Question

1	Volume of Dumas Bulb (L)	0.056 L
2	Mass of Empty Dumas Bulb (g)	50.000 g
3	Mass of Empty Dumas Bulb + condensed acetone (g)	65.714 g
4	Mass of condensed acetone (g) (3-2)	15.714 g

conclusions

1. Determine the number of acetone moles by using the ideal gas law equation. In your calculations, use the volume of the Dumas bulb and the following values: P = 1 atm, T = 373 K and R = 0.0821 L*atm/mole*K. You must show your work.

2. Using the moles found in Question #1 and the mass of acetone, determine the molecular weight of acetone. You must show your work.

3. It is not safe to put aerosol canisters in a campfire because the pressure gets very high and then they can explodes. If a 1.0 L canister can hold 2 moles of gas and the campfire has a temperature of 1400 ^oC, what is the pressure inside the container? Remember, R = 0.0821 L*atm/mole*K

4. How many moles of gas are in a 30 L scuba tank if the temperature is 300 K and the pressure inside the tank is 200 atm. Remember, R = 0.0821 L*atm/mole*K

5. What are the amount in moles of Helium required to fill a 5.0 L balloon to a pressure of 1.1 atm at 25 ^oC? Remember, R = 0.0821 L*atm/mole*K

6. Using the value obtained in Question #5, what is that amount in grams of Helium?

Answer 1