partial pressure, avogadro's law, and the ideal gas law.

12. Using units only slove the ideal gas law for R (use V=L, n= moles, T= K, and P=atm)

13. CH4(g) + Cl2 (gas) ---> CCl4 + HCl. Please balance the equation.
a. calculate how many moles of methane gas would be present at 6.34 atm, 400K, and 38.4L.
b. Using that many moles of gas calculate how many moles of HCl gas would form in the reaction.
c. If that many moles of HCl gas forms; how much volume would it take up at STP (Hint: Avogadro figured out the conversion factor between moles of a gas and Liters of volume for a gas and it's constant)?