Boyles's Law

By Courtney Newman



  1. Get the gas pressure sensor ready to collect data.
  2. Prepare the computer now for the collecting of the data. Do this by opening the "06 Boyle's Law"
  3. To get the corrected volume about you will add .8 mL to your syringe amount.
  4. Once everything is ready to go press the collect button in logger pro.
  5. In between each collected data you pressure keep.
  6. Collect data for the following amounts: 5.0, 7.0, 9.0, 11.0, 13.0, 15.0, 17.0, and 19.0.
  7. Once the data is collect place it within a data table.
  8. Look at the relationship between volume and pressure and try out graphs till you have one you desirer.
  9. Now decide whether the graph is inverse or direct.
  10. With the best fit curve continue to complete lab questions.

What to look for?

Throughout this lab you will be observing the relationship between pressure and volume. When completing the data table and graph notice what the two do to each other. Know that the temperature throughout this experiment stays the same. Ask yourself some of the following questions to help you understand the procedure. Does one increase as the other decreases? Do they both increase together? Is it inverse or direct? What does one do to the other throughout the changes?

Data Table

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Some observations to notice during this experiment would be that when the volume increase the pressure decreases. When slowly increasing the volume a little at a time the pressure begins to decrease. Starting off at 5.8 mL the pressure was at its highest for the experiment being 177.76 kPa. But when the volume was increased to 19.8 mL by the end of the experiment the pressure was at its lowest point for the lab being 53.7 kPa. Following the dots on the logger pro and seeing the graph being created you can observe that this was an inverse graph. When looking through the data and watching the experiment you come to see that two variables change being the volume and pressure as the temp and mass stay constant throughout the experiment.


I've come to conclude that the relationship between pressure and volume are that of an inverse. When the volume increases the pressure decreases. When at the beginning this lab I thought that the relationship would be that of a direct, which would have the pressure and volume both increasing. But when observations were made and I watched the experiment connections between the two were much different then what I thought. I then understood that the relationship was inverse. The relationship can mathematically solved when using the equation of P x V = P x V. The new evidence that I have collected changed my thoughts and my conclusions as for now I understand how the pressure is increased when the volume is lower because the molecules in the gas start to collide. Through this collision process the pressure rises but, when the volume increases the collision process decreases causing the pressure to decrease.

Molecular Model

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