767 Words4 Pages

Purpose/Objective
The purpose of this experiment is to test the validity of Boyle’s Law. The objective is to determine the relationship between the pressure and volume of a confined gas.
Materials
Pencil Lab notebook Pressure sensor Syringe
Chemicals
Air
Data and Results
Volume (mL) Pressure (kPa) P/V PxV
5.0 mL 192.64 kPa 38.53 kPa/mL 963.20 kPa*mL
7.5 mL 136.13 kPa 18.13 kPa/mL 1020.96 kPa*mL
10.0 mL 104.54 kPa 10.45 kPa/mL 1045.40 kPa*mL
12.5 mL 83.50 kPa 6.68 kPa/mL 1043.75 kPa*mL
15.0 mL 70.51 kPa 4.70 kPa/mL 1057.65 kPa*mL
17.5 mL 60.37 kPa 3.45 kPa/mL 1056.48 kPa*mL
20.0 mL 53.22 kPa 2.66 kPa/mL 1064.40 kPa*mL
Boyle’s Law Plot
Sample Calculations
P/V:
53.22 kPa/20.0 mL = 2.66 kPa/mL
PxV:
53.22 kPa x 20.0 mL = 1064.40 kPa*mL
Discussion and Comments
This experiment was a simple and expedient method of proving Boyle’s law by demonstrating that pressure and volume have an indirect relationship. When the volume was doubled from 5.0 mL to 10.0 mL the pressure was nearly halved from 192.64 kPa to 104.54 kPa. When the volume is halved from 20.0 mL to 10.0 mL the pressure is almost doubled from 53.22 kPa to 104.54 kPa.
The relationship between the pressure and volume of a confined gas is inverse. The line of the graph is curved not straight. This indicates an indirect relationship. The amount of the gas and the temperature are assumed to be constant in this experiment. PV=k. Pressure is inversely proportional to volume.
The errors in this experiment were systematic due to not properly attaining the correct amount of gas in the syringe. For example, when the amount of gas was doubled from 5.0 mL to 10.0 mL, the pressure is halved and the reading should have been 96.32 kPa as opposed to 104.54 kPa.
This experiment correlated with the material present in our textbook in

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