Exploring Pressure-Volume Relationships
Results
Exploring Pressure-Volume Relationships
Table 1: Pressure vs. Volume of Container mL Torr
5
1417
7
1089
10
749
11
691.7
13
605.5
17
469.5
20
405.7
Chart 1:
Chart 2:
Part B
Table 2: Data for determining R
Mass Mg
Volume HCl
Volume Of Container
0.29 g
5 mL
144.544 mL
Temperature
Vapor Pressure
19.9℃
17.55 torr
Initial Pressure
Final Pressure
499.9 torr
692.2 torr
Part C
Experimental Design
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.
Chart 3:
Sample Calculations
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 …show more content…
This was done through a setup that helped to stabilize as many factors as possible to obtain a close value of R. The volume of the container and pressure sensor were measured as accurately as possible, and the temperature was kept as stable as possible by placing the system in a water bath at room temperature. When the HCl was added, the water added some vapor pressure, so the vapor pressure at the given temperature was found and subtracted from the total change in pressure. The only factor that could not be completely controlled was the temperature. The reaction of Mg and HCl is exothermic, so there would have been a small change in temperature in the container, which would have affected the
Exploring Pressure-Volume Relationships
Table 1: Pressure vs. Volume of Container mL Torr
5
1417
7
1089
10
749
11
691.7
13
605.5
17
469.5
20
405.7
Chart 1:
Chart 2:
Part B
Table 2: Data for determining R
Mass Mg
Volume HCl
Volume Of Container
0.29 g
5 mL
144.544 mL
Temperature
Vapor Pressure
19.9℃
17.55 torr
Initial Pressure
Final Pressure
499.9 torr
692.2 torr
Part C
Experimental Design
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.
Chart 3:
Sample Calculations
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 …show more content…
This was done through a setup that helped to stabilize as many factors as possible to obtain a close value of R. The volume of the container and pressure sensor were measured as accurately as possible, and the temperature was kept as stable as possible by placing the system in a water bath at room temperature. When the HCl was added, the water added some vapor pressure, so the vapor pressure at the given temperature was found and subtracted from the total change in pressure. The only factor that could not be completely controlled was the temperature. The reaction of Mg and HCl is exothermic, so there would have been a small change in temperature in the container, which would have affected the