{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Scan_Doc0107

# Scan_Doc0107 - 5.5 Dalton's Law of Partial Pressures 199...

This preview shows page 1. Sign up to view the full content.

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 Lawof 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 ••. Dalton's Law of Partial Pressures
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

Ask a homework question - tutors are online