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Published byBirgitte Nygaard Modified over 5 years ago
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Gas Laws The atmosphere is made up of gases so we need to know the basic laws of how gases behave
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Gas laws describe the relationships between the key parameters describing the behavior of gases
Temperature (T): a measure of the kinetic energy (KE) of atoms and molecules. Expressed in °K for calculations. Pressure (P): F/A. Expressed in Pascal (N/m2), Newton per meter squared. Often in terms of hPa (100 N/m2) Density (r): r = Mass/Volume. Expressed in kg/m3 in the Metric system. At the earth’s surface r ~ 1 kg/m3 , 1 kg = 1000 grams~2.2 lbs Volume (V): Expressed in m3
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Boyle’s Law ~1660) PV=constant
Start with a sample of air with temperature (T), pressure (P), and volume (V). If T is kept constant, then: PV=constant
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Boyles Law Basis of air pumps we all use
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Law of Charles and Guy Lussac
If you increases temperature, while keeping pressure constant, volume will increase. V= constant (C)* T (°K) So if you increase T, V will increase Basis of car engines.
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Can combine both gas laws into one: the Perfect Gas Law (a. k. a
Can combine both gas laws into one: the Perfect Gas Law (a.k.a. the Ideal Gas Law) P= rRT Where r is density (kgm-3), R is a gas constant, P is pressure (Nm-2), and T is temperature (K) One of the key relationships of meteorology
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