CRNA Prep
| Content | An ideal gas exerts {{c1::no}} pressure and has {{c1::no}} volume at {{c1::0}} degrees Kelvin. Boyle's Law - pressure and volume are {{c2::inversely}} related with the equation {{c2::PV = Constant}} or {{c2::PV = P1V1}}. Example: An ideal gas at 760 mmHg has a volume of 22.4 liters. If the pressure is increased to 1520 mmHg the new volume will be {{c3::11.2}} liters. Gases always flow from areas of high pressure to areas of {{c3::low}} pressure. By decreasing the volume of the reservoir bag we {{c4::increase}} the pressure in the bag and anesthetic gases flow from the machine to the {{c4::patient's lungs}}. |
| Note | |
| Mnemonics | |
| Extra | |
| Cloze99 |
| Content | Equal volumes of gases under the same conditions of temperature and pressure contain the {{c1::same number of molecules}}. There are {{c1::6.02 x 10²³}} molecules in {{c1::one mole}} of any substance. A mole is the {{c2::molecular weight}} of a substance expressed in {{c2::grams}}. At standard temperature and pressure (0° C and 1 atmosphere) one mole of gas will occupy {{c3::22.4}} liters of volume ({{c3::22.71}} L using SI units). |
| Note | |
| Mnemonics | |
| Extra | |
| Cloze99 |
| Content | Pascal (Pa) = {{c1::1 Newton/square meter}}. The pascal represents a {{c1::very small}} pressure and {{c1::kilopascals (Kpa)}} is more commonly used to express common pressures. 100 kPa = {{c2::1}} bar ({{c2::0.987}} atm); 1 atm = {{c2::1.013}} bar. Atmospheric pressure is the result of {{c3::gravity}} pulling on the {{c3::atmosphere}}. |
| Note | |
| Mnemonics | |
| Extra | |
| Cloze99 |