Figure 5.l.2 The partial pressure of each gas in a mixture of gases in a container depends on the number of moles of that gas. The total pressure is the sum of the partial pressures and depends on the total moles of gas particles present, no matter what they are. Note that the volume re-mains constant. 5.5 Dalton's Law of Partial Pressures 199 How do we get there? ( 1.95~)(0 08206 1::; • atrr1) • Molar mass = dRT = 1::;' R . mol (300. R) P 1.50aan = 32.0 g/mol Reality Check: These are the units expected for molar mass. SEE EXERCISES 5.75 THROUGH 5.78 You could memorize the equation involving gas density and molar mass, but it is better simply to remember the ideal gas equation, the definition of density, and the relationship between number of moles and molar mass. You can then derive the appropriate equation when you need it. This approach ensures that you understand the concepts and means one less equation to memorize. 5.5 ••.
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This note was uploaded on 12/13/2010 for the course CHEM 2301 taught by Professor Bill during the Spring '10 term at South Texas College.