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| {{for|the law of stoichiometry|Law of multiple proportions}}
| | The writer is known as Irwin Wunder but it's not the most masucline name out there. What I love performing is to gather badges but I've been taking on new issues recently. Since she was 18 she's been working as a meter reader but she's always wanted her personal company. For a while I've been in South Dakota and my parents reside nearby.<br><br>Look at my homepage; [http://Ece.Modares.Ac.ir/mnl/?q=node/1015651 at home std testing] |
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| {{unreferenced|date=February 2013}}
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| In [[chemistry]] and [[physics]], '''Dalton's law''' (also called '''Dalton's law of partial pressures''') states that '''the total [[pressure]] exerted by the mixture of non-reactive gases is equal to the sum of the [[partial pressure]]s of individual gases.''' This [[empirical]] law was observed by [[John Dalton]] in 1801 and is related to the [[ideal gas|ideal]] [[gas laws]].
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| Mathematically, the pressure of a mixture of gases can be defined as the summation
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| :<math>P_{\text{total}} = \sum_{i=1} ^ n {p_i}</math> or <math>P_{\text{total}} = p_1 +p_2 + \cdots + p_n</math>
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| where <math>p_{1},\ p_{2},\dots,\ p_{n}</math> represent the partial pressure of each component.
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| It is assumed that the gases do not [[chemical reaction|react]] with each other
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| :<math>\ p_{i} =P_{\text{total}}y_i </math>
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| where <math>y_i</math> is the [[mole fraction]] of the i-th component in the total mixture of ''n'' components .
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| The relationship below provides a way to determine the [[concentration|volume based concentration]] of any individual gaseous component
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| :<math>P_i =\frac{P_{\text{total}}C_i}{1,000,000}</math>
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| where <math>C_i</math> is the concentration of the i-th component expressed in [[Parts per million|ppm]].
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| Dalton's law is not exactly followed by real gases. Those deviations are considerably large at high pressures. In such conditions, the volume occupied by the molecules can become significant compared to the free space between them. In particular, the short average distances between molecules raises the intensity of [[intermolecular force]]s between gas molecules enough to substantially change the pressure exerted by them. Neither of those effects are considered by the ideal gas model.
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| ==See also==
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| {{portal|Underwater diving}}
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| * [[Henry's law]]
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| * [[Amagat's law]]
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| * [[Boyle's law]]
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| * [[Combined gas law]]
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| * [[Gay-Lussac's law]]
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| * [[Mole (unit)]]
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| * [[Partial pressure]]
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| * [[Raoult's law]]
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| * [[Vapour pressure]]
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| {{Distillation}}
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| {{Diving medicine, physiology and physics}}
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| [[Category:Gas laws]]
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| [[Category:Distillation]]
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| [[Category:Physical chemistry]]
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| [[Category:Chemical engineering]]
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| [[de:Partialdruck#Dalton-Gesetz]]
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| [[et:Daltoni seadus]]
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The writer is known as Irwin Wunder but it's not the most masucline name out there. What I love performing is to gather badges but I've been taking on new issues recently. Since she was 18 she's been working as a meter reader but she's always wanted her personal company. For a while I've been in South Dakota and my parents reside nearby.
Look at my homepage; at home std testing