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1. Partial Pressure

   Linked via "total pressure"

   Dalton's Law of Partial Pressures
   Dalton's Law posits that in a mixture of gases, the total pressure exerted is the sum of the partial pressures of the individual constituent gases. This additive relationship holds true provided the gases behave ideally, meaning that intermolecular forces are negligible and the volume occupied by the molecules themselves is insignificant compared to the container volume [1].
   Mathematically,…

2. Partial Pressure

   Linked via "total pressure"

   $$P{\text{Total}} = P1 + P2 + \dots + Pn = \sum{i=1}^{n} Pi$$
   The partial pressure of a specific gas ($Pi$) in an ideal gas mixture is directly proportional to its mole fraction ($xi$) in the mixture and the total pressure ($P_{\text{Total}}$):
   $$Pi = xi P_{\text{Total}}$$

3. Partial Pressure

   Linked via "total pressure"

   Partial Pressure and Gas Diffusion (Fick's First Law Modification)
   The diffusion of gases through a medium, such as air or biological membranes, is fundamentally driven by gradients in partial pressure rather than total pressure differences. Fick's First Law of Diffusion, when applied to gases, relates the molar flux ($Ji$) of component $i$ to the partial pressure gradient ($\nabla Pi$):
   …

4. Partial Pressure

   Linked via "total pressure"

   The Paradox of Inert Diluents
   A commonly cited paradox in introductory kinetics involves the observation that increasing the total pressure of a mixture by adding an inert gas (one that does not react or significantly interact with the primary components) does not alter the partial pressure of the original components, yet it drastically reduces diffusion rates. This is because while the driving force ($\nabla P_i$) remains unchanged, the [mean free path](/entries/mean-free-path…