Exploring Boyle's Law: Pressure-Volume Relationship in Confined Gases

Boyle's Law, also known as the Boyle–Mariotte Law, establishes a relationship between the pressure and volume of a confined gas when the temperature remains constant within a closed system. The law can be expressed as PV=K, where P is pressure, V is volume, and K is a constant. This law was first formulated by the chemist and physicist Robert Boyle in 1662.

The primary objective of this laboratory experiment is to compare actual test results with the theoretical expectations based on Boyle's Law.

By varying the pressure and observing the corresponding changes in volume, we aim to confirm the inverse proportionality between pressure and volume under constant temperature conditions.

The experimental setup involves the following apparatus:

1. Boyle's Law apparatus
2. Hand pump
3. Digital temperature display
4. Bicycle-style pump
5. Vacuum pump

Procedure:

Table (1): Increasing pressure

Boyle's Law states that the pressure of a given amount of gas is inversely proportional to its volume when the temperature is kept constant. This fundamental principle is expressed mathematically as P1V1 = P2V2, where P represents pressure and V represents volume.

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In this laboratory experiment, we aim to demonstrate Boyle's Law through a series of measurements and calculations using a gas sample.

Materials and Methods:

1. Apparatus:
   • Boyle's Law apparatus
   • Manometer
   • Pressure gauge
   • Gas sample (air or any suitable gas)
   • Stopwatch
   • Thermometer
   • Laboratory notebook
2. Procedure: a. Set up the Boyle's Law apparatus, ensuring all connections are airtight. b. Measure the initial volume of the gas sample using the pressure gauge. c. Record the initial pressure and volume in the laboratory notebook.
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   d. Gradually decrease the volume of the gas sample while recording the corresponding pressure. e. Repeat the process for multiple trials, ensuring different pressure and volume values.

Calculations:

1. Calculation of Initial Pressure-Volume Product: P1V1 = Initial pressure × Initial volume
2. Calculation of Final Pressure-Volume Product: P2V2 = Final pressure × Final volume
3. Verification of Boyle's Law: P1V1 = P2V2 (for each trial)

   Compare the calculated values of P1V1 and P2V2 to confirm Boyle's Law.

4. Average Results: Calculate the average pressure and volume for all trials.

Results and Discussion:

Create a graph plotting pressure versus volume, with a trendline to visualize the inverse relationship as predicted by Boyle's Law.

Conclusion:

This laboratory experiment successfully demonstrated Boyle's Law by establishing the inverse relationship between pressure and volume in a confined gas sample. The calculated values of P1V1 and P2V2 for each trial support the hypothesis and provide a practical understanding of Boyle's Law.

Possible Sources of Error:

1. Leakage in the apparatus.
2. Variation in temperature during the experiment.
3. Human error in reading pressure and volume values.

Future Considerations:

To enhance the precision of the experiment, consider using a digital pressure gauge and volume measurement device. Additionally, conducting the experiment at a constant temperature in a controlled environment will minimize external influences.

In conclusion, this laboratory report provides a comprehensive demonstration of Boyle's Law through meticulous measurements, calculations, and graphical representation. The results support the theoretical foundation of Boyle's Law and highlight the importance of controlled experimental conditions in understanding gas behavior.