SCIENCE
Storyboard Text
- CHEMISTRY CLASS
- GOODMORNING CLASS! I'M YOUR TEACHER IN CHEMISTRY CLASS.
- OUR TOPIC FOR TODAY IS ALL ABOUT BOYLE'S LAW. WHO AMONG YOU KNOWS ROBERT BOYLE?
- He performed an experiment wherein he trapped a fixed amount of air in the J-tube, he changed the pressure and controlled the temperature and then, he observed its effect to the volume of the air inside the J-tube. He found out that as the pressure is increased, the volume decreases. He finally concluded that the volume of a fixed amount of gas is inversely proportional to its pressure atconstant temperature.
- NO ONE? OKAY LET ME INTRODUCE TO YOU CLASS ROBERT BOYLE.
- The law can be derived from the kinetic theory of gases assuming a perfect (ideal) gas (see perfect gas). Real gases obey Boyle’s law at sufficiently low pressures, although the product pv generally decreases slightly at higher pressures, where the gas begins to depart from ideal behavior.
- Boyle’s law, also called Mariotte’s law, a relation concerning the compression and expansion of a gas at constant temperature. This empirical relation, formulated by the physicist Robert Boyle in 1662, states that the pressure (p) of a given quantity of gas varies inversely with its volume (v) at constant temperature; i.e., in equation form, pv = k, a constant. The relationship was also discovered by the French physicist Edme Mariotte (1676).
- Hope you learn something new in our class! See you next week, Goodbye Class!
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