Procedure:
1.	Pour water in beaker.
2.	Place beaker on plate.
3.	Place bell jar on plate, covering beaker.
4.	Connect the vacuum to the bell jar.
5.	Pump air out.

Observations:	
After 10 pumps, bubbles started to appear.
After 80 pumps, bubbles got bigger in size.
After 120 pumps, the big bubbles started to rise to the surface.

Conclusion:
The decrease in atmospheric pressure caused the water in the beaker to bubble. The bubbles in the beaker increased in number while the atmospheric pressure was decreased. Water did not boil.

Procedure:
1.	Spray some shaving cream in beaker.
2.	Place beaker on plate.
3.	Place bell jar on plate, covering beaker.
4.	Connect the vacuum to the bell jar.
5.	Pump air out.

Observations:
After 10 pumps, the shaving cream rose up.
After 15 pumps, the shaving cream continued to rise.

Conclusion:
The shaving cream expanded as the atmospheric pressure was decreased. The volume of the shaving cream increased because the atmospheric pressure decreased which made the vapor pressure of the shaving cream to increase. When pressure was stabilized, the shaving cream collapsed because the vapor pressure was turned back to normal.

Question:
What is the relationship between atmospheric pressure and boiling point and vapor pressure of water inside the jar versus outside the jar?
Answer:
Inside the jar, the atmospheric pressure decreased which allowed vapor pressure to increase. The boiling point decreased because with the lower atmospheric pressure, water would be able to boil quicker. Outside the jar, the atmospheric pressure and the vapor pressure remained the same.