Introduction: In this experiment, the problem trying to be solved is what gas laws are being used when the pressure, temperature, and volume are being measured. The three gas laws are Boyle’s Law, Charle’s Law, and Gay-Lussac’s Law. The Boyle’s Law is when volume and pressure are being compared. Pressure and volume are inversely proportional, because when pressure goes up, volume goes down. The Charle’s Law is when volume and temperature are compared. Volume and temperature are also inversely proportional as well.
Lastly, Gay-Lussac’s Law is when pressure and temperature are compared. Pressure and temperature are directly proportional; therefore when pressure goes up, temperature also goes up. The formulas are as follows: Boyle’s Law: P2 P1 = P2 V2 Charle’s Law: V1/T1 = V2/T2 Gay-Lussac’s Law: P1/T1 = P2/T2 Hypothesis: If volume, temperature, and pressure are measured, they will follow the laws and fit under Boyle’s, Charle’s, or Gay-Lussac’s law. Expected Results: It should be expected that when volume and pressure are measured, pressure will go up and volume will go down.
When volume and temperature are compared, volume will go up and temperature will go down. Lastly, when pressure andtemperature are measured, pressure will go up as temperature goes up. Experimental Procedure: Part I Connect a 20mL syringe to a LabQuest Select: File New Then, Mode: Change to Events with Entry Next, Enter Name as Volume Enter Units as mL Select OK Start at 10mL on the syringe and wait for the reading to Select Keep Keep at least 6 data points (any of your choice)
The Essay on Gas Laws Lab
Introduction: The four basic physical properties of a gas sample are pressure, volume, temperature, and number of moles. The volume simply indicates the volume of the container since a gas will take up all space available to it. The temperature indicates the average kinetic energy of the gas particles. For gases, the temperature must be converted to the Kelvin unit. The pressure of the gas ...
Only pull the syringe out (making the mL readings higher each time) Stop the Data Collection and view the graph and points Record Part II Place an Erlenmeyer flask in a beaker big enough to fit the flask Connect a temperature apparatus to the Lab Quest and place probe in beaker Then connect the pressure tube to the Lab Quest in channel 2 and connect the other end of the tube with the rubber stopper to the Erlenmeyer flask Select: File New Then Mode: Change to Selected Events Exit In sensors menu, change units to Kelvin
Tap graph X-axis: chose temperature Place faucet, room temperature water in the beaker Select Keep Place ice in the beaker Select Keep Place room temperature water in the beaker again and place on a hot plate Wait for the water to boil Place temperature probe and Erlenmeyer flask back in beaker Select Keep Record result from graph and chart Results: VOLUME (mL) PRESSURE 10 103. 27 12 87. 6 14 76. 14 16 67. 5 18 60. 96 20 55. 15 This data and chart is comparing volume and pressure.
The graph represents the Boyle’s Law because as the pressure is going up the volume is going down. TYPE OF WATER TEMPERATURE (K) PRESSURE Normal 102. 8 295 Ice 98. 29 275. 4 Boiling 122. 31 357. 4 This data and chart is comparing temperature and pressure. The graph represents Gay-Lussac’s Law because as temperature goes up, pressure goes up as well. Discussion: This experiment went extremely smooth. The data was easy to collect as long as you kept the Lab Quest and tools stable to ensure for accurate readings for temperature, pressure, and volume.
The graphs and data easily coincided correctly with the theories of the gas laws, as was shown accessibly once the graphs were made. Although the data coincided with the theories correctly, the temperature readings for freezing and boiling may have not been completely accurate because the temperatures of the water was not measured accurately for correct boiling and freezing temperatures, but recorded solely for the theories and to prove them. Overall, the experiment held up well and the hypothesis and theories were proven to be correct.
