Exploring Pressure-Volume Relationships
Table 1: Pressure vs. Volume of Container
Table 2: Data for determining R
Volume Of Container
A flask with the same volume as Part B was stoppered and equipped with a pressure sensor. Some water was placed into the flask to give some vapor pressure. The exact volume of the flask was not needed because this experiment involved only pressure and temperature. The flask was then placed in a larger beaker full of water and placed on a hot plate. The temperature and pressure were recorded every 5 seconds as the flask was heated.
Moles Of Hydrogen Gas Produced
0.029 g Mg/(24.31 g/mol) = 0.00119 mol Mg
.00119 mol Mg = mol H2
.00119 mol H2
Partial Pressure Of Hydrogen Gas
Total Pressure Change = 192.3 torr
Vapor Pressure of Water = 17.55 torr
Partial Pressure of H2 = Total Pressure Change - Vapor Pressure of Water
192.3 torr - 17.55 torr = 174.8 Torr
Calculation of R
PV = nRT
R = PV/nT
R = (0.2299 atm)(0.1405 L)/(0.00119 mol H2)(292.9 K)
R = 0.0927 L atm/ mol K
Percent Error R
(0.0927 - 0.08206)/0.08206 x 100% = 12.97% error
Calculation of when P = 0
formula from graph: y = 0.1898x - 68.204
When x = 0 (P = 0 ) y = -68.204 ℃.
This section of the experiment was designed to test Boyle’s law, which relates pressure to volume of the container. The data obtained during experimentation follows Boyle’s law. As the volume of the container decreases, the pressure inside of the container increases. This relationship is because of the behavior of the particles themselves inside of the...
References: Bottomley, L.; Bottomley, L.A.; Chem 1211k/1212k, Chemical Principles 1 & 2 Laboratory Manual, 2013-2014.
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