❖ Procedure and Results:
❖ Boyle’s Law
➢ P = K/V
▪ P is inversely related to V High pressure, low volume
▪ To relate gases of different situation: P1V2 = P2P2
➢ A syringe is fitted into a base and it’s capped off with a wooden platform where weight
was placed on top
▪ Atm pressure: 33ml volume in the syringe
➢ Put a 2.5lbs weigh on the platform, the gas gets compressed as the plunger pushes it
down.
➢ Record the atm pressure as you stack each weight.
❖ Charles Law
➢ V = kT V and T are directly related
▪ When volume goes up, temperature goes up
▪ V1/T1 = V2/T2
➢ Cool a conical flask in an ice bath.
➢ Tighten flask up with clamp stand with thermometer and a syringe within stopper.
➢ Measure the initial temperature: 6.5oC.
➢ Use a blow dryer to heat the flask.
➢ Record the volume stated on the syringe for every 5 oC increase in temperature.
❖ Ideal Gas Law
➢ Part 1: Determine the molar mass of acetone
▪ Measure the mass of the flask and the foil.
• Mass: 112.1373g
▪ 1.8mL of acetone was measured and placed into the flask. Covered with foil
▪ Clamp the flask and set the flask on a water bath
▪ Place a thermometer into the beaker and heat it until it is 66.4OC (10OC more than
boiling point of acetone =56 OC) to ensure all the acetone in the flask is vaporized and
excess acetone comes out the top of the flask.
▪ Remove flask from the water bath and put into a cool flask to recondense acetone
from vapor phase into liquid phase.
▪ When the flask is cooled, take the flask out, unclamp and dry with a laboratory towel
• Water droplets around the flask could add to the mass.
▪ Weigh the mass of the flask. Mass: 112.7900g
▪ Pressure: 09766 atm
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