Boyle's law: Explanation, Limitations and Applications - Explained Details (Animation)
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Boyle's law
Chapters:
0:00 Kinetic school's intro
0:11 About Robert Boyle
0:29 Boyle's Experiment
2:21 Boyle's Observation
2:34 Boyle's Law
3:34 Graphical Representation of Boyle's law
3:59 Limitations of Boyle's Law
5:03 Applications of Boyle's law
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Robert Boyle:
In the seventeenth century, Anglo-Irish Chemist and Physicist Robert Boyle studied the relationship between the pressure and the volume of a gas systematically and quantitatively.
Boyle's Law:
The pressure (P) of a fixed amount of gas maintained at constant temperature is inversely proportional to the volume (V) of the gas.
Therefore,
P ∝ 1 / V
or, PV = k, T & n constant
where, P is pressure, V is volume, k is a constant, and the temperature (T) and amount of gas (n) are held constant.
When a fixed amount of gas, at constant temperature changes from pressure Pi and volume Vi to pressure Pf and volume Vf,
then, PiVi = PfVf
Limitations of Boyle's Law:
• Boyle's law is applicable only to ideal gases.
• The law holds good only at moderate temperatures and pressures.
• The law fails at high pressures and low temperature.
Applications of Boyle's law:
• Pushing Syringe
• Activity of Human lungs
• Bicycle or Ball pumper
• Deep-sea fish • Space
• Scuba Diving
Photo credit: krisztian matyas on unsplash.
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