Science, Tech, Math › Science What Is Dalton's Law of Partial Pressures? Pressures in a Gas Mixture Share Flipboard Email Print ThoughtCo / Max Dodge Science Chemistry Chemical Laws Basics Molecules Periodic Table Projects & Experiments Scientific Method Biochemistry Physical Chemistry Medical Chemistry Chemistry In Everyday Life Famous Chemists Activities for Kids Abbreviations & Acronyms Biology Physics Geology Astronomy Weather & Climate By Todd Helmenstine Todd Helmenstine is a science writer and illustrator who has taught physics and math at the college level. He holds bachelor's degrees in both physics and mathematics. our editorial process Todd Helmenstine Updated January 09, 2019 Dalton's law of partial pressures is used to determine the individual pressures of each gas in a mixture of gases. Dalton's Law of Partial Pressures The total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases. PressureTotal = PressureGas 1 + PressureGas 2 + PressureGas 3 + ... PressureGas n An alternative of this equation can be used to determine the partial pressure of an individual gas in the mixture.If the total pressure is known and the moles of each component gas are known, the partial pressure can be computed using the formula: Px = PTotal ( nx / nTotal ) where: Px = partial pressure of gas x PTotal = total pressure of all gases nx = number of moles of gas x nTotal = number of moles of all gases This relationship applies to ideal gases but can be used in real gases with very little error. Deviations From Dalton's Law Dalton's law is an ideal gas law. It is only an approximation for real gases. The deviation from the law increases with increasing pressure. At high pressure, the volume occupied by a gas becomes significant when compared to the free space between particles. At high pressure, intermolecular forces between particles become more of a consideration. Sources Dalton, J. (1802). "Essay IV. On the expansion of elastic fluids by heat." Memoirs of the Literary and Philosophical Society of Manchester, vol. 5, pt. 2, pp. 595–602.Silberberg, Martin S. (2009). Chemistry: the molecular nature of matter and change (5th ed.). Boston: McGraw-Hill. p. 206. ISBN 9780073048598.