Figure5.l.2The partial pressure of each gas in amixture of gases in a container dependson the number of moles of that gas. Thetotal pressure is the sum of the partialpressures and depends on the totalmoles of gas particles present, no matterwhat they are. Note that the volume re-mains constant.5.5Dalton's LawofPartialPressures199How do we get there?(1.95~)(0 082061::; •atrr1)• Molar mass=dRT=1::;'R .mol(300.R)P1.50aan=32.0g/molRealityCheck:These are the units expected for molar mass.SEEEXERCISES5.75THROUGH5.78You could memorize the equation involving gas density and molar mass, but it is bettersimply to remember the ideal gas equation, the definition of density, and the relationshipbetween number of moles and molar mass. You can then derive the appropriate equationwhen you need it. This approach ensures that you understand the concepts and means oneless equation to memorize.5.5 ••.Dalton's Law of Partial Pressures
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