Ideal (general) gas law
Summary of Ideal (general) gas law
The general gas law explains the relationship of a gas’s temperature, volume, and pressure. The equation is PV = nRT where P is pressure, V is volume, n is mols, R is the gas constant, and T is temperature. In the lungs, for example, if temperature was increased then the pressure would also increase if volume was held constant.
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Physiology
Respiratory system
Anatomy and physiology
Lung volumes and capacities
Breathing mechanics
Ventilation and perfusion
Airflow and gas exchange
Gas transport
Regulation of breathing
Physiologic adaptations of the respiratory system
High Yield Notes
8 pages
![NOTES NOTES GAS EXCHANGE GAS EXCHANGE & LAWS ▪ Diffusion of oxygen (O2), carbon dioxide (CO2) in lungs, peripheral tissues ▪ Alveolar O2 from inhaled gas → pulmonary capillary blood → circulation → tissue capillaries → cells ▪ CO2 from cells → tissue capillaries → circulation → pulmonary capillary blood → CO2 for exhalation from alveoli ▪ Gas exchange, gas behavior in solution is governed by fundamental physical gas properties → represented by gas laws FORMS OF GAS IN SOLUTION Dissolved gas ▪ All gas in solution are to some extent carried in a freely dissolved form ▪ For given partial pressure, the higher the solubility of a gas, the higher the concentration in solution ▪ In solution only dissolved gas molecules contribute to partial pressure ▪ Of the gases inspired as air, only nitrogen is exclusively carried in dissolved form Bound gas ▪ O2, CO2, CO are bound to proteins in blood ▪ O2, CO2, CO can all bind to hemoglobin ▪ CO2 also binds to plasma proteins Chemically modified gas ▪ The ready back and forth conversion of CO2 to bicarbonate (HCO3-) in presence of enzyme carbonic anhydrase allows CO2 to contribute to gas equilibria despite chemical conversion ▪ Majority of CO2 in blood carried as HCO3- IDEAL (GENERAL) GAS LAW osms.it/ideal-gas-law ▪ Relates multiple variables to describe state of a hypothetical “ideal gas” under various conditions ▫ Ideal gas: theoretical gas composed of many randomly moving point particles whose only interactions are perfectly elastic collisions ▫ All gas laws can be derived from general gas law ▪ PV = nRT ▫ P = Pressure (millimeters of mercury (mmHg) ▫ V = Volume (liters (L) ▫ n = Moles (mol) ▫ R = Gas constant (8.314 J/mol) ▫ T = Temperature (Kelvin [K]) ▪ In gas phase: body temperature, pressure (BTPS) used ▫ T = 37°C/98.6°F/310K ▫ P = Ambient pressure ▫ Gas is saturated with water vapor (47mmHg) ▪ In liquid phase/solution: standard temperature, pressure (STPD) used ▫ T = 0°C/32°F/273K ▫ P = 760mmHg ▫ Dry gas (no humidity) ▪ Ideal gas law can be used to interconvert between properties of same gas under BTPS, STPD conditions ▫ E.g. gas volume (V1) at BTPS → gas volume at STPD (V2) OSMOSIS.ORG 603](https://d16qt3wv6xm098.cloudfront.net/Vac47DeSTHa4YINc2NXmx6EqSyKPmG5x/thumb-1.jpg)
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