Experiment # 10 CHEM LAB

Experiment # 10 CHEM LAB - 1 Farley Conor Farley CHM 144...

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1 Farley Conor Farley CHM 144 Section A Deok-Im Jean Mike Eiswerth 27 November 2011 Relationships Between the Physical Properties of Gases
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2 Abstract: Gases have four principle variables that interact with one another. These variables include pressure (atm), volume (L), temperature (K), and number of moles of the gas in question (n). In this experiment, the number of moles, and one of the three variables being tested in a given apparatus, were held constant. This means the results of the experiment regarding the relationships between these variables describe ideal gases. The Ideal Gas Law is given as PV= nRT, which holds true throughout the experimental process. Upon reviewing the results of the lab, pressure and volume were found to be inversely proportional to one another. In turn, pressure and temperature, and volume and temperature were found to be directly proportional. In all three cases, the number of moles was held constant. The graphs also refute the relationships of these variables by showing linear curves for all three cases, save the relationship between pressure and volume, which was inverse and initially showed a downward curve. Methods Experiment 1 (P-V expt.) This experiment was created to demonstrate the relationship between pressure and volume at constant temperature through Boyle’s Law. The apparatus shown in Figure 12- 1, page 151 was set up, with an enclosed gas sample in a 60.0 ml syringe at room temperature. The plunger was used to move the piston of the syringe so that a measured volume of air was trapped in the syringe. The volume was adjusted to 55.0 ml. The foot of the clamp was made to rest on top of the plunger. The LabQuest instrument was turned on, and the gas pressure sensor was connected to the CH 1 port. The units were then changed to atm. The syringe was then attached to the valve of the gas pressure sensor. Gas volume (ml) and pressure (atm) were recorded in the notebook as initial volume and pressure, at 0.983 atm and 55.0 ml respectfully. The plunger was then pushed down by adjusting the clamp handle, and the volume was decreased by 5.00 ml. The new volume and pressure were recorded in the notebook. This was repeated again, decreasing the
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3 Farley volume by another 5.00 ml, with the new volume and pressure recorded. This was repeated for a total of five measurements. The pressure sensor was then disconnected, and the clamp re-adjusted to the original position. Experiment 2 (P-T expt.) This experiment was used to demonstrate the relationship between Pressure and Temperature at Constant Volume, which is based in Gay-Lussac’s Law. The apparatus as seen in Figure 12-2, page 152, was set up using an Erlenmeyer flask, containing an air sample, in a water bath of varying temperature. First, the LabQuest instrument was turned on, and the gas pressure sensor was connected to CH 1, and the temperature probe to CH 2, with the units of pressure turned to “atm” and temperature to “Kelvin.” A 25 ml Erlenmeyer flask was obtained and sealed with a one-holed rubber stopper, and the flask
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This note was uploaded on 02/01/2012 for the course CHEM 141 taught by Professor Crowder during the Fall '11 term at Miami University.

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Experiment # 10 CHEM LAB - 1 Farley Conor Farley CHM 144...

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