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Particulates and Gases
Published in W. David Yates, Safety Professional’s Reference and Study Guide, 2020
Boyle’s law states that at a constant temperature, a fixed mass of gas occupies a volume that is inversely proportional to the pressure exerted upon it. Boyle’s law is written mathematically as P1V1=P2V2
Gases
Published in W. John Rankin, Chemical Thermodynamics, 2019
The combined gas law is a law that combines Boyle’s law (1662), Gay-Lussac’s law (~1700) and Charles’s law (1787). These laws each relate one thermodynamic variable (temperature, pressure and volume) to another mathematically while holding the third variable and the amount of gas constant. Boyle’s law: Pressure and volume are inversely proportional to each other at fixed temperature.Gay-Lussac’s law: Pressure and temperature are directly proportional to each other at fixed volume.Charles’ law: Volume and temperature are directly proportional to each other at fixed pressure.
Molecular Kinetic Theory of Gases and Its Implications
Published in Igor Bello, Vacuum and Ultravacuum, 2017
In a large range of pressures, Boyle’s law is valid only approximately. It can be shown that for different gases at higher pressures, deviations from Boyle’s law are considerable. The product pV is stable up to 5 MPa for hydrogen, but at the same conditions, the pV stability for air and carbon dioxide is satisfied with accuracy of only 3% and 10%, respectively. At higher pressures, all gases are less compressible. The gases whose behaviors can be described by Boyle’s law are considered to be ideal. At STP conditions such gases do not exist, but air and hydrogen exhibit behavior that is very close to the ideal gas properties. Oxygen, nitrogen, and all noble gases can still be classified in this gas group at STP conditions. At vacuum conditions, these gases may certainly be considered ideal.
Current devices used for the monitoring of injection pressure during peripheral nerve blocks
Published in Expert Review of Medical Devices, 2018
Boyle’s Law states that within a closed system containing a compressible gas, the product of the pressure and volume must remain equal (P1V1 = P2V2, where P1 and V1 are the original pressure and volume respectively, and P2 and V2 are the final pressure and volume) [21]. For example, if a syringe containing 10 ml of local anesthetic and 10 ml of air is closed to the atmosphere using a stopcock and the syringe plunger is depressed until the air bubble is reduced to half of its volume (5 ml), the pressure inside the syringe will double (Figure 2).