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Boyle’s Law Lab (Alternate)
Introduction
Boyle’s law explains the relationship between the pressure and volume of an ideal gas when the temperature
and amount of gas inside a container remain constant. The purpose of this lab is to investigate the relationship
between the volume of a container and the pressure of the gas inside the container.
Procedure
1. You may recall that Boyle’s law states that the product of the pressure and volume of an ideal gas is
equal to a constant.
2. The equation that describes Boyle’s Law is
in liters, and k is a constant.
, where P is pressure in atmospheres, V is volume
3. If k is a constant, how will a change in volume change the pressure? One way to think about this is to
choose an arbitrary number to represent k. For example, assume that k always equals 12. What numbers
can be multiplied together to equal 12?
Choose one set of numbers. Assign one of them to represent P and the other to represent V. What
happens to P if V is assigned the larger number? What happens to P if V is assigned the lower number?
Observe the relationship between P and V. Is it a directly proportional relationship or an inversely
proportional relationship?
4. Conducting an experiment that holds the number of particles of a gas and the temperature constant
would allow for an investigation into how volume and pressure are related. Assume 200 particles of a
heavy species gas are pumped into a container that has an adjustable volume.
5. The addition of 200 particles of gas initially results in a pressure of 1.00 atm.
6. The temperature inside the container is 300 K.
7. As the volume is adjusted, the number of particles and the temperature do not change, but the pressure
does.
8. The product of the volume and pressure must stay constant. Predict what will happen to the pressure if
the volume is decreased.
9. The following table shows the data gathered during an experiment with a heavy gas species. Complete
the table by calculating the constant, k.
Heavy Gas Species
Volume (L)
Pressure (atm)
6.00
1.12
5.40
1.29
3.80
1.72
8.00
0.85
10. Assume that the experiment is repeated with 200 particles of a light gas species at a temperature of 300
K. The following table shows the data gathered. Complete the table by calculating the constant, k.
Light Gas Species
Volume (L)
Pressure (atm)
6.00
1.04
5.40
1.15
3.80
1.57
8.00
0.78
Analyze
1. Based on the data, what happens to the pressure of the gas as the volume increases?
2. Look up Boyle’s law in a science textbook. How do the results of the experiment support or contradict
Boyle’s law?
3. Go back to the data tables. Good data may show minor variations, but the values for k should remain
relatively consistent.
What is the average value of k for the heavy gas species?
What is the average value of k for the light gas species?
How does the molecular weight of the gas affect the k-value?
4. Based on the results of this lab, develop a hypothesis to explain why bubbles exhaled by scuba divers
grow in size as they reach the surface of the ocean.
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