57.5
0.1705
Equations and Example Calculations for Part 3:
Pressure/Volume
Overall Results:
From experiment 1, we know pressure is inversely proportional to volume.
In other words,
pressure is proportional to 1/volume. (Greater volumes corresponded to lower pressures and vice
versa.)
From experiment 2, we know pressure is proportional to the number of moles of an ideal gas.
(As the number of moles increased, pressure also steadily increased)
From experiment 3, we know pressure is proportional to temperature.
(As temperature
increased, so did the pressure)
Combining this we know that:
Pressure is proportional to the product of 1/volume, temperature,
and the number of moles.
In equation form we get:
Therefore:
Where K is some constant.
From the ideal gas law we know this constant is actually “R” or
8.314J/mol*K.
Therefore:
With simple algebra we multiply each side by “V” and get:
Discussion:
After completing each of the individual experiments and combining the results, the expected
resultant was reached.
The ideal gas law was at work, and was easily derived from our data as
shown in the
Results
section.
Because the desired result was arrived at, the experiment is clearly
well designed.
One possible improvement would be the utility of the DataStudio program.
It
wasn’t always immediately responsive or as detailed as one would expect, but ultimately it
delivered accurate data.
There is no apparent error as the experiment led to the proper derivation
of the ideal gas law.
What small deviations there were in the data can be attributed to minor
inaccuracies in the pressure/temperature measuring lab equipment, and simple human error.
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 Spring '12
 Dr.Phaneuf
 Physics

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