Boyle’s Law Experiment for Schools, Teachers, and Students
Boyle’s Law states that at constant temperature, the pressure of a fixed amount of gas is inversely proportional to its volume.
Mathematically:
P ∝ 1/V
or
PV = constant
Where:
- P: Pressure of the gas (in Pa or atm)
- V: Volume of the gas (in m³ or L)
- The temperature and amount of gas remain constant.
Equation of Boyle’s Law:
For two states of the gas at constant temperature:
P1V1 = P2V2
Where:
- P1, V1: Initial pressure and volume
- P2, V2: Final pressure and volume
Graphical Representation of Boyle’s Law:
- Pressure-Volume (P-V) Graph: The P-V graph is a hyperbola because pressure and volume are inversely proportional.
P ∝ 1/V - Pressure vs. 1/V Graph: The graph of pressure (P) vs. reciprocal volume (1/V) is a straight line passing through the origin.
Key Points:
- As the volume of a gas decreases, its pressure increases, provided the temperature remains constant.
- Boyle’s law is valid only for ideal gases under isothermal (constant temperature) conditions.
Real-Life Applications of Boyle’s Law:
- Syringes and Pumps: When the plunger of a syringe is pulled, the volume inside increases, reducing the pressure, which causes fluid to be drawn into the syringe.
- Breathing Mechanism: During inhalation, the volume of the lungs increases, reducing the pressure inside the lungs, allowing air to flow in.
- Scuba Diving: As a diver descends, water pressure increases, compressing the volume of air in their lungs and equipment.
- Air Compression: Boyle’s law is used in air compressors where air is compressed to reduce its volume, increasing the pressure.
Observations:
- When volume decreases, pressure increases.
- When volume increases, pressure decreases.
- Boyle’s law applies only to ideal gases and is valid under isothermal conditions.
