Dalton's Law

Dalton's law, also known as Dalton's law of partial pressures, states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas in the mixture.  According to this law, the partial pressure of a gas is the pressure that the gas would exert if it occupied the same volume alone at the same temperature.  The total pressure exerted by the mixture is the sum of these partial pressures. 

Dalton's law assumes that the gases in the mixture behave ideally, meaning that they do not interact or react with each other and occupy the same volume.  It is applicable to a wide range of conditions, including gases at different pressures and temperatures.  This law is particularly useful for understanding the behavior of gas mixtures and for calculating the composition or partial pressure of a specific gas within a mixture.  It finds applications in various fields, such as gas analysis, industrial processes, and atmospheric.  Both Dalton's law and Amagat's law predict the properties of gas mixtures.

 

Dalton's Law formula
\( P_{total} = P_1 + P_2 + P_3\; +...P_n  \)
Symbol	English	Metric
\( P_{total}  \) = Total Pressure of a Gas Mixture	\(lbf\;/\;in^2\)	\( Pa \)
\( P_1 P_2 P_3 ...P_n \) = Partial Pressures of the Individual Gas Components of the Mixture	\(lbf\;/\;in^2\)	\( Pa \)