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An experiment aimed at studying the relationship between the pressure and volume of an air sample at constant temperature. An introduction to boyle's law and the ideal gas law, details the experimental procedure, and suggests an analysis process to determine the constant in boyle's law. The document also includes a data table for the experiment.
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General Physics I
EXPERIMENT 11 BOYLE’s LAW
I. INTRODUCTION The objective of this experiment is to study the relationship between the pressure and volume of an air sample at constant temperature. This will be done by measur- ing the pressure of a constant amount of air contained in a cylinder as the volume of the air is varied. The results will be compared with the predictions of Boyle’s law and the ideal gas law.
II. THEORY Boyle’s law states that, for constant temperature, the product of the volume and the pressure of an ideal gas is a constant.
PV = C (1)
The ideal gas law PV = nRT (2)
states that this constant (nRT) is proportional to the amount of ideal gas in the sam- ple (the number of moles, n) and the absolute temperature, T. The constant R in this equation is the universal gas constant which has a value of R = 8.31 J/(mole.K) in SI units. Note that if T is held constant throughout the experiment, then the ideal gas law reduces to Boyle’s law.
Pressure sensor, syringe and computer.
IV. EXPERIMENTAL PROCEDURE
n =
where R = 8.31 J/(mole.K) and T is the absolute temperature.
P 1 V 1 T 1
Experiment (11) Data Table
Volume of Air Sample V (cm^3 )
Pressure P (kPa)
Average value of PV in Joules, C =
Number of moles in the air sample, n = (^) RTC =
V 1 = 20.0 cm^3 V 2 =
Room Pressure, P 1 = 1.0 atm P 2 = 1.0 atm
Room Temperature, T 1 = T 2 = 273 K
Number of Moles, n = V^2 22, 400 cm^3