John
Dalton visualised that in a mixture of gases, each component gas exerted a pressure as if it were alone in the container. The individual pressure of each gas in the mixture is defined as its Partial Pressure. Based on experimental evidence, in 1807, Dalton enunciated what is commonly known as the Dalton's Law of Partial Pressures. It states that:Daltons law of partial pressure
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The total pressure of a mixture of gases is equal to the sum of the partial pressures of all the gases present.
Mathematically the law can be expressed as Protal = P₁ + P₂ + P3... (V and T are constant) where P. P₂ and P, are partial pressures of the three gases 1, 2 and 3; and so on. 3
Dalton's Law of Partial Pressures follows by application of the ideal-gas equation PV = n RT separately to each gas of the mixture. Thus we can write the partial pressures P₁, P₂ and P3 of the three gases
P1 = n1 (RT/V)
P2 = n2 (RT/V)
P3 = n3(RT/V)
where n₁, n, and n₂ are moles of gases 1, 2 and 3. The total pressure, P, of the mixture is
P=(n1+n2+n3)RT/V
P = nRT/V
In the words, the total pressure of the mixture is determined by the total number of moles present whether of just one gas or a mixture of gases.
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